Abstract
The standard enthalpies of solution (ΔH ? s of cholesterol and cholesteryl methyl ether in carbon tetrachloride and some basic solvents were measured by calorimetery. The obtained ΔH ? s values were used for the determination of the enthalpy of the hydrogen-bond complex formation between cholesterol and proton acceptors using the Arnett “pure base” method. The enthalpy of hydrogen-bond complex formation ranges from −10.4 (diethylcarbonate) to −24.6 kJ mol −1 (hexamethylphosphortriamide), being a linear function of the solvent basicity.
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