Degrees of Dissociation and Hydration Numbers of Twenty Six Strong Electrolytes in Aqueous Solutions at 25 °C

1992 ◽  
Vol 57 (11) ◽  
pp. 2209-2214 ◽  
Author(s):  
Rajalakshmi Heyrovská
Keyword(s):  
Activity Coefficient ◽  
Aqueous Solutions ◽  
Osmotic Coefficients ◽  
Hydration Numbers ◽  
Ionic Activity ◽  
Strong Electrolytes ◽  
The Mean ◽  
First Time ◽  
Degrees Of Dissociation

This paper brings further results on the degrees of dissociation (α) and hydration numbers (nh) of strong electrolytes in aqueous solutions at 25 °C, evaluated for the first time from osmotic coefficients (ϕ). Presented here are also the equations for the non-ideality parameters, ϕ and γ± (the mean molal ionic activity coefficient), in terms of α and nh.

Degrees of dissociation and hydration numbers of six tetra alkyl ammonium halides and nineteen 2:1 strong electrolytes in aqueous solutions at 25 °C

1989 ◽  
Vol 54 (5) ◽  
pp. 1227-1231 ◽  
Author(s):  
Rajalakshmi Heyrovská
Keyword(s):  
Aqueous Solutions ◽  
Osmotic Coefficient ◽  
Hydration Numbers ◽  
Nineteen 2 ◽  
Ionic Concentrations ◽  
Ammonium Halides ◽  
Strong Electrolytes ◽  
Alkyl Ammonium ◽  
First Time ◽  
Degrees Of Dissociation

The actual ionic concentrations and hydration numbers of some tetra alkyl ammonium halides and 2:1 strong electrolytes in aqueous solutions at 25 °C have been evaluated for the first time from the existing osmotic coefficient data.

Interpretation of properties of aqueous electrolyte solutions in terms of hydration and incomplete dissociation

1988 ◽  
Vol 53 (4) ◽  
pp. 686-696 ◽  
Author(s):  
Rajalakshmi Heyrovská
Keyword(s):  
Aqueous Solutions ◽  
Aqueous Electrolyte ◽  
Electrolyte Solutions ◽  
Hydration Numbers ◽  
Concentrated Aqueous Solutions ◽  
Strong Electrolytes ◽  
Strong Acids ◽  
Degrees Of Dissociation ◽  
Concentration Cells ◽  
Existing Data

The existing data on the vapour pressures, densities and e.m.f.s of concentration cells of dilute and concentrated aqueous solutions of strong electrolytes have been interpreted in terms of hydration and incomplete dissociation. Hydration numbers and degrees of dissociation have been presented for several 1 : 1 strong electrolytes at 25 °C. Thus the actual ionic concentrations of strong acids, bases and salts, hitherto inaccessible, have now been made available.

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.

Conductivity study of association of K2Mg[Fe(CN)6], K2Ca[Fe(CN)6] and K2Ba[Fe(CN)6] in aqueous solutions

1980 ◽  
Vol 45 (10) ◽  
pp. 2632-2636
Author(s):  
Alois Fidler ◽  
Jiří Čeleda
Keyword(s):  
Aqueous Solutions ◽  
Stability Constants ◽  
Infinite Dilution ◽  
Ion Pairs ◽  
Electrolyte Mixtures ◽  
Ionic Activity ◽  
Type K ◽  
Strong Electrolytes ◽  
The Stability ◽  
Two Parameter

The stability constants, Kp0, of ion pairs M2+.[Fe(CN)6]4- and their equivalent conductivities, λp0, at infinite dilution were evaluated by means of two-parameter fitting from the conductivities measured in very diluted aqueous solutions of double hexacyanoferrates of the type K2M(II).[Fe(CN)6] at 25 °C with the use of the limiting Debye-Huckel formula for ionic activity coefficients and Onsager limiting formula for the conductivity of strong electrolytes extended to electrolyte mixtures. Thus, Kp0 = 0.66, 0.72, and 0.76 . 104 dm3/mol and λp0 = 46, 49, and 53 S cm2 /val, respectively.

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