**Raw Materials for Production of SrAC**

() (,) (,)

An essential difference between the CDV mechanism and the Arrhenius activation mechanism is that during the interface reactions, a proportion of the energy released on condensation of a non-volatile product is transferred to the solid reactant, reducing the energy barrier for further reactant volatilization. Thus, 'recycled' energy is responsible for the autocatalytic

**•** Models identifying the preferred occurrence of chemical change at reactant/product contact interfaces with (uncharacterized, qualitative) 'strain', 'catalysis of by product', etc., can now

**•** Autocatalytic behaviour, resulting from the redistribution of product condensation energy, occurs when the decomposition proceeds at a reactant/product contact interface. Reactions

**•** Because the energy transfer is responsible for the autocatalysis, the variations in *τ*, found for a number of diverse substances, are identified with supersaturation of the non-volatile

The simplest presumption for the energy redistribution at an interface is that the condensation energy is shared equally between the reactant and the solid products, which is expressed as τ=0.5. The deviations, where *ΔcH*° is distributed unequally between the solid reactant and the product phases in the ratio *τ*/(1-*τ*), are ascribed to the degree of supersaturation of the non-

The Arrhenius model is often represented by the familiar graph of energy variations as the reaction progresses by the "Advance along the Reaction Coordinate". This shows an initial rise to a maximum value, to form the 'transition complex', being followed by a decline thereafter. The activation energy is then the energy required for forming the 'activated' tran‐ sition complex in an assumed "rate-determining step". However, in CDV theory, the value

be discarded as providing no insights into the reaction controls and mechanisms.

yielding non-condensed (non-volatile) product transfer no energy, so that *τ*=0.

component rather than the chemical properties of the different original reactants.

o o (125)

*H T a H AT b H BT*

(,) (,) t

oo o

D =D +D

*c H CT a H AT*

*f c*

For the majority of substances, the condition *τ*=0.5 can be applied [89,90].

*rc f f*

44 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications


behaviour, justifying the following important generalizations [70]:

of parameter *E* represents the vaporization enthalpy [70].

volatile vapor.

## **1. Raw Materials and Raw Material Treatment**

For the synthesis of strontium aluminate cement it is necessary to find the proper source of strontium (SrO) and aluminium oxide (Al2O3).

Two major strontium minerals are its carbonate, strontianite (SrCO3) and more abundant sulfate mineral celestite (SrSO4). William Cruickshank in 1787 and Adair Crawford in 1790 independently detected strontium in the strontianite mineral, small quantities of which are associated with calcium and barium minerals. They determined that the strontianite was an entirely new mineral and was different from barite and other barium minerals known in those times. In 1808, Sir Humphry Davy isolated strontium by the electrolysis of a mixture of moist strontium hydroxide or chloride with mercuric oxide, using mercury cathode. The element was named after the town Strontian in Scotland where the mineral strontianite was found [91].

The **strontium oxide** (SrO) is the first substantial component of strontium aluminate clinker. Therefore, the strontium carbonate (SrCO3) is the most appropriate input material for the synthesis of strontium aluminate clinker. In nature SrCO3 occurs as rare orthorhombic min‐ eral **strontianite**<sup>1</sup> (space group *Pcmn*) and together with isostructural minerals aragonite (CaCO3), witherite (BaCO3) and cerussite (PbCO3) it belongs to anhydrous carbonates from the group of aragonite2 [92,93].

The structure of strontianite (Fig.1(a)) is based on isolated [CO3] 2-triangles which are placed in layers perpendicular to *c*-axis. The layer has two structural planes where [CO3] 2-ions are oriented in the opposite direction. Cations with the coordination number of 9 are placed be‐ tween these layers.

Natural and artificially synthesized binary (**aragonites** up to 14 mol. % Sr [94], **strontianites** up to 27 % Ca [94], **witherites** [94], **baritocalcites** [95]) or ternary solid-solutions (**alstonites** [94]) of these carbonates are intensively studied in order to elucidate the mechanism of their formation, their structure, the thermodynamic stability and the luminescence properties.

<sup>2</sup> There are three main groups of anhydrous carbonates without additional anions. The group of calcite (trigonal, space group R3 ¯c, A = Ca, Mg, Mn, Fe, Co, Ni, Zn and Cd) and aragonite (orthorhombic, space group Pmnc, A = Ca, Sr, Ba and Pb) has the composition given by general formula ACO3. The trigonal group of dolomite (space group R3 ¯ where A = Ca and B = Mg, Fe, Mn and Zn) has general composition given by the general formula AB(CO3)2.

© 2014 The Author(s). Licensee InTech. This chapter is distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

<sup>1</sup> Discovered in 1787 (Strontian, Scotland). Originally was considered the barium bearing mineral; which was dis‐ proved by Crawford and later by Klaproth and Kopp. Named in 1791 by Friedrich Gabriel Sulzer after the locality Strontian in Scotland.

tioned above, also celestite and barite (BaSO4) coexist in the marine environment with significant fractions of Sr and Ba in solid solutions. Therefore it is better to identify barite

The second substantial component of strontium aluminate cement is **aluminium oxide** (Al2O3). The most stable crystalline form of Al2O3 is the polymorphic modification of hexag‐

¯ C space group5

type is typical for other oxides, such as **hematite** (Fe2O3), **eskolaite** (Cr2O3), **karelianite** (V2O3) and **tistarite** (Ti2O3). Therefore, naturally occurring minerals are often colored by the admixture of these elements, e.q. ruby is red colored by Cr and blue sapphire by Fe and Ti. That means that these elements are also interesting from the point of view of modification the properties (course of sintering, hydration and setting) of strontium aluminate cement.

Pure aluminium oxide is relatively rare, but single crystals of gemstones such as sapphire (colorless) or ruby (red due to the content of chromium) can be found in nature [424]. Indus‐ trial production of Al2O3 is based on the Bayer process of bauxite. The main part of pro‐ duced alumina is used in metal industry for the production of aluminium by Hall-Heroult

The application of Al2O3 in ceramics includes the production of alumina porcelain and alu‐ mina oxide ceramics, ZTA (Zirconia Toughened Alumina) ceramics and the applications such as electroceramics, construction ceramics, shaped and unshaped refractory products, abrasive materials, etc [106-112]. From the point of view of the volume of production, poly‐ crystalline alumina is the most frequently used material as ceramics for the structural appli‐ cations. However, in comparison with for example, silicon nitride (Chapter 6), where the influence of various additives on the microstructure and properties is well characterized and understood, alumina remains the material with many unknown factors yet to be revealed.

**• Solid-state sintered aluminas:** enable to prepare nanocrystalline materials with excellent mechanical properties and well-sintered ceramics being transparent to visible light

**• Liquid-phase sintered aluminas (LPS):** are substantial part of industrially produced alu‐ mina-based materials. Silica, alkali oxides and oxides of alkali earth metals are used as

**• Alumina-based composites:** ZTA and alumina based nanocomposites with non-oxide

The preparation of Al2O3 mono-crystals is based on **Verneuil process** consisting in the flame fusion in high temperature region from 1500 to 2500 °C [124-127]. Bauxite (Fig.3) is also used

4 Barite – celestite series from the group of barite. Anhydrous sulfates without additional anions with the composition

Alumina based materials can be roughly divided into three groups [424]:

. The crystal structure of corundum

Raw Materials for Production of SrAC 47

suspended in seawater as the strontian barite (SrxBa1-xSO4) [101].

onal corundum (**α**-Al2O3) from the R 3

Process [102-105].

[113,114].

sintering additives [115-117].

phases such as SiC or TiC [118-123].

given by general formula ASO4, where A = Pb, Ba, Sr.

5 Structure and lattice parameters of corundum are described in Chapter 4.1.

Chapters 4 and 5 are dedicated to this topic [424].

**Figure 1.** Structure of strontianite consists of isolated [CO3] 2-triangles arranged into layers with Sr2+ions in the space between layers.

Calcium carbonate minerals include considerable amount of strontium from seawater as they precipitate. It stands to reason that the solid-solutions of strontianite with calcite and aragonite (CaxSr1-xCO3) are the most explored. There is an immiscibility gap in the range 0.12 (aragonites) < *x* < 0.87 (strontianites) under ambient conditions, which disappears at the tem‐ perature of ~107 °C [92,94,96,97-100].

Therefore natural sources of SrCO3 are rare and have no industrial importance, strontium carbonate as well as other compounds such as strontium nitrate, strontium oxide and chlor‐ ide are prepared from the orthorhombic mineral **celestite**<sup>3</sup> (SrSO4, space group *Pnma* with cell unit parameters *a*=8.359 Å, *b*=5.352 Å, *c*=6.686 Å and *Z*=4) using the techniques descri‐ bed in Chapter 2.1.1. The structure of celestite consists of isolated [SO4]2-tetrahedrons and Sr2+ions (Fig.2).

Figure 2. Structure of celestite (a) and distribution of large celestite deposits in the world (b). **Figure 2.** Structure of celestite (a) and distribution of large celestite deposits in the world (b).

aluminate cement. Chapters 4 and 5 are dedicated to this topic [424].

hexagonal CORUNDUM (

**HEROULT PROCESS** [102-105].

Celestite together with isostructural barite (BaSO4) and anglesite (PbSO4) belong to anhydrous sulfates from the group of barite4. Similarly to the solid solutions of carbonates mentioned above, also celestite and barite (BaSO4) coexist in the marine environment with Celestite together with isostructural barite (BaSO4) and anglesite (PbSO4) belong to anhy‐ drous sulfates from the group of barite4 . Similarly to the solid solutions of carbonates men‐

significant fractions of Sr and Ba in solid solutions. Therefore it is better to identify barite

(Al2O3). The most stable crystalline form of Al2O3 is the polymorphic modification of

corundum type is typical for other oxides, such as **hematite** (Fe2O3), **eskolaite** (Cr2O3), **karelianite** (V2O3) and **tistarite** (Ti2O3). Therefore, naturally occurring minerals are often colored by the admixture of these elements, e.q. ruby is red colored by Cr and blue sapphire by Fe and Ti. That means that these elements are also interesting from the point of view of modification the properties (course of sintering, hydration and setting) of strontium

Pure aluminium oxide is relatively rare, but single crystals of gemstones such as sapphire (colorless) or ruby (red due to the content of chromium) can be found in nature [424]. Industrial production of Al2O3 is based on the **BAYER PROCESS** of bauxite. The main part of produced alumina is used in metal industry for the production of aluminium by **HALL-**

The application of Al2O3 in ceramics includes the production of alumina porcelain and alumina oxide ceramics, ZTA (Zirconia Toughened Alumina) ceramics and the applications such as electroceramics, construction ceramics, shaped and unshaped refractory products, abrasive materials, etc [106-112]. From the point of view of the volume of production, polycrystalline alumina is the most frequently used material as ceramics for the structural

4 Barite – celestite series from the group of barite. Anhydrous sulfates without additional

anions with the composition given by general formula ASO4, where A = Pb, Ba, Sr.

5 Structure and lattice parameters of corundum are described in Chapter 1.2.


suspended in seawater as the strontian barite (SrxBa1-xSO4) [101]. The second substantial component of strontium aluminate cement is **aluminium oxide** 3 Discovered in 1791 and named in 1799 by Abraham Gottlieb Werner from the Greek "cœlestis," for celestial, in allu‐ sion to the faint blue color of the original specimen.

tioned above, also celestite and barite (BaSO4) coexist in the marine environment with significant fractions of Sr and Ba in solid solutions. Therefore it is better to identify barite suspended in seawater as the strontian barite (SrxBa1-xSO4) [101].

The second substantial component of strontium aluminate cement is **aluminium oxide** (Al2O3). The most stable crystalline form of Al2O3 is the polymorphic modification of hexag‐ onal corundum (**α**-Al2O3) from the R 3 ¯ C space group5 . The crystal structure of corundum type is typical for other oxides, such as **hematite** (Fe2O3), **eskolaite** (Cr2O3), **karelianite** (V2O3) and **tistarite** (Ti2O3). Therefore, naturally occurring minerals are often colored by the admixture of these elements, e.q. ruby is red colored by Cr and blue sapphire by Fe and Ti. That means that these elements are also interesting from the point of view of modification the properties (course of sintering, hydration and setting) of strontium aluminate cement. Chapters 4 and 5 are dedicated to this topic [424].

Pure aluminium oxide is relatively rare, but single crystals of gemstones such as sapphire (colorless) or ruby (red due to the content of chromium) can be found in nature [424]. Indus‐ trial production of Al2O3 is based on the Bayer process of bauxite. The main part of pro‐ duced alumina is used in metal industry for the production of aluminium by Hall-Heroult Process [102-105].

Calcium carbonate minerals include considerable amount of strontium from seawater as they precipitate. It stands to reason that the solid-solutions of strontianite with calcite and aragonite (CaxSr1-xCO3) are the most explored. There is an immiscibility gap in the range 0.12 (aragonites) < *x* < 0.87 (strontianites) under ambient conditions, which disappears at the tem‐

46 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

Therefore natural sources of SrCO3 are rare and have no industrial importance, strontium carbonate as well as other compounds such as strontium nitrate, strontium oxide and chlor‐ ide are prepared from the orthorhombic mineral **celestite**<sup>3</sup> (SrSO4, space group *Pnma* with cell unit parameters *a*=8.359 Å, *b*=5.352 Å, *c*=6.686 Å and *Z*=4) using the techniques descri‐ bed in Chapter 2.1.1. The structure of celestite consists of isolated [SO4]2-tetrahedrons and

Figure 2. Structure of celestite (a) and distribution of large celestite deposits in the world (b).

Celestite together with isostructural barite (BaSO4) and anglesite (PbSO4) belong to anhy‐

3 Discovered in 1791 and named in 1799 by Abraham Gottlieb Werner from the Greek "cœlestis," for celestial, in allu‐

suspended in seawater as the strontian barite (SrxBa1-xSO4) [101].

**Figure 2.** Structure of celestite (a) and distribution of large celestite deposits in the world (b).

aluminate cement. Chapters 4 and 5 are dedicated to this topic [424].

Celestite together with isostructural barite (BaSO4) and anglesite (PbSO4) belong to anhydrous sulfates from the group of barite4. Similarly to the solid solutions of carbonates mentioned above, also celestite and barite (BaSO4) coexist in the marine environment with significant fractions of Sr and Ba in solid solutions. Therefore it is better to identify barite

The second substantial component of strontium aluminate cement is **aluminium oxide** (Al2O3). The most stable crystalline form of Al2O3 is the polymorphic modification of

corundum type is typical for other oxides, such as **hematite** (Fe2O3), **eskolaite** (Cr2O3), **karelianite** (V2O3) and **tistarite** (Ti2O3). Therefore, naturally occurring minerals are often colored by the admixture of these elements, e.q. ruby is red colored by Cr and blue sapphire by Fe and Ti. That means that these elements are also interesting from the point of view of modification the properties (course of sintering, hydration and setting) of strontium

Pure aluminium oxide is relatively rare, but single crystals of gemstones such as sapphire (colorless) or ruby (red due to the content of chromium) can be found in nature [424]. Industrial production of Al2O3 is based on the **BAYER PROCESS** of bauxite. The main part of produced alumina is used in metal industry for the production of aluminium by **HALL-**

The application of Al2O3 in ceramics includes the production of alumina porcelain and alumina oxide ceramics, ZTA (Zirconia Toughened Alumina) ceramics and the applications such as electroceramics, construction ceramics, shaped and unshaped refractory products, abrasive materials, etc [106-112]. From the point of view of the volume of production, polycrystalline alumina is the most frequently used material as ceramics for the structural

4 Barite – celestite series from the group of barite. Anhydrous sulfates without additional

anions with the composition given by general formula ASO4, where A = Pb, Ba, Sr.

5 Structure and lattice parameters of corundum are described in Chapter 1.2.

a) b)


. Similarly to the solid solutions of carbonates men‐

2-triangles arranged into layers with Sr2+ions in the space

perature of ~107 °C [92,94,96,97-100].

**Figure 1.** Structure of strontianite consists of isolated [CO3]

hexagonal CORUNDUM (

drous sulfates from the group of barite4

sion to the faint blue color of the original specimen.

**HEROULT PROCESS** [102-105].

Sr2+ions (Fig.2).

between layers.

The application of Al2O3 in ceramics includes the production of alumina porcelain and alu‐ mina oxide ceramics, ZTA (Zirconia Toughened Alumina) ceramics and the applications such as electroceramics, construction ceramics, shaped and unshaped refractory products, abrasive materials, etc [106-112]. From the point of view of the volume of production, poly‐ crystalline alumina is the most frequently used material as ceramics for the structural appli‐ cations. However, in comparison with for example, silicon nitride (Chapter 6), where the influence of various additives on the microstructure and properties is well characterized and understood, alumina remains the material with many unknown factors yet to be revealed. Alumina based materials can be roughly divided into three groups [424]:


The preparation of Al2O3 mono-crystals is based on **Verneuil process** consisting in the flame fusion in high temperature region from 1500 to 2500 °C [124-127]. Bauxite (Fig.3) is also used

<sup>4</sup> Barite – celestite series from the group of barite. Anhydrous sulfates without additional anions with the composition given by general formula ASO4, where A = Pb, Ba, Sr.

<sup>5</sup> Structure and lattice parameters of corundum are described in Chapter 4.1.

for the production of calcium aluminate cements [128] or is calcined and used as opening material for the refractory products [129-131].

**Figure 4.** Process suggested for simultaneous recovery of iron, aluminium and titanium from red mud [146].

[143-146].

of treatment remains elusive [144].

phastes, etc are the major ones [148].

types [149-152]:

The utilization of Bayer's process residues in the cement production is also studied. Previ‐ ous works proposed a method of treating red mud with saturated Ca(OH)2 solution fol‐ lowed by 3% H2SO4, in order to remove Na. After heating, the treated material is suggested for the application in cement manufacturing. The major parts of red mud are hematite and alumina-rich phases (Fig.7), participating in the production of hydraulic crystal phases C3A and C4AF. Fe-rich waste could be then used for the production of sulphate resistant cements [142]. Other option includes the applications such as catalysts and adsorbents, ceramics, coatings and pigments, waste water and gas treatment, recovery of major and minor metals

Raw Materials for Production of SrAC 49

Bayer suggested that [143]: "Red, iron-containing residue, that occurs after digestion, settles well and, with sufficient practice, can be filtered and washed. Due to its high iron content and low aluminium oxide content, it can be, in an appropriate manner, treated or melted with other iron ores to iron". The concept of bauxite residue as an iron resource was tested by a number of workers over the intervening 120 years, however, the "appropriate manner"

The aluminium gels, salts (sulphates, nitrates or chlorides) or alkoxides and advanced ce‐ ramic fabrication techniques can be applied for the preparation of high purity products (please referee to Chapter 9). Bauxite is the mixture of aluminium hydroxides and oxyhydr‐ oxides such as boehmite, diaspore and gibbsite, with varying content of admixture minerals. Goethite, lepidocrocite, hematite, magnetite, kaolinite, chlorites, calcite, anatase, phos‐

Bauxite, as the primary source of aluminum, represents a typical accumulation of weathered continental crust [147,148]. Bauxites are usually considered to be of three major genetic

**1. Lateric bauxites** (sometimes called equatorial) are formed from weathered primary alu‐ minosilicate rocks in equatorial climates comprising ∼90% of the world's exploitable bauxite reserves. Lateritic bauxite is generally formed by in-situ lateritization, therefore, the most important factors in determining the extent and grade of it are thought to be

**Figure 3.** SEM image of calcined bauxite grain.

In order to obtain good quality in abrasive, refractory and pottery products, the content of impurities should be reduced. Chemical processes include the pyrochemical techniques, acid leaching methods or reductive dissolution alternatives. The pyrochemical techniques involve the treatment of bauxite at high temperature with gases such as H2, Cl2 or anhy‐ drous HCl [132,133]. The acid leaching methods are based on the application of strong inor‐ ganic acids such as HCl or H2SO4 [134-137].

