Temperature coefficients of electrode potentials and Gibbs energies, entropies and enthalpies of transfer of Ag+, Na+ and Tl+ from N,N-dimethylformamide to its mixtures with N,N-dimethylthioformamide and with water

1993 ◽  
Vol 89 (12) ◽  
pp. 2007 ◽  
Author(s):  
Gerhard Gritzner ◽  
Andrzej Lewandowski
Keyword(s):  
Enthalpies Of Transfer ◽  
Temperature Coefficients ◽  
Gibbs Energies ◽  
Electrode Potentials

The Temperature Coefficients of Electrode Potentials

1959 ◽  
Vol 106 (7) ◽  
pp. 616 ◽  
Author(s):  
A. J. deBethune ◽  
T. S. Licht ◽  
N. Swendeman
Keyword(s):  
Temperature Coefficients ◽  
Electrode Potentials

Gibbs energies of transfer of individual ions from water to acetone + water solvents

1989 ◽  
Vol 67 (8) ◽  
pp. 1268-1273 ◽  
Author(s):  
Mahmoud Mohamad Elsemongy ◽  
Ahmed Ahmed Abdel-Khalek
Keyword(s):  
Glass Electrode ◽  
Aqueous Mixtures ◽  
Free Energies ◽  
Emf Measurements ◽  
Gibbs Energies ◽  
Electrode Potentials ◽  
Gibbs Energies Of Transfer ◽  
Acetone Water ◽  
Alkali Metal Halides ◽  
Dipolar Aprotic Solvents

The standard absolute potentials of hydrogen, Ag–AgX (X = Cl, Br, and I) and M/M+ (M = Li, Na, K, Rb, and Cs) electrodes in nine different acetone + water solvents containing up to 80 wt. % acetone were determined from the emf data at 25 °C of the cells: glass electrode/HCl (m), solvent/AgCl–Ag and glass electrode (M)/MX (m), solvent/AgX–Ag. The standard Gibbs free energies of a transfer of halogen acids and alkali metal halides as well as their constituent individual ions from water to the respective solvents were computed. The observed increases in [Formula: see text] values of all ions with increasing acetone content of the solvent and their relative order in each solvent were interpreted and discussed. A comparison of the present results with those obtained earlier in the dimethyl sulphoxide (DMSO) + water solvents shows the different nature of the two dipolar aprotic solvents, acetone and DMSO, in their aqueous mixtures. Keywords: acetone + water solvents, electrode potentials, emf measurements, individual ions, transfer free energies.

The distribution of branched octanols between dodecane and water

1985 ◽  
Vol 63 (4) ◽  
pp. 789-792 ◽  
Author(s):  
Norman H. Sagert ◽  
Danny W. P. Lau
Keyword(s):  
Thermodynamic Functions ◽  
Distribution Data ◽  
Standard Entropy ◽  
Standard Thermodynamic Functions ◽  
Enthalpies Of Transfer ◽  
Data Standard ◽  
Gibbs Energies ◽  
Gibbs Energies Of Transfer ◽  
Branched Chain ◽  
Entropy Of Transfer

The distribution of four branched chain octanols, 3-ethyl-3-hexanol, 4-ethyl-3-hexanol, 2-ethyl-4-methylpentanol, and 4-octanol, has been measured between dodecane and water. Measurements were made at alcohol concentrations in the dodecane of less than 0.1 mol/dm3, and as a function of temperature from 10 °C to 35 °C. From these distribution data, standard thermodynamic functions for transfer were calculated. Standard Gibbs energies of transfer from water to dodecane at 25 °C were in the range −14.1 to −15.1 kJ/mol, whereas the standard enthalpies of transfer at 25 °C varied from 29 to 39 kJ/mol. Thus, the change in the standard enthalpy tends to inhibit transfer, but a large standard entropy of transfer results in dodecane being the favoured phase.

Determination of Basicities of Organic Solvents and Absolute Electrode Potentials (E0-Values) of Monovalent Ions in Organic Solvents based on Absolute Values of Gibbs Energies of Solvation of Single Ions

2004 ◽  
Vol 218 (5) ◽  
pp. 515-550 ◽  
Author(s):  
Ranjana Bhattacharyya ◽  
S. C. Lahiri
Keyword(s):  
Organic Solvents ◽  
Gibbs Energies ◽  
Electrode Potentials ◽  
Induced Dipole ◽  
Single Scale ◽  
Monovalent Ions ◽  
Born Equation ◽  
The Absolute ◽  
Single Standard

AbstractSingle ion Gibbs energies of monovalent ions in fourteen solvents (water, methanol, NMF, PC, ethanol, n-propanol, iso-propanol, n-butanol, t-butanol, ethylene glycol, acetone, THF, 1,4-dioxan, acetonitrile) with or without (ion–dipole, ion–induced dipole, ion–quadrupole) interactions were determined. The basicity of the solvents was determined from the absolute values of ΔG0solvation(H+) or ΔG0solution(H+) based on single standard state utilising the modified Born equation suggested by Lahiri. The method involves no arbitrary assumptions. A single scale for the absolute electrode potentials (E0 values) has been determined based on calculated Gibbs energies of solvation or solution of single ions. Appropriation of Gibbs energies of solvation of electrolytes into single ion values is not possible. Gibbs energies of formation of electrolytes in solvents must be taken into consideration. Stabilisation energies of electrolytes (MX) in solvents akin to lattice energies in solids were determined.

scholarly journals Standard electrode potentials involving radicals in aqueous solution: inorganic radicals (IUPAC Technical Report)

2015 ◽  
Vol 87 (11-12) ◽  
pp. 1139-1150 ◽  
Author(s):  
David A. Armstrong ◽  
Robert E. Huie ◽  
Willem H. Koppenol ◽  
Sergei V. Lymar ◽  
Gábor Merényi ◽  
...  
Keyword(s):  
Aqueous Solution ◽  
Literature Review ◽  
Equilibrium Constants ◽  
Experimental Results ◽  
Gibbs Energies ◽  
Electrode Potentials ◽  
Technical Report ◽  
Standard Electrode Potentials ◽  
Best Estimates

AbstractRecommendations are made for standard potentials involving select inorganic radicals in aqueous solution at 25 °C. These recommendations are based on a critical and thorough literature review and also by performing derivations from various literature reports. The recommended data are summarized in tables of standard potentials, Gibbs energies of formation, radical pKa’s, and hemicolligation equilibrium constants. In all cases, current best estimates of the uncertainties are provided. An extensive set of Data Sheets is appended that provide original literature references, summarize the experimental results, and describe the decisions and procedures leading to each of the recommendations.

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