When $3 \ g$ of a non-volatile solute is dissolved in $200 \ mL$ of water, the boiling point of the solution becomes $100.52 \ ^oC$. If $K_b$ for water is $0.6 \ K \ kg \ mol^{-1}$, the molar mass of the solute is ......... $g \ mol^{-1}$.

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

The molal elevation constant of water is $0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar is dissolved in $200 \ g$ of water,at what temperature $(^oC)$ will the solution start to boil under $1 \ bar$ pressure?

Calculate the molar mass of a nonvolatile solute if a solution containing $0.35 \ g$ of solute in $100 \ g$ of water has a boiling point elevation of $0.01 \ K$ $\left[K_{b}=0.50 \ K \ kg \ mol^{-1}\right]$.

What is elevation in boiling point? Explain.

$A$ solution is prepared by dissolving a $2.5 \ g$ sample of an unknown compound in $34 \ g$ of benzene,$C_6H_6$. The solution boils at $1.38 \ ^\circ C$ higher than pure benzene. Which expression gives the molar mass of the unknown compound? $K_b$ of $C_6H_6$ is $2.53 \ ^\circ C \ m^{-1}$.