A serious problem with these techniques is that leaching of iron is often accompanied by substantial co-dissolution of aluminium hydroxides, particularly during the treatment of gibssitic and boehmitic ores. Selective dissolution of iron can be obtained applying mild re‐ ducing conditions. In this case the dissolution of Fe(III) oxides takes place via the reduction of ferric iron to the divalent state. It is widely accepted that biological mechanisms are often involved in the mobilization of iron in natural systems. For the particular case of bauxites the biological activity of iron reducing microorganisms is most probably involved in the generation of gray-colored iron depleted bauxites [138,139].

Since the production of alumina from bauxite ores consumes large amount of caustic soda, and generates large amount of "**red mud**" slurry waste, the alternative processes for the production of aluminium and aluminoalloys via carbothermic reduction of bauxite ores was investigated. The reduction sequence of metal oxides in bauxite ores is iron oxides then silica and titania and then alumina (Fig.4). Metallic iron is formed at the temperatures below 1100 °C. At 1200 °C or above the ferroalloy phase with silicon and aluminium is formed. Carbides of titanium, silicon and aluminium were formed by the carbothermal reduction. The metals were formed and dissolved in the ferroalloy phase, which after saturation, was segregated as metal carbides distributed inside the alloy phase as inclusions or around the alloy particles [140,141].

for the production of calcium aluminate cements [128] or is calcined and used as opening

48 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

In order to obtain good quality in abrasive, refractory and pottery products, the content of impurities should be reduced. Chemical processes include the pyrochemical techniques, acid leaching methods or reductive dissolution alternatives. The pyrochemical techniques involve the treatment of bauxite at high temperature with gases such as H2, Cl2 or anhy‐ drous HCl [132,133]. The acid leaching methods are based on the application of strong inor‐

A serious problem with these techniques is that leaching of iron is often accompanied by substantial co-dissolution of aluminium hydroxides, particularly during the treatment of gibssitic and boehmitic ores. Selective dissolution of iron can be obtained applying mild re‐ ducing conditions. In this case the dissolution of Fe(III) oxides takes place via the reduction of ferric iron to the divalent state. It is widely accepted that biological mechanisms are often involved in the mobilization of iron in natural systems. For the particular case of bauxites the biological activity of iron reducing microorganisms is most probably involved in the

Since the production of alumina from bauxite ores consumes large amount of caustic soda, and generates large amount of "**red mud**" slurry waste, the alternative processes for the production of aluminium and aluminoalloys via carbothermic reduction of bauxite ores was investigated. The reduction sequence of metal oxides in bauxite ores is iron oxides then silica and titania and then alumina (Fig.4). Metallic iron is formed at the temperatures below 1100 °C. At 1200 °C or above the ferroalloy phase with silicon and aluminium is formed. Carbides of titanium, silicon and aluminium were formed by the carbothermal reduction. The metals were formed and dissolved in the ferroalloy phase, which after saturation, was segregated as metal carbides distributed inside the alloy phase as inclusions or around the

material for the refractory products [129-131].

**Figure 3.** SEM image of calcined bauxite grain.

ganic acids such as HCl or H2SO4 [134-137].

alloy particles [140,141].

generation of gray-colored iron depleted bauxites [138,139].

**Figure 4.** Process suggested for simultaneous recovery of iron, aluminium and titanium from red mud [146].

The utilization of Bayer's process residues in the cement production is also studied. Previ‐ ous works proposed a method of treating red mud with saturated Ca(OH)2 solution fol‐ lowed by 3% H2SO4, in order to remove Na. After heating, the treated material is suggested for the application in cement manufacturing. The major parts of red mud are hematite and alumina-rich phases (Fig.7), participating in the production of hydraulic crystal phases C3A and C4AF. Fe-rich waste could be then used for the production of sulphate resistant cements [142]. Other option includes the applications such as catalysts and adsorbents, ceramics, coatings and pigments, waste water and gas treatment, recovery of major and minor metals [143-146].

Bayer suggested that [143]: "Red, iron-containing residue, that occurs after digestion, settles well and, with sufficient practice, can be filtered and washed. Due to its high iron content and low aluminium oxide content, it can be, in an appropriate manner, treated or melted with other iron ores to iron". The concept of bauxite residue as an iron resource was tested by a number of workers over the intervening 120 years, however, the "appropriate manner" of treatment remains elusive [144].

The aluminium gels, salts (sulphates, nitrates or chlorides) or alkoxides and advanced ce‐ ramic fabrication techniques can be applied for the preparation of high purity products (please referee to Chapter 9). Bauxite is the mixture of aluminium hydroxides and oxyhydr‐ oxides such as boehmite, diaspore and gibbsite, with varying content of admixture minerals. Goethite, lepidocrocite, hematite, magnetite, kaolinite, chlorites, calcite, anatase, phos‐ phastes, etc are the major ones [148].

Bauxite, as the primary source of aluminum, represents a typical accumulation of weathered continental crust [147,148]. Bauxites are usually considered to be of three major genetic types [149-152]:

**1. Lateric bauxites** (sometimes called equatorial) are formed from weathered primary alu‐ minosilicate rocks in equatorial climates comprising ∼90% of the world's exploitable bauxite reserves. Lateritic bauxite is generally formed by in-situ lateritization, therefore, the most important factors in determining the extent and grade of it are thought to be the parent rock composition, climate, topography, drainage, groundwater chemistry and movement, location of water table, microbial activity, and the duration of weather‐ ing processes.

**1.1. Industrial and laboratory production of SrCO3**

celestite from gypsum by differential grinding [157].

The shear flocculation7

spectively [159].

HCO3 -

foam.

neously or after the addition of clarifying agents.

Chemical industry consumes over 95 % mined celestite for the conversion to other strontium compounds. The main admixtures in celestite ores are calcite (CaCO3), gypsum (CaSO4 2H2O), quartz (SiO2) and clay minerals. The gravity separation techniques and the flotation6 are mostly used for the separation of those admixtures due to high efficiency and low oper‐ ating costs. Moreover, the process does not require the usage of other chemicals for the puri‐ fication and has low environmental impact. On the other hand, the efficiency of these techniques for the preparation of celestite concentrate depends on the texture of ore as well as the type and quantity of associated impurities [153-155]. The particle size is other most important factor. Extremely fine particle sizes must be achieved by grinding in order to re‐ lease celestite and calcite [156]. The difference in grindabilities makes it possible to separate

C12H25SO4Na) or with anionic alkyl succinate surfactant can be performed in broad pH range (3 – 11) but the highest efficiency is reached at pH 7. Increasing concentration of surfactant has positive effect on the course of process. The most common inorganic dispersants used are sodium silicate, sodium phosphate and sodium polyphosphate. The investigation of mu‐ tual influence of additives shows that sodium silicate strongly prevents celestite with so‐ dium dodecyl sulfate from shear flocculation, but the dispersive effect of SDS is low when anionic alkyl succinate surfactant is used. In the presence of sodium polyphosphate, the shear flocculation of celestite suspension increases slowly for both surfactants. The similar increase can also be observed for sodium phosphate in the presence of SDS. However, so‐ dium phosphate dispersed the celestite suspension in the presence of anionic alkyl succinate surfactant [158]. Sodiumoleate (cis-9-Octadecenoic acid sodium salt) and tallow amine ace‐ tate (TAA) were more effective for celestite suspensions in the pH ranges 7–11 and 6–10, re‐

The surface of celestite becomes hydrophobic by the adsorption of dodecyl sulfate on the surface. Sodium dodecyl sulfate is also effective for the flotation of celestite in the solution free of carbonate species over the broad pH range of 3-11. The surface transformation of cel‐ estite to strontium carbonate which takes place at pH ≥ 7.8 causes that the zeta potential of celestite begins to be more negative and subsequently resembles that of strontium carbo‐ nate. Sulfate ions are exchanged by carbonate ions in the celestite crystal lattice, so CO3

 species are probably responsible for the negative increase in zeta potential. The sur‐ face transformation of celestite to strontium carbonate has no effect on floatability up to the

6 Flotation is an industrial process for the treatment of raw materials. The constituents of fine powdered raw materials are separated from the mixture according to the different wettability of individual solid species. The foam flotation process uses the interaction of gas bubbles with suspended material, which is next concentrated on the liquid level as

7 Flocculation is a special case of coagulation where suspended particles of colloids form flake-like aggregates sponta‐

pH of 10. Once the pH is higher than 10, the concentration of CO3

of fine celestite suspension with sodium dodecyl sulfate (SDS,

2- and

species in

2- and HCO3


Raw Materials for Production of SrAC 51


**Figure 5.** Distribution of superlarge bauxite deposits worldwide [152].

Each genetic group of bauxite experienced the separation of aluminum (Al) and silicon (Si) by the accumulation of Al, and the removal of Si, alkali metals, and rare earth elements from parent rock (sediment) during its weathering [148].

Bauxite deposits (Fig.5) form mainly at ambient pressure and temperature on the (sub)sur‐ face of continents. Abundant bioavailable irons, nutrient elements, sulfurs, and organic car‐ bons make bauxite suitable for microorganisms to inhabit so they become rare geological sites that can preserve records of microbiological activity on the surface of continents under strong weathering effects. The microorganism activities can produce a family of minerals with special morphologies and stable isotope compositions. Bauxite deposits were studied in detail because of their economic value. They play an important role in the study of paleo‐ climate and paleogeography of continents because they contain scarce records of weathering and evolution of continental surfaces [148].

## **1.1. Industrial and laboratory production of SrCO3**

the parent rock composition, climate, topography, drainage, groundwater chemistry and movement, location of water table, microbial activity, and the duration of weather‐

**2. Sedimentary bauxites** are primarily formed by the accumulation of lateritic bauxite de‐ posits during the mechanical transportation of surface flows. In addition, the conse‐ quent weathering and transfer of Al and Fe play substantial roles in bauxitization, which not only supports the formation of bauxite from kaolin clays but also refines the

50 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

**3. Karst bauxites** are named for their confinement to karst zones with karstified or karsti‐ fying carbonate rocks. Karst-type deposits originate from a variety of different materi‐

Each genetic group of bauxite experienced the separation of aluminum (Al) and silicon (Si) by the accumulation of Al, and the removal of Si, alkali metals, and rare earth elements from

Bauxite deposits (Fig.5) form mainly at ambient pressure and temperature on the (sub)sur‐ face of continents. Abundant bioavailable irons, nutrient elements, sulfurs, and organic car‐ bons make bauxite suitable for microorganisms to inhabit so they become rare geological sites that can preserve records of microbiological activity on the surface of continents under strong weathering effects. The microorganism activities can produce a family of minerals with special morphologies and stable isotope compositions. Bauxite deposits were studied in detail because of their economic value. They play an important role in the study of paleo‐ climate and paleogeography of continents because they contain scarce records of weathering

ing processes.

primary clastic ores.

als, depending on the source area.

**Figure 5.** Distribution of superlarge bauxite deposits worldwide [152].

parent rock (sediment) during its weathering [148].

and evolution of continental surfaces [148].

Chemical industry consumes over 95 % mined celestite for the conversion to other strontium compounds. The main admixtures in celestite ores are calcite (CaCO3), gypsum (CaSO4 2H2O), quartz (SiO2) and clay minerals. The gravity separation techniques and the flotation6 are mostly used for the separation of those admixtures due to high efficiency and low oper‐ ating costs. Moreover, the process does not require the usage of other chemicals for the puri‐ fication and has low environmental impact. On the other hand, the efficiency of these techniques for the preparation of celestite concentrate depends on the texture of ore as well as the type and quantity of associated impurities [153-155]. The particle size is other most important factor. Extremely fine particle sizes must be achieved by grinding in order to re‐ lease celestite and calcite [156]. The difference in grindabilities makes it possible to separate celestite from gypsum by differential grinding [157].

The shear flocculation7 of fine celestite suspension with sodium dodecyl sulfate (SDS, C12H25SO4Na) or with anionic alkyl succinate surfactant can be performed in broad pH range (3 – 11) but the highest efficiency is reached at pH 7. Increasing concentration of surfactant has positive effect on the course of process. The most common inorganic dispersants used are sodium silicate, sodium phosphate and sodium polyphosphate. The investigation of mu‐ tual influence of additives shows that sodium silicate strongly prevents celestite with so‐ dium dodecyl sulfate from shear flocculation, but the dispersive effect of SDS is low when anionic alkyl succinate surfactant is used. In the presence of sodium polyphosphate, the shear flocculation of celestite suspension increases slowly for both surfactants. The similar increase can also be observed for sodium phosphate in the presence of SDS. However, so‐ dium phosphate dispersed the celestite suspension in the presence of anionic alkyl succinate surfactant [158]. Sodiumoleate (cis-9-Octadecenoic acid sodium salt) and tallow amine ace‐ tate (TAA) were more effective for celestite suspensions in the pH ranges 7–11 and 6–10, re‐ spectively [159].

The surface of celestite becomes hydrophobic by the adsorption of dodecyl sulfate on the surface. Sodium dodecyl sulfate is also effective for the flotation of celestite in the solution free of carbonate species over the broad pH range of 3-11. The surface transformation of cel‐ estite to strontium carbonate which takes place at pH ≥ 7.8 causes that the zeta potential of celestite begins to be more negative and subsequently resembles that of strontium carbo‐ nate. Sulfate ions are exchanged by carbonate ions in the celestite crystal lattice, so CO3 2- and HCO3 species are probably responsible for the negative increase in zeta potential. The sur‐ face transformation of celestite to strontium carbonate has no effect on floatability up to the pH of 10. Once the pH is higher than 10, the concentration of CO3 2- and HCO3 species in

<sup>6</sup> Flotation is an industrial process for the treatment of raw materials. The constituents of fine powdered raw materials are separated from the mixture according to the different wettability of individual solid species. The foam flotation process uses the interaction of gas bubbles with suspended material, which is next concentrated on the liquid level as foam.

<sup>7</sup> Flocculation is a special case of coagulation where suspended particles of colloids form flake-like aggregates sponta‐ neously or after the addition of clarifying agents.

aqueous solution is very intrinsic and the decrease of floatability is probably caused by the absorption of these species on carbonated surface of celestite [155].

by the partial pressure ratio of *p*CO/*p*CO2. It was also observed that the rate of carbothermic reduction significantly increases if celestite concentrate and carbon are milled together. The temperatures in the range from 1100 to 1300 °C with the excess of metallurgical grade coke

The dissolution of strontium sulfide in hot water can be expressed by the following hetero‐

Eq.4 shows that the pH of leaching solution increases from almost neutral to the value of

should be avoided in order to prevent the system from the precipitation of strontium hy‐

The value of equilibrium constant *K* at 25 °C is 3.55 10-29, i.e. *log K*=-28.45. Therefore, the con‐

That means that leaching of SrS must be carried out in relatively low alkaline medium in order to ensure high concentration of strontium in the solution. The solubility of strontium hydroxide is enhanced by increased temperature. Therefore leaching and precipitation of SrCO3 at higher temperatures mean that the formation of Sr(OH)2 precipitates is reduced.

The generation of hydrogen sulphide gas takes place in early stages of leaching when the

Introducing the carbon dioxide gas or carbonating agent such as soda ash leads to the pre‐ cipitation of strontium carbonate from supersaturated solution (Eq.13). The sequence of re‐ action steps includes the dissolution of carbon dioxide in solution and *in situ* formation of carbonic acid (H2CO3, Eq.8), the dissociation of H2CO3 (Eq.9 with the equilibrium constant

9 Sr(OH)2⋅8H2O precipitates during cooling of hot supersaturated solutions. Strontium hydroxide octahydrate trans‐ forms to monohydrate by ageing of the precipitate. Anhydrous hydroxide can be prepared via thermal treatment of

centration of Sr(OH)2 in leaching solution (Fig.6) can be expressed as:

2

On the other hand, leaching at pH < 7 generates hydrogen sulphide gas:

2+ - - SrS(s)+H O (l) Sr (aq)+HS (aq)+OH (aq) <sup>2</sup> ® (4)

2+ <sup>+</sup> Sr (aq)+2 H O(l) Sr(OH) (s)+2H (aq) 2 2 ® (5)

<sup>10</sup> log 28.45 2 <sup>+</sup> é ù = - ë û *Sr pH* (6)


ions increases. Extremely high pH values (pH > 14)

Raw Materials for Production of SrAC 53

are necessary to produce water-soluble strontium sulfide.

geneous reaction [164]:

droxide9

:

pH of slurry is relatively low.

the precipitate up to 100 °C.

11.5 – 12.5 as the concentration of OH-

The coagulation and flocculation characteristics of celestite by inorganic salts, such as CaCl2, MgCl2 and AlCl3, indicate that magnesium ion was more effective on the celestite suspen‐ sion than calcium and aluminum ions at high pH levels. The effect varied significantly de‐ pending on the concentration. While calcium and magnesium ions were not effective for the suspension below neutral pH, aluminum ion caused the stabilization of the celestite suspen‐ sion at these pH levels [160].

In general, the aggregation of fine particles can be achieved by neutralizing the electrical charge of interacting particles by coagulation, or flocculation can be carried out by crosslink‐ ing the particles with polymolecules [161]. The pH of isoelectric point of celestite deter‐ mined by the hindered settling technique is 2.6 [160].

There are two basic processes to produce SrCO3 from SrSO4 [162]:


The "**pyro-hydrometallurgical process** or **black ash method**" is first of them. Celestite is carbothermically reduced to water soluble sulphide (SrS), which is next dissolved in hot water8 The first solid-state reaction during the carbothermic reduction takes place at up to 400 °C [163]:

$$\text{SrSO}\_4(\text{s}) + 4\text{ C(s)} \to \text{SrS(s)} + 4\text{ CO(g)}\tag{1}$$

After the formation of surface layer of the product the further progress of reaction 1 is inhib‐ ited. Formed carbon dioxide diffuses through the layer and reacts with celestite according to the following reaction:

$$\rm{SrSO\_4(s)+4\ CO(g)\to SrS(s)+4\ CO\_2(g)}\tag{2}$$

Carbon dioxide diffuses further out of reaction zone and generates more CO according to the Boudouard reaction if the temperature is ≥ 720 °C:

$$2\text{ CO}\_2(\text{g}) + \text{C}(\text{s}) \leftrightarrow 2\text{ CO}(\text{g})\tag{3}$$

That means that direct reaction of celestite with carbon (Eq.1) has little importance and SrSO4 can be transformed to SrS at the temperature higher than equilibrium of **Boudouard reaction**. The important factor of the process 2 is the reduction potential of gas phase given

<sup>8</sup> Strontium salt can be then prepared directly by dissolving SrS in acid.

by the partial pressure ratio of *p*CO/*p*CO2. It was also observed that the rate of carbothermic reduction significantly increases if celestite concentrate and carbon are milled together. The temperatures in the range from 1100 to 1300 °C with the excess of metallurgical grade coke are necessary to produce water-soluble strontium sulfide.

aqueous solution is very intrinsic and the decrease of floatability is probably caused by the

52 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

The coagulation and flocculation characteristics of celestite by inorganic salts, such as CaCl2, MgCl2 and AlCl3, indicate that magnesium ion was more effective on the celestite suspen‐ sion than calcium and aluminum ions at high pH levels. The effect varied significantly de‐ pending on the concentration. While calcium and magnesium ions were not effective for the suspension below neutral pH, aluminum ion caused the stabilization of the celestite suspen‐

In general, the aggregation of fine particles can be achieved by neutralizing the electrical charge of interacting particles by coagulation, or flocculation can be carried out by crosslink‐ ing the particles with polymolecules [161]. The pH of isoelectric point of celestite deter‐

The "**pyro-hydrometallurgical process** or **black ash method**" is first of them. Celestite is carbothermically reduced to water soluble sulphide (SrS), which is next dissolved in hot water8 The first solid-state reaction during the carbothermic reduction takes place at up to

After the formation of surface layer of the product the further progress of reaction 1 is inhib‐ ited. Formed carbon dioxide diffuses through the layer and reacts with celestite according to

Carbon dioxide diffuses further out of reaction zone and generates more CO according to

That means that direct reaction of celestite with carbon (Eq.1) has little importance and SrSO4 can be transformed to SrS at the temperature higher than equilibrium of **Boudouard reaction**. The important factor of the process 2 is the reduction potential of gas phase given

SrSO (s)+4 C(s) SrS(s)+4 CO(g) <sup>4</sup> ® (1)

SrSO (s)+4 CO(g) SrS(s)+4 CO (g) 4 2 ® (2)

CO (g)+C(s) 2 CO(g) <sup>2</sup> « (3)

absorption of these species on carbonated surface of celestite [155].

mined by the hindered settling technique is 2.6 [160].

the Boudouard reaction if the temperature is ≥ 720 °C:

8 Strontium salt can be then prepared directly by dissolving SrS in acid.

There are two basic processes to produce SrCO3 from SrSO4 [162]:

**a.** Pyro-hydrometallurgical process or black ash method;

sion at these pH levels [160].

