Thermodynamics of aqueous bile salt solutions: Heat capacity,enthalpy and entropy of dilution

Heat capacity data at various temperatures and enthalpies of dilution at 25°C are reported for aqueous bile salt solutions. The apparent molal heat contents _L have been combined with osmotic and activity coefficients to obtain the excess molal entropies. Measurements of some of these properties have also been carried out with the anionic detergent sodium dodecylsulfate so that the bile salt micellization process may be compared with that of a classical detergent. The observed data have been interpreted in terms of the hydrophobic association properties of bile salts in aqueous solution.     

The enthalpy of dilution as a direct characteristic of the energy spectrum of intermolecular interaction in polymer solutions and gels

Calorimetric data on the concentration dependences of the enthalpy of dilution of polymer solutions are analyzed. The profiles of concentration dependences strongly depend on the nature of intermolecular interactions in polymer solutions and gels and on the specific features of their structure, including phase and relaxation states. Therefore, the concentration dependence of the enthalpy of dilution is treated as a spectral curve containing information on the energy state of the polymer solution and gel as a function of concentration. Theoretical models are considered that allow estimation of quantitative contributions from paired intermolecular and electrostatic interactions in solutions and contributions provided by the metastable state of a glassy polymer and by the presence of crystalline ordering.     

Excess enthalpy and entropy of aqueous tetramethylguanidinium methanesulfonate and trifluoromethanesulfonate solutions

Relative apparent molal heat contents, φ_L, are reported for the tetramethylguanidinium salts of methanesulfonic (MS) and trifluoromethanesulfonic (TFMS) acids. Relative partial molal heat contents, L?₂, are calculated and combined with previously reported activity coefficient data, to yield excess entropies. It is found that the values of L?₂ make the principal contribution to the excess entropies of Me₄GuMS solutions while the excess free energies, as calculated from activity coefficients, make the greatest contribution to the excess entropies of Me₄GuTFMS solutions.     

The effect of temperature on the enthalpy of dilution of polyelectrolyte solutions

The integral enthalpies of dilution of sodium dextran sulphate and sodium alginate have been measured at 15, 25 and 40°. The results are compared with the predictions of the line charge theory. The experimental values show a much greater decrease with temperature than the calculated values and this difference is attributed to a contribution from solute/solvent interactions.     

A macroscopic source of enthalpy—entropy compensation

The characteristics of enthalpy—entropy compensation seen in water can be reproduced by a simple model which considers only the thermal variation of the dielectric constant.     

A relationship between atomic correlation energy and Tsallis entropy

A new relationship between electron correlation energy and Tsallis entropy is presented. This relationship is a generalization of previous equations which correlate the atomic correlation energy and the Shannon entropy. The results, relatively to the atoms with atomic number 2 < Z < 29, put in evidence the crucial role of the p‐parameter in terms of representation of the long‐range interaction contribution in the correlation energy. Moreover, the p‐values, which reproduce the experimental values of the correlation energy, indicate that the atomic wave functions are more localized with respect to those calculated in the limit of p → 1. © 2007 Wiley Periodicals, Inc. Int J Quantum Chem, 2008     

Photon correlation spectroscopy of polymer solutions

A polynomial subdistribution method for analyzing the correlation profile in photon correlation spectroscopy of polymer solutions is described. This method generates a continuous distribution function from the measured photoelectron time-correlation function, which can be related to particle size or molecular weight distribution of solute. The method is tested using simulated data for unimodal and bimodal distributions and compared with cumulant and histogram methods, respectively. The polynomial subdistribution method has an advantage in that it not only generates a continuous distribution curve but also works well for bimodal distributions whose peaks are close together.     

Correlation between entropy and enthalpy factors during heterogeneous complex catalytic reactions

The correlation equations are discussed between entropy and enthalpy factors during complex heterogeneous catalytic reactions based on the dependence of the Gibbs energy on the surface coverage. The existence of the entropy heterogeneity in the adsorption layer leads to the correlations between S and H. In the cases where the increase of H is accompanied by an increase of S, i. e. when the entropy factors lead to a decrease of the interval of heterogeneity, the known thermodynamic compensation effect is observed.

---

, . S H. H S, , .

     

The enthalpy and entropy of activation for ethyl acetate saponification

The saponification of ethyl acetate was measured by conductimetry at different temperatures within a batch reactor. A new mathematical model for obtaining concentration profiles from conductivity was presented and used for reaction‐kinetics' determination. The Arrhenius parameters (A, E_a) showed good agreement with the previously published values. Basic transition‐state theory was used for obtaining the Gibbs energy (ΔG?), the enthalpy (ΔH?), and the entropy (ΔS?) of activation. The low enthalpy of activation and negative entropy of activation were consistent with a reaction pathway when forming a transition‐state complex. The suggested mechanism involves OH^?, acting as a general base for removing proton from one of the hydroxide hydrating water, placed directly between it and the ester. The nucleophile from the water then attacks at the electrophilic C of the ester, breaking the π bond, and creating a tetrahedral intermediate. © 2012 Wiley Periodicals, Inc. Int J Chem Kinet 44: 692–698, 2012 This article was published online on 24 January 2012. An error was subsequently identified. This notice is included in the online and print versions to indicate that both have been corrected on 16 July 2012.     

