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Thermodynamic behavior of electrolytes in mixed solvents --II based on a symposium sponsored by the Division of Industrial and Engineering Chemistry at the 175th meeting of the American Chemical Society, Anaheim, California, March 13-16, 1978 by

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Published by ACS in Washington .
Written in English

Subjects:

  • Electrolytes -- Congresses.,
  • Solvents -- Congresses.

Book details:

Edition Notes

Including bibliographical references and index.

StatementWilliam F. Furter, editor.
SeriesAdvances in chemistry series ;, 177
ContributionsFurter, William F., American Chemical Society. Division of Industrial and Engineering Chemistry.
Classifications
LC ClassificationsQD1 .A355 no. 177, QD565 .A355 no. 177
The Physical Object
Paginationx, 400 p. :
Number of Pages400
ID Numbers
Open LibraryOL4406858M
ISBN 100841204284
LC Control Number79010009

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Thermodynamic behavior of electrolyte solutions. Part II. Prediction of vapor-liquid equilibria for mixed-solvent electrolyte systems. Fluid Phase Equilibria A predictive model for vapor-liquid equilibria of ternary systems, composed of two solvents and one electrolyte, is by: Thermodynamic behavior of electrolytes in mixed solvents --II: based on a symposium sponsored by the Di Thermodynamic behavior of electrolytes in mixed solvents: a symposium sponsored by the Division of Indu. Thermodynamics of electrolytes. II. Activity and osmotic coefficients for strong electrolytes with one or both ions univalent liquid-phase nonideality for aqueous and mixed-solvent electrolyte.   In solution thermodynamics, the quantity par excellence is the activity coefficient, which gives the non-ideal behavior of the solute species. Since electrolyte solutions obey the same thermodynamics, we shall give a brief review of solution thermodynamics.

of the thermodynamic behavior of aqueous electrolytes: II. The density and dielectric constant of H2 0 together with their par­ tial derivatives have been computed as functions of pressure and tem­ perature from to 5 kb and 25° to °C (Helgeson and Kirkham, la). The results of these calculations were used in the present studyFile Size: 2MB. Abstract. Molar excess volume V E and enthalpy H E data have been measured at 25°C for pyridine A saturated with anhydrous cupric chloride (S) [A(S)]+ B [where B is aniline or o-toluidine (OT) or formamide (FD) or N, N-dimethylformamide (NND)] mixtures on the assumption that while the standard state of B is that of pure components B, the standard state of A(S) is that of A Cited by: 4. Thermodynarnics of solubility in mixed solvent systems convenient choice is p = xi''), the solvent mole fraction of solvent component 2. The chemical potential of the salt in solvent i, with i = 1, 2 or 12, is: where R is the gas constant, T the thermodynamic temperature, v the sum of the stoichiometric coefficients v + and v of ions of the completely-ionized salt, p,O('), y s(i), in:) the.   Theoretical prediction of the thermodynamic behavior of aqueous electrolytes by high pressures and temperatures; IV, Calculation of activity coefficients, osmotic coefficients, and apparent molal and standard and relative partial molal properties to degrees C and 5kb.

Get this from a library! Thermodynamic behavior of electrolytes in mixed solvents --II: based on a symposium sponsored by the Division of Industrial and Engineering Chemistry at the th meeting of the American Chemical Society, Anaheim, California, March , [William F Furter; American Chemical Society. Division of Industrial and Engineering Chemistry.;]. Thermodynamic Characteristics of Solvents: A Review Mohd Shafique 1, Sayyed Hussain 2, But it is fairly soluble or extremely soluble in mixed solvent systems. Such behavior of organic compounds varies electrolytes in presence of ions such as salting out of soap andCited by: 3. A comprehensive thermodynamic framework for mixed-solvent electrolyte systems has been applied to the simultaneous computation of phase behavior and acid–base equilibria. Full text of "Electrolyte behavior in solvents of high dielectric constant" These mixed solvents have dielectric constants varying from 87 to at 35°C. Standard potentials obtained at nine different temperatures from 5 to 45°C were used to derive the mean ionic activity coefficients and the standard thermodynamic constants for the X2.