**b.** Hydro metallurgical process.

400 °C [163]:

the following reaction:

The dissolution of strontium sulfide in hot water can be expressed by the following hetero‐ geneous reaction [164]:

$$\text{SrS(s)} + \text{H}\_2\text{O(l)} \rightarrow \text{Sr}^{2+}\text{(aq)} + \text{HS}^{\cdot}\text{(aq)} + \text{OH}^{\cdot}\text{(aq)}\tag{4}$$

Eq.4 shows that the pH of leaching solution increases from almost neutral to the value of 11.5 – 12.5 as the concentration of OH ions increases. Extremely high pH values (pH > 14) should be avoided in order to prevent the system from the precipitation of strontium hy‐ droxide9 :

$$\text{Sr}^{2+}\text{(aq)} + 2\text{ H}\_2\text{O(l)} \rightarrow \text{Sr(OH)}\_2\text{(s)} + 2\text{H}^+\text{(aq)}\tag{5}$$

The value of equilibrium constant *K* at 25 °C is 3.55 10-29, i.e. *log K*=-28.45. Therefore, the con‐ centration of Sr(OH)2 in leaching solution (Fig.6) can be expressed as:

$$\log\_{10}\left[Sr^{2+}\right] = 28.4\text{S} - 2\text{ }pH\tag{6}$$

That means that leaching of SrS must be carried out in relatively low alkaline medium in order to ensure high concentration of strontium in the solution. The solubility of strontium hydroxide is enhanced by increased temperature. Therefore leaching and precipitation of SrCO3 at higher temperatures mean that the formation of Sr(OH)2 precipitates is reduced.

On the other hand, leaching at pH < 7 generates hydrogen sulphide gas:

$$\text{HS}^\cdot(\text{aq}) \text{+H}^+(\text{aq}) \leftrightarrow \text{H}\_2\text{S}(\text{g})\tag{7}$$

The generation of hydrogen sulphide gas takes place in early stages of leaching when the pH of slurry is relatively low.

Introducing the carbon dioxide gas or carbonating agent such as soda ash leads to the pre‐ cipitation of strontium carbonate from supersaturated solution (Eq.13). The sequence of re‐ action steps includes the dissolution of carbon dioxide in solution and *in situ* formation of carbonic acid (H2CO3, Eq.8), the dissociation of H2CO3 (Eq.9 with the equilibrium constant

<sup>9</sup> Sr(OH)2⋅8H2O precipitates during cooling of hot supersaturated solutions. Strontium hydroxide octahydrate trans‐ forms to monohydrate by ageing of the precipitate. Anhydrous hydroxide can be prepared via thermal treatment of the precipitate up to 100 °C.

(*K*´) given by Eq.10), the dissociation of bicarbonate species (Eq.11 with the equilibrium con‐ stant (*K*´´) given by Eq.12) and the precipitation of strontium carbonate (Eq.13 with the ion product (*P*) given by Eq.14) [163-165].

$$\rm{CO}\_2(g) + \rm{H}\_2\rm{O(l)} \leftrightarrow \rm{H}\_2\rm{CO}\_3 \tag{8}$$

$$\text{H}\_2\text{CO}\_3 \leftrightarrow \text{H}^+\text{(aq)} + \text{HCO}\_3^\cdot\text{(aq)}\tag{9}$$

$$\text{K}^{\prime} = \frac{\left[\text{H}^{+}\right]\left[\text{HCO}\_{3}^{\cdot}\right]}{\left[\text{H}\_{2}\text{CO}\_{3}\right]} \tag{10}$$

$$\text{HCO}\_3^\cdot \leftrightarrow \text{H}^+ + \text{CO}\_3^{2\cdot} \tag{11}$$

The second technique for the preparation of strontium carbonate is the **direct conversion method** or **hydrometallurgical method**. Strontium carbonate is prepared by introducing SrSO4 powder into hot solution of Na2CO3, where the following conversion process takes

The effect of experimental conditions on the process includes the influence of temperature, solid to liquid ratio, particle size, stirring rate, Na2CO3 : SrSO4 molar ratio, etc. The conver‐ sion rate of celestite to strontium carbonate increases with temperature up to 70 °C [165-170]. Prepared carbonate or sulphide is further converted to other strontium salts [91].

3

**Figure 6.** Influence of pH on the equilibrium concentration of Sr2+ and SrOH+ ions in solution.

It is also possible to use ammonium carbonate ((NH4)2CO3)

(in boiling mixture) SrSO4+(NH4)2CO3→SrCO3+2NH3+SO3+H2O

stead of soda ash for the conversion [165,171-174]:

10 Since NH4+ species as well as Na+

obtained for both processes.

SrSO +Na CO SrCO +Na SO 4 2 3 3 24 ® (16)

2- 2- SrSO (s)+CO (aq) SrCO (s)+SO (aq) <sup>4</sup> ® 3 4 (17)

SrSO +(NH ) CO SrCO +(NH ) SO 4 42 3 3 42 4 ® (18)

ion in Eq.16 does not participate in the reaction, the same equation 17 will be

10 and bicarbonate (NH4HCO3) in‐

Raw Materials for Production of SrAC 55

place:

or better:

$$\mathbf{K} = \frac{\left[\text{H}^{+}\right]\left[\text{CO}\_{3}^{2-}\right]}{\left[\text{HCO}\_{3}^{\*}\right]}\tag{12}$$

$$\text{Sr}^{2+}\text{(aq)} + \text{CO}\_3^{2-}\text{(aq)} \rightarrow \text{SrCO}\_3\text{(s)}\tag{13}$$

$$\mathbf{P} = \left[ \mathbf{S} \mathbf{r}^{2^+} \right] \left[ \mathbf{C} \mathbf{O}\_3^{2^\*} \right] \tag{14}$$

The solubility of strontium carbonate is 5.6 10-10 at the temperature of 25 °C and decreases to 1.32 10-10 at the temperature of 100 °C. The hydrolysis reaction leads to alkaline character of aqueous solution of SrCO3.

Eqs.8-14 show that one mole of gaseous CO2 is required for the precipitation of each mole of SrCO3. The concentration of CO3 2- ions in leaching solution for given pH is expressed by the following law:

$$\log\_{10}\left[\text{CO}\_3^{2\cdot}\right] = \log\_{10}\text{K}"+\text{pH}+\log\_{10}\left[\text{HCO}\_3^{\cdot}\right] \tag{15}$$

If the pH of leaching solution is higher than 7, H+ ions formed by the reaction 11 neutraliz‐ ing OH anions are released during leaching of SrS (Eq.4).

In general, the black ash method is concluded to be more the more economical than other alternatives [165].

**Figure 6.** Influence of pH on the equilibrium concentration of Sr2+ and SrOH+ ions in solution.

The second technique for the preparation of strontium carbonate is the **direct conversion method** or **hydrometallurgical method**. Strontium carbonate is prepared by introducing SrSO4 powder into hot solution of Na2CO3, where the following conversion process takes place:

$$\text{SrSO}\_4 + \text{Na}\_2\text{CO}\_3 \to \text{SrCO}\_3 + \text{Na}\_2\text{SO}\_4 \tag{16}$$

or better:

(*K*´) given by Eq.10), the dissociation of bicarbonate species (Eq.11 with the equilibrium con‐ stant (*K*´´) given by Eq.12) and the precipitation of strontium carbonate (Eq.13 with the ion

54 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

[ ]

H CO é ùé ù

H HCO

K =

K =

2 3

+ 2- 3 - 3

é ùé ù ë ûë û ¢¢ é ù ë û

H CO

HCO

2+ 2- P= Sr CO3 é ùé ù

The solubility of strontium carbonate is 5.6 10-10 at the temperature of 25 °C and decreases to 1.32 10-10 at the temperature of 100 °C. The hydrolysis reaction leads to alkaline character of

Eqs.8-14 show that one mole of gaseous CO2 is required for the precipitation of each mole of

2- -

In general, the black ash method is concluded to be more the more economical than other

+ - 3

CO (g)+H O(l) H CO 2 2 23 « (8)

+ - H CO H (aq)+HCO (aq) 2 3 « <sup>3</sup> (9)

ë ûë û ¢ (10)


2+ 2- Sr (aq)+CO (aq) SrCO (s) 3 3 ® (13)

ë ûë û (14)

2- ions in leaching solution for given pH is expressed by the

ions formed by the reaction 11 neutraliz‐

10 3 10 10 3 log CO =log K +pH+log HCO é ù ¢¢ é ù ë û ë û (15)

(12)

product (*P*) given by Eq.14) [163-165].

aqueous solution of SrCO3.

following law:

ing OH-

alternatives [165].

SrCO3. The concentration of CO3

If the pH of leaching solution is higher than 7, H+

anions are released during leaching of SrS (Eq.4).

$$\text{SrSO}\_4(\text{s}) \text{+CO}\_3^{2-}(\text{aq}) \rightarrow \text{SrCO}\_3(\text{s}) \text{+SO}\_4^{2-}(\text{aq}) \tag{17}$$

The effect of experimental conditions on the process includes the influence of temperature, solid to liquid ratio, particle size, stirring rate, Na2CO3 : SrSO4 molar ratio, etc. The conver‐ sion rate of celestite to strontium carbonate increases with temperature up to 70 °C [165-170]. Prepared carbonate or sulphide is further converted to other strontium salts [91].

It is also possible to use ammonium carbonate ((NH4)2CO3) 10 and bicarbonate (NH4HCO3) in‐ stead of soda ash for the conversion [165,171-174]:

$$\text{SrSO}\_4 + (\text{NH}\_4)\_2\text{CO}\_3 \rightarrow \text{SrCO}\_3 + (\text{NH}\_4)\_2\text{SO}\_4 \tag{18}$$

(in boiling mixture) SrSO4+(NH4)2CO3→SrCO3+2NH3+SO3+H2O

<sup>10</sup> Since NH4+ species as well as Na+ ion in Eq.16 does not participate in the reaction, the same equation 17 will be obtained for both processes.

$$\rm{SrSO\_4(s)\text{-}2HCO\_3^-(aq)\to SrCO\_3(s)\text{+}SO\_4^{2-}(aq)\to H\_2O(l)\text{+}CO\_2(g)}\tag{19}$$

Strontium is also obtained by the reduction of its amalgam, hydride, and other salts. Amal‐ gam is heated and the mercury is separated by the distillation. If hydride is used, it is heated at 1 000°C in vacuum for the decomposition and removal of hydrogen. Such thermal reduc‐ tions yield high–purity metal which, when exposed to air, oxidizes to SrO. The metal is py‐ rophoric, both SrO and SrO2 (strontium peroxide) are formed via ignition in air. When heated with chlorine gas or bromine vapor, strontium burns brightly, forming its halides

Strontium reacts vigorously with water and hydrochloric acid forming hydroxide Sr(OH)2

When heated under hydrogen it forms ionic hydride (SrH2), a stable crystalline salt. Heating

Pure alumina, which is required for the production of aluminum by the Hall process, is made by the Bayer process [91]. The Bayer process was developed in 1887 by Carl Josef Bayer (1847-1904). It is the method for industrial production of aluminium oxide from bauxite. This method replaces earlier techniques developed by Henri Étienne Sainte-Claire Deville (1818-1881). Fine milled bauxite powder is leached in the solution of sodium hydroxide in autoclave under the temperature range from 160 to 250 °C and the pressure from 0.4 to 0.8 MPa. The basic components of bauxite are dissolved and soluble salts

Sr+2 H O Sr(OH) +H <sup>2</sup> ® 2 2 (20)

Raw Materials for Production of SrAC 57

Sr+2 HCl SrCl +H ® 2 2 (21)

T,p Al(OH) +NaOH NaAl(OH) 3 4 ¾¾® (22)

T,p SiO +2 NaOH Na SiO +H O <sup>2</sup> ¾¾® 2 32 (23)

T,p Fe O +2 NaOH Na FeO +H O 2 3 ¾¾® 2 22 (24)

T,p TiO +2 NaOH Na TiO +H O <sup>2</sup> ¾¾® 2 32 (25)

(SrCl2 or SrBr2). When heated with sulfur, it forms sulfide (SrS) [91].

metallic Sr in a stream of nitrogen above 380°C forms nitride (Sr3N2).

according to the following reaction scheme are formed [189]:

or chloride (SrCl2) with liberation of hydrogen [91]:

**1.2. Bayer process**

There is also an alternative in mechanochemical synthesis, where the mixture of SrSO4 and NH4HCO3 is intensively milled. The soluble ammonium sulphate is next removed by leach‐ ing of the product in water [165].

Moreover lots of special techniques for the preparation of SrCO3 were described in current literature. These methods include the preparation of strontium carbonate via solid-state de‐ composition route from inorganic precursor [746]. Simple solution techniques [175], solvo‐ thermal synthesis [176-178], refluxing method [188] hydrothermal synthesis [179-182], ultrasonic method or sonochemical-assisted synthesis [183,184], microwave assisted synthe‐ sis [185,186] and mechanochemical synthesis [168,187] were described. Depending on ap‐ plied preparation technique, the strontium carbonate particles of different shape can be prepared, such as spheres, rods, whiskers and ellipsoids, needles, flowers, ribbons, wires, etc. [188].


The solubility of strontium salts is mostly either higher or lower than for corresponding cal‐ cium and barium salts (Table 1).

**Table 1.** The solubility of salts of alkaline earth metals at the temperature of 20 °C.

Metallic strontium can be prepared by the electrolysis of mixed melt of strontium chloride and potassium chloride in a graphite crucible using iron rod as cathode. The upper cathode space is cooled and metallic strontium collects around cooled cathode and forms a stick. Metallic strontium can also be prepared by thermal reduction of its oxide with aluminum. Strontium oxide-aluminum mixture is heated at high temperature in vacuum. Strontium is collected by the distillation in vacuum. Strontium is also a reducing agent. It reduces oxides and halides of metals at elevated temperatures to the metallic form.

Strontium is also obtained by the reduction of its amalgam, hydride, and other salts. Amal‐ gam is heated and the mercury is separated by the distillation. If hydride is used, it is heated at 1 000°C in vacuum for the decomposition and removal of hydrogen. Such thermal reduc‐ tions yield high–purity metal which, when exposed to air, oxidizes to SrO. The metal is py‐ rophoric, both SrO and SrO2 (strontium peroxide) are formed via ignition in air. When heated with chlorine gas or bromine vapor, strontium burns brightly, forming its halides (SrCl2 or SrBr2). When heated with sulfur, it forms sulfide (SrS) [91].

Strontium reacts vigorously with water and hydrochloric acid forming hydroxide Sr(OH)2 or chloride (SrCl2) with liberation of hydrogen [91]:

$$\text{Sr} + 2\,\text{H}\_2\text{O} \to \text{Sr(OH)}\_2\text{+H}\_2\tag{20}$$

$$\text{Sr} + 2\text{ HCl} \rightarrow \text{SrCl}\_2 + \text{H}\_2 \tag{21}$$

When heated under hydrogen it forms ionic hydride (SrH2), a stable crystalline salt. Heating metallic Sr in a stream of nitrogen above 380°C forms nitride (Sr3N2).

### **1.2. Bayer process**


There is also an alternative in mechanochemical synthesis, where the mixture of SrSO4 and NH4HCO3 is intensively milled. The soluble ammonium sulphate is next removed by leach‐

56 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

Moreover lots of special techniques for the preparation of SrCO3 were described in current literature. These methods include the preparation of strontium carbonate via solid-state de‐ composition route from inorganic precursor [746]. Simple solution techniques [175], solvo‐ thermal synthesis [176-178], refluxing method [188] hydrothermal synthesis [179-182], ultrasonic method or sonochemical-assisted synthesis [183,184], microwave assisted synthe‐ sis [185,186] and mechanochemical synthesis [168,187] were described. Depending on ap‐ plied preparation technique, the strontium carbonate particles of different shape can be prepared, such as spheres, rods, whiskers and ellipsoids, needles, flowers, ribbons, wires,

The solubility of strontium salts is mostly either higher or lower than for corresponding cal‐

**Cations Ca2+ Sr2+ Ba2+**

OH- 0.160 0.810 3.890 F- 0.0017 0.0175 0.1600 Cl- 74.5 53.1 36.2 NO3 2- 128.8 70.4 9.10

**Table 1.** The solubility of salts of alkaline earth metals at the temperature of 20 °C.

and halides of metals at elevated temperatures to the metallic form.

CO3 2- 0.0014 (25 °C) 0.00155 (25 °C) 0.0022 (18 °C) SO<sup>4</sup> 2- 0.20 0.0148 0.00023 C2O<sup>4</sup> 2- 0.00058 0.0048 0.0125 CrO<sup>4</sup> 2- 2.25 0.204 0.00037

Metallic strontium can be prepared by the electrolysis of mixed melt of strontium chloride and potassium chloride in a graphite crucible using iron rod as cathode. The upper cathode space is cooled and metallic strontium collects around cooled cathode and forms a stick. Metallic strontium can also be prepared by thermal reduction of its oxide with aluminum. Strontium oxide-aluminum mixture is heated at high temperature in vacuum. Strontium is collected by the distillation in vacuum. Strontium is also a reducing agent. It reduces oxides

ing of the product in water [165].

cium and barium salts (Table 1).

Anions Solubility [g∙100 cm-3]

etc. [188].

Pure alumina, which is required for the production of aluminum by the Hall process, is made by the Bayer process [91]. The Bayer process was developed in 1887 by Carl Josef Bayer (1847-1904). It is the method for industrial production of aluminium oxide from bauxite. This method replaces earlier techniques developed by Henri Étienne Sainte-Claire Deville (1818-1881). Fine milled bauxite powder is leached in the solution of sodium hydroxide in autoclave under the temperature range from 160 to 250 °C and the pressure from 0.4 to 0.8 MPa. The basic components of bauxite are dissolved and soluble salts according to the following reaction scheme are formed [189]:

$$\text{Al(OH)}\_{3} + \text{NaOH} \xrightarrow{\text{T}\_{2}\text{p}} \text{NaAl(OH)}\_{4} \tag{22}$$

$$\text{NiO}\_2 + 2\text{ NaOH} \xrightarrow{\text{T}\_3\text{p}} \text{Na}\_2\text{SiO}\_3 + \text{H}\_2\text{O} \tag{23}$$

$$\text{Na}\_2\text{O}\_3 + 2\text{ NaOH} \xrightarrow{\text{T}\_2\text{p}} \text{Na}\_2\text{FeO}\_2 + \text{H}\_2\text{O} \tag{24}$$

$$\text{TiO}\_2 + 2\text{ NaOH} \xrightarrow{\text{T}, \text{p}} \text{Na}\_2\text{TiO}\_3 + \text{H}\_2\text{O} \tag{25}$$

Significant amount of impurities which remains in the dissolved solid rest, so called "**red mud**" (Fig.7), is next separated from the solution by filtration11. The IEP values vary with red mud ranging from 6.35 to 8.70 [347]. The liquid filtrate is then diluted so that the concen‐ tration of Al2O3 in the solution reaches the value of 150 kg Al2O3∙m-3 and the nuclei of Al(OH)3 are introduced [190].

$$\text{Al(OH)}\_{4}\text{I}^{\ast} \xrightarrow{\text{seed}} \text{Al(OH)}\_{3}\text{+OH}^{\ast} \tag{26}$$

The flowing diagram of the process is shown in Fig.9. For the applications where high con‐ tent of **α**-Al2O3 is necessary, the mineralization is accelerated by AlF3 (Eq.29). Several micro‐

Tricalcium aluminate hexahydrate (hydrogarnet) is used as a filter aid during the purifica‐ tion of sodium aluminate liquors. Furthermore, C3AH6 reduces the TiO2 content of precipi‐ tated gibbsite and the formation of hydrogarnet at high-temperature (250 °C) leaching

Fig.8 reveals that aluminium hydroxide can precipitate from the solution by introducing the

The ultrasound [193] and the addition of organics such as methanol [194] and crown ether [195] intensify the nucleation and crystallization of sodium aluminate solution, which has the potential to enhance the throughput of a Bayer process. On the contrary, polyols [196], oleic acid [197] and alditols of hydroxycarboxili acids [198] inhibit the gibbsite precipitation

4 2 3 32 2 Al[OH] +CO 2 Al(OH) +CO +H O ® (30)

carbon dioxide gas. The process can be expressed by the following reaction scheme:


α-Al2O3+3 H2O (29)

Raw Materials for Production of SrAC 59

meter sized plate-like corundum crystals are formed.

minimizes the soda content of red-mud waste [191,192].

