The temperature-dependent solubilities of several series of phenols in a 0.15 M sodium chloride solution have been measured. Experimentally determined heats of solution are compared with calculated values based on solubility principles. The solution process of all phenols is entropy-dominated and functional group contributions to the solubility are attributed mainly to their relative sizes and hydrophobicities. The correlation between experimental and calculated solubilities is excellent within a given series of phenols but not so good between different series. Correlations found between aqueous solubilities and partition coefficients of compounds can be explained in terms of the entropy change of the process in each case. © 1982.
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