If $1$ mole of a solute dissociates to give $n$ number of ions,then the degree of dissociation $\alpha$ in terms of the van't Hoff factor $i$ is given by:

Calculate the approximate $\Delta T_b$ (in $K$) for $0.001 \ m$ $KCl$ solution, if its van't-Hoff factor is $1.98$ [$K_b$ of water is $0.52 \ K \ kg \ mol^{-1}$].

$A$ solution of $CaCl_2$ is prepared by dissolving $0.0112 \ g$ of $CaCl_2$ in $1 \ kg$ of distilled water. If the molal freezing point depression constant $(K_f)$ of water is $2 \ K \ kg \ mol^{-1}$,what is the depression in the freezing point of the solution? (Assume $100\%$ ionization of $CaCl_2$)

$0.01 \ M$ 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? ............. $^oC$

The van't Hoff factor $(i)$ for the reaction of $HNO_3$ with $H_2SO_4$ is:

$1$ molal aqueous solution of an electrolyte $A_{2}B_{3}$ is $60\%$ ionised. The boiling point of the solution at $1 \ atm$ is ......... $K$.
(Rounded-off to the nearest integer)
[Given $K_{b}$ for $H_{2}O = 0.52 \ K \ kg \ mol^{-1}$]