**Figure 8.** Bayer process of the production of alumina.

from seeded sodium aluminate liquors.

2 Al(OH)3 →

1250°C,AlF3

The dilution means decreasing the pH of alkaline solution12 and the precipitation of alumini‐ um hydroxide. Precipitated gibbsite (Eq.27), which is the main product of Bayer process, is washed and calcined to Al2O3 in the rotary kiln (Eq.28).

**Figure 7.** Composition of red mud [145].

The purity of prepared aluminium oxide is about 99.5 % and Na2O is the main admixture in the product.

$$\text{NaAl(OH)}\_{4} \rightarrow \gamma\text{-Al(OH)}\_{3} + \text{NaOH} \tag{27}$$

$$2\text{ Al(OH)}\_3 \xrightarrow{950\text{-}1250^\circ \text{C}} \text{Al}\_2\text{O}\_3 + 3\text{ H}\_2\text{O} \tag{28}$$

<sup>11</sup> The deposition lagoon of red mud may be significant ecological load as was demonstrated by industrial accident in Hungary (Aika, 2010).

<sup>12</sup> According to the definition law pH = -log [H3O+ ] = 14 – pOH = 14 – log[OH- ], the teen times dilution causes the decrease of pH by 1.

The flowing diagram of the process is shown in Fig.9. For the applications where high con‐ tent of **α**-Al2O3 is necessary, the mineralization is accelerated by AlF3 (Eq.29). Several micro‐ meter sized plate-like corundum crystals are formed.

$$\text{2Al(OH)}\_{3} \quad \text{\rightarrow} \quad \text{a-Al}\_{2}\text{O}\_{3} + \text{3H}\_{2}\text{O} \tag{29}$$

Tricalcium aluminate hexahydrate (hydrogarnet) is used as a filter aid during the purifica‐ tion of sodium aluminate liquors. Furthermore, C3AH6 reduces the TiO2 content of precipi‐ tated gibbsite and the formation of hydrogarnet at high-temperature (250 °C) leaching minimizes the soda content of red-mud waste [191,192].

Fig.8 reveals that aluminium hydroxide can precipitate from the solution by introducing the carbon dioxide gas. The process can be expressed by the following reaction scheme:

$$2\text{ Al[OH]}\_4 + \text{CO}\_2 \rightarrow 2\text{ Al(OH)}\_3 + \text{CO}\_3^{2\text{\textdegree}} + \text{H}\_2\text{O} \tag{30}$$

**Figure 8.** Bayer process of the production of alumina.

Significant amount of impurities which remains in the dissolved solid rest, so called "**red mud**" (Fig.7), is next separated from the solution by filtration11. The IEP values vary with red mud ranging from 6.35 to 8.70 [347]. The liquid filtrate is then diluted so that the concen‐ tration of Al2O3 in the solution reaches the value of 150 kg Al2O3∙m-3 and the nuclei of

58 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications


The dilution means decreasing the pH of alkaline solution12 and the precipitation of alumini‐ um hydroxide. Precipitated gibbsite (Eq.27), which is the main product of Bayer process, is

The purity of prepared aluminium oxide is about 99.5 % and Na2O is the main admixture in

11 The deposition lagoon of red mud may be significant ecological load as was demonstrated by industrial accident in

] = 14 – pOH = 14 – log[OH-

950-1250°C

NaAl(OH)4→γ-Al(OH)3+NaOH (27)

<sup>3</sup> 23 2 2 Al(OH) ¾¾¾¾¾®Al O +3 H O (28)

], the teen times dilution causes the

4 3 [Al(OH) ] Al(OH) +OH ¾¾¾® (26)

Al(OH)3 are introduced [190].

**Figure 7.** Composition of red mud [145].

12 According to the definition law pH = -log [H3O+

the product.

Hungary (Aika, 2010).

decrease of pH by 1.

washed and calcined to Al2O3 in the rotary kiln (Eq.28).

The ultrasound [193] and the addition of organics such as methanol [194] and crown ether [195] intensify the nucleation and crystallization of sodium aluminate solution, which has the potential to enhance the throughput of a Bayer process. On the contrary, polyols [196], oleic acid [197] and alditols of hydroxycarboxili acids [198] inhibit the gibbsite precipitation from seeded sodium aluminate liquors.

## **1.3. Utilization of red mud**

The treatment and utilization of red mud waste are major challenge for the alumina indus‐ try. The main environmental risks associated with bauxite residue are related to high pH and alkalinity and minor and trace amounts of heavy metals and radionuclides. Many ef‐ forts are being globally made to find suitable applications for red mud so that the alumina industry may end up with no residue [199].

absorbed by solar collectors [214,215], as the catalyst [216,217] and for rubidium recovery

Ammonium aluminum sulfate (AAlSD14) dodecahydrate undergoes the phase transitions at 58 K and 71 K on cooling and heating, respectively. At room temperature NH4Al(SO4)2∙12 H2O crystals have a cubic structure and belong to the space group with four molecules per unit cell with the lattice parameters *a*=12.242 Å. The structural phase transition mechanism is related to the hydrogen-bond transfer involving the breakage of weak part of the hydro‐

The process of alum derived synthesis of alumina often produces nanosized powders con‐ sisting of amorphous or transition aluminas (Chapter 4.1). The thermal decomposition of

The preparation of submicrometer-grained aluminas requires well-defined pure nanopow‐ ders which have many exploitable characteristics, such as low-temperature sinterability, greater chemical reactivity and enhanced plasticity. Therefore, whole range of methods was developed for the preparation of nanopowders with desired properties. These can be rough‐

**• High temperature/ flame/ laser synthesis:** the method usually comprises the injection of suitable gaseous or liquid aluminium-containing precursors (e.g. aluminum tri-sec-butox‐ ide) into the source of intensive heat (flame, laser or plasma), where the precursor decom‐ poses and converts into oxide. In most cases, the transient aluminas are formed. Therefore

**• Chemical method including the sol-gel process:** obviously utilizes the low-and mediumtemperature decomposition of inorganic aluminium salts and hydroxides or metal-organ‐ ic compounds of aluminium. Typical precursors include aluminium nitrate and

**• Mechanically assisted synthesis:** the method is based on high-energy milling of coarsergrained powder. In this case, the minimum particle size is limited to approximately 40 nm.

further high-temperature treatment is necessary in order to obtain *α*-Al2O3.

14 Abbreviation, another example is CsAlSeD (CsAl(SeO4)⋅12H2O).

~225 °C NH Al(SO ) ×12 H O NH Al(SO ) +12 H O 4 42 2 ¾¾¾¾® 4 42 2 (31)

4 42 2 43 3 3 2 2 NH Al(SO ) ¾¾¾¾®Al (SO ) +2 NH +SO +H O (32)

~900 °C Al (SO ) 2 42 ¾¾¾¾®Al O +3 SO 23 3 (33)

Raw Materials for Production of SrAC 61

aluminium alum can be described according to the following reaction scheme [219]:

~600 °C

from the processing of zinnwaldite [218].

gen bond [208].

ly devided to [424]:

hydroxides.

The possible applications of red mud include [199-204]:


## **1.4. Methods of production of high purity Al2O3**

Aluminium oxide of high purity and high specific surface area can be prepared by thermal decomposition of alum (NH4Al(SO4)2⋅12 H2O)13. Pure ammonium alum crystal is colorless and transparent and belongs to cubic crystal system. Melting temperature of ammonium alum crystal is 94.5 °C with the phase transition enthalpy of 122.2 kJ mol-1. [205-209]. NH4Al(SO4)2∙12 H2O is widely applied in industries and in water treatment [210,211]. Re‐ cently, ammonium alum is used as a promising material for Raman laser converters with a large frequency shift [212], for ferroelectricity [213] and phase transitions for storing energy

<sup>13</sup> Alums can be described by general formula M+ Me3+(RO4)2⋅12H2O, where M+ is monovalent cation such as Na+ , K+ , Rb+ , Cs+ or NH4 + , Me3+ is trivalent cation such as Al3+, Fe3+, Cr3+ and R is S or Se. Each M+ and Me3+ ion is surrounded by an octahedron of six water molecules. A complex network of H-bonds is one of the main features of alum structures. Alums are classified into α (RbAl(SO4)2⋅12H2O and NH4Al(SO4)2⋅12H2O), β (CsAl(SO4)2⋅12H2O), and γ (NaAl(SO4)2⋅12H2O) modifications depending upon three slightly different arrangements of ions and molecules within the cubic lattice. The different structures are characterized by different orientations of sulfate ions with respect to the trigonal axes of unit cell [208,209].

absorbed by solar collectors [214,215], as the catalyst [216,217] and for rubidium recovery from the processing of zinnwaldite [218].

**1.3. Utilization of red mud**

industry may end up with no residue [199].

and low density foamed products.

The possible applications of red mud include [199-204]:

tion concretes, repairs of roads, pavements, dykes.

**•** Foamed paper in wood pulp and paper industry.

**•** Special use as inorganic chemicals, adsorbents, etc.

er) for iron ores, flux in steel making, etc.

13 Alums can be described by general formula M+

trigonal axes of unit cell [208,209].

Rb+ , Cs+ or NH4 +

The treatment and utilization of red mud waste are major challenge for the alumina indus‐ try. The main environmental risks associated with bauxite residue are related to high pH and alkalinity and minor and trace amounts of heavy metals and radionuclides. Many ef‐ forts are being globally made to find suitable applications for red mud so that the alumina

60 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

**•** Building/construction materials such as bricks, stabilized blocks, light weight aggregates

**•** In cement industry as cements, special cements, additives to cements, mortars, construc‐

**•** In metallurgical industries, as raw material in iron and steel industry as a sinter aid (bind‐

Aluminium oxide of high purity and high specific surface area can be prepared by thermal decomposition of alum (NH4Al(SO4)2⋅12 H2O)13. Pure ammonium alum crystal is colorless and transparent and belongs to cubic crystal system. Melting temperature of ammonium alum crystal is 94.5 °C with the phase transition enthalpy of 122.2 kJ mol-1. [205-209]. NH4Al(SO4)2∙12 H2O is widely applied in industries and in water treatment [210,211]. Re‐ cently, ammonium alum is used as a promising material for Raman laser converters with a large frequency shift [212], for ferroelectricity [213] and phase transitions for storing energy

Me3+(RO4)2⋅12H2O, where M+

an octahedron of six water molecules. A complex network of H-bonds is one of the main features of alum structures. Alums are classified into α (RbAl(SO4)2⋅12H2O and NH4Al(SO4)2⋅12H2O), β (CsAl(SO4)2⋅12H2O), and γ (NaAl(SO4)2⋅12H2O) modifications depending upon three slightly different arrangements of ions and molecules within the cubic lattice. The different structures are characterized by different orientations of sulfate ions with respect to the

, Me3+ is trivalent cation such as Al3+, Fe3+, Cr3+ and R is S or Se. Each M+

is monovalent cation such as Na+

and Me3+ ion is surrounded by

, K+ ,

**•** Extracting rare-earth metals and alumo-ferric coagulants as technical raw materials.

**•** Colouring agents for paint works for ground floors of industrial and other buildings.

**•** Reinforced red mud polymer products, ceramic/refractory products.

**•** Micro-fertilizer and a neutralizer of pesticides in agriculture.

**1.4. Methods of production of high purity Al2O3**

Ammonium aluminum sulfate (AAlSD14) dodecahydrate undergoes the phase transitions at 58 K and 71 K on cooling and heating, respectively. At room temperature NH4Al(SO4)2∙12 H2O crystals have a cubic structure and belong to the space group with four molecules per unit cell with the lattice parameters *a*=12.242 Å. The structural phase transition mechanism is related to the hydrogen-bond transfer involving the breakage of weak part of the hydro‐ gen bond [208].

The process of alum derived synthesis of alumina often produces nanosized powders con‐ sisting of amorphous or transition aluminas (Chapter 4.1). The thermal decomposition of aluminium alum can be described according to the following reaction scheme [219]:

$$\text{NH}\_4\text{Al(SO}\_4)\_2 \times 12\text{ H}\_2\text{O} \xrightarrow{\text{-}225\text{ °C}} \text{NH}\_4\text{Al(SO}\_4)\_2 + 12\text{ H}\_2\text{O} \tag{31}$$

$$2\text{ NH}\_4\text{Al}(\text{SO}\_4)\_2 \xrightarrow{-600^\circ \text{C}} \text{Al}\_2(\text{SO}\_4)\_3 + 2\text{ NH}\_3 + \text{SO}\_3 + \text{H}\_2\text{O} \tag{32}$$

$$\text{Al}\_2(\text{SO}\_4)\_2 \xrightarrow{\text{-}900 \text{ V}} \text{Al}\_2\text{O}\_3 + 3 \text{ SO}\_3 \tag{33}$$

The preparation of submicrometer-grained aluminas requires well-defined pure nanopow‐ ders which have many exploitable characteristics, such as low-temperature sinterability, greater chemical reactivity and enhanced plasticity. Therefore, whole range of methods was developed for the preparation of nanopowders with desired properties. These can be rough‐ ly devided to [424]:


<sup>14</sup> Abbreviation, another example is CsAlSeD (CsAl(SeO4)⋅12H2O).

**•** Other options include the combustion synthesis [220-224], the spray pyrolysis of aerosol of nitrate or other aluminum salts [225-227], the sol-gel process [228,229], the emulsion synthesis [230,231], etc.

#### **2. Adjustment of clinker composition**

Strontium aluminate is formed via solid-state reaction of equimolar amount of aluminium oxide with strontium oxide:

$$\rm Al\_2O\_3 + SrO \to SrAl\_2O\_4 \tag{34}$$

first eutectic melt is formed at the temperature of 1760 °C instead of 1505 °C for the cement

The composition of mixture of raw materials is calculated from required composition of

The preparation of raw meal using only two components is a simple process. The example could be strontium carbonate with 98.4 % SrCO3 and alumina which does not contain any strontium carbonate. The analysing techniques are described in Chapter 2.4. From Eq.34 it can be read that equimolar mixture of SrCO3 and Al2O3 (*x*Al2O3=0.5) should be prepared. That means that *x*SrCO3=0.5 and *x*Al2O3=1 – *x*SrCO3=0.5. The molar ratio can be recalculated to the

=1

1 1 1 1

= = å å = Þ = *k k i ki i i*

From the relationships introduced above we can calculate:

3

15 Please see Eqs.18 and 19 in Chapter 1.

*j*

*x M <sup>w</sup>*

*i i k*

*j j*

0.5 147.6 0,591 59.1% 0.5 147.6 0.5 102,0 <sup>×</sup> <sup>=</sup> = Þ

1

× +× *wSrCO* (44)


= å

SrCO =1.425 SrO <sup>3</sup> (39)

Raw Materials for Production of SrAC 63

Al(OH) =0.765×Al O <sup>3</sup> 2 3 (40)

3 3 others=100-SrCO -Al(OH) (41)

*x M* (42)

*w ww* (43)

with *SD*SrO > 100.

weight ratio as follows15:

clinker according to the following relations:

**3. Calculation of the raw meal composition**

With regard to the molar weight ratios of SrO/Al2O3=1.016 and SrO/Fe2O3=0.65, the proper amount of SrO should be calculated as follows:

$$\text{SrO=1.016 Al}\_2\text{O}\_3 + 0.65 \,\text{Fe}\_2\text{O}\_3 \tag{35}$$

The mass ratio of used SrO and the theoretical amount calculated according to Eq.34 should be termed as the "**Saturation Degree**" or "**Strontium saturation factor**" of clinker by stronti‐ um oxide (*SD*SrO):

$$\text{SD}\_{\text{SrO}} = \frac{100 \,\text{SrO}}{1.016 \,\text{Al}\_2\text{O}\_3 + 0.65 \,\text{Fe}\_2\text{O}\_3} \qquad \left[ \,^{\text{[\%]}} \right] \tag{36}$$

Analogically to ordinary Portland cement, the hydraulic module (*M*H) and the alumina module (*M*A) of strontium aluminate clinker should be defined:

$$\text{M}\_{\text{H}} = \frac{\text{SrO}}{\text{Al}\_2\text{O}\_3 + \text{Fe}\_2\text{O}\_3} \tag{37}$$

$$\mathbf{M}\_{\rm A} = \frac{\mathbf{A}\mathbf{l}\_2 \mathbf{O}\_3}{\mathbf{F}\mathbf{e}\_2 \mathbf{O}\_3} \tag{38}$$

To use the strontium aluminate cements for the production of refractory materials the value of *SD*SrO < 100 and low content of Fe2O3 are required. These compositions ensure that the first eutectic melt is formed at the temperature of 1760 °C instead of 1505 °C for the cement with *SD*SrO > 100.

The composition of mixture of raw materials is calculated from required composition of clinker according to the following relations:

$$\text{SrCO}\_3 \text{=} 1.425 \,\text{SrO} \tag{39}$$

$$\text{Al(OH)}\_{3} = 0.765 \times \text{Al}\_{2}\text{O}\_{3} \tag{40}$$

$$\text{Tothers} = 100 \text{-SrCO}\_3 \text{-Al(OH)}\_3 \tag{41}$$

#### **3. Calculation of the raw meal composition**

**•** Other options include the combustion synthesis [220-224], the spray pyrolysis of aerosol of nitrate or other aluminum salts [225-227], the sol-gel process [228,229], the emulsion

62 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

Strontium aluminate is formed via solid-state reaction of equimolar amount of aluminium

With regard to the molar weight ratios of SrO/Al2O3=1.016 and SrO/Fe2O3=0.65, the proper

The mass ratio of used SrO and the theoretical amount calculated according to Eq.34 should be termed as the "**Saturation Degree**" or "**Strontium saturation factor**" of clinker by stronti‐

> SrO [ ] 23 23

Analogically to ordinary Portland cement, the hydraulic module (*M*H) and the alumina

23 23

2 3

2 3

To use the strontium aluminate cements for the production of refractory materials the value of *SD*SrO < 100 and low content of Fe2O3 are required. These compositions ensure that the

100 SrO SD = %

module (*M*A) of strontium aluminate clinker should be defined:

H

SrO M =

A

Al O M =

Al O +SrO SrAl O 2 3 ® 2 4 (34)

SrO=1.016 Al O +0.65 Fe O 23 23 (35)

1.016 Al O +0.65 Fe O (36)

Al O +Fe O (37)

Fe O (38)

synthesis [230,231], etc.

oxide with strontium oxide:

um oxide (*SD*SrO):

**2. Adjustment of clinker composition**

amount of SrO should be calculated as follows:

The preparation of raw meal using only two components is a simple process. The example could be strontium carbonate with 98.4 % SrCO3 and alumina which does not contain any strontium carbonate. The analysing techniques are described in Chapter 2.4. From Eq.34 it can be read that equimolar mixture of SrCO3 and Al2O3 (*x*Al2O3=0.5) should be prepared. That means that *x*SrCO3=0.5 and *x*Al2O3=1 – *x*SrCO3=0.5. The molar ratio can be recalculated to the weight ratio as follows15:

$$\begin{aligned} \lambda w &= \frac{\boldsymbol{\chi}\_i \boldsymbol{M}\_i}{\sum\_{j=1}^k \boldsymbol{\chi}\_j \boldsymbol{M}\_j} \\ &\sum\_{j=1}^k \boldsymbol{\chi}\_j \boldsymbol{M}\_j \end{aligned} \tag{42}$$

$$\sum\_{i=1}^{k} w\_i = 1 \quad \Rightarrow \quad w\_k = 1 - \sum\_{i=1}^{k-1} w\_i \tag{43}$$

From the relationships introduced above we can calculate:

$$\text{Cov}\_{SrCO\_3} = \frac{0.5 \cdot 147.6}{0.5 \cdot 147.6 + 0.5 \cdot 102.0} = 0,591 \Rightarrow 59.1\% \tag{44}$$

<sup>15</sup> Please see Eqs.18 and 19 in Chapter 1.

$$\text{Cov}\_{Al\_2O\_3} = 1 - 0.591 \Longrightarrow 0.409 \Longrightarrow 40.9\% \tag{45}$$

<sup>22</sup> *a* = - × =- 0 0.98 99.8 97.8 (51)

**Raw meal**

<sup>123</sup> *www* ++=100 (53)

21 1 22 2 23 3 *aw aw aw* ++= 0 (54)

(52)

Raw Materials for Production of SrAC 65

From the substitution of 48 by 50 and 51 the following relationship results:

1 2 22

*w w*


100 98.2 97.8 0

21 2 1 22 21

*<sup>a</sup> w w <sup>a</sup>*


1 98.4 0 0.2 49.9 48,3 0 0,1 2 0 98.2 1.6 50.1 0 49,2 0,8 Total 100.0 49,1 49,2 0,9

× - == = -

100 100 ( 97.8) 49.9% -97.8-98.2 100 ( ) 100 50.1%

**[%]**

Another case is that the mixture requires the preparation via **mixing of three raw materials**, e.g. we have strontium carbonate, calcined bauxite and corundum. Corundum is necessary to keep the value of hydraulic module (*M*H)=0.98 and alumina module (*M*A)=57. The compo‐

**Raw material SrO Al2O3 Fe2O3 Z =Al2O3+Fe2O3**

SrCO3 1 98.4 0 0.2 0.2 Calcined bauxite 2 0 98.2 1.6 99.8 Corundum 3 0 99.5 0.1 99.6

**Table 3.** Composition of three raw materials for the preparation of raw meal.

**SrO Al2O3 Fe2O3 SrO Al2O3 Fe2O3**

22 11

a

Now it is possible to check, if the calculated results are correct:

**Composition wi**

MH 49,1/ (49.2 + 0,9) = 0.98

sition of raw materials is listed in Table 3.

