The addition of a polar solvent to a solid electrolyte results in

If for a sucrose solution the elevation in boiling point is $0.1\,^{\circ}C$,then what will be the elevation in boiling point of a $NaCl$ solution for the same molal concentration? (in $^{\circ}C$)

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 $K_b = 0.52 \ K \ kg \ mol^{-1}$)

Of the following four aqueous solutions,the total number of those solutions whose freezing point is lower than that of $0.10 \, M \, C_{2}H_{5}OH$ is (Integer answer).
$(i)$ $0.10 \, M \, Ba_{3}(PO_{4})_{2}$
$(ii)$ $0.10 \, M \, Na_{2}SO_{4}$
$(iii)$ $0.10 \, M \, KCl$
$(iv)$ $0.10 \, M \, Li_{3}PO_{4}$

$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \%$ ionised. The freezing point of this solution is .......... $^oC$. ($K_f = 1.86 \, K \cdot kg \cdot mol^{-1}$ for water) :-

Which of the following equimolar aqueous solutions has the highest freezing point?