$A$ solution containing $12.5 \ g$ of non-electrolyte substance in $250 \ g$ of water shows boiling point elevation of $0.52 \ K$. Calculate the molar mass of the substance. $(K_b = 0.52 \ K \ kg \ mol^{-1})$ ......... $g \ mol^{-1}$.

Calculate the molality of a solution of a nonvolatile solute having a boiling point elevation of $1.89 \ K$,if the boiling point elevation constant of the solvent is $3.15 \ K \ kg \ mol^{-1}$. (in $m$)

Which one of the following would produce maximum elevation in boiling point?

If the boiling point of a solution is $T_1$ and the boiling point of the pure solvent is $T_2$,then the elevation in boiling point is given by:

To observe an elevation of boiling point of $0.05^{\circ} C$, the amount of a solute (mol. wt. $= 100$) to be added to $100 \ g$ of water $(K_{b} = 0.5)$ is (in $g$)

Calculate the boiling point of an aqueous solution containing $18 \text{ g}$ of glucose in $100 \text{ g}$ of water, given that the molal elevation constant $(K_b)$ of water is $0.5 \text{ K kg mol}^{-1}$. [Molar mass of glucose $= 180 \text{ g mol}^{-1}$ and boiling point of pure water $= 100^{\circ}\text{C}$] (in $^{\circ}\text{C}$)