1 2

*w w*

+ =

*<sup>a</sup> <sup>w</sup> a a*

1

**Raw material**

The amount of raw mixture constituent can be then calculated:

$$\begin{array}{ccccc} \text{SrCO}\_3 & 98.4 & \text{SrO} & 100 \times \text{59.1} (\text{\"(59.1+39.3)=60.1\text{\"(} }\\ & & \text{59.1} & & \\ \text{Al}\_2\text{O}\_3 & 0 & & \text{39.3} & \text{\text{\"(} } \text{100} \times \text{\"(59.1+39.3)=39.9\text{\"(} }\end{array} \tag{46}$$

The raw meal contains 60.1 % of strontium carbonate and 39.9 % of alumina, i.e. both com‐ ponents are mixed in the weight ratio of 1.5 : 1.

#### **3.1. Calculation of required hydraulic module**

The preparation of raw meal of given value of hydraulic module (Eq.37) is demonstrated in this chapter. As an example the raw meal for the strontium aluminate clinker with *M*H=0.98 will be prepared. There are **two raw materials** with the composition given in Table 2.


**Table 2.** Composition of two raw materials for the preparation of raw meal.

Hence we have two equations:

$$\mathbf{w}\_1 + \mathbf{w}\_2 = 100 \tag{47}$$

$$a\_{21}w\_1 + a\_{22}w\_2 = 0\tag{48}$$

where:

$$a\_{2i} = SrO - M\_H Z\_i \qquad \left(i = 1, 2\right) \tag{49}$$

From the relationships introduced above we can calculate:

$$a\_{21} = 98.4 - 0.98 \cdot 0.2 = 98.2\tag{50}$$

$$a\_{22} = 0 - 0.98 \cdot 99.8 = -97.8\tag{51}$$

From the substitution of 48 by 50 and 51 the following relationship results:

2 3 *wAl O* =- Þ Þ 1 0,591 0.409 40.9% (45)

1 2 *w w*+ =100 (47)

21 1 22 2 *aw aw* + = 0 (48)

<sup>2</sup> =- = ( ) 1, 2 *<sup>i</sup> H i a SrO M Z i* (49)

<sup>21</sup> *a* = - ×= 98.4 0.98 0.2 98.2 (50)

(46)

The amount of raw mixture constituent can be then calculated:

59.1

SrCO 98.4 59.1 Þ 100×59.1/(59.1+39.3)=60.1%

64 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

Al O 0 39.3 Þ 100×39.3/(59.1+39.3)=39.9%

The raw meal contains 60.1 % of strontium carbonate and 39.9 % of alumina, i.e. both com‐

The preparation of raw meal of given value of hydraulic module (Eq.37) is demonstrated in this chapter. As an example the raw meal for the strontium aluminate clinker with *M*H=0.98

will be prepared. There are **two raw materials** with the composition given in Table 2.

**Raw material SrO Al2O3 Fe2O3 Z =Al2O3+Fe2O3**

SrCO3 1 98.4 0 0.2 0.2 Calcined bauxite 2 0 98.2 1.6 99.8

**Table 2.** Composition of two raw materials for the preparation of raw meal.

From the relationships introduced above we can calculate:

3

ponents are mixed in the weight ratio of 1.5 : 1.

**3.1. Calculation of required hydraulic module**

2 3

Hence we have two equations:

where:

$$\begin{aligned} \begin{cases} w\_1 + w\_2 = 100 \\ 98.2 \ w\_1 - 97.8 \ w\_2 = 0 \\ w\_1 = \frac{100 \ a\_{22}}{a\_{22} - a\_{11}} = \frac{100 \cdot (-97.8)}{\cdot 97.8 \ - 98.2} = 49.9\% \\ w\_2 = \frac{100 \ (-a\_{21})}{a\_{22} - a\_{21}} = 100 - w\_{11} = 50.1\% \end{cases} \end{aligned} \tag{52}$$

Now it is possible to check, if the calculated results are correct:


Another case is that the mixture requires the preparation via **mixing of three raw materials**, e.g. we have strontium carbonate, calcined bauxite and corundum. Corundum is necessary to keep the value of hydraulic module (*M*H)=0.98 and alumina module (*M*A)=57. The compo‐ sition of raw materials is listed in Table 3.


**Table 3.** Composition of three raw materials for the preparation of raw meal.

$$\mathbf{w}\_1 + \mathbf{w}\_2 + \mathbf{w}\_3 = 100 \tag{53}$$

$$a\_{21}w\_1 + a\_{22}w\_2 + a\_{23}w\_3 = 0\tag{54}$$

66 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

$$a\_{31}w\_1 + a\_{32}w\_2 + a\_{33}w\_3 = 0\tag{55}$$

The composition of raw meal is then:

**Raw material**

1

2

100

3

100

100

3 12

*w ww*

**Composition wi**

MH 49.10/ (49.24 + 0.86) = 0.98

**Raw material SrO Al2O3 Fe2O3** SrCO3 1 97.3 0 0.3 Calcined bauxite 2 0 96.5 2.6 Corundum 3 0 99.7 0.1

MA 49.24/ 0.86 = 57

**Table 4.** Composition of three raw materials for the preparation of raw meal.

**3.2. Calculation from the saturation degree**

ed in Table 4 will be prepared.

=-+ =

*aa aa <sup>w</sup> <sup>D</sup>*

( 22 33 32 23 )

( 21 33 31 23 )

( )

21 32 31 22

( )

100 2.5 %

Now it is possible, as previously, to check, if the calculated results are correct:

 98.4 0 0.2 49.9 49.10 0 0.10 0 98.2 1.6 47.6 0 46.74 0.76 0 99.5 0.1 2.5 0 2.50 0 Total 100 49.10 49.24 0.86

**[%]**

The method of calculation of raw meal for the preparation of strontium aluminate clinker with given Saturation Degree (*SD*SrO) and alumina module (*M*A) is described. As an example the mixture with *SD*SrO=0.95 and *M*A=60 using three raw materials with the composition list‐

**SrO Al2O3 Fe2O3 SrO Al2O3 Fe2O3**


49.9% - - = = *aa aa <sup>w</sup> <sup>D</sup>* (66)

47.6% - - = = *aa aa <sup>w</sup> <sup>D</sup>* (67)

**Raw meal**

(68)

Raw Materials for Production of SrAC 67

2.5% or

Where:

$$a\_{2i} = \text{SrO} - M\_H Z\_{\text{ii}} \tag{56}$$

$$a\_{3i} = Al\_2O\_3 - M\_AFe\_2O\_3 \qquad \text{ ( $i = 1, 2, 3$ )}\tag{57}$$

From the relationships introduced above we can calculate:

$$a\_{21} = 98.4 - 0.98 \cdot 0.2 = 98.2\tag{58}$$

$$a\_{22} = 0 - 0.98 \cdot 99.8 = -97.8\tag{59}$$

$$a\_{23} = 0 - 0.98 \cdot 99.6 = -97.6\tag{60}$$

$$a\_{31} = 0 - \\$0 \cdot 0.2 = -1 \,\text{l.}\,4\tag{61}$$

$$a\_{32} = 98.2 - 50 \cdot 1.6 = 7.0\tag{62}$$

$$a\_{33} = 99.5 - 50 \cdot 0.1 = 93.8 \tag{63}$$

The substitution of equations 53-55 by Eq.58-63 yields to:

$$\begin{aligned} \left(\boldsymbol{\mu}\_{1} + \boldsymbol{\mu}\_{2} + \boldsymbol{\mu}\_{3} = 100 \\ \text{98.2 } \boldsymbol{\mu}\_{1} - 97.8 \text{ } \boldsymbol{\mu}\_{2} - 97.6 \text{ } \boldsymbol{\mu}\_{3} = 0 \\ \boldsymbol{\mu}\_{1} - 11.4 \text{ } \boldsymbol{\mu}\_{1} + 7.0 \text{ } \boldsymbol{\mu}\_{2} + 93.8 \text{ } \boldsymbol{\mu}\_{3} = 0 \end{aligned} \tag{64}$$

The value of determinant *D* can be calculated as follows:

$$\begin{aligned} D &= a\_{22} \ a\_{33} - a\_{32} \ a\_{23} - \left( a\_{21} \ a\_{33} - a\_{31} \ a\_{23} \right) + a\_{21} \ a\_{32} - a\_{31} \ a\_{22} \\ D &= -9174.0 - 683.3 - \left( 9211.5 - 1112.7 \right) + 687.4 - 1115.0 \\ D &= -17017.1 \end{aligned} \tag{65}$$

The composition of raw meal is then:

31 1 32 2 33 3 *aw aw aw* ++= 0 (55)

<sup>2</sup>*<sup>i</sup>* = - *H i a SrO M Z* (56)

3 23 23 =- = ( ) 1, 2, 3 *i A a Al O M Fe O i* (57)

<sup>21</sup> *a* = - ×= 98.4 0.98 0.2 98.2 (58)

<sup>22</sup> *a* = - × =- 0 0.98 99.8 97.8 (59)

<sup>23</sup> *a* = - × =- 0 0.98 99.6 97.6 (60)

<sup>31</sup> *a* = - × =- 0 50 0.2 11.4 (61)

<sup>32</sup> *a* = -× = 98.2 50 1.6 7.0 (62)

<sup>33</sup> *a* = -× = 99.5 50 0.1 93.8 (63)

(64)

(65)

Where:

From the relationships introduced above we can calculate:

66 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

The substitution of equations 53-55 by Eq.58-63 yields to:

The value of determinant *D* can be calculated as follows:

17017.1

= -

*D D* 123

*www*

++=

123 12 3

*ww w ww w*



( ) ( ) 22 33 32 23 21 33 31 23 21 32 31 22 9174.0 683.3 9211.5 1112.7 687.4 1115.0

=-- - +- =- - - - + -

*D aa aa aa aa aa aa*

100 98.2 97.8 97.6 0 11.4 7.0 93.8 0

$$\text{cov}\_{\text{l}} = \frac{-100 \left(a\_{22} \ a\_{33} - a\_{32} \ a\_{23}\right)}{D} = 49.9\% \tag{66}$$

$$\%w\_2 = \frac{-100\left(a\_{21}\ a\_{33} - a\_{31}\ a\_{23}\right)}{D} = 47.6\% \tag{67}$$

$$\begin{aligned} \text{aw}\_3 &= \frac{100 \left( a\_{21} a\_{32} - a\_{31} a\_{22} \right)}{D} = 2.5\text{\%} & \text{or} \\ \text{aw}\_3 &= 100 - \left( w\_1 + w\_2 \right) = 2.5 \text{\%} \end{aligned} \tag{68}$$

Now it is possible, as previously, to check, if the calculated results are correct:


#### **3.2. Calculation from the saturation degree**

The method of calculation of raw meal for the preparation of strontium aluminate clinker with given Saturation Degree (*SD*SrO) and alumina module (*M*A) is described. As an example the mixture with *SD*SrO=0.95 and *M*A=60 using three raw materials with the composition list‐ ed in Table 4 will be prepared.


**Table 4.** Composition of three raw materials for the preparation of raw meal.

The composition of raw meal results from the solution of the following set of three equa‐ tions:

$$
\hbar \mathbf{w}\_1 + \mathbf{w}\_2 + \mathbf{w}\_3 = 100 \tag{69}
$$

The composition of raw meal is then:

1

2

100

3

**Raw material**

100

100

3 12

*w ww*

**Composition wi**

MH 48.48/ (49.23 + 0.82) = 0.97

MA 49.23/ 0.82 = 60

**3.3. Calculation with SDSrO, MA and other parameter**

mina module can be redefined as follows:

=-+ =

*aa aa <sup>w</sup> <sup>D</sup>*

( 22 33 32 23 )

( 21 33 31 23 )

( )

21 32 31 22

( )


100 25.3 %

Now it is possible, as previously, to check, if the calculated results are correct:

 97.3 0 0.3 49.8 48.48 0 0,15 0 96.5 2.6 24.8 0 23.97 0,65 0 99.7 0.1 25.3 0 25,27 0,03 Total 100 48,48 49,23 0,82

**[%]**

Using four raw materials for the preparation of raw meal where other parameter can be used for calculation. That can be useful for the preparation of cement with exceeding substi‐ tution of alumina. For example, the Saturation Degree of clinker by strontium oxide and alu‐

> [ ] \* 23 23 23

> > 23 23 Al O Fe O +Cr O

1.016 Al O +0.65 Fe O +0.68 Cr O

\* 2 3

100 SrO %

*SDSrO* = (84)

*M <sup>A</sup>* = (85)

**SrO Al2O3 Fe2O3 SrO Al2O3 Fe2O3**

49.8% - - = = *aa aa <sup>w</sup> <sup>D</sup>* (81)

24.8% - - = = *aa aa <sup>w</sup> <sup>D</sup>* (82)

**Raw meal**

(83)

Raw Materials for Production of SrAC 69

25.3% or

$$a\_{21}w\_1 + a\_{22}w\_2 + a\_{23}w\_3 = 0\tag{70}$$

$$a\_{31}w\_1 + a\_{32}w\_2 + a\_{33}w\_3 = 0\tag{71}$$

where

$$a\_{2i} = \text{SrO-SD}\_{\text{SiO}} \left( 1.016 \,\text{Al}\_2\text{O}\_3 + 0.65 \,\text{Fe}\_2\text{O}\_3 \right) \tag{72}$$

$$\mathbf{a}\_{3i} = \mathbf{A} \mathbf{l}\_2 \mathbf{O}\_3 \text{-M}\_\text{A} \text{ Fe}\_2\text{O}\_3 \qquad \text{ (} i = \text{l, 2, 3)}\tag{73}$$

From the relationships introduced above we can calculate:

$$a\_{21} = 90.3 - 0.96 \left( 1.016 \cdot 0 + 0.65 \cdot 0.3 \right) = 90.2 \tag{74}$$

$$a\_{22} = 0 - 0.96 \left( 1.016 \cdot 96.5 + 0.65 \cdot 2.6 \right) = -95.6 \tag{75}$$

$$a\_{23} = 0 - 0.96 \left( 1.016 \cdot 99.7 + 0.65 \cdot 0.1 \right) = -97.2 \tag{76}$$

$$a\_{31} = 0 - 60 \cdot 0.3 = -18.0\tag{77}$$

$$a\_{32} = 96.5 - 60 \cdot 2.6 = -59.5\tag{78}$$

$$a\_{33} = 99.7 - 60 \cdot 0.1 = 93.7\tag{79}$$

The value of determinant *D* can be calculated as follows:

$$\begin{aligned} D &= a\_{22} \ a\_{33} - a\_{32} \ a\_{23} - \left( a\_{21} \ a\_{33} - a\_{31} \ a\_{23} \right) + a\_{21} \ a\_{32} - a\_{31} \ a\_{22} \\ D &= -8960.3 - \ $783.9 - \left( 9099.7 - 1749.8 \right) - \$ 778.4 - 1721.3 \\ D &= -29593.8 \end{aligned} \tag{80}$$

The composition of raw meal is then:

The composition of raw meal results from the solution of the following set of three equa‐

68 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

From the relationships introduced above we can calculate:

The value of determinant *D* can be calculated as follows:

29593.8

= -

*D D*

( ) ( ) 22 33 32 23 21 33 31 23 21 32 31 22 8960.3 5783.9 9099.7 1749.8 5778.4 1721.3

=-- - +- =- - - - - -

*D aa aa aa aa aa aa*

<sup>123</sup> *www* ++=100 (69)

21 1 22 2 23 3 *aw aw aw* ++= 0 (70)

31 1 32 2 33 3 *aw aw aw* ++= 0 (71)

*a*2*<sup>i</sup>* = SrO-SD 1.016 Al O +0.65 Fe O SrO 2 3 2 3 ( ) (72)

*a i* 3 23 A 23 *<sup>i</sup>* = = Al O -M Fe O 1, 2, 3 ( ) (73)

*a*<sup>21</sup> = - ×+ × = 90.3 0.96 1.016 0 0.65 0.3 90.2 ( ) (74)

*a*<sup>22</sup> = - × + × =- 0 0.96 1.016 96.5 0.65 2.6 95.6 ( ) (75)

*a*<sup>23</sup> = - × + × =- 0 0.96 1.016 99.7 0.65 0.1 97.2 ( ) (76)

<sup>31</sup> *a* = - × =- 0 60 0.3 18.0 (77)

<sup>32</sup> *a* = - × =- 96.5 60 2.6 59.5 (78)

<sup>33</sup> *a* = -× = 99.7 60 0.1 93.7 (79)

(80)

tions:

where

$$\text{cov}\_{\text{l}} = \frac{-100 \left( a\_{22} \ a\_{33} - a\_{32} \ a\_{23} \right)}{D} = 49.8\% \tag{81}$$

$$\%w\_2 = \frac{-100\left(a\_{21}\ a\_{33} - a\_{31}\ a\_{23}\right)}{D} = 24.8\% \tag{82}$$

$$\begin{aligned} \text{aw}\_3 &= \frac{100 \left( a\_{21} \, a\_{32} - a\_{31} \, a\_{22} \right)}{D} = 25.3\% \qquad \text{or} \\ \text{aw}\_3 &= 100 - \left( w\_1 + w\_2 \right) = 25.3 \, \% \end{aligned} \tag{83}$$

Now it is possible, as previously, to check, if the calculated results are correct:


#### **3.3. Calculation with SDSrO, MA and other parameter**

Using four raw materials for the preparation of raw meal where other parameter can be used for calculation. That can be useful for the preparation of cement with exceeding substi‐ tution of alumina. For example, the Saturation Degree of clinker by strontium oxide and alu‐ mina module can be redefined as follows:

$$\text{SD}\_{\text{SnO}}^{\bullet} = \frac{100 \text{ SrO}}{1.016 \text{ Al}\_2\text{O}\_3 + 0.65 \text{ Fe}\_2\text{O}\_3 + 0.68 \text{ Cr}\_2\text{O}\_3} \qquad \text{[\%]} \tag{84}$$

$$\boldsymbol{M}\_A^\* = \frac{\text{Al}\_2\text{O}\_3}{\text{Fe}\_2\text{O}\_3 + \text{Cr}\_2\text{O}\_3} \tag{85}$$

Therefore a new type of module can be applied:

$$M\_{\rm Fe} = \frac{\rm Fe\_2O\_3}{\rm Cr\_2O\_3} \tag{86}$$

From the relationships introduced above we can calculate:

From the relationships introduced above we can further calculate:

*a*<sup>21</sup> = - ×+ × + × = 97.3 0.90 1.016 0 0.65 0.3 0.68 0 97.1 ( ) (94)

Raw Materials for Production of SrAC 71

*a*<sup>22</sup> = - × + × + × =- 0 0.90 1.016 96.5 0.65 2.6 0.68 0 89.8 ( ) (95)

*a*<sup>23</sup> = - × + × + × =- 0 0.90 1.016 99.7 0.65 0.1 0.68 0 91.2 ( ) (96)

*a*<sup>24</sup> = - × + × + × =- 0 0.90 1.016 2.8 0.65 1.5 0.68 32.6 23.4 ( ) (97)

*a*<sup>31</sup> = - + =- 0 58.0 0.3 0 17.4 ( ) (98)

*a*<sup>32</sup> = - + =- 96.5 58.0 2.6 0 54.3 ( ) (99)

*a*<sup>33</sup> = - += 99.7 58.0 0.1 0 93.9 ( ) (100)

*a*<sup>34</sup> = - + =- 2.8 58.0 1.5 32.6 1975.0 ( ) (101)

<sup>41</sup> *a* = - ×= 0.3 10.0 0 0.3 (102)

<sup>42</sup> *a* = - ×= 2.6 10.0 0 2.6 (103)

<sup>43</sup> *a* = - ×= 0.1 10.0 0 0.1 (104)

<sup>44</sup> *a* = - × =- 1.5 10.0 32.6 324.5 (105)

<sup>1234</sup> *wwww* +++=100 (106)

12 3 4 97.1 89.8 91.2 23.4 0 *ww w w* - +- - = (107)

This is the case of raw meal the preparation of strontium aluminate clinker with following parameters *SD*SrO\* =0.90, *M*<sup>A</sup> \* =58 and *M*F=10. The composition of raw materials is listed in Ta‐ ble 5.


