**3. Isothermal titration calorimetry**

As its name indicates, ITC measures the heat change accompanying the injection of a titrant into titrate at constant temperature. In contemporary instruments, this is accomplished by compensating for any temperature difference between the sample and reference cells (the latter lacking titrate, usually just water). The raw ITC signal is therefore power *P*, a timedependent variable. Integration with respect to time therefore yields heat *q* which is the primary dependent variable that tracks the progress of the titration of interest:

$$q(\Delta t) = \int\_0^\infty Pdt\,\,.\tag{12}$$

Typically, ITC is operated in incremental mode in which the titrant is injected in preset aliquots after successive re-equilibration periods. A feature of ITC that distinguishes it from most titration techniques is that the measured heat does not accumulate from one injection to the next, but dissipates as the instrument measures the heat signal by returning the sample and reference cells to isothermal conditions. ITC is therefore a differential technique

Probing Solution Thermodynamics by Microcalorimetry 879

If the interaction under investigation occurs in a buffered solution, the earlier discussion on the temperature dependence of p*K*a would again be relevant. More generally, binding that involves coupled uptake or release of protons will contain the buffer's enthalpy of ionization

<sup>e</sup> <sup>e</sup>

[X]t x 10-6 M

Finally, ITC has been used as an "analog" of DSC for studying the stability of complexes. A concentrated solution of complex in the syringe is titrated into pure water or buffer in the cell. The resulting dilution drives complex dissociation and the attendant enthalpy is measured. This method has been used to characterize complexes through the spectrum of stoichiometries, from dimers (Burrows et al. 1994; Lovatt et al. 1996) to higher oligomers (Lassalle et al. 1998; Luke et al. 2005) to polymeric species (Stoesser and Gill 1967; Arnaud and Bouteiller 2004). Again, given the sensitivity of ITC, relatively high concentrations are required, so this technique is limited to the measurement of relatively weak complexes. It has been shown (Poon 2010) that the ITC data can be used to diagnose a dimeric or higher-

Two types of baselines are operative in an ITC experiment. One is instrument noise. Drifts on the order of 0.02 µW/h are routinely achievable in contemporary instruments. Another source of baseline arises from the injection of titrant. At the very least, viscous mixing makes a measurable if small exothermic contribution to the observed heat. This effect can be observed in a blank-to-blank injection (Figure 4), and serves as a casual useful indicator of the cleanliness of the cell and syringe between sample runs. Moreover, any mismatch in the matrices of the titrant and titrate will be manifest as a dilution enthalpy with each injection.

Fig. 3. The differential nature of ITC data. The volume and enthalpy are intentionally omitted to illustrate the differential nature of ITC data with respect to total titrant concentration. *S*imulated 1:1 binding to 10 µM titrate is shown in Panel *A*, with the corresponding integrated binding curves in Panel *B*. The values of *K* are as follows: a, 10-9 M; b, 10-8 M; c, 10-7 M; d, 10-6 M; and e, 10-5 M. The values of *c*titrate/K range from 104 to 1.

order complex based on the presence of an inflection point in the latter.

<sup>d</sup> <sup>d</sup> c c

. (15)

B a,b

0 5 10 15 20

0

2

4

[X]b x 10-6 M

6

8

10

p *d HT*( ) *<sup>C</sup> dT*

in the apparent binding enthalpy (Fisher and Singh 1995).

a,b A

0 5 10 15 20

0.0

**3.1.1 Baseline signals** 

0.2

0.4

0.6

d[X]b/d[X]t

0.8

1.0

with respect to the concentration of the titrant (X) *i.e.*, the derivative of *q* with respect to the total titrant concentration, [X]t:

$$\frac{dq}{d[\mathbf{X}]\_\iota} = V \sum\_{i=1}^n \Delta H\_i \frac{d[\mathbf{X}\_i]\_\iota}{d[\mathbf{X}]\_\iota} \,. \tag{13}$$

where [X*i*]b is the concentration of X in the *i*-th bound state. This contrasts with most other physical binding signals (*e.g.*, absorbance, fluorescence intensity or anisotropy, pH) which are integrative in nature.

### **3.1 Experimental conditions for ITC**

As a thermodynamic tool for studying molecular interactions, the singular strength of ITC is the direct measurement of binding enthalpies. Model-based analysis of ITC data, the subject of Section 3.2, allows the extraction of binding affinity and additional parameters in complex systems. As a label-free technique, ITC compares favorably with other titration techniques such as fluorescence and radioactivity. However, despite much-improved sensitivity (minimum detectable thermal energy <0.1 µJ), baseline stability, and titrant control found in contemporary instruments, sensitivity of ITC is relatively limited. The actual limit of detection depends primarily on the intrinsic enthalpy of the binding system at the temperature of interest, and to a lesser extent, the physical configuration of the instrument. Roughly speaking, a typical ITC experiment requires at least 10-6 M of titrate in a 1-mL volume and 10-4 M of titrant in a 100-µL syringe. (Recently, so-called "low volume" instruments equipped with 200-µL cells and 50-µL syringes have become available.)

The sensitivity of ITC is helped considerably by the differential nature of its signal (which is proportional to <sup>t</sup> [X] *dq <sup>d</sup>* ) with respect to titrant concentration (Figure 3). In practice, the

requirement for sufficient concentration in the sample cell to produce sufficient heat signals poses a direct limit on the tightest binding that may be reliably determined. Specifically, depletion of titrant dominates at titrate concentrations that are high relative to the dissociation constant *K*. Under this condition, the titration approaches a discontinuity in the first derivative at the equivalence point (Poon 2010). In the case of simple 1:1 binding, an empirical relationship that the product 1 < *c*titrate/*K* < 1000, where *c*titrate is the titrate concentration, is optimal for reliable estimation of *K* (Wiseman et al. 1989). One way of getting around this problem for very tight binding is to lower the apparent value of *K* by including a suitable, fixed concentration of competitor in the cell. Another possibility is continuous ITC, which will be discussed in Section 3.1.2. It should be noted that even under conditions where *K* cannot be determined, *H* can still be determined by integration of the measured heat:

$$
\Delta H = \frac{1}{c\_{\text{intra}}} \int\_{0}^{\upsilon} \frac{q(v)}{v} dv \, \, \, \tag{14}
$$

where *V* is the volume of the (fixed) sample cell. (A volume correction is generally necessary; see Section 3.2.1.3.) A requirement for Eq (14) is, of course, that the titration is complete. Whichever the case, repeating the titration at different temperatures provides an estimate of the change in heat capacity by Kirchoff's relation:

with respect to the concentration of the titrant (X) *i.e.*, the derivative of *q* with respect to the

1 t t

[X] [X] *n*

where [X*i*]b is the concentration of X in the *i*-th bound state. This contrasts with most other physical binding signals (*e.g.*, absorbance, fluorescence intensity or anisotropy, pH) which

As a thermodynamic tool for studying molecular interactions, the singular strength of ITC is the direct measurement of binding enthalpies. Model-based analysis of ITC data, the subject of Section 3.2, allows the extraction of binding affinity and additional parameters in complex systems. As a label-free technique, ITC compares favorably with other titration techniques such as fluorescence and radioactivity. However, despite much-improved sensitivity (minimum detectable thermal energy <0.1 µJ), baseline stability, and titrant control found in contemporary instruments, sensitivity of ITC is relatively limited. The actual limit of detection depends primarily on the intrinsic enthalpy of the binding system at the temperature of interest, and to a lesser extent, the physical configuration of the instrument. Roughly speaking, a typical ITC experiment requires at least 10-6 M of titrate in a 1-mL volume and 10-4 M of titrant in a 100-µL syringe. (Recently, so-called "low volume"

instruments equipped with 200-µL cells and 50-µL syringes have become available.)

