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.
Read more about this topic: Ideal Solution
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