**Table 5.** Composition of four raw materials for the preparation of raw meal.

The composition of raw meal results from the solution of the following set of four equations:

$$\mathbf{w}\_1 + \mathbf{w}\_2 + \mathbf{w}\_3 + \mathbf{w}\_4 = 100 \tag{87}$$

$$a\_{21}w\_1 + a\_{22}w\_2 + a\_{23}w\_3 + a\_{24}w\_4 = 0\tag{88}$$

$$a\_{31}w\_1 + a\_{32}w\_2 + a\_{33}w\_3 + a\_{34}w\_4 = 0\tag{89}$$

$$a\_{41}w\_1 + a\_{42}w\_2 + a\_{43}w\_3 + a\_{44}w\_4 = 0\tag{90}$$

Where:

$$a\_{2i} = \text{SrO-SD}^\*\_{\text{SiO}} \left( 1.016 \,\text{Al}\_2\text{O}\_3 + 0.65 \,\text{Fe}\_2\text{O}\_3 + 0.68 \,\text{Cr}\_2\text{O}\_3 \right) \tag{91}$$

$$a\_{3i} = \text{Al}\_2\text{O}\_3\text{-M}\_A^"\text{ (Fe}\_2\text{O}\_3 + \text{Cr}\_2\text{O}\_3) \tag{92}$$

$$a\_{4i} = \text{Fe}\_2\text{O}\_3\text{-M}\_\text{F}\text{Cr}\_2\text{O}\_3 \qquad \left(\text{i} = 1, 2, 3, 4\right) \tag{93}$$

From the relationships introduced above we can calculate:

Therefore a new type of module can be applied:

=0.90, *M*<sup>A</sup>

\*

**Table 5.** Composition of four raw materials for the preparation of raw meal.

parameters *SD*SrO\*

ble 5.

Where:

2 3

*M* (86)

=58 and *M*F=10. The composition of raw materials is listed in Ta‐

<sup>1234</sup> *wwww* +++=100 (87)

21 1 22 2 23 3 24 4 *aw aw aw aw* +++ = 0 (88)

31 1 32 2 33 3 34 4 *aw aw aw aw* +++ = 0 (89)

41 1 42 2 43 3 44 4 *aw aw aw aw* +++ = 0 (90)

3 23 A 23 23 = Al O -M (Fe O +Cr O ) *<sup>i</sup> a* (92)

*a*4 23 F 23 *<sup>i</sup>* = Fe O -M Cr O i=1, 2, 3, 4 ( ) (93)

2 3 Fe O <sup>=</sup> Cr O

This is the case of raw meal the preparation of strontium aluminate clinker with following

The composition of raw meal results from the solution of the following set of four equations:

( ) \*

\*

<sup>2</sup>*<sup>i</sup>* = SrO-SD 1.016 Al O +0.65 Fe O +0.68 Cr O SrO 2 3 2 3 2 3 *a* (91)

**Raw material SrO Al2O3 Fe2O3 Cr2O3 Y=Fe2O3+Cr2O3**

SrCO3 1 97.3 0 0.3 0 0.3 Calcined bauxite 2 0 96.5 2.6 0 2.6 Corundum 3 0 99.7 0.1 0 0.11 Cr2O3 4 0 2.8 1.5 32.6 34.1

Fe

70 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

$$a\_{21} = 97.3 - 0.90 \left( 1.016 \cdot 0 + 0.65 \cdot 0.3 + 0.68 \cdot 0 \right) = 97.1 \tag{94}$$

$$a\_{22} = 0 - 0.90 \left( 1.016 \cdot 96.5 + 0.65 \cdot 2.6 + 0.68 \cdot 0 \right) = -89.8 \tag{95}$$

$$a\_{23} = 0 - 0.90 \left( 1.016 \cdot 99.7 + 0.65 \cdot 0.1 + 0.68 \cdot 0 \right) = -91.2 \tag{96}$$

$$a\_{24} = 0 - 0.90 \left( 1.016 \cdot 2.8 + 0.65 \cdot 1.5 + 0.68 \cdot 32.6 \right) = -23.4 \tag{97}$$

$$a\_{31} = 0 - 58.0 \left( 0.3 + 0 \right) = -17.4 \tag{98}$$

$$a\_{32} = 96.5 - 58.0 \, (2.6 + 0) = -54.3 \, \tag{99}$$

$$a\_{33} = 99.7 - 58.0 \, (0.1 + 0) = 93.9 \, \tag{100}$$

$$a\_{34} = 2.8 - 58.0 \left( 1.5 + 32.6 \right) = -1975.0 \tag{101}$$

$$a\_{41} = 0.3 - 10.0 \cdot 0 = 0.3\tag{102}$$

$$a\_{42} = 2.6 - 10.0 \cdot 0 = 2.6\tag{103}$$

$$a\_{43} = 0.1 - 10.0 \cdot 0 = 0.1\tag{104}$$

$$a\_{44} = 1.5 - 10.0 \cdot 32.6 = -324.5\tag{105}$$

From the relationships introduced above we can further calculate:

$$\mathbf{w}\_1 + \mathbf{w}\_2 + \mathbf{w}\_3 + \mathbf{w}\_4 = 100 \tag{106}$$

$$97.1\text{ w}\_1 - 89.8\text{ w}\_2 + -91.2\text{ w}\_3 - 23.4\text{ w}\_4 = 0\tag{107}$$

$$-17.4\text{ w}\_1 - 54.3\text{ w}\_2 + 93.9\text{ w}\_3 - 1975.0\text{ w}\_4 = 0\tag{108}$$

**Rule**

**Raw material**

SD\*

system.

**i k**

**Table 6.** Numerical solution for raw meal four raw materials.

MA \* 50.69/ (0.79 + 0.08) = 58.0

MFe 0.79/ 0.08 = 10.0

**Composition wi**

**Matrix Test: 4 Test:**

1 2 3 4 I II III

6 : 6a2 XX 10 0.00 1.00 1.01 0.64 2.65 51.97 54.62 -7a2 ∙ 10 + 7 11 0.00 0.00 148.49 -1933.8 -1785.32 3657.70 1872.38 -8a2 ∙ 10 + 8 12 0.00 0.00 -2.52 -326.28 -328.80 -149.53 -478.33 -9a3 ∙ 15 + 9 13 1.00 0.00 0.00 0.25 1.25 48.22 49.48 -10a3 ∙ 15 + 10 14 0.00 1.00 0.00 17.77 14.77 27.14 41.91 11 : 11a3 XX 15 0.00 0.00 1.00 -13.02 -12.02 24.63 12.61 -12a3 ∙ 15 + 12 16 0.00 0.00 0.00 -359.08 -359.08 -87.51 -446.58 -13a4 ∙ 20 + 13 17 1.00 0.00 0.00 0.00 1.00 48.16 49.16 -14a4 ∙ 20 + 14 18 0.00 1.00 0.00 0.00 1.00 23.79 24.79 -15a4 ∙ 20 + 15 19 0.00 0.00 1.00 0.00 1.00 27.81 28.81 16 : 16a4 XX 20 0.00 0.00 0.00 0.00 1.00 0.24 1.24

Now it is possible, as previously, to check, if the calculated results are correct:

 97.3 0 0.3 0 48.16 46.86 0 0.14 0 0 96.5 2.6 0 23.76 0 22.96 0.62 0 0 99.7 0.1 0 27.81 0 27.72 0.03 0 0 2.8 1.5 32.6 0.24 0 0.01 0 0.08 Total 100.00 46.86 50.69 0.79 0.08

SrO 46.86/ (1.016∙50.69 + 0.65∙0.79 + 0.68∙0.08) = 0.90

**[%]**

It is also possible to define another kind of module using V2O3, Ti2O3 or their mixture with Fe2O3 and to calculate the raw meal composition by the same way. This calculation certainly requires the redefinition of Saturation Degree of clinker from strontium oxide to applied

**SrO Al2O3 Fe2O3 Cr2O3 SrO Al2O3 Fe2O3 Cr2O3**

**Raw meal**

**Σi ib I+II.**

Raw Materials for Production of SrAC 73

$$0.3\,\mathrm{w}\_1 + 2.6\,\mathrm{w}\_2 + 0.1\,\mathrm{w}\_3 - 324.5\,\mathrm{w}\_4 = 0\tag{109}$$

The solution based on the Sauruss law is time consuming without specialized software. Nevertheless, it is possible to use the calculation according to Table 6. This solution is based on the Gauss inversion method. The symbols *i* and *k* denote the line and column of matrix for mathematical operation according to given rule, e.g. 2*a*1 is the second line and the first column member of matrix. The solution consists of the following steps:




**Table 6.** Numerical solution for raw meal four raw materials.

12 3 4 -- + - = 17.4 54.3 93.9 1975.0 0 *ww w w* (108)

123 4 0.3 2.6 0.1 324.5 0 *www w* + +- = (109)

The solution based on the Sauruss law is time consuming without specialized software. Nevertheless, it is possible to use the calculation according to Table 6. This solution is based on the Gauss inversion method. The symbols *i* and *k* denote the line and column of matrix for mathematical operation according to given rule, e.g. 2*a*1 is the second line and the first

72 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

**i.** Inserting the coefficients from the left side of Eqs.106-109 into proper line (1-4) of

**iii.** The column II contains the coefficients from the right side of Eqs.106-109 for the

**iv.** The operation on line 6 (-2*a*1 ∙ 5+2) means:-97.13 ∙ 1.00+97.13=0, where 2*a*1 is the co‐

**v.** The last four lines of column II provide the solution for the composition of raw

1 :1a1 XX 5 1.00 1.00 1.00 1.00 4.00 100.00 104.00 -2a1 ∙ 5 + 2 6 0.00 -186.89 -188.35 -120.51 -495.75 -9712.45 -10208.2 -3a1 ∙ 5 + 3 7 0.00 -36.90 111.30 -1957.6 -1883.2 1740.00 -143.2 -4a1 ∙ 5 + 4 8 0.00 2.30 -0.20 -324.80 -322.70 -30.00 -352.7 -5a2 ∙ 10 + 5 9 1.00 0.00 -0.01 0.36 -1.35 48.03 49.38

Table 6. For example the coefficient *a*11 from Eq.106 should be written in the first line and first column; the coefficient *a*32 belongs to the third line and second col‐

line from 1 to 4. Other lines refer to the results of mathematical operation defined

efficient related to the second line and first column. The operation 1 : 1*a*1 means

**Matrix Test: 4 Test:**

1 2 3 4 I II III

1 1.00 1.00 1.00 1.00 4.00 100.00 104.00 2 97.13 -89.76 -91.22 -23.39 -107.25 0.00 -107.25 3 -17.40 -54.30 93.90 -1975.0 -1952.8 0.00 -1952.8 4 0.30 2.60 0.10 -324.50 -321.50 0.00 -321.50

**Σi ib I+II.**

column member of matrix. The solution consists of the following steps:

**ii.** The column I contains the sum of members 1-4 for given line.

that all numbers in the first line are divided by given term.

umn, etc.

meal.

**Rule**

i ak

in the column rule.

**i k** Now it is possible, as previously, to check, if the calculated results are correct:


It is also possible to define another kind of module using V2O3, Ti2O3 or their mixture with Fe2O3 and to calculate the raw meal composition by the same way. This calculation certainly requires the redefinition of Saturation Degree of clinker from strontium oxide to applied system.

## **4. Method of analysis of raw material and clinker**

The calculation mentioned above requires the analysis of raw materials to calculate the cor‐ rection of working mixture composition. Some techniques applicable for the analysis of raw materials or cements are presented in this chapter. Chemical analysis, microscopy, XRD and other methods of examination should be carried out on the same, representative sample of material [7].

#### **4.1. Determination of SrO**

The EDTA disodium salt (Ethylenediaminetetraacetic acid disodium salt dehydrate, Na2H2Y⋅2H2O) titration is the most common technique used for the determination of stronti‐ um oxide in the strontium carbonate:

$$\text{Sr}^{2+} + \text{H}\_2\text{Y}^{2\text{-}} \rightarrow \text{SrY}^{2\text{-}} + 2\text{H}^+ \tag{110}$$

Depending on the concentration of oxalic acid and ammonium oxalate as precipitating agents, both forms can be obtained. At sufficiently low pH, the stoichiometric compound SrC2O4⋅ ½H2C2O4⋅H2O is formed. The morphologies of precipitated particles (bi-pyramids, rods, peanuts, spheres, etc.) depend on the experimental conditions such as pH, tempera‐

The structure of acidic strontium oxalate is shown in Fig.9(a). Oxalate and hydrogen oxalate anions are present in such a way that each asymmetric unit contains exactly one molecule with the structural formula Sr(HC2O4)⋅1/2(C2O4)H2O instead of Sr(C2O4)⋅1/2(H2C2O4)⋅H2O. Similarly to other known strontium oxalates, strontium is eight-fold coordinated by oxygen. In this coordination sphere, both, oxalate and hydrogen oxalate anions act once as bidentate and once as monodentate. Two remaining positions are occupied by H2O molecules. The SrO8 polyhedron can be described as distorted bicapped trigonal prism, with O7…O2… O5…Ow3 forming the square face. These polyhedrons are connected to each other only by

**Figure 9.** Strontium oxalate: Structure of SrO8 polyhedron (a) and connection of polyhedrons via shared edge (b) ac‐

The shared edges are O4…O4´ and Ow3…Ow3´(Fig.9 (b)), which means that H2O acts as bridging ligand between two strontium atoms. This is in contrast to all other Sr oxalates, where H2O is also coordinated to Sr, but without any bridging function. In the *ac* plane, the

O5 and D3…O2 along the *bc* plane) as well as interchain (Dw1…O6 along the *ac* plane) hy‐ drogen bridges, which give the whole network an extra stability. Until now the four types of acid strontium oxalates are known, the type 2 and 4 are conformers (Fig.10) with calculated

Many analytical techniques were suggested for the determination of strontium in the cement matrix [238,247-250], i.e. under conditions including high concentration of calcium in the sample, based on complicated separation techniques of low selectivity. The atomic absorp‐

2- groups, while in the *bc* plane the connection is

Raw Materials for Production of SrAC 75

groups. In addition, there is the possibility to form intrachain (Dw2…

ture, ageing time and concentration of additives [246].

cording to [243].

made by the HC2O4

polyhedra chains are connected by the C2O4

energy difference of ~6.69 kJ mol-1 [242,243].


edge sharing it to form one-dimensional chains along the c-axis [242].

with the stability constant of complex:

$$\mathrm{K}\left(\mathrm{SrY}^{2^{\*}}\right) = \frac{[\mathrm{SrY}^{2^{\*}}][\mathrm{H}^{+}]^{2}}{[\mathrm{Sr}^{2^{+}}][\mathrm{H}\_{2}\mathrm{Y}^{\cdot}]} = 398.1 \tag{111}$$

$$\log \mathbf{K} \left( \text{SrY}^{2\*} \right) = 8.6 \tag{112}$$

The formation of stable complex during the assessment requires the pH ≥ 10 (the same pH range as for Mg2+and Ba2+).

#### **4.2. Determination of SrO in OPC**

In compliance with the current ASTM Standard Test Methods for chemical analysis of hy‐ draulic cement (C 114) [241], strontium (usually present in Portland cement as minor constit‐ uent), is led to precipitate (Table 1) with calcium (CaC2O4) as oxalate (SrC2O4, monoclinic, space group P21/n [242,243]) and next it is subsequently titrated and calculated as CaO, or alternative correction of CaO for SrO is made, if the SrO content is known. Therefore, the development of a new, direct, sensitive and accurate method for the determination of stron‐ tium as minor constituent in cement is of upmost importance [244].

Strontium oxalate exists in two different forms [245]:


Depending on the concentration of oxalic acid and ammonium oxalate as precipitating agents, both forms can be obtained. At sufficiently low pH, the stoichiometric compound SrC2O4⋅ ½H2C2O4⋅H2O is formed. The morphologies of precipitated particles (bi-pyramids, rods, peanuts, spheres, etc.) depend on the experimental conditions such as pH, tempera‐ ture, ageing time and concentration of additives [246].

**4. Method of analysis of raw material and clinker**

( )

tium as minor constituent in cement is of upmost importance [244].

Strontium oxalate exists in two different forms [245]:

**1.** Neutral strontium oxalate hydrate, SrC2O4 *x*H2O.

**2.** Acid salt of strontium oxalate, SrC2O4 *y*H2C2O4 xH2O.

2-

material [7].

**4.1. Determination of SrO**

range as for Mg2+and Ba2+).

**4.2. Determination of SrO in OPC**

um oxide in the strontium carbonate:

with the stability constant of complex:

The calculation mentioned above requires the analysis of raw materials to calculate the cor‐ rection of working mixture composition. Some techniques applicable for the analysis of raw materials or cements are presented in this chapter. Chemical analysis, microscopy, XRD and other methods of examination should be carried out on the same, representative sample of

74 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

The EDTA disodium salt (Ethylenediaminetetraacetic acid disodium salt dehydrate, Na2H2Y⋅2H2O) titration is the most common technique used for the determination of stronti‐

2- + 2

2+ - 2

The formation of stable complex during the assessment requires the pH ≥ 10 (the same pH

In compliance with the current ASTM Standard Test Methods for chemical analysis of hy‐ draulic cement (C 114) [241], strontium (usually present in Portland cement as minor constit‐ uent), is led to precipitate (Table 1) with calcium (CaC2O4) as oxalate (SrC2O4, monoclinic, space group P21/n [242,243]) and next it is subsequently titrated and calculated as CaO, or alternative correction of CaO for SrO is made, if the SrO content is known. Therefore, the development of a new, direct, sensitive and accurate method for the determination of stron‐

[SrY ] [H ] K SrY = =398.1

2+ 2- 2- + Sr +H Y SrY +2 H <sup>2</sup> ® (110)

[Sr ] [H Y ] (111)

( ) 2- log K SrY 8.6 = (112)

The structure of acidic strontium oxalate is shown in Fig.9(a). Oxalate and hydrogen oxalate anions are present in such a way that each asymmetric unit contains exactly one molecule with the structural formula Sr(HC2O4)⋅1/2(C2O4)H2O instead of Sr(C2O4)⋅1/2(H2C2O4)⋅H2O. Similarly to other known strontium oxalates, strontium is eight-fold coordinated by oxygen. In this coordination sphere, both, oxalate and hydrogen oxalate anions act once as bidentate and once as monodentate. Two remaining positions are occupied by H2O molecules. The SrO8 polyhedron can be described as distorted bicapped trigonal prism, with O7…O2… O5…Ow3 forming the square face. These polyhedrons are connected to each other only by edge sharing it to form one-dimensional chains along the c-axis [242].