The sensitivity of ITC is helped considerably by the differential nature of its signal (which is

requirement for sufficient concentration in the sample cell to produce sufficient heat signals poses a direct limit on the tightest binding that may be reliably determined. Specifically, depletion of titrant dominates at titrate concentrations that are high relative to the dissociation constant *K*. Under this condition, the titration approaches a discontinuity in the first derivative at the equivalence point (Poon 2010). In the case of simple 1:1 binding, an empirical relationship that the product 1 < *c*titrate/*K* < 1000, where *c*titrate is the titrate concentration, is optimal for reliable estimation of *K* (Wiseman et al. 1989). One way of getting around this problem for very tight binding is to lower the apparent value of *K* by including a suitable, fixed concentration of competitor in the cell. Another possibility is continuous ITC, which will be discussed in Section 3.1.2. It should be noted that even under conditions where *K* cannot be determined, *H* can still be determined by integration of the

> 0 titrate <sup>1</sup> *<sup>V</sup> q v*( ) *<sup>H</sup> dv c v*

where *V* is the volume of the (fixed) sample cell. (A volume correction is generally necessary; see Section 3.2.1.3.) A requirement for Eq (14) is, of course, that the titration is complete. Whichever the case, repeating the titration at different temperatures provides an

estimate of the change in heat capacity by Kirchoff's relation:

, (14)

*<sup>d</sup>* ) with respect to titrant concentration (Figure 3). In practice, the

*i dq <sup>d</sup> V H d d*

b

. (13)

[X ]

*i i*

total titrant concentration, [X]t:

are integrative in nature.

proportional to

measured heat:

**3.1 Experimental conditions for ITC** 

<sup>t</sup> [X] *dq*

$$
\Delta \mathcal{C}\_p = \frac{d \Delta H(T)}{dT} \,. \tag{15}
$$

If the interaction under investigation occurs in a buffered solution, the earlier discussion on the temperature dependence of p*K*a would again be relevant. More generally, binding that involves coupled uptake or release of protons will contain the buffer's enthalpy of ionization in the apparent binding enthalpy (Fisher and Singh 1995).

Fig. 3. The differential nature of ITC data. The volume and enthalpy are intentionally omitted to illustrate the differential nature of ITC data with respect to total titrant concentration. *S*imulated 1:1 binding to 10 µM titrate is shown in Panel *A*, with the corresponding integrated binding curves in Panel *B*. The values of *K* are as follows: a, 10-9 M; b, 10-8 M; c, 10-7 M; d, 10-6 M; and e, 10-5 M. The values of *c*titrate/K range from 104 to 1.

Finally, ITC has been used as an "analog" of DSC for studying the stability of complexes. A concentrated solution of complex in the syringe is titrated into pure water or buffer in the cell. The resulting dilution drives complex dissociation and the attendant enthalpy is measured. This method has been used to characterize complexes through the spectrum of stoichiometries, from dimers (Burrows et al. 1994; Lovatt et al. 1996) to higher oligomers (Lassalle et al. 1998; Luke et al. 2005) to polymeric species (Stoesser and Gill 1967; Arnaud and Bouteiller 2004). Again, given the sensitivity of ITC, relatively high concentrations are required, so this technique is limited to the measurement of relatively weak complexes. It has been shown (Poon 2010) that the ITC data can be used to diagnose a dimeric or higherorder complex based on the presence of an inflection point in the latter.

#### **3.1.1 Baseline signals**

Two types of baselines are operative in an ITC experiment. One is instrument noise. Drifts on the order of 0.02 µW/h are routinely achievable in contemporary instruments. Another source of baseline arises from the injection of titrant. At the very least, viscous mixing makes a measurable if small exothermic contribution to the observed heat. This effect can be observed in a blank-to-blank injection (Figure 4), and serves as a casual useful indicator of the cleanliness of the cell and syringe between sample runs. Moreover, any mismatch in the matrices of the titrant and titrate will be manifest as a dilution enthalpy with each injection.

Probing Solution Thermodynamics by Microcalorimetry 881

(phosphates). The so-called Donnan ratio, *r*D, is significantly above unity even at low polyion:salt ratios (). Eq (16) shows that a ten-fold excess of salt concentrations (=0.1) leads to a 10% exclusion of A or B from the compartment occupied by polyion. If AB is a buffer salt, the result is also a change of pH. Such asymmetry will modify the heat observed by ITC. As is well known, and illustrated by Eq (16), Donnan effects can be suppressed by ensuring a sufficient excess of diffusible salt in the dialysate. Unfortunately, the required salt concentrations may interfere with the investigation of interactions mediated substantially by electrostatic effects (as is usually the case for polyions). If possible, therefore, it is advisable

to arrange for the polyionic species to be in the cell, where concentrations are lower.

more appropriate solution is to add a constant parameter *B* to the fitting equation:

**3.1.2 Continuous ITC titrations** 

binding.

integration of thermal power is performed to obtain

obsd b 1 t t

While incremental titrations most commonly performed in ITC, an alternative mode of operation is a continuous titration (cITC) (Markova and Hallén 2004). In cITC, the titrant is continuously into injected the cell at a low rate (~0.1 µL/s). The primary advantage of cITC is throughput. An incremental ITC experiment typically requiring 20 injections of 5 µL at intervals of 300 s takes (neglecting time for baseline stabilization) 100 min; at 0.1 µL/s, cITC would require approximately 17 min. Another potential motivation for cITC is increased resolution in terms of model-dependent analysis. In incremental ITC, peak-by-peak

collected data points (typically 1 s-1 over 103 s, or about one to two hours) for nonlinear regression to the number of injections (usually 10 to 30). By using the thermal power data directly for fitting, cITC can in principle discriminate the curvature required to define tight

Maintenance of quasi-equilibrium conditions throughout the titration is essential to correct interpretation of derived thermodynamic parameters and is a major concern for cITC. To this end, the stirring rate in cITC must be considerably increased (up to 700 rpm) relative to incremental ITC to facilitate mixing of titrant into the titrate solution. Additionally, the

[X] [X] *n*

*i dq <sup>d</sup> VH B d d*

[X ]

*i i*

> <sup>t</sup> [X] *dq*

. (17)

*<sup>d</sup>* . This step reduces the number of

In practical terms, none of these baselines effects are significant if the heat generated by the interaction of interest is sufficiently strong. This is not always achievable, however, for several reasons. Availability or solubility of the sample, particularly biological samples, may be limiting. It may also be desirable, for example, to perform titrations at a range of cell concentrations for binding to oligomerizing systems. Characterization of binding to a polyion at low salt concentration may require a reduced concentration. Thus, strategies for handling relatively low signal-to-noise situations are helpful in many situations. The most basic of these involve inspection and, where necessary, manual editing of the power baseline to mitigate the occasion excursion due to instrumental noise. To this end, an increase in the time between injection may be indicated to unambiguously identify the restoration of baseline. In addition, the residual heats (which may be up to 10 µJ) after the equivalence point are unlikely to be negligible. Subtraction with data from a titrant-to-blank run would likely introduce more noise into the data and be no more helpful than taking a simple average of the final post-equivalence heats. If the data is to be fitted to models, a

For small molecules, solids or lyophilized samples are usually dissolved in water or buffer. To complicate matters, hydrophobic solutes often require a cosolvent such as DMSO or DMF to achieve initial solubility before addition of the aqueous solvent; dilution of the cosolvent will therefore contribute to the observed heat at each injection. In other cases, ionizable solutes can perturb solution pH due to their substantial (>10-3 M) concentration in the syringe. Unless the solvent is adequately buffered, the pH in the cell and syringe will differ significantly and neutralization heats will contribute to the observed signal.

Fig. 4. Typical water-water control "titration." *Inset*, integrated areas of the water peaks. Given the low signal-to-noise ratios, the values must be considered very crude. However, the scatter also attests to the cleanliness of the cell and syringe.

