$A$ $0.2 \ m$ solution of acid $HX$ is $20\%$ ionized in the solution. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the freezing point of the solution is ........... $^oC$.

The freezing point of a $2\%$ aqueous solution of $[Ag(CH_3NH_2)_2]Cl$ is:

Which one of the following $0.10 \ M$ aqueous solutions will exhibit the largest freezing point depression?

$0.6 \, mL$ of acetic acid $(CH_{3}COOH)$,having density $1.06 \, g \, mL^{-1}$,is dissolved in $1 \, L$ of water. The depression in freezing point observed for this strength of acid was $0.0205^{\circ} \, C$. Calculate the van't Hoff factor and the dissociation constant of acid.

Molal depression constant for a solvent is $4.0 \, K \, kg \, mol^{-1}$. The depression in the freezing point of the solvent for $0.03 \, mol \, kg^{-1}$ solution of $K_2SO_4$ is .............. $K$ (Assume complete dissociation of the electrolyte).

If the relative decrease in vapour pressure is $0.4$ for a solution containing $1 \, mol$ of $NaCl$ in $3 \, mol$ of $H_2O$,the degree of ionization of $NaCl$ is .......... $\%$.