**Figure 9.** Strontium oxalate: Structure of SrO8 polyhedron (a) and connection of polyhedrons via shared edge (b) ac‐ cording to [243].

The shared edges are O4…O4´ and Ow3…Ow3´(Fig.9 (b)), which means that H2O acts as bridging ligand between two strontium atoms. This is in contrast to all other Sr oxalates, where H2O is also coordinated to Sr, but without any bridging function. In the *ac* plane, the polyhedra chains are connected by the C2O4 2- groups, while in the *bc* plane the connection is made by the HC2O4 groups. In addition, there is the possibility to form intrachain (Dw2… O5 and D3…O2 along the *bc* plane) as well as interchain (Dw1…O6 along the *ac* plane) hy‐ drogen bridges, which give the whole network an extra stability. Until now the four types of acid strontium oxalates are known, the type 2 and 4 are conformers (Fig.10) with calculated energy difference of ~6.69 kJ mol-1 [242,243].

Many analytical techniques were suggested for the determination of strontium in the cement matrix [238,247-250], i.e. under conditions including high concentration of calcium in the sample, based on complicated separation techniques of low selectivity. The atomic absorp‐

riously, even when present in amounts higher than 0.1 mg. The interference due to Mn and Zn was eliminated by the addition of ammonium hydroxide, and that of Ca and Mg was overcome by using the derivative ratio zero crossing method. Using the proposed method, it is possible to determine Sr, Mg, and Ca simultaneously in mixtures containing 1.5-18 μg⋅cm-3 of strontium, 0.5-5.0 μg⋅cm-3 of magnesium and 1.0-8.0 μg⋅cm-3 of calcium [262].

Raw Materials for Production of SrAC 77

**4.3. Application of strontium isotopes to determine the origin of cements in concrete**

[264,265].

against Ca/Sr [266].

into account [7].

to 208Pb, 207Pb, 206Pb; 147Sm to 143Nd [264].

**4.4. Determination of Al2O3 and Fe2O3**

**5. Method for analysis of SrAC cement**

In many disciplines of science it is important to be able to determine the source of material or to characterize its transportation history. The chemical composition has been used exten‐ sively to determine the source of materials by fingerprinting the chemical composition of the material to be identified and comparing it to the chemical composition of potential sources. This approach has been used extensively for major elements as well as for trace elements

Forensic isotope geochemistry relies on subtle differences in isotopic abundance of element to characterize particular material. These different isotopic abundances give rise to unique isotopic composition that will identify the material come from particular region. Many rocks composed of different minerals have distinctive isotopic compositions and their unique composition can be used to fingerprint them. This distinctive rock/mineral composition usu‐ ally arises from the decay of radiogenic elements e.g., 87Rb to 87Sr; the transuranic elements

Combined chemical and Sr isotopic analysis may provide the geochemical fingerprints from raw materials, which can be used to identify them in concrete. For successful chemical fin‐ gerprinting of cement in concrete, it is important to leach cement without significantly at‐ tacking the aggregate, but this can be minimized by using slightly alkaline or neutral EDTA as solvent in preference to weak mineral acids such as HNO3. Combined chemical and Sr isotopic analysis of commonly used New Zealand cements showed that they contain charac‐ teristic fingerprints, which may be used to identify them in concrete of unknown origin. Al‐ though cements have typically 87Sr/86Sr values similar to their mid-Tertiary limestone source rocks (0.7078 – 0.7085) most are easily distinguishable when their 87Sr/86Sr values are plotted

Different forms of alumina may be identified by x-ray diffraction analysis [91]. Classical, wet analysis gives inaccurate results for Al2O3 unless the effects of P2O5 and TiO2 are not taken

The standard test methods for the chemical analysis of hydraulic cement are specified by ASTM C 114-13. The chemical analysis of hydraulic cement is specified by ASTM C 114-88

**Figure 10.** Coordination types of acid strontium oxalate: type 4 (a) and type 2 (b).

tion spectrometric method can be used for the determination of calcium, magnesium and strontium in soils [236] but the assessment requires the removal of the silicon.

Derivative spectrophotometry is analytical technique combining high selectivity [251-255] and sensitivity [244,256-258]. The accuracy of assessment depends on the shape of normal absorption spectra of analyte and interfering substances, as well as on the instrumental pa‐ rameters and the applied technique of measurement, e.g. peak-to-trough or zero-crossing [259-261]. Salinas et al. [262] developed the derivative spectrophotometric method for re‐ solving binary mixtures when the spectra of components are overlapped. The method uses the first derivation of the spectra. The concentration of other component is then determined from the calibration graph. Later, the method was extended to the resolution of ternary mix‐ tures in combination with zero-crossing method [263].

The determination of strontium and simultaneous determination of strontium oxide, magne‐ sium oxide and calcium oxide content in Portland cement by derivative ratio spectropho‐ tometry uses alizarin Complexone (alizarin-3-methylamine-N, N-diacetic acid, AC) as one of the most common reagents used for the spectrophotometric determination of metal ions. The AC reagent yields five colored acid–base forms in the solutions of pH ∼3.2–10.5: H4L, H3L<sup>−</sup> , H2L2 − , HL3− and L4−, exhibiting the absorption maxima at 270, 335, 423, 525, and 580 nm, respectively. Distinct isosbestic points are observed for the particular acid–base equili‐ brium. The formation of SrL2-complex with liberation of one proton occurs in pH range from 7 to 10 [262]:

$$\rm{Sr^{2+} + LH^{3-} \to SrL^{2+} + H^{+}} \tag{113}$$

The determination of strontium as SrL2− complex was possible in the presence of Li+ , Na+ , K+ , Cs+ , Cd2+, Al3+, Fe3+, Mo6+, SO4 2−, SO3 2−, NO3−, Cl<sup>−</sup> , Br<sup>−</sup> , I<sup>−</sup> and PO4 3− (20.0 mg); Co2+,Ni2+, Pb+ , Cr3+, Ti4+, C2O4 2− and CO3 2− (1.0 mg). Investigated ions Ca2+, Mg2+, Mn2+and Zn2+interfered se‐ riously, even when present in amounts higher than 0.1 mg. The interference due to Mn and Zn was eliminated by the addition of ammonium hydroxide, and that of Ca and Mg was overcome by using the derivative ratio zero crossing method. Using the proposed method, it is possible to determine Sr, Mg, and Ca simultaneously in mixtures containing 1.5-18 μg⋅cm-3 of strontium, 0.5-5.0 μg⋅cm-3 of magnesium and 1.0-8.0 μg⋅cm-3 of calcium [262].

#### **4.3. Application of strontium isotopes to determine the origin of cements in concrete**

In many disciplines of science it is important to be able to determine the source of material or to characterize its transportation history. The chemical composition has been used exten‐ sively to determine the source of materials by fingerprinting the chemical composition of the material to be identified and comparing it to the chemical composition of potential sources. This approach has been used extensively for major elements as well as for trace elements [264,265].

Forensic isotope geochemistry relies on subtle differences in isotopic abundance of element to characterize particular material. These different isotopic abundances give rise to unique isotopic composition that will identify the material come from particular region. Many rocks composed of different minerals have distinctive isotopic compositions and their unique composition can be used to fingerprint them. This distinctive rock/mineral composition usu‐ ally arises from the decay of radiogenic elements e.g., 87Rb to 87Sr; the transuranic elements to 208Pb, 207Pb, 206Pb; 147Sm to 143Nd [264].

Combined chemical and Sr isotopic analysis may provide the geochemical fingerprints from raw materials, which can be used to identify them in concrete. For successful chemical fin‐ gerprinting of cement in concrete, it is important to leach cement without significantly at‐ tacking the aggregate, but this can be minimized by using slightly alkaline or neutral EDTA as solvent in preference to weak mineral acids such as HNO3. Combined chemical and Sr isotopic analysis of commonly used New Zealand cements showed that they contain charac‐ teristic fingerprints, which may be used to identify them in concrete of unknown origin. Al‐ though cements have typically 87Sr/86Sr values similar to their mid-Tertiary limestone source rocks (0.7078 – 0.7085) most are easily distinguishable when their 87Sr/86Sr values are plotted against Ca/Sr [266].

## **4.4. Determination of Al2O3 and Fe2O3**

tion spectrometric method can be used for the determination of calcium, magnesium and

Derivative spectrophotometry is analytical technique combining high selectivity [251-255] and sensitivity [244,256-258]. The accuracy of assessment depends on the shape of normal absorption spectra of analyte and interfering substances, as well as on the instrumental pa‐ rameters and the applied technique of measurement, e.g. peak-to-trough or zero-crossing [259-261]. Salinas et al. [262] developed the derivative spectrophotometric method for re‐ solving binary mixtures when the spectra of components are overlapped. The method uses the first derivation of the spectra. The concentration of other component is then determined from the calibration graph. Later, the method was extended to the resolution of ternary mix‐

The determination of strontium and simultaneous determination of strontium oxide, magne‐ sium oxide and calcium oxide content in Portland cement by derivative ratio spectropho‐ tometry uses alizarin Complexone (alizarin-3-methylamine-N, N-diacetic acid, AC) as one of the most common reagents used for the spectrophotometric determination of metal ions. The AC reagent yields five colored acid–base forms in the solutions of pH ∼3.2–10.5: H4L,

nm, respectively. Distinct isosbestic points are observed for the particular acid–base equili‐ brium. The formation of SrL2-complex with liberation of one proton occurs in pH range from

The determination of strontium as SrL2− complex was possible in the presence of Li+

2−, NO3−, Cl<sup>−</sup>

2−, SO3

, HL3− and L4−, exhibiting the absorption maxima at 270, 335, 423, 525, and 580

, Br<sup>−</sup>

2+ 3- 2- + Sr +LH SrL +H ® (113)

, I<sup>−</sup> and PO4

2− (1.0 mg). Investigated ions Ca2+, Mg2+, Mn2+and Zn2+interfered se‐

, Na+ , K+ ,

,

3− (20.0 mg); Co2+,Ni2+, Pb+

strontium in soils [236] but the assessment requires the removal of the silicon.

76 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

**Figure 10.** Coordination types of acid strontium oxalate: type 4 (a) and type 2 (b).

tures in combination with zero-crossing method [263].

H3L<sup>−</sup>

Cs+

, H2L2 −

7 to 10 [262]:

Cr3+, Ti4+, C2O4

, Cd2+, Al3+, Fe3+, Mo6+, SO4

2− and CO3

Different forms of alumina may be identified by x-ray diffraction analysis [91]. Classical, wet analysis gives inaccurate results for Al2O3 unless the effects of P2O5 and TiO2 are not taken into account [7].

## **5. Method for analysis of SrAC cement**

The standard test methods for the chemical analysis of hydraulic cement are specified by ASTM C 114-13. The chemical analysis of hydraulic cement is specified by ASTM C 114-88 standard. The mineralogy of cement cannot be determined from the chemical composition because the thermodynamic equilibrium usually is not reached during the production proc‐ ess. The phase (mineralogical) composition of strontium aluminate cement can be in princi‐ ple determined by the same methods as for aluminous cements:

**4.** Air voids.

The solid hydration products occupy a greater volume than the volume of reacted cement (Fig.11), but slightly smaller volume than the sum of volumes of cement and water due to chemical shrinkage [273,278]. Chemical shrinkage associated with hydration of OPC and AC

Raw Materials for Production of SrAC 79

The methodology for the estimation of initial cement content, water content and water/ cement ratio of hardened cement-based materials by electron microscopy was developed by Wong and Buenfeld [273] and Sahu at al. [275]. The acoustic-ultrasonic approach for nondestructive determination of *w*/*c* ratio was described by Philippidis and Aggelis [274]. Betch‐ er at al. [277] published the method using 2.45 GHz microwave radiation which can be conveniently and accurately used for the on-site determination of the water-to-cement (*w*/*c*)

Grinding occurs at the beginning and at the end of cement making process [279]. In recent years, the matrix model and the kinetic model, which were suggested by investigators, are used in laboratories and industrial areas. The kinetic model, which is an alternative ap‐ proach, considers the combination as a continuous process in which the rate of breakage of particle size is proportional to the mass of particles of that size. The analysis of size reduc‐ tion in tumbling ball mills using the concepts of specific rate of breakage and primary daughter fragment distribution has received considerable attention in the last years [280,320].

To optimize the cement grinding, the standard Bond grinding calculations [281] can be used as well as the modeling and simulation techniques based on the population balance model (PBM) [284,285]. The mill power draw prediction can be carried out using the Morrell power

is about 5 and 10 – 12 ml per 100 g of cement, respectively [12].

**Figure 11.** Proportion of main phases in hardened cement stone [273].

ratio in a batch of fresh rapid-setting concrete.

model for tumbling mills [279,282].

**7. Grinding**


Due to recent developments in cement clinker engineering, the optimization of chemical substitutions in the main clinker phases offers a promising approach to improve both reac‐ tivity and grindability of clinkers. Thus, the monitoring of chemistry of phases may become a part of the quality control at cement plants, along with usual measurements of the abun‐ dance of mineralogical phases [270].

## **6. Determination of water to cement ratio**

The chemical reactions which take place after mixing cement with water are generally more complex than simple conversion of anhydrous compounds into the corresponding hydrates. The mixtures of cement with water, where the hydration reactions, setting and hardening take place are termed as pastes [271], while the hardened material can be termed as cement stone or hardened cement stone. The water to cement ratio (*w*/*c*) refers to the proportion by mass that is related to water and cement used for the preparation of cement paste [12,271].

The value water-to-cement (*w/c*) ratio is one of the most fundamental parameters in concrete mixture proportioning. The *w*/*c* ratio has a significant influence on most properties of hard‐ ened concrete, in particular on strength and durability due to its relationship with the amount of residual space i.e. capillary porosity, in the cement stone. Since the *w*/*c* ratio is an indication of quality of concrete mix, the situations often arise in which it is desirable to de‐ termine the original *w*/*c* ratio of particular concrete some time after it has hardened. This of‐ ten happens when the disputes suspecting the noncompliance with the mix specification arise. The determination of the *w*/*c* ratio is also important for the quality control during the concrete production and for general quality assurance purposes [273-277].

Unfortunately, once concrete has set, it is very difficult to ascertain the exact amounts of ce‐ ment and water which were originally added during batching. At any moment after setting, the hardened cement stone can be considered to consist of four main phases [273]:


## **4.** Air voids.

standard. The mineralogy of cement cannot be determined from the chemical composition because the thermodynamic equilibrium usually is not reached during the production proc‐ ess. The phase (mineralogical) composition of strontium aluminate cement can be in princi‐

78 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

Due to recent developments in cement clinker engineering, the optimization of chemical substitutions in the main clinker phases offers a promising approach to improve both reac‐ tivity and grindability of clinkers. Thus, the monitoring of chemistry of phases may become a part of the quality control at cement plants, along with usual measurements of the abun‐

The chemical reactions which take place after mixing cement with water are generally more complex than simple conversion of anhydrous compounds into the corresponding hydrates. The mixtures of cement with water, where the hydration reactions, setting and hardening take place are termed as pastes [271], while the hardened material can be termed as cement stone or hardened cement stone. The water to cement ratio (*w*/*c*) refers to the proportion by mass that is related to water and cement used for the preparation of cement paste [12,271].

The value water-to-cement (*w/c*) ratio is one of the most fundamental parameters in concrete mixture proportioning. The *w*/*c* ratio has a significant influence on most properties of hard‐ ened concrete, in particular on strength and durability due to its relationship with the amount of residual space i.e. capillary porosity, in the cement stone. Since the *w*/*c* ratio is an indication of quality of concrete mix, the situations often arise in which it is desirable to de‐ termine the original *w*/*c* ratio of particular concrete some time after it has hardened. This of‐ ten happens when the disputes suspecting the noncompliance with the mix specification arise. The determination of the *w*/*c* ratio is also important for the quality control during the

Unfortunately, once concrete has set, it is very difficult to ascertain the exact amounts of ce‐ ment and water which were originally added during batching. At any moment after setting,

**2.** Crystalline and semi-crystalline hydration products including their intrinsic gel pores;

concrete production and for general quality assurance purposes [273-277].

the hardened cement stone can be considered to consist of four main phases [273]:

ple determined by the same methods as for aluminous cements:

**4.** Quantitative X-Ray Diffraction Analysis (QXDA) [7,267-270,599],

**1.** Selective dissolution [269];

**2.** Electron Microscopy [7,269];

**3.** Reflected Light Microscopy [7,269];

dance of mineralogical phases [270].

**1.** Rest of unreacted cement;

**3.** Capillary pores;

**6. Determination of water to cement ratio**

The solid hydration products occupy a greater volume than the volume of reacted cement (Fig.11), but slightly smaller volume than the sum of volumes of cement and water due to chemical shrinkage [273,278]. Chemical shrinkage associated with hydration of OPC and AC is about 5 and 10 – 12 ml per 100 g of cement, respectively [12].

**Figure 11.** Proportion of main phases in hardened cement stone [273].

The methodology for the estimation of initial cement content, water content and water/ cement ratio of hardened cement-based materials by electron microscopy was developed by Wong and Buenfeld [273] and Sahu at al. [275]. The acoustic-ultrasonic approach for nondestructive determination of *w*/*c* ratio was described by Philippidis and Aggelis [274]. Betch‐ er at al. [277] published the method using 2.45 GHz microwave radiation which can be conveniently and accurately used for the on-site determination of the water-to-cement (*w*/*c*) ratio in a batch of fresh rapid-setting concrete.

## **7. Grinding**

Grinding occurs at the beginning and at the end of cement making process [279]. In recent years, the matrix model and the kinetic model, which were suggested by investigators, are used in laboratories and industrial areas. The kinetic model, which is an alternative ap‐ proach, considers the combination as a continuous process in which the rate of breakage of particle size is proportional to the mass of particles of that size. The analysis of size reduc‐ tion in tumbling ball mills using the concepts of specific rate of breakage and primary daughter fragment distribution has received considerable attention in the last years [280,320].

To optimize the cement grinding, the standard Bond grinding calculations [281] can be used as well as the modeling and simulation techniques based on the population balance model (PBM) [284,285]. The mill power draw prediction can be carried out using the Morrell power model for tumbling mills [279,282].

The Bonds equation describes the specific power required to reduce the feed from specified feed *F*80 to the product with specified *P*80 [279,281]:

$$W\_m = W\_i \left(\frac{10}{\sqrt{P\_{80}}} - \frac{10}{\sqrt{F\_{80}}}\right) \tag{114}$$

the mill and breakage within the mill. Because the mill or section of it is perfectly mixing a

Steady state operation conditions can be described by the following relation:

1

1

charge rate of particle size *i* [h-1]. If the breakage distribution function is known, the calibra‐ tion of the model to a ball mill involves the calculation of *r/d* values using the feed and product size distribution obtained under known operating conditions. Where the size distri‐ bution of the mill content is available, the breakage and discharge rates can be calculated

The model consists of two important parameters, the breakage function (*a*ij) that describes

machine characteristics and can be calculated when the feed and product size distributions are known and the breakage function is available. The air classifier controls the final product quality. Therefore, the air classifier has a crucial role in the circuit and a strong attention is paid regarding the design and operation of the air classifier. The classification action is mod‐ eled using the efficiency curve approach. The effect of the classifier design and of operation‐ al parameters on the efficiency is complicated and the works proceed to improve the current

The consumption of steel grinding media plays an important role in the economics of grinding and as a consequence also in the overall processing of a large variety of ores. The cost associated with grinding media is chiefly determined by two factors; the price and the wear performance of the grinding media. The mass losses of grinding media can be

= - + -= å *<sup>i</sup> i i i i ij j i i i j*

is the mass fraction of particle of size that appears at size *i* after breakage, *r*<sup>i</sup>

the material characteristics and the breakage/discharge rate function (*r*<sup>i</sup>

= -+ - = å *i i i i ij j j i i j*

leads to the equation:

, for each size fraction is an important variable for defining the product

0

0

is the amount of size *i* particles inside the mill [t], *d*<sup>i</sup>

*f rs a r s d s* (119)

*p p f r ar p d d* (120)

is the product flow of size fraction [t⋅h-1], *a*ij

/*d*i

is the breakage

Raw Materials for Production of SrAC 81

) which defines the

is the dis‐

*p ds i ii* = (118)

discharge rate, *d*<sup>i</sup>

The substitution of *s*<sup>i</sup>

rate of particle size *i* [h-1], *s*<sup>i</sup>

where *f*<sup>i</sup>

separately.

models [279].