In the case of macromolecular titrant and titrates, the solution matrices can be closely matched by extensive co-dialysis in the same solution. Care must be taken, however, with ionic polymers such as nucleic acids. These solutes can alter the distribution of ions in their compartment during dialysis due to the Donnan effect. Specifically, a non-diffusible polyionic solute excludes diffusible ions of the same charge from their compartment and therefore induces an asymmetric distribution of diffusible ions across the semipermeable membrane at equilibrium. To illustrate, for a simple system consisting only of the nondiffusible polyion M and a monovalent salt AB, the ratio concentrations of A+ or B across the membrane is (Cantor and Schimmel 1980):

$$r\_{\rm D} = \frac{z[\rm M]}{2[\rm AB]\_{\rm t}} + \sqrt{1 + \left(\frac{z[\rm M]}{2[\rm AB]\_{\rm t}}\right)^2} = \Psi + \sqrt{1 + \Psi^2} \,, \tag{16}$$

where *z* is the charge on the polyion (shown simply as M for brevity). At the concentrations required for the syringe, *z*[M] can be substantial. For example, a duplex oligonucleotide consisting of 20 base-pairs represents at 100 µM contributes 4 mM in total anions

For small molecules, solids or lyophilized samples are usually dissolved in water or buffer. To complicate matters, hydrophobic solutes often require a cosolvent such as DMSO or DMF to achieve initial solubility before addition of the aqueous solvent; dilution of the cosolvent will therefore contribute to the observed heat at each injection. In other cases, ionizable solutes can perturb solution pH due to their substantial (>10-3 M) concentration in the syringe. Unless the solvent is adequately buffered, the pH in the cell and syringe will

0 1000 2000 3000 4000 5000 6000

q, J

across

, (16)


Time, s

In the case of macromolecular titrant and titrates, the solution matrices can be closely matched by extensive co-dialysis in the same solution. Care must be taken, however, with ionic polymers such as nucleic acids. These solutes can alter the distribution of ions in their compartment during dialysis due to the Donnan effect. Specifically, a non-diffusible polyionic solute excludes diffusible ions of the same charge from their compartment and therefore induces an asymmetric distribution of diffusible ions across the semipermeable membrane at equilibrium. To illustrate, for a simple system consisting only of the nondiffusible polyion M and a monovalent salt AB, the ratio concentrations of A+ or B-

2

2

Fig. 4. Typical water-water control "titration." *Inset*, integrated areas of the water peaks. Given the low signal-to-noise ratios, the values must be considered very crude. However,

t t

2[AB] 2[AB] *z z*

[M] [M] 1 1

 

where *z* is the charge on the polyion (shown simply as M for brevity). At the concentrations required for the syringe, *z*[M] can be substantial. For example, a duplex oligonucleotide consisting of 20 base-pairs represents at 100 µM contributes 4 mM in total anions

the scatter also attests to the cleanliness of the cell and syringe.

the membrane is (Cantor and Schimmel 1980):

D

*r*


P, W

differ significantly and neutralization heats will contribute to the observed signal.

(phosphates). The so-called Donnan ratio, *r*D, is significantly above unity even at low polyion:salt ratios (). Eq (16) shows that a ten-fold excess of salt concentrations (=0.1) leads to a 10% exclusion of A or B from the compartment occupied by polyion. If AB is a buffer salt, the result is also a change of pH. Such asymmetry will modify the heat observed by ITC. As is well known, and illustrated by Eq (16), Donnan effects can be suppressed by ensuring a sufficient excess of diffusible salt in the dialysate. Unfortunately, the required salt concentrations may interfere with the investigation of interactions mediated substantially by electrostatic effects (as is usually the case for polyions). If possible, therefore, it is advisable to arrange for the polyionic species to be in the cell, where concentrations are lower.

In practical terms, none of these baselines effects are significant if the heat generated by the interaction of interest is sufficiently strong. This is not always achievable, however, for several reasons. Availability or solubility of the sample, particularly biological samples, may be limiting. It may also be desirable, for example, to perform titrations at a range of cell concentrations for binding to oligomerizing systems. Characterization of binding to a polyion at low salt concentration may require a reduced concentration. Thus, strategies for handling relatively low signal-to-noise situations are helpful in many situations. The most basic of these involve inspection and, where necessary, manual editing of the power baseline to mitigate the occasion excursion due to instrumental noise. To this end, an increase in the time between injection may be indicated to unambiguously identify the restoration of baseline. In addition, the residual heats (which may be up to 10 µJ) after the equivalence point are unlikely to be negligible. Subtraction with data from a titrant-to-blank run would likely introduce more noise into the data and be no more helpful than taking a simple average of the final post-equivalence heats. If the data is to be fitted to models, a more appropriate solution is to add a constant parameter *B* to the fitting equation:

$$\frac{dq\_{\text{closed}}}{d[\mathbf{X}]\_{\text{h}}} = V \sum\_{i=1}^{n} \Delta H\_{i} \frac{d[\mathbf{X}\_{i}]\_{\text{s}}}{d[\mathbf{X}]\_{\text{h}}} + B \,. \tag{17}$$

### **3.1.2 Continuous ITC titrations**

While incremental titrations most commonly performed in ITC, an alternative mode of operation is a continuous titration (cITC) (Markova and Hallén 2004). In cITC, the titrant is continuously into injected the cell at a low rate (~0.1 µL/s). The primary advantage of cITC is throughput. An incremental ITC experiment typically requiring 20 injections of 5 µL at intervals of 300 s takes (neglecting time for baseline stabilization) 100 min; at 0.1 µL/s, cITC would require approximately 17 min. Another potential motivation for cITC is increased resolution in terms of model-dependent analysis. In incremental ITC, peak-by-peak

integration of thermal power is performed to obtain <sup>t</sup> [X] *dq <sup>d</sup>* . This step reduces the number of

collected data points (typically 1 s-1 over 103 s, or about one to two hours) for nonlinear regression to the number of injections (usually 10 to 30). By using the thermal power data directly for fitting, cITC can in principle discriminate the curvature required to define tight binding.

Maintenance of quasi-equilibrium conditions throughout the titration is essential to correct interpretation of derived thermodynamic parameters and is a major concern for cITC. To this end, the stirring rate in cITC must be considerably increased (up to 700 rpm) relative to incremental ITC to facilitate mixing of titrant into the titrate solution. Additionally, the

Probing Solution Thermodynamics by Microcalorimetry 883

where *r* = *K*/[X]t and = [X]t/[Y]t. Eq (21) is sometimes referred to as the Wiseman isotherm (Wiseman et al. 1989). As complexity of the model increases, however, the algebra involved rapidly becomes prohibitive. In any case, numerical methods provide the means

Given the usual practice of formulating models in terms of total or unbound concentrations, rather than their derivatives, conventional ITC data analysis has handled the differential nature of calorimetric data by fitting to a finite-difference version of Eq (13). Thus, for the *j*-

*j jj j* <sup>1</sup> *qqq q*

where *q*j is a volume-correction factor. This approach has the apparent advantage that models which have been formulated in terms of [X]b vs. [X]t can be used directly. However, Eq (22) represents poor practice in nonlinear regression. Since each computation of *qj* requires evaluation of *q* corresponding to two consecutive injections, *j* and *j*-1, the data points (and their errors, albeit small) are not independent. Independence of observations constitutes a major assumption of nonlinear regression, one which the recursive form of Eq (22) clearly violates. Specifically, the residual in *q*j during fitting becomes increasing correlated with increasing *j*. In addition, the resultant propagation of error likely violates the assumption of homoscedasticity (uniform variance) as well. Unless specialized regression techniques are employed (such as correlated least-squares), violations of these assumptions potentially calls the errors of the parameters, and possibly the parameters themselves, into

From the perspective of numerical analysis, Eq (22) is also entirely unnecessary. As stated previously, the most appropriate approach to handling ITC data is to fit Eq (13) directly.

classic initial value problems (IVPs). IVPs are first-order ordinary differential equations (ODEs) with a specific initial condition ([X]b = 0 at [X]t = 0) for which numerical methods for their solution are well-established. In addition avoiding the statistical pitfalls of Eq (22), formulating ITC models as differential equations simplify the algebra considerably. This is because implicit differentiation offers a welcome shortcut that obviates the need for an

b b

*d d <sup>K</sup> d d <sup>d</sup> <sup>K</sup>*

t t

Recognizing that [X]t, [Y]t are constants (and *K* being the parameter to be estimated), Eq (23) takes on a noticeable simpler (but equivalent) form compared to the Wiseman isotherm, Eq (21). More importantly, implicit differentiation always yields an explicit ODE even when no

[X] (2[X] [Y] [X] ) [X] [Y] [X]

btt bt

*d*

b b t t btt

*d K*

[X] [X] [Y] [X] 2[X] [Y] [X]

Posed in the form of Eq (13), ITC models (more specifically, the solution of b

explicit solution for [X]b. This is illustrated for X + Y XY with Eq (20):

[X] [X] [Y] ([Y] [X] ) [X] 2[X] 0 [X] [X]

t tt b b

b

t

*d*

, (22)

t [X] [X] *d*

*<sup>d</sup>* ) represent

. (23)

for generating solutions for Eq (13).

th injection:

question.

