1987
DOI: 10.1016/0040-6031(87)88345-4
|View full text |Cite
|
Sign up to set email alerts
|

Thermodynamics of electrolytic dissociation

Help me understand this report

Search citation statements

Order By: Relevance

Paper Sections

Select...
1
1

Citation Types

0
4
0

Year Published

1995
1995
2008
2008

Publication Types

Select...
5
2

Relationship

0
7

Authors

Journals

citations
Cited by 7 publications
(4 citation statements)
references
References 10 publications
0
4
0
Order By: Relevance
“…Thus the behavior of [Co(dien)(en)Cl] in acetone-water mixtures is not typical of halogenopentamminecobalt(III) ions where the solute-solvent interaction plays its important role. The situation for the aquation in aqueous ethanol is puzzling, the rate constant increases gradually with increasing mole fraction of ethanol, which is opposite to the normal trend for the spontaneous aquation of chloropentamminecobalt(III) [2,21] in that solvent. This behavior was previously observed for the aquation of some other octahedral complexes in aqueous ethanol [22,23] and in aqueous t-butyl alcohol [24] which could be due simply to differences in free energies of solvation of initial or transition states leading to great destabilization of the initial state relative to the transition state.…”
Section: Resultsmentioning
confidence: 96%
“…Thus the behavior of [Co(dien)(en)Cl] in acetone-water mixtures is not typical of halogenopentamminecobalt(III) ions where the solute-solvent interaction plays its important role. The situation for the aquation in aqueous ethanol is puzzling, the rate constant increases gradually with increasing mole fraction of ethanol, which is opposite to the normal trend for the spontaneous aquation of chloropentamminecobalt(III) [2,21] in that solvent. This behavior was previously observed for the aquation of some other octahedral complexes in aqueous ethanol [22,23] and in aqueous t-butyl alcohol [24] which could be due simply to differences in free energies of solvation of initial or transition states leading to great destabilization of the initial state relative to the transition state.…”
Section: Resultsmentioning
confidence: 96%
“…Acetic acid and benzoic acid and their alkali-metal salts have been of particular use as buffers for pH measurements in aqueous media as well as for pH*(s) measurements in mixed solvents (7). There have been extensive studies on the dissociation constants of acids and bases in various mixed and nonaqueous solvents (2)(3)(4)(5)(6)(7)(8)(9)(10)(11)(12)(13)(14)(15)(16). In this paper we determined the dissociation constants of the biologically important monocarboxylic acids acetic, benzoic, 3-phenylpropenoic, 2-methylpropionic, and pentanoic by potentiometric pH titrations in pure water and water + methanol, water + ethanol, water + dimethylformamide, water + dimethyl sulfoxide, and water + acetonitrile.…”
Section: Introductionmentioning
confidence: 99%
“…13,14 Dissociation constants have been determined for some dicarboxylic acids in an aqueous medium and in mixed solvents. [15][16][17][18][19][20][21] Acetonitrile (MeCN) is one of the most important dipolar aprotic solvents, it is used extensively as a reaction medium for mechanistic studies, in electrochemistry, and in HPLC and it is also employed as a solvent for non aqueous titrations. 22 MeCN behaves as a weaker base and as a much weaker acid and a small autoprotolysis constant (pKs MeCN acts as a strongly differentiating solvent with a modest solvating power for many polar ionic solutes.…”
mentioning
confidence: 99%