Find the expected value of $\Delta T_{b}$ for $1 \ m \ AlCl_3$ solution in water if a solution of a nonelectrolyte of the same concentration has a $\Delta T_{b}$ value of '$x$' $K$.

Van't Hoff factor of $Hg_{2}Cl_{2}$ in its aqueous solution will be : ($Hg_{2}Cl_{2}$ is $80\%$ ionized in the solution) :- (in $.6$)

$A$ $0.1 \ mol$ of a binary electrolyte undergoes complete dissociation in $250 \ g$ of a protic solvent. If the elevation in boiling point is $1.5 \ K$,the molal elevation constant $(K_b)$ is ............. $K \ kg \ mol^{-1}$.

$0.6 \, mL$ 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.

For $0.01 \, M$ solutions of urea, common salt $(NaCl)$, and $Na_2SO_4$, the ratio of depression of freezing point is:

For a $0.1 \ M \ Ba(NO_3)_2$ solution, the van't Hoff factor is $2.74$. The degree of dissociation is .............