Thermodynamic Properties of Ideal Solutions

In an ideal solution, each component’s standard state is its pure form at the same temperature and pressure, which serves as the reference for measuring changes in its thermodynamic properties upon mixing.

The chemical potentials of these components in the ideal solution can be compared to those of the pure substances in their standard states.

Mixing quantities of the ideal solution refers to the thermodynamic properties, like change in Gibbs free energy, volume, and enthalpy during mixing. It describes the changes that occur when two or more substances are mixed to form a solution.

As a measurable thermodynamic property, vapor pressure connects mixing behavior to phase equilibrium. It is the pressure exerted by the vapor phase of a substance when in equilibrium with its liquid phase.

In an ideal solution, vapor pressure is the sum of the partial pressures of the components in the solution.

Further, Raoult’s law states that the partial pressure of a component in the vapor phase is equal to the product of its mole fraction in the liquid phase and the vapor pressure of the pure component at the same temperature