**3.2.1 Numerical aspects of ITC data analysis** 

instrument must be able to provide sufficient thermal compensation during the titration to maintain isothermal conditions. Finally, the kinetics of the interaction of interest must be fast relative to the injection rate. Generally speaking, these criteria are most likely met by relatively high-affinity interactions with moderate binding enthalpies.

### **3.2 Analysis of ITC data**

The direct measurement of *H* is considered a significant advantage over non-calorimetric binding methods since the latter access the binding thermodynamics indirectly in terms of the equilibrium constant *K* via the van't Hoff equation:

$$\frac{d\ln K}{d(1/T)} = -\frac{\Delta H\_{\text{vH}}}{R} \,. \tag{18}$$

Estimation of *C*p by non-calorimetric methods, therefore, involves taking a second derivative of the measured data. Another potential source of difficulty is the interpretation of *K*, which is model-dependent. As in DSC, however, ITC becomes a considerably more useful analytical technique when model fitting is used for parameter estimation and hypothesis testing. Moreover, agreement between the directly-fitted, calorimetric *H* and the van't Hoff *H*vH obtained from Eq (18) is a strong indication of the physical correctness of the model at hand.

The most fundamental concept in the analysis of ITC data is the differential nature of the heat signal with respect to titrant concentration (Figure 3). Recalling Eq (13),

$$\frac{dq}{d[\![\mathbf{X}]\!]\_\iota} = V \sum\_{i=1}^\iota \Delta H\_i \frac{d[\mathbf{X}\_i]\_\iota}{d[\mathbf{X}]\_\iota} \cdot \iota$$

Integration of this fundamental equation gives the is the functional form of conventional binding models:

$$q(\left[\mathbf{X}\_{i}\right]\_{\flat}) = V \sum\_{i=1}^{n} \Delta H\_{i} [\mathbf{X}\_{i}]\_{\flat} (\left[\mathbf{X}\_{i}\right]\_{\flat}) \tag{19}$$

The ideal approach to fitting ITC data is to directly fit Eq (13) (Poon 2010). For simple models, it is possible to write analytical expressions for b t [X ] [X] *<sup>i</sup> d <sup>d</sup>* explicitly in terms of [X]t i.e.,

the functional form of Eq (19). Take, for example, simple 1:1 binding of X + Y XY:

$$\begin{aligned} \left[\mathbf{X}\right]\_{\mathbf{i}} \left[\mathbf{Y}\right]\_{\mathbf{i}} - \left(\mathbf{X}\right)\_{\mathbf{i}} + \left[\mathbf{Y}\right]\_{\mathbf{i}} + \mathbf{K} \left[\mathbf{X}\right]\_{\mathbf{i}} + \left[\mathbf{X}\right]\_{\mathbf{i}} \stackrel{\circ}{=} 0\\ \left[\mathbf{X}\right]\_{\mathbf{i}} = \frac{\left[\mathbf{X}\right]\_{\mathbf{i}} + \left[\mathbf{Y}\right]\_{\mathbf{i}} + \mathbf{K} - \sqrt{\left[\mathbf{X}\right]\_{\mathbf{i}} + \left[\mathbf{Y}\right]\_{\mathbf{i}} + \mathbf{K}\right)^{2} - 4\left[\mathbf{X}\right]\_{\mathbf{i}}\mathbf{Y}\mathbf{I}\_{\mathbf{i}}}}{2} \end{aligned} \tag{20}$$

where b [X][Y] [X][Y] [XY] [X] *K* is the equilibrium dissociation constant. Its derivative is

$$\frac{d[\mathbf{X}]\_{\mathbf{i}}}{d[\mathbf{X}]\_{\mathbf{i}}} = \frac{1}{2} + \frac{1 - \Phi - r}{2\sqrt{(\Phi + 1 + r)^2 - 4\Phi}},\tag{21}$$

instrument must be able to provide sufficient thermal compensation during the titration to maintain isothermal conditions. Finally, the kinetics of the interaction of interest must be fast relative to the injection rate. Generally speaking, these criteria are most likely met by

The direct measurement of *H* is considered a significant advantage over non-calorimetric binding methods since the latter access the binding thermodynamics indirectly in terms of

vH ln

Estimation of *C*p by non-calorimetric methods, therefore, involves taking a second derivative of the measured data. Another potential source of difficulty is the interpretation of *K*, which is model-dependent. As in DSC, however, ITC becomes a considerably more useful analytical technique when model fitting is used for parameter estimation and hypothesis testing. Moreover, agreement between the directly-fitted, calorimetric *H* and the van't Hoff *H*vH obtained from Eq (18) is a strong indication of the physical correctness

The most fundamental concept in the analysis of ITC data is the differential nature of the

1 t t

b b t 1 ([X ] ) [X ] ([X ] ) *n i ii i i q VH* 

The ideal approach to fitting ITC data is to directly fit Eq (13) (Poon 2010). For simple

the functional form of Eq (19). Take, for example, simple 1:1 binding of X + Y XY:

*K* is the equilibrium dissociation constant. Its derivative is

[X] 2 2( 1 ) 4 *d r d r*

2

b

[X] 1 1

b

t

.

[X] [X] *n*

Integration of this fundamental equation gives the is the functional form of conventional

*i dq <sup>d</sup> V H d d*

b

(19)

*<sup>d</sup>* explicitly in terms of [X]t i.e.,

2

, (20)

t [X ] [X] *<sup>i</sup> d*

[X] [Y] ([X] [Y] ) 4[X] [Y] [X] <sup>2</sup>

2

t t t t t t

, (21)

*K K*

[X ]

*i i*

heat signal with respect to titrant concentration (Figure 3). Recalling Eq (13),

models, it is possible to write analytical expressions for b

tt t t b b

b

[X][Y] [X][Y] [XY] [X]

[X] [Y] ([X] [Y] )[X] [X] 0

*K*

. (18)

*dK H dT R*

(1 / )

relatively high-affinity interactions with moderate binding enthalpies.

the equilibrium constant *K* via the van't Hoff equation:

**3.2 Analysis of ITC data** 

of the model at hand.

binding models:

where

where *r* = *K*/[X]t and = [X]t/[Y]t. Eq (21) is sometimes referred to as the Wiseman isotherm (Wiseman et al. 1989). As complexity of the model increases, however, the algebra involved rapidly becomes prohibitive. In any case, numerical methods provide the means for generating solutions for Eq (13).

## **3.2.1 Numerical aspects of ITC data analysis**

Given the usual practice of formulating models in terms of total or unbound concentrations, rather than their derivatives, conventional ITC data analysis has handled the differential nature of calorimetric data by fitting to a finite-difference version of Eq (13). Thus, for the *j*th injection:

$$
\Delta \boldsymbol{q}\_{j} = \boldsymbol{q}\_{j} - \boldsymbol{q}\_{j-1} - \delta \boldsymbol{q}\_{j} \,\tag{2}
$$

t

where *q*j is a volume-correction factor. This approach has the apparent advantage that models which have been formulated in terms of [X]b vs. [X]t can be used directly. However, Eq (22) represents poor practice in nonlinear regression. Since each computation of *qj* requires evaluation of *q* corresponding to two consecutive injections, *j* and *j*-1, the data points (and their errors, albeit small) are not independent. Independence of observations constitutes a major assumption of nonlinear regression, one which the recursive form of Eq (22) clearly violates. Specifically, the residual in *q*j during fitting becomes increasing correlated with increasing *j*. In addition, the resultant propagation of error likely violates the assumption of homoscedasticity (uniform variance) as well. Unless specialized regression techniques are employed (such as correlated least-squares), violations of these assumptions potentially calls the errors of the parameters, and possibly the parameters themselves, into question.

