Abstract
The stability constants and thermodynamic values of complex formation of nonionic surfactants with alkali and alkaline-earth cations were determined by calorimetric titration in methanol. The purity of the ligands examined was checked by calorimetric end point titration. This method gives good results only if 1 : 1 complexes are formed. For the smallest ligands a ligand:cation ratio of x : 1 is found. In contrast the surfactant with the longest oligoethylene glycol chain forms 1 : x complexes. With increasing number of donor atoms the reaction enthalpies become more negative but the stability constants do not change very much due to compensating changes in entropies. Compared with the monocyclic ligand 18-crown-6 it is possible to obtain higher values of the reaction enthalpies and the high stability constants for crown complexes are caused mainly by favourable entropic factors.
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