Abstract
The complex formation between nickel(II) and thioglycolic acid was studied by a potentiometric method at 25°C and in 0.5 M KN0 3. In solution two polynuclear complexes, B 3A 4 and B 4A 6, and one mononuclear complex, BA 2, were detected, and the following stability constants were determined: log β 3.4=32.219; log β 4.6=49.157; log β 1.2=12.759. The enthalpies of formation of the double (Ni-S-Ni) and single (Ni-S) bond were determined by calorimetric titration, and were found to be -5 kcal mol -1 and -1.5 kcal mol -1, respectively. It was shown that the stability of the polynuclear complexes is due to the enthalpy term, whereas the stability of the mononuclear complexes can be ascribed principally to the entropy term.
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