From the perspective of numerical analysis, Eq (22) is also entirely unnecessary. As stated previously, the most appropriate approach to handling ITC data is to fit Eq (13) directly.

Posed in the form of Eq (13), ITC models (more specifically, the solution of b [X] [X] *d <sup>d</sup>* ) represent

classic initial value problems (IVPs). IVPs are first-order ordinary differential equations (ODEs) with a specific initial condition ([X]b = 0 at [X]t = 0) for which numerical methods for their solution are well-established. In addition avoiding the statistical pitfalls of Eq (22), formulating ITC models as differential equations simplify the algebra considerably. This is because implicit differentiation offers a welcome shortcut that obviates the need for an explicit solution for [X]b. This is illustrated for X + Y XY with Eq (20):

$$\begin{aligned} \left[ \mathbf{Y} \right]\_{\mathbf{i}} - \left( \mathbf{[Y} \right)\_{\mathbf{i}} + \left[ \mathbf{X} \right]\_{\mathbf{i}} + K \right) \frac{d[\mathbf{X}]\_{\mathbf{i}}}{d[\mathbf{X}]\_{\mathbf{i}}} - \left[ \mathbf{X} \right]\_{\mathbf{i}} + 2 [\mathbf{X}]\_{\mathbf{i}} \frac{d[\mathbf{X}]\_{\mathbf{i}}}{d[\mathbf{X}]\_{\mathbf{i}}} = 0 \end{aligned}$$
 
$$\frac{d[\mathbf{X}]\_{\mathbf{i}}}{d[\mathbf{X}]\_{\mathbf{i}}} (2[\mathbf{X}]\_{\mathbf{i}} - [\mathbf{Y}]\_{\mathbf{i}} - [\mathbf{X}]\_{\mathbf{i}} - K) = [\mathbf{X}]\_{\mathbf{i}} - [\mathbf{Y}]\_{\mathbf{i}} \qquad . \tag{23}$$
 
$$\frac{d[\mathbf{X}]\_{\mathbf{i}}}{d[\mathbf{X}]\_{\mathbf{i}}} = \frac{[\mathbf{X}]\_{\mathbf{i}} - [\mathbf{Y}]\_{\mathbf{i}}}{2[\mathbf{X}]\_{\mathbf{i}} - [\mathbf{Y}]\_{\mathbf{i}} - [\mathbf{X}]\_{\mathbf{i}} - K}$$

Recognizing that [X]t, [Y]t are constants (and *K* being the parameter to be estimated), Eq (23) takes on a noticeable simpler (but equivalent) form compared to the Wiseman isotherm, Eq (21). More importantly, implicit differentiation always yields an explicit ODE even when no

Probing Solution Thermodynamics by Microcalorimetry 885

The observed heat is now the sum of the enthalpy of unbinding of X2 from Y and the

X Y X Y t 1 t 1 t 1 2

2t t 2 2t t 2 2t t

B

[X1 ] t x 10-6 M

Fig. 5. Titrant-titrate binding in the presence of a competitor. *A*, simulated 1:1 titrant-titrate binding in the absence of competitor. The parameters are *K*1 = 10-10 M, *H*1 = -10 kcal mol-1, and [*Y*]t = 10 µM. Data representing this level of affinity would be unfit for model-fitting; *K*1/[Y]t = 104. *B*, in the presence a competitor, X2, at 10 µM (*K*2 = 10-8 M, *H*2 = -5 kcal mol-1).

Explicit titration models are also amenable to formulating models for continuous ITC. In the case of cITC, thermal power *P* is directly used in model fitting, so Eq (19) needs to be

> b 1 1 ( ) [X ] ( ) [X ] ( ) *n n*

*i i dq t <sup>d</sup> d t P VH tV H dt dt dt*

*i i i*

. (28)

[X] [X ] [X ] *dq d d VH H d dd*

As shown in Figure 5, a judicious choice of competitor reduces the apparent affinity of the titrant to a range more amenable for regression. In this case, the initial condition for [X2Y] is *not* zero because the titrate is essentially pre-equilibrated with competitor before any titrant

> [X ] [Y] ([X ] [Y] ) 4[X ] [Y] [X Y] <sup>2</sup> *K K* .

Thus, the competitive model requires prior knowledge of both the concentration and affinity of the competitor. Since the competitor would therefore require its own characterization, a weak competitor is preferred, which means it would need to be present at significant concentrations (i.e., [Y]t *K*). Since binding of the titrate involves the unbinding of the competitor, the enthalpy of competitor unbinding may be substantially convoluted in the

has been injected. The initial value for numerical integration is supplied by Eq (20):

1 2

2

0 5 10 15 20

b

*i*

[X2Y] x 10


M

. (27)

[X Y] [X Y]

binding of X1 to Y:

2

observed heat as indicated by Eq (27).


*Inset*, titration of the competitor.

differentiated with respect to *time*:




1/V dq/d[X1]t, cal mol-1


0 5 10 15 20

analytical expression for [X]b exists *e.g.*, polynomials of order >4. Direct substitution of Eq (23) into Eq (13) directly yields the ODE needed to generate values for nonlinear regression. This approach of formulating explicit titration models for ITC has been demonstrated for many empirical models in common use, including the multi-site model, homotropic cooperativity, and two-state self-association (Poon 2010). To further illustrate the this approach, a competitive binding model will be examined. This is a method of measuring tight binding by ITC by adding a competitive species in the cell to reduce the apparent affinity (Sigurskjold 2000). The mechanism is an example of the general multi-site model involving two ligands competing for a single site (Wells 1992). The equilibrium distribution of bound titrate is a function of the affinities of the titrant X1 and competitor X2 for the titrate Y as well as the total concentrations of all three species. For the titrant-titrate complex, X1Y:

$$a\_{\diamond} + a\_{\diamond}[\mathcal{X}\_{\diamond}\mathcal{Y}] + a\_{\diamond}[\mathcal{X}\_{\diamond}\mathcal{Y}]^2 + a\_{\diamond}[\mathcal{X}\_{\diamond}\mathcal{Y}]^3 = 0 \,\,\,\,\,\tag{24}$$

where

$$\begin{aligned} a\_0 &= -K\_2[\mathbf{X}\_1]\_\iota^\mathbf{r}[\mathbf{Y}]\_\iota \\ a\_1 &= [\mathbf{X}\_1]\_\iota \{ K\_1(\mathbf{K}\_2 + [\mathbf{X}\_2]\_\iota - [\mathbf{Y}]\_\iota) + K\_2([\mathbf{X}\_1]\_\iota + 2[\mathbf{Y}]\_\iota) \} \\ a\_2 &= K\_1^2 - K\_2(2[\mathbf{X}\_1]\_\iota + [\mathbf{Y}]\_\iota) - K\_1(K\_2 - [\mathbf{X}\_1]\_\iota + [\mathbf{X}\_2]\_\iota - [\mathbf{Y}]\_\iota) \\ a\_3 &= K\_2 - K\_1 \end{aligned}$$

and *K*1 and *K*2 are the equilibrium dissociation constants of X1 and X2 for the titrate, respectively. The corresponding expression for the competitor-titrate complex, X2Y, can be obtained from symmetry arguments:

$$\left[b\_0 + b\_1[\mathbf{X}\_2\mathbf{Y}] + b\_2[\mathbf{X}\_2\mathbf{Y}]^2 + b\_3[\mathbf{X}\_2\mathbf{Y}]^3 = \mathbf{0}\right],\tag{25}$$

.

