Assuming $100\%$ dissociation of $1 \ m$ $KCl$ solution in water,the freezing point of the solution will be ........ $^oC$. $(K_f = 1.86 \ K \ kg \ mol^{-1})$

The elevation in boiling point of a solution of $13.44 \ g$ of $CuCl_2$ in $1 \ kg$ of water using the following information will be (Molecular weight of $CuCl_2 = 134.4 \ g \ mol^{-1}$ and $K_b = 0.52 \ K \ kg \ mol^{-1}$)

An aqueous solution of a salt $MX_2$ at a certain temperature has a van't Hoff factor of $2$. The degree of dissociation for this solution of the salt is

If the $O.P.$ (Osmotic Pressure) of $1 \ M$ solutions of the following compounds in water can be measured,which one will show the maximum $O.P.$?

If $13.44 \ g$ of $CuCl_2$ is dissolved in $1 \ kg$ of water,calculate the elevation in boiling point of the solution. $[K_b = 0.5 \ K \ kg \ mol^{-1}$,molar mass of $CuCl_2 = 134.1 \ g \ mol^{-1}]$

Consider the dissociation of the weak acid $HX$ as given below:
$HX_{(aq)} \rightleftharpoons H^{+}_{(aq)} + X^{-}_{(aq)}, K_{a} = 1.2 \times 10^{-5}$
$[K_{a}: \text{ dissociation constant}]$
The osmotic pressure of $0.03 \ M$ aqueous solution of $HX$ at $300 \ K$ is ............... $\times 10^{-2} \ bar$ (nearest integer).
$[\text{Given: } R = 0.083 \ L \ bar \ mol^{-1} \ K^{-1}]$