Thermodynamics of aqueous solutions of nonelectrolytes. I. Enthalpies of transfer of 1-methyl-2-pyrrolidinone from water to aqueous methanol

1974 ◽  
Vol 3 (1) ◽  
pp. 71-79 ◽  
Author(s):  
Sachio Murakami ◽  
Reiji Tanaka ◽  
Ryoichi Fujishiro
Keyword(s):  
Aqueous Solutions ◽  
Aqueous Methanol ◽  
Enthalpies Of Transfer

Interactions between cations and sugars. III. Free energies, enthalpies, and entropies of association of Ca2+, Sr2+, Ba2+, La3+, Gd3+ with D-ribose in water at 25 °C

1987 ◽  
Vol 65 (11) ◽  
pp. 2656-2660 ◽  
Author(s):  
Alfredo Maestre Alvarez ◽  
Nicole Morel-Desrosiers ◽  
Jean-Pierre Morel
Keyword(s):  
Thermodynamic Properties ◽  
Aqueous Solutions ◽  
Equilibrium Constant ◽  
The Other ◽  
Free Energies ◽  
Mean Values ◽  
Enthalpies Of Transfer ◽  
Other Hand ◽  
Solutions Of Electrolytes

The standard enthalpies of transfer of ribose and arabinose from water to aqueous solutions of electrolytes (CaCl2, SrCl2, BaCl2, LaCl3, and GdCl3) have been measured at 25 °C. A method is described to calculate from these data the equilibrium constant and the enthalpy for the association between the cations and the complexing isomers of ribose. Mean values relative to these isomers are given: the constants vary from 2.0 to 4.3 and the enthalpies from −5.9 to −17.9 kJ mol−1 for the different cations studied. The thermodynamic properties of association are not related to the size nor to the charge of the complexed cation in a simple way. On the other hand, the enthalpies of reaction are linearly correlated to the entropies of reaction.

Enthalpies of transfer of amino acids from water to aqueous solutions of formamide

2005 ◽  
Vol 432 (1) ◽  
pp. 20-22 ◽  
Author(s):  
Lin Ma ◽  
Nan Xu ◽  
Guimei Lin ◽  
Ruisen Lin
Keyword(s):  
Amino Acids ◽  
Aqueous Solutions ◽  
Enthalpies Of Transfer

Enthalpies of Transfer of Amino Acids from Water to Aqueous Solutions of Alkali Metal Nitrates

2005 ◽  
Vol 50 (6) ◽  
pp. 2094-2096 ◽  
Author(s):  
Chunli Liu ◽  
Ruisen Lin ◽  
Nan Xu
Keyword(s):  
Amino Acids ◽  
Alkali Metal ◽  
Aqueous Solutions ◽  
Enthalpies Of Transfer ◽  
Metal Nitrates

Enthalpies of transfer of Mebicarum from water to aqueous solutions of carbamide and its methyl-substituted derivatives at 298.15 K

2006 ◽  
Vol 80 (11) ◽  
pp. 1795-1798 ◽  
Author(s):  
V. K. Abrosimov ◽  
E. V. Ivanov ◽  
D. V. Batov
Keyword(s):  
Aqueous Solutions ◽  
Enthalpies Of Transfer

Solvation of Fluoride Ions. II. Enthalpies and Entropies of Transfer From Water to Aqueous Methanol

1988 ◽  
Vol 41 (12) ◽  
pp. 1971 ◽  
Author(s):  
GT Hefter ◽  
PJ Mclay
Keyword(s):  
Composition Range ◽  
Potassium Fluoride ◽  
Alkali Metal Ions ◽  
Halide Ions ◽  
Aqueous Methanol ◽  
Fluoride Ions ◽  
Solvent Interactions ◽  
Enthalpies Of Transfer ◽  
Complex Dependence ◽  
The Individual

Enthalpies of transfer of potassium fluoride from water to water-methanol mixtures over the whole composition range have been determined by calorimetry. Combination of these values with literature data has enabled calculation of the enthalpies and entropies of transfer for the individual ions through the tetraphenylarsonium tetrapbenylborate ( tatb ) assumption. The values of ΔtH°(F-) and ΔtS°(F-) show a complex dependence on solvent composition which closely parallels the dependence of the other halide ions. These effects are discussed in terms of ion-solvent and solvent-solvent interactions. The halide ions appear to be (weakly) preferentially solvated by H2O, and the alkali metal ions by MeOH.

Excess partial molar entropy of alkane-mono-ols in aqueous solutions at 25°C

2003 ◽  
Vol 81 (2) ◽  
pp. 150-155 ◽  
Author(s):  
Yoshikata Koga ◽  
Peter Westh ◽  
Keiko Nishikawa
Keyword(s):  
Aqueous Solutions ◽  
Key Words ◽  
Preceding Paper ◽  
Aqueous Methanol ◽  
Model Free ◽  
Chemical Potentials ◽  
Hydrophobic Nature ◽  
Mixing Schemes ◽  
Partial Molar Entropy ◽  
Partial Molar Enthalpies

In the preceding paper, we reported the values of model-free chemical potentials for aqueous methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, and 1-hexanol at 25°C over the entire compositional region. Using alcohol excess partial molar enthalpies, HEAL, determined earlier in this laboratory (Can. J. Chem. 74, 713 (1996)), we have calculated excess partial molar entropies for the alcohols, SEAL, where AL stands for an alcohol. We then calculated, numerically, the entropic interaction, SEAL–AL = N([Formula: see text]SEAL/[Formula: see text]nAL)p,T,nW, where nAL is the amount of AL, nW is the amount of H2O, and N is the total amount of solution. SEAL–AL signifies the effect of addition of AL upon the entropic situation of existing AL in solution. Using these quantities, the mixing schemes in aqueous alcohols have been studied. The earlier conclusions, which used HEAL and HEAL–AL alone, are confirmed. Furthermore, the order of the relative hydrophobic nature of alcohols is established from the behaviour of SEAL–AL and of HEAL–AL as methanol < ethanol < 2-propanol < 1-propanol. Key Words: aqueous alcohols, excess partial molar entropies, entropic interaction mixing schemes, hydrophobicity ranking.

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