The solute particles increase the intermolecular forces between solvent molecules.

The solute particles decrease the kinetic energy of the solvent molecules.

The solute particles occupy some surface area, reducing the solvent's ability to evaporate.

The solute particles react with the solvent molecules, reducing the amount of solvent available.

Unsaturated solution

Saturated solution

Supersaturated solution

Dilute solution

ΔH_mix = 0

ΔV_mix = 0

ΔG_mix < 0

ΔH_mix > 0

It obeys Raoult's law.

The enthalpy of mixing is zero.

The volume change on mixing is zero.

The interaction between unlike molecules is stronger than the interaction between like molecules.

Increases with increasing temperature

Decreases with increasing temperature

Is independent of temperature

Increases with increasing pressure and decreasing temperature

$ΔH_{mix} > 0$

$ΔV_{mix} > 0$

$ΔH_{mix} < 0$

A-B interactions are weaker than A-A and B-B interactions

Sugar in water

Salt in water

Brass

Air

It halves.

It remains the same.

It doubles.

It quadruples.

Solid solution

Liquid solution

Gaseous solution

Colloidal solution

The total vapour pressure of the solution is greater than the ideal vapour pressure.

The intermolecular forces between A-A and B-B are stronger than those between A-B.

The enthalpy of mixing ($\Delta H_{mix}$) is positive.

The volume of mixing ($\Delta V_{mix}$) is positive.

Moist air

Dry air

Au-Hg

${{\rm{C}}_2}{{\rm{H}}_5}{\rm{OH}} + {{\rm{H}}_2}{\rm{O}}$