Conductance behavior of some potassium and tetraalkylammonium salts in sulfolane + water

Abstract

The conductance behavior of potassium plcrate, salicylate, bromide, and Iodide as well as tetraethylammonlum bromide and tetrabutylammonlum tetraphenylboride and Iodide has been studied at x = 0.20, 0.40, 0.60, and 0.80 (at 25 °C) and 1.0 (at 30 °C) for mixtures of x sulfolane + (1 -x) water. The conductance data are organized and treated on the basis of the Fuoss (1978) equation using the Fuoss computer program. Values of the limiting molar conductance (A,), association constant (AfA), and cosphere diameter (j?) are obtained as a result of the treatment. The limiting Ionic mobilities of the Individual Ions have been reported on the basis of tetrabutylammonlum tetraphenylboride reference electrolyte. The Walden product for each system Interestingly showed maxima and minima at different mole fractions of sulfolane studied.

Ionic Conductivity in Binary Solvent Mixtures. 2. Ethylene Carbonate + Water at 25 °C

“…The ionic mobility decreases with the increasing amount of ethylene carbonate in the mixture in all cases except the picrate ion, as expected because of the gradual increase in viscosity of the solvent at the ethylene carbonate rich region. The unusual behavior of the picrate ion has also been observed in propylene carbonate and propylene carbonate + ethylene carbonate mixtures (12) and also in sulfolane + water mixtures (11) earlier.…”

“…Conductivity Measurements. All conductivity measurements were made at (25 ( 0.05) °C using a dip-type cell (cell constant 1.073 cm -1 ) with a lightly platinized electrode, as described earlier (11). The conductivity meter was regularly standardized using standard potassium chloride solutions.…”

Ionic Conductivity in Binary Solvent Mixtures. 1. Propylene Carbonate (20 mass %) + Ethylene Carbonate at 25 .degree.C

“…Conductivity Measurements. All conductivity measurements were made at 25 ± 0.05 °C using a dip-type cell (cell constant 1.010 cm-1) with a lightly platinized electrode as described earlier (10). All molar conductivities reported here have been calculated after correcting for the solvent conductivity.…”