Pure HCl

Pure water

Pure water as well as HCl

Neither HCl nor $\;{{\rm{H}}_2}{\rm{O}}$ in their pure states

$\Delta H_{mix} > 0$ and $\Delta V_{mix} > 0$

$\Delta H_{mix} = 0$ and $\Delta V_{mix} = 0$

$\Delta H_{mix} < 0$ and $\Delta V_{mix} < 0$

$\Delta H_{mix} > 0$ and $\Delta V_{mix} < 0$

$0.1\;{\rm{M }}\;{\rm{BaC}}{{\rm{l}}_2}$

0.1 M glucose

$0.1\;{\rm{M }}\;{\rm{MgS}}{{\rm{O}}_4}$

Urea

120 torr

36 torr

88 torr

180 torr

252 mm Hg

336 mm Hg

408 mm Hg

504 mm Hg

Density

Osmotic Pressure

Mass

Volume

$\left( {{P_0} - {P_s}} \right)/{P_0} = {N_1}/\left( {{N_1} + {N_2}} \right)$

$\left( {{P_0} - {P_s}} \right)/{P_s} = {N_1}/{N_2}$

${P_s} = {P_0}.{N_2}/\left( {{N_1} + {N_2}} \right)$

All of the above

Relative lowering of vapour pressure is independent of the solute and the solvent.

The relative lowering of vapour pressure is a colligative property.

Vapour pressure of a solution is lower than the vapour pressure of the solvent.

The relative lowering of vapour pressure is directly proportional to the original pressure.

Volatile solute in a volatile solvent

Non-volatile solute in a volatile solvent

Volatile solute in a non-volatile solvent

Non-volatile solute in a non-volatile solvent

Positive deviations from ideal behaviour

Negative deviations from ideal behaviour

Positive deviations for lower concentrations and negative deviations for higher concentration

None of the above

Minimum boiling azeotrope

Maximum boiling azeotrope

Ideal solution

Supersaturated solution