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

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.

Which of the following aqueous solutions will exhibit the highest boiling point?

The elevation in boiling point for a $0.1 \ m$ solution of a solute in $500 \ g$ of benzene is $0.51 \ K$. If $1000 \ g$ of a $0.1 \ m$ solution of the same solute in benzene is added to the above solution,the $\Delta T_b$ for the resulting solution will be ............... $K$.

If $0.15 \ g$ of a solute dissolved in $15 \ g$ of solvent is boiled at a temperature higher by $0.216 \ ^oC$ than that of the pure solvent,what is the molecular weight of the substance? (Given: molal elevation constant for the solvent is $2.16 \ ^oC \ kg \ mol^{-1}$)

Which of the following statements is correct for the boiling point of a solvent containing a dissolved solid substance?