Seema Saini Solutions for Chapter: Solutions, Exercise 3: DPP 2.3

$\mathrm{Y} \mathrm{gm}$ of a non-volatile solute of molar mass $\mathrm{M}$is dissolved in $250 \mathrm{g}$of benzene. If ${\mathrm{K}}_{\mathrm{b}}$ is molal elevation constant, then the value of $\mathrm{\Delta T}$ is given by

The vapour pressure of pure liquid $\mathrm{A}$ is $10 \mathrm{torr}$ and at the same temperature when $1 \mathrm{g}$ of solute $\mathrm{B}$ is dissolved in $20 \mathrm{g}$ of $\mathrm{A}$, its vapour pressure is reduced to $9.0 \mathrm{torr}$. If the molecular mass of $\mathrm{A}$ is $200 \mathrm{amu}$, then the molecular mass of $\mathrm{B}$ is:

Calculate the ebullioscopic constant for water. The heat of vaporization is $40.685 \mathrm{kJ} {\mathrm{mol}}^{-1}$.

An aqueous solution of urea is found to boil at $100.52°\mathrm{C}$. Given, ${\mathrm{K}}_{\mathrm{b}}$ for water is, $0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. Then, the mole fraction of urea in the solution is

When common salt is dissolved in water, the

Which of the following is (are) correct for non-volatile solute?

If ${\mathrm{P}}^0$ and ${\mathrm{P}}_{\mathrm{S}}$ are the $\mathrm{V}.\mathrm{P}.$ of a solvent and solution, respectively, and ${\mathrm{N}}_1$ and ${\mathrm{N}}_2$ are the mole of the solute and the solvent, then

The ebullioscopic constant depends upon