Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.

(N/A) An ideal solution is one that obeys Raoult's law over the entire range of concentration. In an ideal solution,the solute-solute $(A-A)$ and solvent-solvent $(B-B)$ interactions are similar to the solute-solvent $(A-B)$ interactions. Consequently,the enthalpy of mixing $(\Delta_{mix}H = 0)$ and the volume of mixing $(\Delta_{mix}V = 0)$ are zero.
$A$ non-ideal solution is one that does not obey Raoult's law over the entire range of concentration. In these solutions,the solute-solvent $(A-B)$ interactions are either stronger or weaker than the solute-solute $(A-A)$ and solvent-solvent $(B-B)$ interactions. This leads to deviations from Raoult's law:
$1$. Positive deviation: $A-B$ interactions are weaker than $A-A$ and $B-B$ interactions,resulting in $\Delta_{mix}H > 0$ and $\Delta_{mix}V > 0$.
$2$. Negative deviation: $A-B$ interactions are stronger than $A-A$ and $B-B$ interactions,resulting in $\Delta_{mix}H < 0$ and $\Delta_{mix}V < 0$.