Ideal Solution - Consequences

Consequences

Solvent-Solute interactions are similar to solute-solute and solvent-solvent interactions

Since the enthalpy of mixing (solution) is zero, the change in Gibbs free energy on mixing is determined solely by the entropy of mixing. Hence the molar Gibbs free energy of mixing is

or for a two component solution

where m denotes molar i.e. change in Gibbs free energy per mole of solution, and is the mole fraction of component .

Note that this free energy of mixing is always negative (since each is positive and each must be negative) i.e. ideal solutions are always completely miscible.

The equation above can be expressed in terms of chemical potentials of the individual components

where is the change in chemical potential of on mixing.

If the chemical potential of pure liquid is denoted, then the chemical potential of in an ideal solution is

Any component of an ideal solution obeys Raoult's Law over the entire composition range:

where

is the equilibrium vapor pressure of the pure component
is the mole fraction of the component in solution

It can also be shown that volumes are strictly additive for ideal solutions.

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