Difference between Ideal Solution and Non-ideal Solution

Examples of ideal solutions include benzene and toluene, hexane and heptane. Examples of non-ideal solutions include ethanol and acetone, phenol and aniline, and chloroform and acetone.

Non-ideal solutions show positive or negative deviations from Raoult’s law because the intermolecular interactions between solute and solvent are either weaker (positive deviation) or stronger (negative deviation) than those between the pure components.

Yes, non-ideal solutions can form azeotropes, which are mixtures that boil at a constant temperature and retain the same composition in the vapor phase as in the liquid phase.

In ideal solutions, the total vapor pressure is the same as predicted by Raoult’s law. In non-ideal solutions, the total vapor pressure is either higher or lower than the value predicted by Raoult’s law.

A non-ideal solution is one that does not obey Raoult’s law. It may show positive or negative deviation from Raoult’s law, and the enthalpy and volume changes upon mixing are not zero.

An ideal solution is a solution where the intermolecular interactions between solute-solute (A-A) and solvent-solvent (B-B) are similar to the interaction between solute-solvent (A-B). It obeys Raoult’s law, has zero enthalpy and volume change upon mixing.