The Ionic Activity Coefficient Product and Ionization of Water in Uni-univalent Halide Solutions—A Numerical Summary

1937 ◽  
Vol 59 (11) ◽  
pp. 2304-2305 ◽  
Author(s):  
Herbert S. Harned ◽  
Melvin A. Cook
Keyword(s):  
Activity Coefficient ◽  
Ionic Activity ◽  
Ionization Of Water

Mixture Property: Mean Ionic Activity and Mean Ionic Activity Coefficient

2016 ◽  
Author(s):  
Michael Frenkel ◽  
Robert D. Chirico ◽  
Vladimir Diky ◽  
Paul L. Brown ◽  
John H. Dymond ◽  
...  
Keyword(s):  
Activity Coefficient ◽  
Ionic Activity

Dissociation Degree of HSO-4 and Mean Ionic Activity Coefficient of Aqueous Sulfuric Acid of Different Molalities up to 473 K and 975 bar

1994 ◽  
Vol 49 (10) ◽  
pp. 939-942
Author(s):  
B. A. Bilal ◽  
E. Müller
Keyword(s):  
Sulfuric Acid ◽  
Activity Coefficient ◽  
Thermodynamic Data ◽  
Formation Constant ◽  
Saturation Pressure ◽  
Ionic Activity ◽  
The Real ◽  
Aqueous Sulfuric Acid ◽  
Dissociation Degree

AbstractThe apparent formation constant and the dissociation degree of HSO-4 in aqueous H2SO4 of the molalities 0.1, 0.5, and 1.0 m, as well as the real mean ionic coefficient have been calculated up to 473 K and 975 bar using the thermodynamic data reported by Holmes and Mesmer at saturation pressure and those given by the authors at higher pressure.

Activity coefficients of potassium perrhenate in aqueous mixtures with KCl, NaCl and KI at 298.15 K

1975 ◽  
Vol 28 (3) ◽  
pp. 665 ◽  
Author(s):  
C Chan
Keyword(s):  
Activity Coefficient ◽  
Aqueous Solutions ◽  
Activity Coefficients ◽  
Aqueous Mixtures ◽  
Ionic Activity ◽  
Activity Product ◽  
Dilute Aqueous Solutions ◽  
Mean Ionic Activity Coefficients

The solubilities of potassium perrhenate in aqueous NaCl, KCl and KI solutions are reported. The solubility activity product for this electrolyte was determined using extrapolation functions involving three different mean ionic activity coefficient expressions. Mean ionic activity coefficients have been computed for potassium perrhenate in dilute aqueous solutions and there is no justification for considering ion association1,2 in these solutions.

Activity coefficient assumptions m the determination of the association constant of thallons chloride. II. Effect of interactions between freeions

1966 ◽  
Vol 19 (6) ◽  
pp. 915 ◽  
Author(s):  
JB Macaskill ◽  
MH Panckhurst
Keyword(s):  
Sodium Chloride ◽  
Activity Coefficient ◽  
Association Constant ◽  
Sodium Perchlorate ◽  
Barium Chloride ◽  
Specific Interactions ◽  
Ionic Activity ◽  
Caesium Chloride ◽  
Free Ions

The solubility of thallous chloride has been measured in solutions of hydrochloric acid, caesium chloride, caesium perchlorate, barium chloride, and in various mixtures of sodium chloride and sodium perchlorate. These measurements are analysed to give the association constant for thallous chloride, paying particular attention to ionic activity coefficient formulae. It is shown that an activity coefficient expression which assumes no specific interactions between free ions is unsatisfactory in contrast to an expression which assumes such interactions. The consequences of this are discussed.

THE IONIZATION BEHAVIOR OF AMIDES IN CONCENTRATED SULFURIC ACIDS: III. INDICATOR ACTIVITY COEFFICIENT VARIATION

1966 ◽  
Vol 44 (20) ◽  
pp. 2395-2404 ◽  
Author(s):  
Linda M. Sweeting ◽  
Keith Yates
Keyword(s):  
Sulfuric Acid ◽  
Activity Coefficient ◽  
Acid Concentration ◽  
Acidity Function ◽  
Total Acidity ◽  
Relative Importance ◽  
Ionic Activity ◽  
Tetraethylammonium Ion ◽  
Ionization Behavior ◽  
Substituted Benzamides

Activity coefficient data for ten substituted benzamides and two benzamide salts have been obtained from solubility measurements in 0–70% sulfuric acid. The ionic activity coefficients have been referred to a standard ion, the tetraethylammonium ion. The variations of activity coefficient with acid concentration are discussed and compared with available data for anilines and anilinium ions. Estimates have been made of the relative importance of the various terms contributing to the total acidity function for sulfuric acid. Up to 40% acid the order of importance of these terms is [Formula: see text] and in more concentrated acids becomes [Formula: see text].

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