Titration calorimetric determination of the pairwise interaction parameters of glycerol, D-threitol, mannitol, and D-glucitol in dilute aqueous solutions

Soldi, Luca; Marcus, Yizhak; Blandamer, Michael J.; Cullis, Paul M.

doi:10.1007/bf00979189

Cited by 11 publications

(4 citation statements)

References 15 publications

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“…Other authors report another equation for calculating the coefficients for alkanols up to pentan-1-ol and for hexane-m,ndiols and alditols : however, we veriÐed that it fails for longer hydroxylated substances. 23 In the present work, ethanol is chosen as cosolvent in order to study how a hydrophobic-structure maker substance inÑuences hydrophobic interactions in the aqueous solutions of alkane-1,2-diols and alkane-a,u-diols. In Figs.…”

Section: Discussionmentioning

confidence: 99%

Effect of a cosolvent on the hydrophobic interactions. A calorimetric study of alkane-m,n-diols in concentrated aqueous solutions of ethanol

Castronuovo¹,

Elia²,

Moniello³

et al. 1999

Phys. Chem. Chem. Phys.

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Calorimetric measurements were carried out at 298.15 K on concentrated aqueous solutions of ethanol, ranging from 0 to 9 m, containing alkane-m,n-diols from C-2 to C-9. The purpose of this study is to obtain more information about the influence of ethanol on hydrophobic hydration and interactions. The pairwise interaction coefficients of the virial expansion of the excess enthalpies were evaluated, and the results rationalized according to the preferential configuration model. The effect of ethanol depends on its concentration, on the alkyl chain length of the diol and on the OH positions. The hydrophilic interactions between the hydroxy groups determine the strength of hydrophobic interactions. The presence of the cosolvent ethanol, which lowers the relative permittivity of the medium, at first enhances the forcing action of hydrophilic interactions, making the hydrophobic interactions more cooperative. The enthalpic interaction coefficients are larger than those in water and reach a maximum at 2-3 m ethanol. Then, they decrease with the increasing structuring effect of the cosolvent on water. Evidences are given that, at low concentration of ethanol, the alkyl chains of the diols are preferentially hydrated. At higher concentration, instead, they are to some extent ethanolated. The results obtained are compared with those found for diols in concentrated solutions of urea: some comments are made on the possible mode of action of ethanol and urea as protein denaturants

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Section: Discussionmentioning

confidence: 99%

Effect of a cosolvent on the hydrophobic interactions. A calorimetric study of alkane-m,n-diols in concentrated aqueous solutions of ethanol

Castronuovo¹,

Elia²,

Moniello³

et al. 1999

Phys. Chem. Chem. Phys.

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“…This pattern is not surprising in that the same titration calorimeter can be used to probe soluteÈsolute interactions for simple neutral solutes in dilute aqueous solutions. 16 In general terms, the c.m.c. of ionic surfactants increase with a decrease in alkyl chain length.10 Consequently, in order that the concentration of surfactant in the simple cell changes from below to above the c.m.c.…”

Section: Type B Enthalpogramsmentioning

confidence: 99%

Classification of calorimetric titration plots for alkyltrimethylammonium and alkylpyridinium cationic surfactants in aqueous solutions

Bijma¹,

Engberts²,

Blandamer³

et al. 1997

Faraday Trans.

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Classification of calorimetric titration plots for alkyltrimethylammonium and alkylpyridinium cationic surfactants in aqueous solutions Bijma, K; Engberts, Jan; Blandamer, M.J; Cullis, P.M.; Last, P.M.; Irlam, K.D.; Soldi, L.G. Take-down policy If you believe that this document breaches copyright please contact us providing details, and we will remove access to the work immediately and investigate your claim. Calorimetric titration plots for deaggregation of micelles formed by alkylpyridinium and alkyltrimethylammonium surfactants are classiÐed into three types, A, B and C, depending on the shape of the plot of the enthalpy of dilution as a function of surfactant concentration. For Type A plots the recorded heat of injection q changes sharply between two parts of the titration curve over which the recorded heats are e †ectively independent of the composition of the solution in the sample cell. For Type B plots, the change is less sharp and both parts of the plot show dependences of heat q on solution composition, a pattern accounted for in terms of soluteÈsolute interactions. Type C plots are complicated, in that no sharp change in q is recorded, the complexity of the plots being accounted for in terms of micelleÈmonomer equilibria over a range of surfactant concentrations and related enthalpies of deaggregation.

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“…2. Partial dehydration of the hydration shell of the polylol, 18,19 which makes another positive contribution to h 2 .…”

Section: Resultsmentioning

confidence: 99%

Enthalpies of Dilution of (2S,3R,4R,5R)-Hexane-1,2,3,4,5,6-hexol in Water and Aqueous Sodium Halide Solutions at T = (293.15 to 318.15) K

et al. 2010

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The enthalpies of dilution of (2S,3R,4R,5R)-hexane-1,2,3,4,5,6-hexol in water and aqueous sodium halide solutions have been determined by isothermal flow-mix microcalorimetry at T = (293.15 to 318.15) K. Experiential equations of apparent enthalpies of dilution varying with the concentration of the polylol have been obtained from the experimental data in terms of the improved McMillan−Mayer theory. Enthalpic interaction coefficients, h 2, h 3, and h 4, pairwise entropic interaction coefficient s 2, and Gibbs free energy pairwise coefficient g 2 have been calculated. The values of pairwise enthalpic interaction coefficient, h 2, have been discussed in the light of solute−solute and solute−solvent interactions. The results indicate that the values of h 2 show quite well that the straight-line dependence on temperature and pairwise entropic interaction coefficient, s 2, is a constant in the experimental range of temperature.

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Titration calorimetric determination of the pairwise interaction parameters of glycerol, D-threitol, mannitol, and D-glucitol in dilute aqueous solutions

Cited by 11 publications

References 15 publications

Effect of a cosolvent on the hydrophobic interactions. A calorimetric study of alkane-m,n-diols in concentrated aqueous solutions of ethanol

Effect of a cosolvent on the hydrophobic interactions. A calorimetric study of alkane-m,n-diols in concentrated aqueous solutions of ethanol

Classification of calorimetric titration plots for alkyltrimethylammonium and alkylpyridinium cationic surfactants in aqueous solutions

Enthalpies of Dilution of (2S,3R,4R,5R)-Hexane-1,2,3,4,5,6-hexol in Water and Aqueous Sodium Halide Solutions at T = (293.15 to 318.15) K

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