Abstract
The experimental data published for the cadmium-thiodipropionate system, which had been studied polarographically at the ionic strength of 1·2 and a temperature of 30 ± 1, 40 ± 1 and 50 ± 1°C, as well as the experimental data reported for the thallium-ethylthioglicolate system, studied also polarographically at the ionic strength of 2 and temperature of 20 and 30°C have been analyzed. As a result, for the above systems stability constants of the complexes formed have been found, which satisfy the following relation: β n=A· a n n! where β n is the overall stability constant of the complex ML n , n is the number of ligands in a given complex ( I ⩽ n ⩽ N), N is the coordination number of the complex forming metal M, A and a are constants. The free energy change, the enthalpy and entropy of the complex formation have been obtained. The values obtained for these quantities are in accordance with the thermodynamic considerations underlying the complex formation. This fact has been interpreted as an indication that the mathematical model developed in the first paper of this series can be regarded as a good approximation of the complex formation process.
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