$0.01 \ M$ solutions of $KCl$ and $BaCl_2$ are prepared in water. The freezing point of $KCl$ is found to be $-2 \ ^oC$. What is the freezing point of $BaCl_2$ if it is completely ionised? ............. $^oC$

$19.5 \ g$ of $CH_2FCOOH$ is dissolved in $500 \ g$ of water. The depression in the freezing point of water observed is $1.0 \ ^\circ C$. Calculate the van't Hoff factor and dissociation constant of fluoroacetic acid.

Which one of the following is the ratio of the lowering of vapour pressure of $0.1 \ M$ aqueous solutions of $BaCl_2, NaCl$ and $Al_2(SO_4)_3$ respectively?

$0.8 \ mL$ of acetic acid of density $1.06 \ g \ mL^{-1}$ when dissolved in $1 \ kg$ of water causes a depression in freezing point by $0.0325^{\circ} C$. The Van't Hoff factor is:
$(K_{f} \text{ of } H_2O = 1.86 \ K \ kg \ mol^{-1})$

If a compound $AB$ dissociates to the extent of $75\,\%$ in an aqueous solution,the molality of the solution which shows a $2.5\, K$ rise in the boiling point of the solution is $......$ molal.
(Rounded-off to the nearest integer) $[K_{b} = 0.52\, K\, kg\, mol^{-1}]$

$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \% $ ionised. The freezing point of this solution is .............. $^o C$ (Given ${K_f} = 1.86 \, ^o C/m$ for water)