Abstract
The enthalpies of solution of ordinary (H 2O) and heavy (D 2O) water in dimethylsulphoxide (DMSO), N, N-dimethylformamide (DMF) and N, N-dimethylacetamide (DMA) have been measured using an isoperibol sealed calorimeter at 298.15 K. Standard (at infinite dilution) enthalpies of solution and solvation, together with D 2O–H 2O solute isotope effects on the quantities in question, were calculated. The enthalpies of solution of water H/D isotopologues have been found to be negative by sign and increasing in magnitude on going from DMF to DMSO and DMA. The corresponding positive solute isotope effects are very insignificant and slightly increase in a consequence: DMF < DMSO ≤ DMA. It has been concluded that the enthalpy-isotopic effects of water solvation are qualitatively connected with the donor-accepting and structure-packing properties of the aprotic dipolar solvents compared.
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