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The solubility of 6-methylcoumarin in water, ethanol and nine aqueous ethanol mixtures was determined from 293.15 to 323.15 K. 6-Methylcoumarin solubility expressed in mole fraction was correlated with some well-known correlation/prediction models. Gibbs energy, enthalpy and entropy, for dissolution and mixing processes, were computed using van’t Hoff and Gibbs equations. The plot of enthalpy  vs . Gibbs energy of dissolution exhibited negative slopes from water to  w1  = 0.20 and from  w1  = 0.90 to ethanol but positive slopes in the interval 0.20 &lt;  w1  &lt; 0.90. 6-Methylcoumarin transfer from water to  w1  = 0.20 is entropy-driven that could be attributed to water molecules releasing originally bounded as ‘icebergs’ around the drug-non-polar groups. In mixtures of 0.20 &lt;  w1  &lt; 0.90, enthalpy-driving mechanism for drug transfer from more-polar to less-polar systems is observed, probably owing to better solvation by ethanol. Inverse Kirkwood–Buff integrals show that 6-methylcoumarin is preferentially solvated by water in water-rich mixtures but preferentially solvated by ethanol in 0.24 &lt;  x1  &lt; 1.00.

Equilibrium solubility of 6-methylcoumarin in some (ethanol + water) mixtures: determination, correlation, thermodynamics and preferential solvation