$A$ solution of non-volatile solute has boiling point elevation $0.5 \ K$. Calculate molality of solution $[K_{b} = 2.40 \ K \ kg \ mol^{-1}]$.

$18 \ g$ 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 following graph shows the vapour pressure (in $atm$) on the $y$-axis versus temperature $T$ (in $K$) on the $x$-axis for pure water and an aqueous urea solution. What is the boiling point (in $K$) of the urea solution? (Atmospheric pressure $= 1 \ atm$)

What is molal elevation? Explain.

When $3.3 \ g$ of an unknown substance is dissolved in $125 \ g$ of benzene (boiling point $80^\circ \text{C}$),the boiling point of the resulting solution is $80.66^\circ \text{C}$. What is the molar mass of the unknown substance? $(K_b = 3.28 \ \text{K kg mol}^{-1})$

Which of the following equations correctly represents the molar mass of a solute by knowing the boiling point elevation?