Thermodynamic parameters (∆Hº, ∆Gº, ∆Sº) and the activation energy (∆Es) were calculated to explain the limiting equivalent conductance (Λ0) and ion association constant (KA) of s-acetylthiocholine halides and perchlorate in acetonitrile at different temperatures by using conductance measurements. It has been evaluated by using Fuoss-Onsager equation. It is evident that the values of (Λ0) increase regularly with increase in temperature. For all salts of s-acetylthiocholine, (Λ0) indicates less solvation or higher mobility of the ions in all solvent systems studied. The free energy change ∆Gº values are negative for all salts (Br -, Iand ClO4 -). Clearly strengthening to interionic association at higher temperatures is largely caused by a decrease in the permitivity of the solvent. The positive values of (∆Hº) for three salts (Br -, Iand ClO4 -) show that the association processes are endothermic in nature. Entropy change (∆Sº) values are positive for all salts indicate the randomness of ions in all solvent systems studied.

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The conductance data of sodium diethyldithiocarbamate (NaDDC) in methanol at different temperatures (25, 30, 35 and 40°C)

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