Calculate the molal elevation constant $(K_b)$ of a solvent if the boiling point of a $0.12 \ m$ solution is $319.8 \ K$ (Boiling point of pure solvent = $319.5 \ K$).

The rise in the boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of a solvent is $0.1 \ ^\circ C$. The molal elevation constant of the liquid is .......... $K/m$.

Sea water contains $29.25\%$ $NaCl$ and $19\%$ $MgCl_2$ by weight of solution. The normal boiling point of the sea water is $..........{}^{\circ}C$ (Nearest integer).
Assume $100\%$ ionization for both $NaCl$ and $MgCl_2$.
Given: $K_b(H_2O) = 0.52 \, K \, kg \, mol^{-1}$.
Molar mass of $NaCl$ and $MgCl_2$ is $58.5$ and $95 \, g \, mol^{-1}$ respectively.

Calculate the molality of a solution containing a non-volatile solute if the boiling point elevation of the solution is $0.2 \ K$ $[K_{b} = 0.52 \ K \ kg \ mol^{-1}]$.

$13.44 \ g$ of $CuCl_2$ is dissolved in $1 \ kg$ of water. Determine the elevation in boiling point of the solution. [$K_b = 0.52 \ K \ kg \ mol^{-1}$,$mol \ wt$ of $CuCl_2 = 134.4$]

$Y \ g$ of non-volatile organic substance of molecular mass $M$ is dissolved in $250 \ g$ benzene. The molal elevation constant of benzene is $K_b$. The elevation in its boiling point is given by: