An aqueous dilute solution containing non-volatile solute boils at $100.52^{\circ} C$. What is the molality of the solution (in $m$)? ($K_b = 0.52 \ K \ kg \ mol^{-1}$, boiling temperature of water $= 100^{\circ} C$)

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 $= 1 \ atm$)

Calculate the molal elevation constant $(K_b)$ of a solvent if the boiling point of a $0.12 \ m$ solution is $319.8 \ K$ (Boiling point of pure solvent = $319.5 \ K$).

If the boiling point of water is $100 \,^{\circ}C$,how many grams of $NaCl$ must be added to $500 \,g$ of water to increase the boiling point by approximately $1 \,^{\circ}C$ (in $,g$)? Given $(K_{b})_{H_2O} = 0.52 \,K \cdot kg/mol$.

The boiling point of benzene is $353.23 \, K$. When $1.80 \, g$ of a nonvolatile solute was dissolved in $90 \, g$ of benzene,the boiling point is raised to $354.11 \, K$. The molar mass of the solute is $........ \, g \, mol^{-1}$. $[K_b \text{ for benzene} = 2.53 \, K \, kg \, mol^{-1}]$

When $0.5 \ g$ of anthracene is dissolved in $35 \ g$ of chloroform,the boiling point increases by $0.3 \ K$. If the $K_b$ value for $CHCl_3$ is $3.9 \ K \ kg \ mol^{-1}$,the experimental molar mass of anthracene is ......... $g \ mol^{-1}$.