THERMODYNAMIC STUDY ON THE TRANSFER OF THE TIN(II), LEAD(II) AND ALKALINE-EARTH-METAL IONS FROM WATER TO METHANOL, DIMETHYL-SULFOXIDE, ACETONITRILE, PYRIDINE AND N,N-DIMETHYLTHIOFORMAMIDE

The thermodynamic functions for the transfer reactions of the tin(II), lead(II) and alkaline-earth-metal ions from water to methanol, aceton itrile, dimethyl sulfoxide and pyridine, and of the tin(II) and lead(I I) ions to N,N-dimethylthioformamide, are reported. The Gibbs energies of transfer, Delta(t)G(-) have been calculated from the standard elec trode potentials of the Sn2+/Sn(s) and Pb2+/Pb(s) couples, which have been determined potentiometrically with the Ag(s)/Ag+ electrode as ref erence in the title solvents, and the Gibbs energies of transfer of th e silver ion. The Gibbs energies of transfer of the alkaline-earth-met al ions were calculated from electrode or halfwave potentials of the M (2+)/M(am) couples in the title solvents and the difference in standar d electrode potential between the M(2+)/M(am) and M(2+)/M(s) couples r eported in the literature. The enthalpies of transfer, Delta(t)H(e), h ave been obtained from calorimetrically determined enthalpies of solut ion of the anhydrous metal trifluoromethylsulfonates. The entropies of transfer, Delta(t)S(-), have been calculated from the experimentally determined Delta(t)G(-) and Delta(t)H(-) values. All measurements have been carried out at 25 degrees C. The extrathermodynamic tetraphenyla rsonium tetraphenylborate (TATB) assumption has been applied in order to calculate the contributions from the single ions. The tin(II)) and lead(II) ions are solvated more strongly in dimethyl sulfoxide and N,N -dimethylthioformamide than in water, while they are solvated more wea kly in methanol and acetonitrile. The small tin(II) ion is solvated mo re weakly and the larger lead(II) ion is solvated more strongly in pyr idine than in water. The alkaline-earth-metal ions are solvated more s trongly in dimethyl sulfoxide than in water, while methanol and the ni trogen donor solvents acetonitrile and pyridine solvate these ions mor e weakly than water. The enthalpies of transfer for these ions to the solvents studied are exothermic except for the tin(II), calcium and st rontium ions to acetonitrile. The entropies of transfer to all solvent s are markedly negative except for N,N-dimethylthioformamide where the T Delta(t)S(-) values are close to zero. The difference in solvation of an ion between two solvents is mainly dependent on the bonding char acter of the ion-solvate bonds and on the way in which the ion affects the solvent bulk.