Calculate the molality of the solution containing a nonvolatile solute if the boiling point elevation of the solution is $0.39 \ K$.
[$K_{b}$ of water $= 0.52 \ K \ kg \ mol^{-1}$]

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.

If the boiling point of a urea solution is $100.18^{\circ}C$ and $K_b$ for water is $0.512 \ K \ kg \ mol^{-1}$,what is the molality of the solution? (Boiling point of water $= 100^{\circ}C$)

By studying the elevation in boiling point of an aqueous solution of glucose,the value of $K_b$ for water is found to be $0.51 \ K \ kg \ mol^{-1}$. What value of $K_b$ can be expected from an aqueous solution of $K_4[Fe(CN)_6]$?

Elevation in boiling point was $0.52 \, ^\circ C$ when $6 \, g$ of a compound $X$ was dissolved in $100 \, g$ of water. The molecular weight of $X$ is: ($K_b$ for water is $0.52 \, K \, kg \, mol^{-1}$)

$A$ solution containing $0.1050 \ g$ of a substance in $15.84 \ g$ of ether has a boiling point $1 \ ^\circ C$ higher than that of pure ether. What is the molar mass of the substance? [Given: Molar elevation constant for ether per $100 \ g = 21.6$]