Single-ion Setschenow coefficients for several hydrophobic non-electrolytes in aqueous electrolyte solutions

1990 ◽  
Vol 68 (2) ◽  
pp. 243-246 ◽  
Author(s):  
P. Perez-Tejeda ◽  
A. Maestre ◽  
P. Delgado-Cobos ◽  
J. Burgess
Keyword(s):  
Aqueous Solutions ◽  
Alkali Halide ◽  
Aqueous Electrolyte ◽  
Electrolyte Solutions ◽  
Salt Solutions ◽  
Tetraalkylammonium Bromide ◽  
Chemical Potentials ◽  
Tetraalkylammonium Cations ◽  
Aqueous Salt Solutions ◽  
Tetraphenylarsonium Chloride

Setschenow coefficients have been derived from solubility measurements on cyclohexane, benzene, naphthalene, 1-naphthol, 1,5-dihydroxynaphthalene, and anthracene in alkali halide, tetraalkylammonium bromide, and tetraphenylarsonium chloride aqueous solutions at 298.2 K. Single ion Setschenow coefficients have thence been obtained by an assumption involving extrapolation of the tetraalkylammonium bromide results to zero cation volume. Setschenow coefficients for the tetraalkylammonium cations correlate well with a hydrophobicity parameter based on their transfer chemical potentials from water into 1,2-dichloroethane. Keywords: solubilities, aqueous salt solutions, Setschenow coefficients.

Hydrolysis in Some Aqueous Salt Solutions

1895 ◽  
Vol 20 ◽  
pp. 255-263
Author(s):  
James Walker
Keyword(s):  
Aqueous Solutions ◽  
Chemical Equilibrium ◽  
Free Acid ◽  
Free Base ◽  
Salt Solutions ◽  
Weak Acids ◽  
Organic Bases ◽  
Weak Bases ◽  
Aqueous Salt Solutions ◽  
Acid And Base

Some years ago, in an investigation on the affinity of organic bases, I was led to study the amount of decomposition suffered by various salts when dissolved in water, for a knowledge of this amount gives us a method of comparing the relative strengths of weak bases. When these bases are made to unite with a given acid, the extent to which the resulting salts are decomposed, in equivalent aqueous solutions, into acid and base, depends directly on the strength of the various bases. The same process of decomposition by water, or hydrolysis, can also be made use of to determine the strengths of weak acids, and experiments in this direction have been executed by Lellmann and his pupils, and by Shields. As the amount of free acid or free base in a hydrolysed solution cannot be determined directly by neutralisation, on account of the progressive disturbance of the chemical equilibrium involved in the process, it must be determined by taking advantage of some property of the acid or base which is susceptible of accurate measurement, and does not destroy the chemical equilibrium, or else does so in a manner amenable to calculation.

scholarly journals Negligible cation effect on the vibrational relaxation dynamics of water molecules in NaClO4 and LiClO4 aqueous electrolyte solutions

RSC Advances ◽  
2017 ◽  
Vol 7 (82) ◽  
pp. 52111-52117 ◽  
Author(s):  
Qianshun Wei ◽  
Dexia Zhou ◽  
Hongtao Bian
Keyword(s):  
Aqueous Solutions ◽  
Vibrational Relaxation ◽  
Aqueous Electrolyte ◽  
Electrolyte Solutions ◽  
Water Molecules ◽  
Relaxation Dynamics ◽  
Cation Effects ◽  
Aqueous Electrolyte Solutions ◽  
Cation Effect

Negligible cation effects on the vibrational relaxation dynamics of water molecules in NaClO4 and LiClO4 aqueous solutions.

scholarly journals Charge regulation of colloidal particles in aqueous solutions

2020 ◽  
Vol 22 (42) ◽  
pp. 24712-24728 ◽  
Author(s):  
Amin Bakhshandeh ◽  
Derek Frydel ◽  
Yan Levin
Keyword(s):  
Aqueous Solutions ◽  
Colloidal Particles ◽  
Aqueous Electrolyte ◽  
Electrolyte Solutions ◽  
Charge Regulation ◽  
Aqueous Electrolyte Solutions

We study the charge regulation of colloidal particles inside aqueous electrolyte solutions.

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.

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