Mark the correct relationship between the boiling points of very dilute solutions of $BaCl_2$ $(t_1)$ and $KCl$ $(t_2)$,having the same molarity.

In an aqueous solution of $NaCl$,the mole fraction of the solvent is $0.9$. Then,the relative lowering in vapour pressure will be ......... $atm$.

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution,the change in freezing point of water $(\Delta T_f),$ when $0.01 \ mol$ of sodium sulphate is dissolved in $1 \ kg$ of water,is $(K_f = 1.86 \ K \ kg \ mol^{-1})$ (in $K$).

Van't Hoff factor of $BaCl_2$ in its aqueous solution will be: ($BaCl_2$ is $60 \%$ ionized in the solution)

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 $CuCl_2 = 134.1 \ g \ mol^{-1}]$

$17.4\% (W/V)$ of potassium sulphate $(mol. wt. = 174)$ is isotonic with $4\% (W/V)$ aqueous solution of $NaOH$. If $NaOH$ is $100\%$ ionised,the degree of ionisation of potassium sulphate is $.......... \%$.