Thermodynamic properties from conductance data are reported for solutions of Ph4PBr in 2-methoxyethanol-water binary solvent mixtures, at 19 temperatures in the range -10 to +80-degrees-C and for six mixtures in the composition range 0.1865 less-than-or-equal-to X1 less-than-or-equal-to 1. The experimental conductivity values were analysed by the Fuoss-Hsia equation, and the salt was found to be associated to some extent in these mixtures. The experimental dissociation constant (K) of the ion pair for this electrolyte has been used to test some empirical equations representing the functions K = K(T), K = K(X1) and K = K(T, X1).
Thermodynamic properties from conductance data are reported for solutions of Ph4PBr in 2-methoxyethanol-water binary solvent mixtures, at 19 temperatures in the range -10 to +80°C and for six mixtures in the composition range 0.1865 ≤ X1 ≤ 1. The experimental conductivity values were analysed by the Fuoss-Hsia equation, and the salt was found to be associated to some extent in these mixtures. The experimental dissociation constant (K) of the ion pair for this electrolyte has been used to test some empirical equations representing the functions K = K(T), K = K(X1) and K = K(T, X1).
Conductivity of tetraphenylphosphonium bromide in 2-methoxyethanol - water / F., Corradini; Franchini, Giancarlo; Marchetti, Andrea; M., Tagliazucchi; Tassi, Lorenzo; G., Tosi. - In: JOURNAL OF THE CHEMICAL SOCIETY. FARADAY TRANSACTIONS. - ISSN 0956-5000. - STAMPA. - 89:16(1993), pp. 3043-3047. [10.1039/FT9938903043]
Conductivity of tetraphenylphosphonium bromide in 2-methoxyethanol - water
FRANCHINI, Giancarlo;MARCHETTI, Andrea;TASSI, Lorenzo;
1993
Abstract
Thermodynamic properties from conductance data are reported for solutions of Ph4PBr in 2-methoxyethanol-water binary solvent mixtures, at 19 temperatures in the range -10 to +80°C and for six mixtures in the composition range 0.1865 ≤ X1 ≤ 1. The experimental conductivity values were analysed by the Fuoss-Hsia equation, and the salt was found to be associated to some extent in these mixtures. The experimental dissociation constant (K) of the ion pair for this electrolyte has been used to test some empirical equations representing the functions K = K(T), K = K(X1) and K = K(T, X1).
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