Abstract
The changes in the enthalpy of formation of complexes of nicotinamide with Ag+ ion at 25 ± 0.1°C and ionic strength of 0.25 (NaClO4) were obtained in the composition range of water-ethanol solvent from 0.1 to 0.9 mole fractions using precise calorimetry. We ascertained the stabilization of nicotinamide-silver(I) complexes in water-ethanol solvents and the maximum increase in exothermicity of the reaction in ethanol concentration range from 0 to 0.3 mole fractions. The enthalpy component of the change in the Gibbs energy of the complexation of Ag+ ions with NicNH2 was shown to dominate over the entropy component; the changes in thermodynamic argue for the prevailing contribution of the solvation state of a ligand to the exothermicity of complexation process at low ethanol concentrations.
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Original Russian Text © M.A. Zevakin, S.V. Dushina, V.A. Sharnin, 2010, published in Zhurnal Fizicheskoi Khimii, 2010, Vol. 84, No. 5, pp. 838–842.
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Zevakin, M.A., Dushina, S.V. & Sharnin, V.A. The thermochemistry of complexation of silver(I) with nicotinamide in water-ethanol solvents. Russ. J. Phys. Chem. 84, 741–744 (2010). https://doi.org/10.1134/S0036024410050055
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DOI: https://doi.org/10.1134/S0036024410050055