Application of scanning methods to distinguish between entropy and enthalpy driven phase transitions

All phase transitions can be divided into enthalpy and entropy driven. The driving forces of phase transitions in aqueous soft matter systems can be resolved by applying scanning methods. In this review three experimental methods — sorption calorimetry, differential scanning calorimetry and humidity scanning quartz crystal microbalance with dissipation monitoring are described. Advantages and disadvantages of the methods are discussed. The driving forces of phase transitions can be directly measured using sorption calorimetry or calculated using van der Waals differential equation using experimental data obtained by other methods. The results of experimental studies show that in surfactant and lipid systems the phase transitions to phases with higher curvature are driven by enthalpy, while phase transitions to phases with lower curvature are driven by entropy.     

Balance of enthalpy and entropy in depletion forces

Solutes added to solutions often dramatically impact molecular processes ranging from the suspension or precipitation of colloids to biomolecular associations and protein folding. Here we revisit the origins of the effective attractive interactions that emerge between and within macromolecules immersed in solutions containing cosolutes that are preferentially excluded from the macromolecular interfaces. Until recently, these depletion forces were considered to be entropic in nature, resulting primarily from the tendency to increase the space available to the cosolute. However, recent experimental evidence indicates the existence of additional, energetically-dominated mechanisms. In this review we follow the emerging characteristics of these different mechanisms. By compiling a set of available thermodynamic data for processes ranging from protein folding to protein–protein interactions, we show that excluded cosolutes can act through two distinct mechanisms that correlate to a large extent with their molecular properties. For many polymers at low to moderate concentrations the steric interactions and molecular crowding effects dominate, and the mechanism is entropic. To contrast, for many small excluded solutes, such as naturally occurring osmolytes, the mechanism is dominated by favorable enthalpy, whereas the entropic contribution is typically unfavorable. We review the available models for these thermodynamic mechanisms, and comment on the need for new models that would be able to explain the full range of observed depletion forces.     

A relationship between atomic correlation energy of neutral atoms and generalized entropy

In a previous article, hereafter named as Paper I, we have showed a relationship between atomic correlation energy of neutral atoms with 2 < Z < 29 and Tsallis entropy. In this article, we generalize this relation showing the link between the atomic correlation energy and a general form of entropy obtained from deformed algebra. The results evidence the role of both q and Δ parameters of the general entropy, in terms of contribution of the long‐range interactions in the correlation energy. The q and Δ values, obtained as best fit of the atomic correlation energies 2 < Z < 29, indicate that this general form of entropy reduces to the Tsallis one, reproducing well the trend of the correlation energy for low Z. Moreover, as a consequence of these values of the parameters, the state atomic wave function is more localized with respect to the wave function calculated in the limit of Shannon entropy. © 2010 Wiley Periodicals, Inc. Int J Quantum Chem, 2011     

Equation for the interfacial tension between demixed polymer solutions

The theory of Cahn and Hilliard is used to derive an equation for the interfacial tension (free energy) between some demixed polymer solutions, applying a simple solution model treated by Debye in his theory of light scattering near the critical solution temperature. For a (symmetrical) system containing two polymers in a common solvent it is found that the interfacial tension is given by σ = (l/12^½)Ω_φp ²σ_r, where l is the Debye l parameter for the range of molecular interaction—here equal to (2S² )^½, where (S² )^½ is the radius of gyration of both polymers, Ω is a heat of mixing parameter for polymer-polymer interaction, φ_p is the total volume fraction of polymer and σ_r is a function of the ratio of temperature and critical solution temperature. The equation is in qualitative agreement with experiments of Langhammer and Nestler.     

Some aspects of the enthalpy of dilution of biological polyelectrolytes

It is shown that calorimetric experiments on the dilution process of polyelectrolytes, i.e. on the excess enthalpy of electrostatic origin, can give information on the conformational state of the polymer. Analytical expression are obtained relating the enthalpy of dilution to the charge density on the polymer, from Manning's theory. The experimental data reported on some ionic biopolymers are interpreted on the basis of the theoretical prediction of the electrostatic contribution to the enthalpy of dilution in water of a polyelecrolytic salt and of a weak polyacid. The procedure outlined provides a means of calculating the actual charge/per unit length and of disclosing possible non-electrostatic effects arising from conformational transitions.     