where

$$\begin{aligned} b\_0 &= -K\_1 [\mathbf{X}\_2]\_\mathbf{i}^\natural [\mathbf{Y}]\_\mathbf{i} \\ b\_1 &= [\mathbf{X}\_2]\_\mathbf{i} \{ K\_2 ([\mathbf{X}\_1]\_\mathbf{i} - [\mathbf{Y}]\_\mathbf{i}) + K\_1 (K\_2 + [\mathbf{X}\_2]\_\mathbf{i} + 2[\mathbf{Y}]\_\mathbf{i}) \} \\ b\_2 &= K\_2 (K\_2 - [\mathbf{X}\_1]\_\mathbf{i} + [\mathbf{X}\_2]\_\mathbf{i} + [\mathbf{Y}]\_\mathbf{i}) - K\_1 (K\_2 + 2[\mathbf{X}\_2]\_\mathbf{i} + [\mathbf{Y}]\_\mathbf{i}) \\ b\_3 &= K\_1 - K\_2 \end{aligned}$$

It is possible to solve the cubic equation in Eqs (24) and (25) explicitly, followed by differentiation of the solutions to obtain 1 1 t [X Y] [X ] *d d* and 2 1 t [X Y] [X ] *d d* as was done with the Wiseman isotherm. All of this is avoided, however, by implicit differentiation with respect to [X1]t which directly yields the required derivatives:

$$\begin{split} \frac{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]} &= \frac{-\left(\frac{da\_{2}}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]^{2} + \frac{da\_{1}}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}] + \frac{da\_{0}}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}\right)}{\Im a\_{3}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]^{2} + 2a\_{2}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}] + a\_{1}} \\ \frac{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]} &= \frac{-\left(\frac{db\_{2}}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]^{2} + \frac{db\_{1}}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}] + \frac{db\_{0}}{d[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]}\right)}{\Im b\_{3}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}]^{2} + 2b\_{2}[\mathbf{X}\_{\mathrm{i}}\mathbf{Y}] + b\_{1}} \end{split} \tag{26}$$

analytical expression for [X]b exists *e.g.*, polynomials of order >4. Direct substitution of Eq (23) into Eq (13) directly yields the ODE needed to generate values for nonlinear regression. This approach of formulating explicit titration models for ITC has been demonstrated for many empirical models in common use, including the multi-site model, homotropic cooperativity, and two-state self-association (Poon 2010). To further illustrate the this approach, a competitive binding model will be examined. This is a method of measuring tight binding by ITC by adding a competitive species in the cell to reduce the apparent affinity (Sigurskjold 2000). The mechanism is an example of the general multi-site model involving two ligands competing for a single site (Wells 1992). The equilibrium distribution of bound titrate is a function of the affinities of the titrant X1 and competitor X2 for the titrate Y as well as the total concentrations of all three species. For the titrant-titrate complex, X1Y:

> 2 0 2 1t t

*a KK K aKK K K*

[X ] [Y]

2 0 1 2t t

*b K K K b KK K K*

[X ] [Y]

2

*a K*

3 21

3 12

*bKK*

differentiation of the solutions to obtain 1

which directly yields the required derivatives:

*b K*

*aKK*

obtained from symmetry arguments:

1 1t 1 2 2t t 2 1t t

1 2t 2 1t t 1 2 2t t 2 2 2 1t 2t t 1 2 2t t

[X ] { ([X ] [Y] ) ( [X ] 2[Y] )}

It is possible to solve the cubic equation in Eqs (24) and (25) explicitly, followed by

1 t [X Y] [X ] *d d*

isotherm. All of this is avoided, however, by implicit differentiation with respect to [X1]t

[X Y] [X Y] [X Y] [X ] [X ] [X ]

[X Y] [X Y] [X Y] [X ] [X ] [X ]

[X ] 3 [X Y] 2 [X Y]

*d d dd d a aa*

*d d dd d b bb*

[X ] 3 [X Y] 2 [X Y]

( [X ] [X ] [Y] ) ( 2[X ] [Y] )

and 2

2 10 2 1 1 1 1 t 1 t 1 t 2 1 t 3 1 21 1

*da da da*

 

2 10 2 2 2 2 1 t 1 t 1 t 2 1 t 3 2 22 1

*db db db*

 

1 t [X Y] [X ] *d d*

2 1 2 1t t 1 2 1t 2t t

and *K*1 and *K*2 are the equilibrium dissociation constants of X1 and X2 for the titrate, respectively. The corresponding expression for the competitor-titrate complex, X2Y, can be

[X ] { ( [X ] [Y] ) ([X ] 2[Y] )}

where

where

2 3

(2[X ] [Y] ) ( [X ] [X ] [Y] )

2 3

0 12 22 32 *bb b b* [X Y] [X Y] [X Y] 0 , (25)

.

as was done with the Wiseman

. (26)

0 11 21 31 *aa a a* [X Y] [X Y] [X Y] 0 , (24)

The observed heat is now the sum of the enthalpy of unbinding of X2 from Y and the binding of X1 to Y:

$$\frac{dq}{d[\mathbf{X}]\_\iota} = V \left( \Delta H\_{\chi\_{\mathbf{Y}} \chi} \frac{d[\mathbf{X}\_\iota \mathbf{Y}]}{d[\mathbf{X}\_\iota]\_\iota} + \Delta H\_{\chi\_{\mathbf{Y}} \chi} \frac{d[\mathbf{X}\_\iota \mathbf{Y}]}{d[\mathbf{X}\_\iota]\_\iota} \right). \tag{27}$$

As shown in Figure 5, a judicious choice of competitor reduces the apparent affinity of the titrant to a range more amenable for regression. In this case, the initial condition for [X2Y] is *not* zero because the titrate is essentially pre-equilibrated with competitor before any titrant has been injected. The initial value for numerical integration is supplied by Eq (20):

$$\mathbb{E}\left[\mathbf{X}\_{\texttt{z}}\mathbf{Y}\right] = \frac{\left[\mathbf{X}\_{\texttt{z}}\right]\_{\texttt{i}} + \left[\mathbf{Y}\right]\_{\texttt{i}} + K\_{\texttt{z}} - \sqrt{\left(\left[\mathbf{X}\_{\texttt{z}}\right]\_{\texttt{i}} + \left[\mathbf{Y}\right]\_{\texttt{i}} + K\_{\texttt{z}}\right)^{2} - 4\left[\mathbf{X}\_{\texttt{z}}\right]\_{\texttt{i}}\left[\mathbf{Y}\right]\_{\texttt{i}}}{2} \dots$$

Thus, the competitive model requires prior knowledge of both the concentration and affinity of the competitor. Since the competitor would therefore require its own characterization, a weak competitor is preferred, which means it would need to be present at significant concentrations (i.e., [Y]t *K*). Since binding of the titrate involves the unbinding of the competitor, the enthalpy of competitor unbinding may be substantially convoluted in the observed heat as indicated by Eq (27).

Fig. 5. Titrant-titrate binding in the presence of a competitor. *A*, simulated 1:1 titrant-titrate binding in the absence of competitor. The parameters are *K*1 = 10-10 M, *H*1 = -10 kcal mol-1, and [*Y*]t = 10 µM. Data representing this level of affinity would be unfit for model-fitting; *K*1/[Y]t = 104. *B*, in the presence a competitor, X2, at 10 µM (*K*2 = 10-8 M, *H*2 = -5 kcal mol-1). *Inset*, titration of the competitor.