**7.1. Consumption of grinding media**

 by *p*<sup>i</sup> /*d*i

is the feed rate of size fraction [t⋅h-1], *p*<sup>i</sup>

[279,284,285]:

where *W*m is the mill specific motor output power (kWh⋅t-1), *W*<sup>i</sup> is the Bond ball mill work index (kWh⋅t-1) *P*80 is the sieve size passing 80 % of the mill product (μm), *F*<sup>80</sup> is the sieve size passing 80 % of the mill feed (μm). It was found in the crushing area that there are sig‐ nificant differences between the real plant data and the Bond calculations and therefore the empirical corrections were introduced. The following modified Bond equation was pro‐ posed for crushing [283]:

$$W\_c = \frac{A}{\sqrt{P\_c}} W\_i \left(\frac{10}{\sqrt{P\_c}} - \frac{10}{\sqrt{F\_c}}\right) \tag{115}$$

where *W*c is the energy consumed for crushing the clinker (kWh t-1), *W*<sup>i</sup> is the Bond ball mill work index (kWh t-1), *P*<sup>c</sup> is the sieve size passing 80% of clinker after crushing (μm), *F*c is the sieve size passing 80% of clinker before crushing (μm) and *A* is the empirical coefficient, which depends on clinker and crusher properties.

Based on the above considerations for crushing and grinding, the energy consumption for the clinker pre-crushing and ball milling can be estimated using the following Bond based model:

$$W = W\_c + W\_m \tag{116}$$

Since the pre-crushing product size *P*c is equal to the mill feed size *F*80 then [279]:

$$\begin{aligned} W &= \frac{A}{\sqrt{F\_{80}}} W\_i \left( \frac{10}{\sqrt{P\_{80}}} - \frac{10}{\sqrt{F\_c}} \right) + 1.3 \left( \frac{2.44}{D} \right)^{0.2} \\\ &\left[ \left\{ R\_r + (W\_i - 7) \left( \frac{F\_{80} - F\_0}{F\_0} \right) \right\} \Big| \begin{matrix} R\_{80} \\ R\_r \end{matrix} \right] \frac{P\_{80} + 10.3}{1.145 \ P\_{80}} W\_i \left( \frac{10}{\sqrt{P\_{80}}} - \frac{10}{\sqrt{F\_{80}}} \right) \end{aligned} \tag{117}$$

where *D* is the interior mill diameter and *R*r=*F*80/*P*80.

The basis of the population balance model for modeling the two-compartment ball mill is the perfect mixing ball mill model. This model considers a ball mill or a section of it as a perfectly stirring tank. Then the process can be described in the terms of transport through the mill and breakage within the mill. Because the mill or section of it is perfectly mixing a discharge rate, *d*<sup>i</sup> , for each size fraction is an important variable for defining the product [279,284,285]:

$$\mathbf{p}\_i = \mathbf{d}\_i \,\mathbf{s}\_i \tag{118}$$

Steady state operation conditions can be described by the following relation:

$$\Box f\_i - r\_i \mathbf{s}\_i + \sum\_{j=1}^{i} a\_{ij} r\_j \mathbf{s}\_j - d\_i \mathbf{s}\_i = \mathbf{0} \tag{119}$$

The substitution of *s*<sup>i</sup> by *p*<sup>i</sup> /*d*i leads to the equation:

The Bonds equation describes the specific power required to reduce the feed from specified

80 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

80 80

index (kWh⋅t-1) *P*80 is the sieve size passing 80 % of the mill product (μm), *F*<sup>80</sup> is the sieve size passing 80 % of the mill feed (μm). It was found in the crushing area that there are sig‐ nificant differences between the real plant data and the Bond calculations and therefore the empirical corrections were introduced. The following modified Bond equation was pro‐

> æ ö 10 10 <sup>=</sup> ç ÷ è ø *c i c cc*

where *W*c is the energy consumed for crushing the clinker (kWh t-1), *W*<sup>i</sup> is the Bond ball mill work index (kWh t-1), *P*<sup>c</sup> is the sieve size passing 80% of clinker after crushing (μm), *F*c is the sieve size passing 80% of clinker before crushing (μm) and *A* is the empirical coefficient,

Based on the above considerations for crushing and grinding, the energy consumption for the clinker pre-crushing and ball milling can be estimated using the following Bond based

0.2

0 80 80 80

*F P P F*

10.3 10 10 <sup>7</sup> 1.145

The basis of the population balance model for modeling the two-compartment ball mill is the perfect mixing ball mill model. This model considers a ball mill or a section of it as a perfectly stirring tank. Then the process can be described in the terms of transport through

Since the pre-crushing product size *P*c is equal to the mill feed size *F*80 then [279]:

80 0 80

ì ü é ù æ ö - + æ ö ï ï í ý ê ú + - ç ÷ ç ÷ ï ï î þ ë û è ø è ø

10 10 2.44 1.3

è ø è ø

*c*

*r i r i*

*F F <sup>P</sup> R W R W*

æ ö æ ö = -+ ç ÷ ç ÷

*F PF D*

*W W m i P F* (114)

*P PF* (115)

*WW W* = +*c m* (116)

is the Bond ball mill work

(117)

æ ö 10 10 = - ç ÷ è ø

feed *F*80 to the product with specified *P*80 [279,281]:

which depends on clinker and crusher properties.

( )

where *D* is the interior mill diameter and *R*r=*F*80/*P*80.

80 80

*i*

*<sup>A</sup> W W*

posed for crushing [283]:

model:

where *W*m is the mill specific motor output power (kWh⋅t-1), *W*<sup>i</sup>

*<sup>A</sup> W W*

$$\Box f\_i - r\_i \frac{p\_i}{d\_i} + \sum\_{j=1}^i a\_{ij} r\_j \frac{p\_i}{d\_i} - p\_i = 0 \tag{120}$$

where *f*<sup>i</sup> is the feed rate of size fraction [t⋅h-1], *p*<sup>i</sup> is the product flow of size fraction [t⋅h-1], *a*ij is the mass fraction of particle of size that appears at size *i* after breakage, *r*<sup>i</sup> is the breakage rate of particle size *i* [h-1], *s*<sup>i</sup> is the amount of size *i* particles inside the mill [t], *d*<sup>i</sup> is the dis‐ charge rate of particle size *i* [h-1]. If the breakage distribution function is known, the calibra‐ tion of the model to a ball mill involves the calculation of *r/d* values using the feed and product size distribution obtained under known operating conditions. Where the size distri‐ bution of the mill content is available, the breakage and discharge rates can be calculated separately.

The model consists of two important parameters, the breakage function (*a*ij) that describes the material characteristics and the breakage/discharge rate function (*r*<sup>i</sup> /*d*i ) which defines the machine characteristics and can be calculated when the feed and product size distributions are known and the breakage function is available. The air classifier controls the final product quality. Therefore, the air classifier has a crucial role in the circuit and a strong attention is paid regarding the design and operation of the air classifier. The classification action is mod‐ eled using the efficiency curve approach. The effect of the classifier design and of operation‐ al parameters on the efficiency is complicated and the works proceed to improve the current models [279].

#### **7.1. Consumption of grinding media**

The consumption of steel grinding media plays an important role in the economics of grinding and as a consequence also in the overall processing of a large variety of ores. The cost associated with grinding media is chiefly determined by two factors; the price and the wear performance of the grinding media. The mass losses of grinding media can be attributed to three basic mechanisms; the abrasion, the impact and the corrosion. These mechanisms can be simultaneously active in given grinding environment, leading to complex interactions [286].

1, 1,

The value *S*1 for different particle sizes can be estimated by performing the same experi‐ ment with uniform-sized material. Different values of *S*1 versus the size can then be plotted on *log*–*log* plot to give a straight line if all the sizes follow the first-order law of grinding

The primary breakage distribution (*B*i,j) is also defined in an empirical form in literature as

parameters *φ*, *γ* and *β* define the size distribution of the material being ground. When plot‐ ting the size versus *B*i,j on log paper, the slope of the lower part of the curve gives the value of *γ*, the slope of the upper part of the curve gives the value of *β*, and *φ* is the intercept [319].

The spheroidal aggregate of particles is called a granule, ball, pellet, or an agglomerate. The nucleation, compaction, size enlargement, and spheroidization of pellets take place in the course of balling and granulation and related agglomeration processes [291]. The granula‐ tion converts fine powder and/or sprayable liquids (e.g. suspensions, solutions or melts) into granular solid products with more desirable physical and/or chemical properties than the original feed material. This size enlargement technique constitutes a key process in many in‐ dustries such as the pharmaceutical, food, ore processing and fertilizers ones. Particularly, the granulation process has clear advantages regarding the storage, handling and transpor‐

The new king of agglomeration technology is binder-less granulation, where the original co‐ hesiveness of powder material is utilized to arrange them into granules. The strength of product granules can be much weaker. However, if the product granules are just an inter‐ mediate product in a larger process, such weakness has significant advantages. In many ma‐ terial-forming processes, the boundary between granules remains even after shaping due to unnecessary strength of granules. With weaker granules, the density of green bodies pro‐ duced by the application of the same pressure as for conventional granules can be much higher. In many cases, the binder removal cannot be done completely leaving possible de‐ fects caused by carbonacious pyrolysis residues. Weaker granules can also be advantageous

in pharmaceutical processes depending on the purpose of granulation [294].

*b*

*x x <sup>B</sup> ni j x x* (123)

*<sup>w</sup>* (122)

is the largest size, and the

Raw Materials for Production of SrAC 83

1,0 log 2.3 = - *w S t t*

( ) 1 1 , 1 ; g

*i i ij i <sup>j</sup>*

 j - - æö æö = +- ç÷ ç÷ ³ ³ èø èø

*j j*

j

where *B*i,j is the mass fraction of primary breakage products, *x*<sup>i</sup>

kinetics.

[280,290,319,320]:

**8. Granulation**

tation of the final product [292,293].

#### **7.2. Grinding aids**

The action of grinding media within the rotating mill not only crushes the existing clinker particles, but also sharply compresses them, which in fact leads to the formation of electro‐ static surface charges of opposed polarity. The cement particles agglomerate as a result of the forces of attraction acting on them. Consequently, the cement particle agglomeration re‐ duces the efficiency of mill. The extent of agglomeration depends on [287]:


Additives, such as water, organic liquids and some inorganic electrolytes are used to reduce the surface free energy of the material being ground with a view to improve the grinding efficiency.

In the grinding process, a variety of grinding aids are used. There are aliphatic amines such as triethylenetetramine (TETA), tetraethylenepentamine (TEPA) and aminealcohols such as diethanolamine (DEA), triethanolamine (TEA) and triisopropanolamine (TIPA). Glycol com‐ pounds are represented such as ethyleneglycol (EG), diethyleneglycol (DEG). In addition, there are more complex compounds such as aminoethylethanolamine (AEEA) and hydrox‐ yethyl diethylenetriamine (HEDETA). Phenol and phenol-derivates are also used as grind‐ ing aids, as well as other compounds, such as amine acetate, higher polyamines and their hydroxyethyl derivates [287,322].

#### **7.3. Grinding kinetics**

Assuming that a grinding mill is equivalent to a chemical reactor with a first-order phenom‐ enological rate of reaction kinetics [288], the rate of decrease in particle size during the batch grinding of brittle material in ball mill can be described by the first-order equation. The breakage rate of such material was expressed in literature as [289]:

$$\mathbf{w}\_{i,t} = \mathbf{w}\_{i,0} \exp\left(-S\_i t\right) \tag{121}$$

where *S*<sup>i</sup> is the specific rate of breakage of feed size *i* and *w*i,t is the mass fraction of total charge. For single component (*i*=1) Eq.121 can be rewritten as:

$$\log \frac{\mathbf{w}\_{\mathbf{l},t}}{\mathbf{w}\_{\mathbf{l},0}} = -\frac{S\_{\mathbf{l},t}}{2.3} \tag{122}$$

The value *S*1 for different particle sizes can be estimated by performing the same experi‐ ment with uniform-sized material. Different values of *S*1 versus the size can then be plotted on *log*–*log* plot to give a straight line if all the sizes follow the first-order law of grinding kinetics.

The primary breakage distribution (*B*i,j) is also defined in an empirical form in literature as [280,290,319,320]:

$$B\_{i,j} = \phi\_i \left(\frac{\mathbf{x}\_{i-1}}{\mathbf{x}\_j}\right)^\gamma + \left(1 - \phi\_j\right) \left(\frac{\mathbf{x}\_{i-1}}{\mathbf{x}\_j}\right)^b; n \ge i \ge j \tag{123}$$

where *B*i,j is the mass fraction of primary breakage products, *x*<sup>i</sup> is the largest size, and the parameters *φ*, *γ* and *β* define the size distribution of the material being ground. When plot‐ ting the size versus *B*i,j on log paper, the slope of the lower part of the curve gives the value of *γ*, the slope of the upper part of the curve gives the value of *β*, and *φ* is the intercept [319].

#### **8. Granulation**

attributed to three basic mechanisms; the abrasion, the impact and the corrosion. These mechanisms can be simultaneously active in given grinding environment, leading to

82 Strontium Aluminate - Cement Fundamentals, Manufacturing, Hydration, Setting Behaviour and Applications

The action of grinding media within the rotating mill not only crushes the existing clinker particles, but also sharply compresses them, which in fact leads to the formation of electro‐ static surface charges of opposed polarity. The cement particles agglomerate as a result of the forces of attraction acting on them. Consequently, the cement particle agglomeration re‐

**•** The internal operating conditions of mill (humidity, temperature, ventilation, condition of

Additives, such as water, organic liquids and some inorganic electrolytes are used to reduce the surface free energy of the material being ground with a view to improve the grinding

In the grinding process, a variety of grinding aids are used. There are aliphatic amines such as triethylenetetramine (TETA), tetraethylenepentamine (TEPA) and aminealcohols such as diethanolamine (DEA), triethanolamine (TEA) and triisopropanolamine (TIPA). Glycol com‐ pounds are represented such as ethyleneglycol (EG), diethyleneglycol (DEG). In addition, there are more complex compounds such as aminoethylethanolamine (AEEA) and hydrox‐ yethyl diethylenetriamine (HEDETA). Phenol and phenol-derivates are also used as grind‐ ing aids, as well as other compounds, such as amine acetate, higher polyamines and their

Assuming that a grinding mill is equivalent to a chemical reactor with a first-order phenom‐ enological rate of reaction kinetics [288], the rate of decrease in particle size during the batch grinding of brittle material in ball mill can be described by the first-order equation. The

is the specific rate of breakage of feed size *i* and *w*i,t is the mass fraction of total

, ,0 = - exp ( ) *w w St it i <sup>i</sup>* (121)

breakage rate of such material was expressed in literature as [289]:

charge. For single component (*i*=1) Eq.121 can be rewritten as:

duces the efficiency of mill. The extent of agglomeration depends on [287]:

**•** The specific characteristics of materials to be ground;

**•** The efficiency and distribution of grinding media;

**•** The operating parameters of mill;

**•** The fineness of cement particles;

hydroxyethyl derivates [287,322].

**7.3. Grinding kinetics**

where *S*<sup>i</sup>

armor plating, etc.).

efficiency.

complex interactions [286].

**7.2. Grinding aids**

The spheroidal aggregate of particles is called a granule, ball, pellet, or an agglomerate. The nucleation, compaction, size enlargement, and spheroidization of pellets take place in the course of balling and granulation and related agglomeration processes [291]. The granula‐ tion converts fine powder and/or sprayable liquids (e.g. suspensions, solutions or melts) into granular solid products with more desirable physical and/or chemical properties than the original feed material. This size enlargement technique constitutes a key process in many in‐ dustries such as the pharmaceutical, food, ore processing and fertilizers ones. Particularly, the granulation process has clear advantages regarding the storage, handling and transpor‐ tation of the final product [292,293].

The new king of agglomeration technology is binder-less granulation, where the original co‐ hesiveness of powder material is utilized to arrange them into granules. The strength of product granules can be much weaker. However, if the product granules are just an inter‐ mediate product in a larger process, such weakness has significant advantages. In many ma‐ terial-forming processes, the boundary between granules remains even after shaping due to unnecessary strength of granules. With weaker granules, the density of green bodies pro‐ duced by the application of the same pressure as for conventional granules can be much higher. In many cases, the binder removal cannot be done completely leaving possible de‐ fects caused by carbonacious pyrolysis residues. Weaker granules can also be advantageous in pharmaceutical processes depending on the purpose of granulation [294].

Using large pellets for the processing of strontium aluminate clinker (Fig.31 in Chapter 4.5) may change the behaviour during thermal treatment as well as some properties of the prod‐ uct due to increasing influence of partial pressure of carbon dioxide on the thermal decom‐ position of strontium carbonate. The material forming the diffusion barrier as the reaction zone is shifted from the surface into the deeper zones of pellet. Increasing partial pressure of carbon dioxide slows down the rate of thermal decomposition of strontium carbonate and increases the temperature required for the thermal decomposition (please see the discussion in Chapter 4.2) and temporary lack of SrO in the reaction zone. Therefore, the influence of large pellets on prepared strontium aluminate clinker is similar to the usage of mixture with lower saturation degree (discussed in Chapter 4).

**Chapter 3**

**Technology of Thermal Treatment**

this understanding for the performance enhancement [297].

[295,296].

[297,299,300].

Cement is made of clinker and ground gypsum, whereas clinker is produced from fired limestone and clay mixed in particular percentages. Portland cement clinker was first made in 1842 in modified form of traditional static limekiln. Around 1885, the experiments began on the design of continuous kilns. One of the designs was the shaft kiln, similar in design to a blast furnace. The raw meal in the form of lumps and fuel were continuously added at the top, and clinker was continually withdrawn at the bottom. Compressed air was blown through from the base to combust the fuel. The shaft kiln had been used for only short period of time before it was forced out by the rotary kiln, but it has had a limited renaissance from 1970 onward in China and elsewhere, when it has been used for the small-scale, low-tech plants in rural areas away from transport access. A typical shaft kiln can produce 100–200 tons/day. Nowadays, rotary kiln is one of the key equipment in cement industry used to convert calcineous raw meal to cement clinker. Raw meal for the cement production is a mixture of predetermined proportions of limestone, silica, and small quantities of alumina and iron oxide

The cement making processes are extremely energy consuming. Typically for the production of one ton of cement, a well-equipped plant consumes nearly 3 GJ. For each ton of produced clinker an equivalent amount of greenhouse gases is emitted. The manufacture of cement is the focus of considerable attention worldwide because of giant amount of used energy and high environmental impact of the process. Considering the recent impetus on the emission of greenhouse gases reductions and on the reduction of energy consumption, a renewed emphasis arises on developing the computational models for cement industry and on applying

The most important plant unit in cement manufacturing is the kiln [298]. The raw material passes sequentially through pre-heater, calciner, kiln and cooler to form the cement clinker. In a pre-heater section the raw meal is pre-heated to the calcination temperature via hot gases coming from calciner. In calciner, the raw meal is partially calcined. The energy required for the endothermic calcination reaction is provided by combusting a suitable fuel. In most cases, coal is used to provide the required energy, especially in India. The calciner is supplied with tertiary air from the cooler and with air coming out of kiln exhaust. The former is to supply coal with O2 sufficiently during the combustion and the later to utilize the heat of kiln gases to enhance the calcination reaction. Hot gases from calciner are sent to pre-heater assembly to pre-heat the solids. Partially calcined solids from the calciner are fed slowly to a rotary kiln. In rotary kiln, remaining calcination and other reactions of formation of clinker phases proceed

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