**2. Experimental**

All chemicals were bought in analytical purity and were used without further purification. The main chemicals, calcium chloride and ferrous sulfate, were purchased from Vetec. The manganese and nickel solutions (1000 mg L−1) were prepared and used as stock solutions.

Sodium alginate was supplied by Sigma-Aldrich Chemicals Co. The industrial wastewater used in this work was provided by a large metallurgical company, more particularly from the E-coat painting line pretreatment, which is a water-based immersion coating process for application on metal parts.

## **2.1 Synthesis of nanomagnetic absorbent**

The nanomagnetic absorbent were prepared according to the method described in Llanes et al. [14] with some adaptations. It was synthesized an iron oxide-alginate nanocomposites in situ, as follows. A aqueous solution of sodium alginate (50 mL) was added dropwise, at room temperature, to a degassed ferrous sulfate heptahydrate solution (0.3 mol L−1) using a syringe fitted with a needle. The pale-yellow Fe(II)-crosslinked beads were formed immediately. The solution was gently stirred, during the whole addition, and remained under stirring for 45 min. The beads were separated by filtration and washed, several times, with ethanol/water (1/1), to remove the excess ferrous ions. Then an aqueous solution of sodium hydroxide (0.5 mol L−1) was added to the beads, resulting in a change in the color of the beads from light orange to dark green. The suspension was stirred for 30 min. and then heated at 65 ± 5°C in a water bath. A solution of hydrogen peroxide (10% v/v) was added dropwise. The suspension was stirred at 65 ± 5°C for 60 min. Nitrogen was bubbled in the suspension before the oxidation stage. The resulting beads were washed with ethanol/water (1/1) and added to an aqueous solution of calcium chloride (0.3 mol L−1) and stirred for 24 h. Finally, the beads were separated, washed some times and placed in a kiln at 40°C for 24 h, to obtain reddish-brown beads.

#### **2.2 Characterization**

The content of mannuronate (M) and guluronate (G) units of sodium alginate sample was 62.8% and 37.2%, respectively, calculated by 13C CP-MAS NMR in our previous study [15]. The viscosity average molar mass (− Mv) of sodium alginate was calculated by applying the equation of Mark-Houwink-Sakurada, using K = 7.3 x 10–5 dL/g and a = 0.92, obtaining a value of 4.7 x 104 g mol−1 [15].

The iron oxide particle size was determined by transmission electron microscopy (TEM) using an FEI Tecnai G2 F20 microscope. The samples were ground in an agate mortar along with methyl alcohol, after which the supernatant was removed from the mortar and diluted in 1 mL of methyl alcohol. The resulting solution was kept in an ultrasound bath for 10 minutes. A drop of the mixture was then deposited on a copper mesh with carbon film. The magnetic properties were analyzed by a vibrating sample magnetometer (VSM) calibrated with a nickel standard cylinder at room temperature (25° C). The total analysis time was 10 minutes and the magnetic field ranged from 2,000 to 12,000 G, and each spot was measured at 1.5 second intervals. The Mössbauer spectrum was obtained at room temperature with constant acceleration with 1024 channels, encompassing a velocity range of −11 to +11 mm/s with increments of about 0.045 mm/s per channel. Through the X-ray diffraction (XRD) it was possible to identify the metals present in the hydrogel sample. The samples were macerated with the help of pistil and gral. The diffractograms were obtained in a Shimadzu diffractometer, model XRD

6000, equipped with iron tube and graphite monochromator. The scans were made between 15 and 60° (2θ), with a goniometer speed of 2°/ min.

The morphological properties were analyzed by granulometry using a Retsch AS 200 Basic shaker with analytical sieves of 15 to 50 mesh, optical microscopy (OM) with an Olympus SZX10 microscope, for which the samples were placed on a glass slide subjected to the action of a light beam for observation, and scanning electron microscopy (SEM) with a JOEL JSM-6510LV apparatus, after coating samples with a thin gold layer. For image capture, secondary electron detectors and energy dispersive X-ray analysis (EDX) were used, with acceleration voltage of 20 kV. The metal ion concentration in the aqueous solution and industrial wastewater was determined using a Varian AA240 atomic absorption spectrophotometer (AAS), with samples diluted in order to adjust them to the calibration curve previously obtained for each metal, followed by addition of nitric acid (HNO3) to prepare the samples for analysis.

#### **2.3 Water uptake (WU) of nanomagnetic absorbent**

The *WU* capacities were determined at room temperature through the Eq. (1).

$$
\Delta WU = \frac{\left(\mathbf{W}\_{\text{w}} - \mathbf{W}\_{\text{d}}\right)}{\mathbf{W}\_{\text{d}}}.\text{100}\tag{1}
$$

Ww is the weight of swelled absorbent in water at equilibrium and Wd is the weight of dried absorbent (average weight of 100 mg). These experiments were performed in triplicate.