Explicit titration models are also amenable to formulating models for continuous ITC. In the case of cITC, thermal power *P* is directly used in model fitting, so Eq (19) needs to be differentiated with respect to *time*:

$$P = \frac{d\boldsymbol{q}(t)}{dt} = \frac{d}{dt}\left\{\boldsymbol{V}\sum\_{i=1}^{n}\Delta H\_{i}[\mathbf{X}\_{i}]\_{\mathbf{b}}(t)\right\} = \boldsymbol{V}\left[\sum\_{i=1}^{n}\Delta H\_{i}\frac{d[\mathbf{X}\_{i}]\_{\mathbf{b}}(t)}{dt}\right].\tag{28}$$

Probing Solution Thermodynamics by Microcalorimetry 887

t btt t t

The simultaneous equations (32) and (34) represent another formulation of the same model, except now [X] is the explicit dependent variable instead of [X]b. (The initial condition is [X] = 0 at [X]t = 0.) Of course, we have previously derived Eq (23) directly, so this approach is regressive for this simple model. However, The flexibility to use any dependent variable of [X]t is useful, for example, for models that are formulated in terms of the binding

Successful implementation of Eq (13) requires numerical procedures for solving IVPs. The explicit, closed-form ODEs encountered in most models are typically ratios of polynomials. These functions are generally amenable any of the standard Runge-Kutta methods, which are widely available. A fast CPU is helpful, but not required. To this end, the tolerance for iteration should not be unnecessarily stringent in relation to the concentrations used and the value of *K* expected. Generally, a value of 10-6 will suffice. Even average single-core CPUs will handle ODEs of practical complexity with reasonable dispatch. Any significant delay is almost always related to input/output issues and can be alleviated by suppressing intermediate output. Numerical failures, if they occur, usually does so when there are two or more very different scales of the independent variable on which the dependent variable is changing *e.g.*, extremely tight binding to one site in the multi-site model. One such example is competitive binding in the presence of a very strong competitor in Eq (27). These pathological scenarios are associated with "stiff" differential equations that require more specialized algorithms for numerical solution. Fortunately, these situations are unlikely to be encountered as they are usually incompatible with experimental data in the first place. Several technical software suites, such as Mathematica (Wolfram Research, Champaign, IL, USA), MATLAB (the MathWorks, Natick, MA USA), Maple (Maplesoft, Waterloo, Ontario, Canada), and IgorPro (WaveMetrics, OR, USA) which have built-in numerical ODE and least-square minimization capabilities, represent full-featured, integrated solutions. Alternatively, pre-compiled libraries containing optimized algorithms for numerical ODEs and least-square minimization are available commercially (the Numerical Algorithm Group Library; Numerical Algorithms Group [NAG], Oxford, UK) or free (GNU Scientific Library [GSL]) for most computing platforms. Functions from these libraries can be called under standard programming environments (*e.g.*, C/C++, FORTRAN) to perform the required procedures. Some commercial data analysis software such as Origin (Northampton, MA, USA) can interface with external libraries such as the NAG Library or GSL to perform numerical ODEs within their least-squares routines. If access to external libraries is not available, an adequate alternative is to code a numerical ODE algorithm (such as Runge-Kutta-Fehlberg) as part of the target function within the data fitting routines of the analysis program. "Cookbook" recipes for a variety of ODE solvers are straightforward and can be

The sample and reference cells are typically overfilled for both DSC and ITC. Overfilling maximizes heat transfer between the solution and the wall of the cell as air is a poor thermal conductor. In the case of ITC, overfilling also minimizes stray signal arising from mechanical agitation of the solution-air-cell interface caused by the stirring paddle.

(34)

b t

polynomial which is based on [L] (Schellman 1975; Freire et al. 2009). **3.2.1.2 Practical considerations in implementing explicit ITC models** 

found in most texts of numerical analysis (Press 2007).

**3.2.1.3 Volume correction** 

[X] [X] [X] [X] <sup>1</sup> [X] 2[X] [X] [Y] 2[X] [X] [Y] *d K d KK* 

Applying the chain rule and the relation syr inj tot [X ]*<sup>i</sup> c v <sup>V</sup>* , where *c*syr is the concentration of titrant in the syringe and *v*inj is the injection volume,

$$\frac{d[\mathbf{X}\_i]\_\mathbf{b}}{dt} = \frac{d[\mathbf{X}\_i]\_\mathbf{b}}{d[\mathbf{X}\_i]\_\mathbf{b}} \frac{d[\mathbf{X}\_i]\_\mathbf{b}}{dt} = \frac{d[\mathbf{X}\_i]\_\mathbf{b}}{d[\mathbf{X}\_i]\_\mathbf{b}} \left(\frac{c\_{\mathbf{y}\tau}}{V} \frac{dv\_{\text{inj}}}{dt}\right). \tag{29}$$

(The subscript "tot" has been used to denote total concentration to avoid ambiguity with the variable *t* for time.) Note that inj *dv dt* is the (constant) injection rate. Substituting into Eq (28) gives

$$P = c\_{\text{sym}} \frac{d\upsilon\_{\text{inj}}}{dt} \left[ \sum\_{i=1}^{n} \Delta H\_i \frac{d[\mathbf{X}\_i]\_{\text{b}}}{d[\mathbf{X}\_i]\_{\text{tot}}} \right]. \tag{30}$$

Thus explicit expressions of b tot [X ] [X ] *i i d d* can be directly used as in incremental ITC. At a

sufficiently low injection rate, Eq (30) has the potential of "flattening out" the titration by transforming it in the time domain. This feature, in addition to the higher density of data points available for regression, may allow cITC to characterize much tighter binding than is practicable with incremental ITC (Markova and Hallén 2004).

In the foregoing discussion, the need to correct for various displacement and dilution effects due to the injection process has not been considered. In the author's experience, this is best handled during preliminary data reduction, before nonlinear regression. This aspect will be discussed in Section 3.2.1.3.

#### **3.2.1.1 Choice of dependent variable**

Another benefit of formulating ITC models as explicit ODEs is the flexibility in the choice of dependent variable for implicit differentiation, as long as it is a function in [X]t. For the 1:1 binding model, formulation in terms of the unbound titrant X gives the (and simple) functional form of the familiar Langmuir isotherm:

$$\mathbb{I}\left[\mathbf{X}\right]\_{\mathbb{h}} = \frac{\left[\mathbf{X}\right]\left[\mathbf{Y}\right]\_{\mathbb{h}}}{\left[\mathbf{X}\right] + K}.\tag{31}$$

Applying the chain rule of calculus,

$$\frac{d[\mathbf{X}]\_\flat}{d[\mathbf{X}]\_\flat} = \frac{d[\mathbf{X}]\_\flat}{d[\mathbf{X}]} \frac{d[\mathbf{X}]}{d[\mathbf{X}]\_\flat} = \frac{[\mathbf{X}]\mathbf{X}}{([\mathbf{X}] + \mathbf{X})^2} \frac{d[\mathbf{X}]}{d[\mathbf{X}]\_\flat} \tag{32}$$

At the same time, using the equation of state [X] = [X]t - [X],

$$\frac{d[\mathbf{X}]}{d[\mathbf{X}]\_\star} = \frac{d([\mathbf{X}]\_\star - [\mathbf{X}]\_\star)}{d[\mathbf{X}]\_\star} = 1 - \frac{d[\mathbf{X}]\_\star}{d[\mathbf{X}]\_\star} \,. \tag{33}$$

Substituting the results from Eq (23) into Eq (33),

*c v*

*dt* is the (constant) injection rate. Substituting into Eq (28)

. (30)

*d* can be directly used as in incremental ITC. At a

*<sup>V</sup>* , where *c*syr is the concentration of

. (31)

. (32)

. (29)

tot [X ]*<sup>i</sup>*

b bto syr inj t b tot tot

[X ] [X ] *i ii i*

*i i d dd d c dv dt d dt d V dt* 

(The subscript "tot" has been used to denote total concentration to avoid ambiguity with the

*n*

sufficiently low injection rate, Eq (30) has the potential of "flattening out" the titration by transforming it in the time domain. This feature, in addition to the higher density of data points available for regression, may allow cITC to characterize much tighter binding than is

In the foregoing discussion, the need to correct for various displacement and dilution effects due to the injection process has not been considered. In the author's experience, this is best handled during preliminary data reduction, before nonlinear regression. This aspect will be

Another benefit of formulating ITC models as explicit ODEs is the flexibility in the choice of dependent variable for implicit differentiation, as long as it is a function in [X]t. For the 1:1 binding model, formulation in terms of the unbound titrant X gives the (and simple)

> b [X][Y] [X] [X] *<sup>K</sup>*

b b

At the same time, using the equation of state [X] = [X]t - [X],

Substituting the results from Eq (23) into Eq (33),

t

t b b

tt t [X] [X] [X] [X] [X] [X] [X] [X] ([X] ) [X] *d d d Kd d d d Kd*

tt t [X] ([X] [X] ) [X] <sup>1</sup> [X] [X] [X] *dd d dd d*

2

. (33)

*dv <sup>d</sup> Pc H dt d*

inj b

1 tot

*i i i*

[X ] [X ]

*i*

[X ] [X ] [X ] [X ]

syr

tot [X ] [X ] *i i*

*d*

practicable with incremental ITC (Markova and Hallén 2004).

