Assertion:- Ideal solutions are one which obeys Raoult's law at all temperature and concentration.

Reason: -Very dilute solution can be treated as ideal solution.

Assertion: - In positive deviation of non-ideal solution attraction between solute solvent is less than the attraction between solute-solute and solvent-solvent.

Reason:-In negative deviation of non-ideal solution attraction between solute-solvent is more than the attraction between solute-solute and solvent-solvent.

Assertion:- Isotonic solutions don't show net phenomenon of osmosis.

Reason:- Isotonic solutions have equal osmotic pressure at constant temp.

Assertion:- When Benzoic acid is dissolved in benzene its vant Hoff factor is less than one.

Reason:- In benzene, benzoic acid has tendency to form dimer.

Assertion:- van't Hoff factor for benzoic acid in benzene is one.

Reason:- Benzoic acid behaves as a weaker electrolyte in benzene.

Assertion:- van't Hoff factor is always more or equal to one.

Reason:- van't Hoff factor is the ratio of experimental colligative properties to observed colligative properties.

Assertion:- Azeotropic mixture can not be separated by fractional distillation.

Reason:- Azeotropic mixtures are constant boiling mixtures.

Assertion:- ${\mathrm{\Delta H}}_{\mathrm{mix}}$and ${\mathrm{\Delta V}}_{\mathrm{mix}}$ for the preparation of ideal solution is zero.

Reason :- $\mathrm{A}-\mathrm{B}$ interactions in ideal solution are same as between $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$ in the two liquids before mixing.

Assertion:- $0.1 \mathrm{M}$ solution of $\mathrm{NaCl}$ have low freezing point than $0.1\mathrm{M}$ urea solution.

Reason:- Van't Hoff factor (No. of particles) for $\mathrm{NaCl}$ is more than urea.