Heat capacity,enthalpy and entropy of calcium niobates

Heat capacity and enthalpy increments of calcium niobates CaNb₂O₆ and Ca₂Nb₂O₇ were measured by the relaxation time method (2–300 K), DSC (260–360 K) and drop calorimetry (669–1421 K). Temperature dependencies of the molar heat capacity in the form C _pm=200.4+0.03432T−3.450·10⁶/T ² J K⁻¹ mol⁻¹ for CaNb₂O₆ and C _pm=257.2+0.03621T−4.435·10⁶/T ² J K⁻¹ mol⁻¹ for Ca₂Nb₂O₇ were derived by the least-squares method from the experimental data. The molar entropies at 298.15 K, S _m⁰(CaNb₂O₆, 298.15 K)=167.3±0.9 J K⁻¹ mol⁻¹ and S _m⁰(Ca₂Nb₂O₇, 298.15 K)=212.4±1.2 J K⁻¹ mol⁻¹, were evaluated from the low temperature heat capacity measurements. Standard enthalpies of formation at 298.15 K were derived using published values of Gibbs energy of formation and presented heat capacity and entropy data: Δ_f H ⁰(CaNb₂O₆, 298.15 K)= −2664.52 kJ mol^t-1 and Δ_f H ⁰(Ca₂Nb₂O₇, 298.15 K)= −3346.91 kJ mol⁻¹.     

Hydration of dimethyldodecylamine-N-oxide: enthalpy and entropy driven processes

Dimethyldodecylamine-N-oxide (DDAO) has only one polar atom that is able to interact with water. Still, this surfactant shows very hydrophilic properties: in mixtures with water, it forms normal liquid crystalline phases and micelles. Moreover, there is data in the literature indicating that the hydration of this surfactant is driven by enthalpy while other studies show that hydration of surfactants and lipids typically is driven by entropy. Sorption calorimetry allows resolving enthalpic and entropic contributions to the free energy of hydration at constant temperature and thus directly determines the driving forces of hydration. The results of the present sorption calorimetric study show that the hydration of liquid crystalline phases of DDAO is driven by entropy, except for the hydration of the liquid crystalline lamellar phase which is co-driven by enthalpy. The exothermic heat effect of the hydration of the lamellar phase arises from formation of strong hydrogen bonds between DDAO and water. Another issue is the driving forces of the phase transitions caused by the hydration. The sorption calorimetric results show that the transitions from the lamellar to cubic and from the cubic to the hexagonal phase are driven by enthalpy. Transitions from solid phases to the liquid crystalline lamellar phase are entropically driven, while the formation of the monohydrate from the dry surfactant is driven by enthalpy. The driving forces of the transition from the hexagonal phase to the isotropic solution are close to zero. These sorption calorimetric results are in good agreement with the analysis of the binary phase diagram based on the van der Waals differential equation. The phase diagram of the DDAO-water system determined using DSC and sorption calorimetry is presented.     

Spectrochemistry of solutions,part 23. Changes of enthalpy and entropy in the formation of contact ion pairs: A vibrational spectroscopic appraisal using thiocyanate and azide solutions

Summary The vibrational spectra of solutions have been analyzed to assess both qualitatively and quantitatively the changes in enthalpy and entropy for ion pair formation in solutions of LiNCS, Mg(NCS)₂, and LiN₃ in liquid ammonia, dimethylformamide, dimethylsulphoxide and acetonitrile. Contrary to predictions both the H _ass and S _ass terms are all positive in the cases examined, indicating that the driving force in the ion association process derives from solvent-solute restructuring, and not the energy of the interaction between the cation and anion. This characteristic of contact ion pair formation is likely to be found to be applicable over a wide range of solvents. The following specific values of the thermodynamic parameters at 298 K have been obtained: LiNCS/DMF, G=–1.3 (1) kJ mol^–1, H _ass =+1.8 (5) kJ mol^–, S _ass =+10 (2) J mol^–1 K^–1; LiNCS/DMSO, G=+0.9 (2) kJ mol^–1, H _ass =+0.3 (3) kJ mol^–1; Mg(NCS)₂/DMF, G _ass =–4.0 (3) kJ mol^–1, H _ass =+15 (4) kJ mol^–1, S=+64 (17) kJ mol^–1; LiN₃/DMSO, G _ass =–2.5 (3) kJ mol^–1, H _ass =+4.9 (9) kJ mol^–1, S _ass =+25 (10) J K^–1 mol^–1.Submitted to celebrate the 70th Birthday of Professor Viktor Gutmann, and in recognition of his considerable contributions towards the better understanding of Chemistry in the Solution Phase