Applying the chain rule and the relation syr inj

titrant in the syringe and *v*inj is the injection volume,

variable *t* for time.) Note that inj *dv*

Thus explicit expressions of b

discussed in Section 3.2.1.3.

**3.2.1.1 Choice of dependent variable** 

Applying the chain rule of calculus,

functional form of the familiar Langmuir isotherm:

gives

$$\frac{d[\mathbf{X}]}{d[\mathbf{X}]\_\circ} = 1 - \frac{[\mathbf{X}]\_\circ - [\mathbf{X}]\_\circ}{2[\mathbf{X}]\_\circ - [\mathbf{X}]\_\circ - [\mathbf{Y}]\_\circ - K} = \frac{[\mathbf{X}] + K}{2[\mathbf{X}] - [\mathbf{X}]\_\circ + [\mathbf{Y}]\_\circ + K} \tag{34}$$

The simultaneous equations (32) and (34) represent another formulation of the same model, except now [X] is the explicit dependent variable instead of [X]b. (The initial condition is [X] = 0 at [X]t = 0.) Of course, we have previously derived Eq (23) directly, so this approach is regressive for this simple model. However, The flexibility to use any dependent variable of [X]t is useful, for example, for models that are formulated in terms of the binding polynomial which is based on [L] (Schellman 1975; Freire et al. 2009).

### **3.2.1.2 Practical considerations in implementing explicit ITC models**

Successful implementation of Eq (13) requires numerical procedures for solving IVPs. The explicit, closed-form ODEs encountered in most models are typically ratios of polynomials. These functions are generally amenable any of the standard Runge-Kutta methods, which are widely available. A fast CPU is helpful, but not required. To this end, the tolerance for iteration should not be unnecessarily stringent in relation to the concentrations used and the value of *K* expected. Generally, a value of 10-6 will suffice. Even average single-core CPUs will handle ODEs of practical complexity with reasonable dispatch. Any significant delay is almost always related to input/output issues and can be alleviated by suppressing intermediate output. Numerical failures, if they occur, usually does so when there are two or more very different scales of the independent variable on which the dependent variable is changing *e.g.*, extremely tight binding to one site in the multi-site model. One such example is competitive binding in the presence of a very strong competitor in Eq (27). These pathological scenarios are associated with "stiff" differential equations that require more specialized algorithms for numerical solution. Fortunately, these situations are unlikely to be encountered as they are usually incompatible with experimental data in the first place.

Several technical software suites, such as Mathematica (Wolfram Research, Champaign, IL, USA), MATLAB (the MathWorks, Natick, MA USA), Maple (Maplesoft, Waterloo, Ontario, Canada), and IgorPro (WaveMetrics, OR, USA) which have built-in numerical ODE and least-square minimization capabilities, represent full-featured, integrated solutions. Alternatively, pre-compiled libraries containing optimized algorithms for numerical ODEs and least-square minimization are available commercially (the Numerical Algorithm Group Library; Numerical Algorithms Group [NAG], Oxford, UK) or free (GNU Scientific Library [GSL]) for most computing platforms. Functions from these libraries can be called under standard programming environments (*e.g.*, C/C++, FORTRAN) to perform the required procedures. Some commercial data analysis software such as Origin (Northampton, MA, USA) can interface with external libraries such as the NAG Library or GSL to perform numerical ODEs within their least-squares routines. If access to external libraries is not available, an adequate alternative is to code a numerical ODE algorithm (such as Runge-Kutta-Fehlberg) as part of the target function within the data fitting routines of the analysis program. "Cookbook" recipes for a variety of ODE solvers are straightforward and can be found in most texts of numerical analysis (Press 2007).

#### **3.2.1.3 Volume correction**

The sample and reference cells are typically overfilled for both DSC and ITC. Overfilling maximizes heat transfer between the solution and the wall of the cell as air is a poor thermal conductor. In the case of ITC, overfilling also minimizes stray signal arising from mechanical agitation of the solution-air-cell interface caused by the stirring paddle.

Probing Solution Thermodynamics by Microcalorimetry 889

Unfortunately, the "black-box" nature of commercial software has engendered unwarranted reliance by many users on the turnkey software accompanying their instruments, and an attendant tendency to fit data to models of questionable relevance to the actual chemistry. This chapter discusses several novel aspects and potential pitfalls in the experimental practice and analysis of both DSC and ITC. This information should enable users to tailor

Financial support by the College of Pharmacy at Washington State University is

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**5. Acknowledgement** 

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**6. References** 

However, the introduction of titrant into an overfilled ITC sample cell leads to displacement effects that need to be taken into account. Specifically, each injected volume of titrant simultaneously displaces an equal volume of titrate and any previously injected titrant out of the sample cell (into the access tube). The accounting for these displaced volumes and their effect on titrant and titrate concentration is made on the assumption that the displaced material is immediately and completely excluded from the titration. This implies that no mixing occurs between the injected and displaced materials at the time injection. The concentrations of the titrant X after the *i*-th injection in the cell is therefore

$$\begin{bmatrix} \mathbf{X} \end{bmatrix}\_{\iota\iota} = \frac{\upsilon\_{\text{in}}\mathfrak{C}\_{\text{sys}} + [\mathbf{X}]\_{\iota, i-1}(V - \upsilon\_{\text{in}})}{V}, \quad \begin{bmatrix} \mathbf{X} \end{bmatrix}\_{\iota\iota} = \mathbf{0} \tag{35}$$

where *V* is the cell volume and *v*inj is the injection volume. The corresponding concentrations of the titrate Y is

$$\left[\mathbf{Y}\right]\_{i,i} = \frac{\left[\mathbf{Y}\right]\_{i,i-1}\left(V - \upsilon\_{\text{inj}}\right)}{V}.\tag{36}$$

There are two ways to handle volume corrections. One is to incorporate Eqs (35) and (36) as additional terms in the fitting equation. In the author's experience (Poon 2010), it is more efficient instead to perform the volume corrections on the dataset at the outset, and simply treat [Y]t,*i* as an additional dependent variable in the least-square procedure.

#### **3.2.1.4 Error analysis in ITC**

Compared to other titrations, particularly in the biochemical laboratory, that requires extensive manual manipulation *e.g.*, electrophoretic mobility shift, filter binding, ITC instrumentation offers a greatly reduced level of statistical error in the measured data. Nonetheless, detailed theoretical and experimental studies of the nature and magnitude of statistical errors in ITC have offered insight into how instrumental errors can be minimized in fitted parameters. Although such studies have so far only focused on 1:1 binding, it has become clear that at least two régimes of instrumental errors exist (Tellinghuisen 2003; 2005b). Specifically, for titrations associated with relatively large heats (>300 µcal or "high*q*"), proportional errors in the injected volumes dominate, and the inclusion of statistical weights is indicated to optimize fitted parameters. For "low-*q*" titrations, which typify lowconcentration titrations needed for tight binding interactions, constant errors in thermal detection and compensation dominate, and unweighted fitting does not adversely affect parameter optimization. In either case, the optimal number of injections is considerably lower than the norm of 20 to 25 injections, especially if variable volume procedures are employed (Tellinghuisen 2005a). This approach could substantially reduce titration time and increase experimental throughput. It may be pointed out, however, that in some applications, sample-to-sample variation may be greater than any statistical error inherent in the analytical technique. In these cases, standard errors in parameters estimated from replicate experiments will be higher but more representative indicators of experimental uncertainty than the fitting error extracted from the variance-covariance matrix.

### **4. Conclusion**

Commercial development of microcalorimetry has greatly increased the accessibility of this technique for the thermodynamic characterization of chemical systems in solution. Unfortunately, the "black-box" nature of commercial software has engendered unwarranted reliance by many users on the turnkey software accompanying their instruments, and an attendant tendency to fit data to models of questionable relevance to the actual chemistry. This chapter discusses several novel aspects and potential pitfalls in the experimental practice and analysis of both DSC and ITC. This information should enable users to tailor their experiments and model-dependent analysis to the particular requirements.
