Molal elevation constant is the elevation in boiling point produced by

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.

For water,$K_b = 0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $200 \ mL$ of water,at what temperature will the resulting solution boil at $1 \ atm$ pressure (in $^oC$)?

$18 \ g$ of glucose,$C_6H_{12}O_6$,is dissolved in $1 \ kg$ of water in a saucepan. At what temperature will water boil at $1.013 \ bar$ (in $K$)? $K_b$ for water is $0.52 \ K \ kg \ mol^{-1}$.

The molal elevation constant is the ratio of the elevation in $B.P.$ to

$A$ solution of $6 \ g$ of solute in $100 \ g$ of water boils at $100.52^{\circ} C$. The molal elevation constant of water is $0.52 \ K \ kg \ mol^{-1}$. What is the molar mass of the solute?