#### **2.4 Adsorption experiments**

The adsorption experiments were performed for 1 h contact time at room temperature by shaking with a constant weight of the nanomagnetic absorbent (100 mg). The initial concentrations of Mn(II) and Ni(II) in the solutions were varied from 50 mg L−1 and then 100 to 500 mgL−1 at intervals of 100 mgL−1.

Adsorption experiments of the metal ions in the industrial wastewater were performed at 1 hour of contact time at room temperature by shaking with the sample natural pH (pH = 6.5). The absorbent mass ranged from 50 mg and then 100–300 mg in 100 mg intervals.

### **3. Results and discussion**

The swelling of a polymer depends on the degree of interaction between the solvent and polymer molecules. The swelling kinetic is shown in **Figure 1**. The swelling degree at equilibrium was reached in 60 min and its value was 52%.

The size distribution curve of nanomagnetic absorbent (NA) is shown in **Figure 2(a)**. The size of the NAs produced ranged from 500 to 850 μm. The shape of the beads was mostly spherical, according to **Figure 2(b)**.

**Figure 3** depicts the SEM images of NAs. In general, the beads were mostly spherical, confirming the results of OM images, and the surfaces were rough, which favors the adsorption of the NAs. The composition maps (**Figure 3**) reveal a homogeneous distribution of calcium and iron elements throughout the polymeric matrix surface. To confirm the presence of both components (calcium and iron)

*Nanomagnetic Polymeric Absorbent Based on Alginate and Gamma-Maghemite Synthesized… DOI: http://dx.doi.org/10.5772/intechopen.98611*

**Figure 1.** *Swelling kinetic of nanomagnetic absorbent, in deionized water.*

**Figure 2.** *Size distribution of synthesized NAs (a); optical microscopic image of NAs (b).*

#### **Figure 3.** *SEM micrograph of NA external surface and composition maps of iron (Fe) and calcium (Ca) (magnification: 100X).*

#### **Figure 4.**

*SEM micrograph of NA internal surface and composition maps of iron (Fe) and calcium (Ca) (magnification: 300X).*

#### **Figure 5.**

*TEM images of maghemite nanoparticles synthesized into the NA (in situ).*

inside the microspheres, a cut as made in one of the samples ([Alg-Na] = 3% m/v; [FeSO4] = 0.3 mol L−1; [CaCl2] = 0.3 mol L−1) as shown in **Figure 4**. It can be seen that the microsphere has a massive internal surface containing both components.

The transmission electron microscopic (TEM) images and EDX spectra (**Figure 5**) proved that the magnetic iron oxide particles were dispersed in the NA with nanometric size (< 20 nm), confirming the formation of a nanocomposite with superparamagnetic behavior.

The VSM curve (**Figure 6**) demonstrates that the NA did not present a hysteresis cycle, a phenomenon that causes a delay between the magnetic flux density and the magnetic field. The saturation magnetization was found to be 9.88 emu/g. The values of coercivity (Hc) and remanence were 17.50 G and 0.30 emu/g, respectively. Besides that, all the samples were sensitive to magnetic stimulus by a magnet (**Figure 6**). A video is shown in Supplementar Material.

*Nanomagnetic Polymeric Absorbent Based on Alginate and Gamma-Maghemite Synthesized… DOI: http://dx.doi.org/10.5772/intechopen.98611*

**Figure 6.** *Magnetization curve of NA and digital photograph of the samples responding to the stimulus of a magnet.*

The Mössbauer spectrum (**Figure 7a**) showed the dominance of a central doublet and the presence of a low intensity diffuse sextet, typical of superparamagnetic relaxation [16].

The hyperfine parameters indicated the presence of a compound containing Fe3+ and maximum magnetic field probability less than 200 kOe. For the doublet, the quadrupole splitting and isomer shift of the sample were 0.70 mm/s and 0.35 mm/s, respectively. These values again indicate the presence of a phase containing Fe3+ [17, 18].

The superparamagnetic behavior is caused by the presence of nanometric particles, of the order of 10 nm. According to the XRD diffractogram (**Figure 7b**), the diffuse peaks of the carrier phase of iron indicate the presence of nanosized particles. The phase of iron (III) oxide (maghemite, γ-Fe2O3) was identified in the X-ray diffraction patterns by the rays at the approximate positions of 2θ = 36°, 45° and 52°.

#### **3.1 Adsorption of metallic ions from industrial wastewater by the NAs**

After preparing and characterizing the nanomagnetic absorbent (NA), we investigated their adsorption capacity for removal of metallic ions from wastewater samples from the metallurgical industry.

The untreated wastewater was analyzed by atomic absorption spectrometry to ascertain the concentration of metals. The results are shown in **Table 1**.

Among the metals analyzed, manganese and nickel had the highest concentrations, both derived from surface protective coating by cathodic electrodeposition, in both cases above the thresholds allowed for discharge into the environment [19]. In view of these results, we decided to evaluate the ability of the NA to adsorb these metals (Mn and Ni) to reduce their concentration.

We first performed kinetic studies of the adsorption of these metals present in an aqueous solution prepared in the laboratory to verify the adsorption equilibrium time of each metal contaminant. The results showed that the adsorption

**Figure 7.** *Mössbauer spectrum (a) and XRD diffractogram (b) of NA.*

equilibrium time for both ions was about 60 minutes, as shown in **Figure 8**, where the quantity of each metal adsorbed at equilibrium (Qe) can also be seen.

From the adsorption kinetic curves of Ni(II) and Mn(II), it can be seen that the nanomagnetic absorbent presented satisfactory removal potential. After 60 minutes, the adsorption capacity (Qe) of nickel 12.9 mg/g of NA, which corresponds to removal potential of 52%, while for manganese it was 12.3 mg/g of NA, corresponding to removal potential of 49%.

The fact that the adsorption capacity was much more pronounced in the first 30minutes can be explained by the adsorption mechanism, which occurs in three steps [20, 21]:


*Nanomagnetic Polymeric Absorbent Based on Alginate and Gamma-Maghemite Synthesized… DOI: http://dx.doi.org/10.5772/intechopen.98611*


**Table 1.**

*Concentration of the metals presented in the industrial wastewater sample.*

#### **Figure 8.**

*Adsorption capacity (Qe) and removal percentage (%) of ions from aqueous solutions by NAs in function of time: (a) [Ni2+]onset = 50 mg L−1; V = 50 mL; m = 100 mg e (b) [Mn2+]onset = 50 mg L−1; V = 50 mL; mMHB = 100 mg (pH = 6.5).*

#### **Figure 9.**

*Effect of NA mass on adsorption of Ni(II) (a) and Mn(II) from industrial wastewater (b) [experimental condition: pH = 6.5 and V = 50 mL].*

3.Immeasurably fast step, when the adsorption itself takes place (adsorption of the adsorbate on the internal surface of the adsorbent particles). The third step does not offer any resistance to the process, so that the mass transfer and intraparticle diffusion are the steps that determine the adsorption speed.

The maximum adsorption equilibrium times observed for the two metals in question were short (60 minutes), indicating rapid reaction between the adsorbent material and the metallic ions in solution. This means the NA prepared in this study has good potential for application on industrial scale.

Two experiments were performed with the industrial wastewater, one to analyze the kinetics in function of the NA mass and the other to assess the adsorption mechanism of these ions. The intention of applying the NA for commercial treatment of wastewater is to remove metallic ions without the need to adjust the pH. Therefore, all the experiments were performed at the natural pH of the sample, 6.5.

### **3.2 Analysis of the adsorption kinetics in function of NA mass (for treatment of wastewater)**

To ascertain the most suitable quantity of nanomagnetic absorbent to remove Ni2+ and Mn2+ from the industrial wastewater, we performed studies in which the *Nanomagnetic Polymeric Absorbent Based on Alginate and Gamma-Maghemite Synthesized… DOI: http://dx.doi.org/10.5772/intechopen.98611*

NA mass was varied (**Figure 9**). The results showed that 300 mg of NAs removed 60.5% and 56.6% of Ni (II) and Mn (II), respectively. Also, the higher the NA mass, the greater the removal percentages of Ni (II) and Mn (II) were. That was expected, considering that with the increase of NA mass, the availability of binding sites with metals also increases.

#### **3.3 Competitiveness between the metals: adsorption mechanism**

We performed analysis by atomic absorption spectrometry of calcium, iron, nickel and manganese ions after application of the hydrogel in the wastewater sample, for the purpose of determining the interaction between these ions and the alginate (**Figure 10**). Both nickel and manganese were adsorbed by the hydrogel (concentrations in the wastewater diminished) while calcium was desorbed by

#### **Figure 10.**

*Concentration of Ni2+ (a), Mn2+ (b), Ca2+ and Fe2+ ions in the wastewater as a function of contact time with the nanomagnetic absorbent (experimental conditions: mNA = 300 mg; pH = 6.5 and V = 50 mL).*

the hydrogel (concentration in the medium increased). This indicates the occurrence of ionic exchange of Ni2+ and Mn2+ with Ca2+. The iron concentration remained unchanged, proving no loss of magnetic material occurred from the hydrogel.
