Because a solute increases the entropy of the liquid phase while the enthalpy is left unchanged,there is a decrease in the molar free energy of the solvent.

Question

Quizplus · Accepted Answer

Adding a solute to a solvent increases the disorder (entropy) of the system without significantly changing the enthalpy, leading to a decrease in the molar free energy of the solvent according to the Gibbs free energy equation, ΔG = ΔH - TΔS, where ΔG is the change in free energy, ΔH is the change in enthalpy, T is the temperature, and ΔS is the change in entropy.

Because a Solute Increases the Entropy of the Liquid Phase