Question #44744

An aqueous solution of a weak monoprotic acid \ce{HA} (molar mass $= 120 \text{ g mol}^{-1}$) has a mass concentration of $0.048 \text{ g cm}^{-3}$ and a density of $1.088 \text{ g cm}^{-3}$ at $298 \text{ K}$. The electrolytic conductivity ($\kappa$) of the solution is $3.2 \times 10^{-3} \text{ S cm}^{-1}$. Given the limiting molar conductivities $\Lambda^\circ_m(\ce{H^+}) = 350 \text{ S cm}^2 \text{ mol}^{-1}$ and $\Lambda^\circ_m(\ce{A^-}) = 50 \text{ S cm}^2 \text{ mol}^{-1}$, calculate the boiling point of this solution at $1 \text{ atm}$. (Assume $K_b$ for water is $0.52 \text{ K kg mol}^{-1}$ and the boiling point of pure water is $373.150 \text{ K}$.)