Two beakers of capacity $500 \mathrm{mL}$ were taken. One of these beakers, labelled as $"\mathrm{A}"$, was filled with $400 \mathrm{mL}$ water whereas the beaker labelled $"\mathrm{B}"$ was filled with $400 \mathrm{mL}$ of $2 \mathrm{M}$ solution of $\mathrm{NaCl}$. At the same temperature, both the beakers were placed in closed containers of the same material and same capacity as shown in Figure.

At a given temperature, which of the following statement is correct about the vapour pressure of pure water and that of $\mathrm{NaCl}$ solution.

(i) Solution is a homogeneous mixture of two or more chemically non-reacting substances whose composition can be varied within certain limits.

(ii) Solute and Solvent. In a binary solution, the component present in smaller amount is called solute while the other present in larger amount is called solvent. If water is the solvent, solution is called aqueous solution.

2. Concentration terms of solutions

(i) Molarity$\left(\mathrm{M}\right)=\frac{\text{No. of Moles of solute }}{\text{ Vol. of solution (in mL) }}\times 1000$

(ii) Molality$\left(\mathrm{m}\right)=\frac{\text{ Moles of solute }}{\text{ Mass of solvent }\text{(in }\mathrm{g}\text{)}}\times 1000$

(iii) Mole fraction$\left(\mathrm{x}\right)=\frac{\text{No. of Moles of solute }}{\text{ Moles of solute}+\text{Moles of solvent }}$

(iv) Mole fraction of solute$+$mole fraction of solvent$=1$

3. Laws governing solutions:

(i) Henry’s law: The mass of the gas dissolved in a given volume of the liquid at constant temperature is directly proportional to the pressure of the gas in equilibrium with the liquid or for a mixture of gases in equilibrium with a liquid, the partial pressure of the gas is directly proportional to the mole fraction of the gas in the solution

$\mathrm{m}=\mathrm{k}.\mathrm{p}\mathrm{ }$or $\mathrm{p}={\mathrm{K}}_{\mathrm{H}}.\mathrm{x}$

KH is Henry’s law constant.

(ii) Raoult’s law in its general form can be stated as, for any solution the partial vapour pressure of each volatile component in the solution is directly proportional to its mole fraction.

4. Colligative properties:

(i) Relative lowering in vapour pressure:

$\frac{{\mathrm{p}}_1^{\mathrm{ }0}-{\mathrm{p}}_1}{{\mathrm{p}}_1^{\mathrm{ }0}}={\mathrm{x}}_2$ and ${\mathrm{M}}_{\mathrm{2}}=\frac{{\mathrm{w}}_2{\mathrm{M}}_{\mathrm{1}}}{{\mathrm{w}}_1\times \left(\frac{{\mathrm{p}}_1^{\mathrm{ }0}-{\mathrm{p}}_1}{{\mathrm{p}}_1^{\mathrm{ }0}}\right)}$

(ii) Elevation in boiling point ${\mathrm{\Delta T}}_{\mathrm{b}}={\mathrm{K}}_{\mathrm{b}}\mathrm{ }\mathrm{m}$ and ${\mathrm{M}}_{\mathrm{2}}=\frac{{\mathrm{K}}_{\mathrm{b}}\times {\mathrm{w}}_2\times 1000}{{\mathrm{\Delta T}}_{\mathrm{b}}\times {\mathrm{w}}_1}$

(iii) Depression in freezing point $\mathrm{\Delta }{\mathrm{T}}_{\mathrm{f}}={\mathrm{K}}_{\mathrm{f}}\mathrm{m}\mathrm{ }$ and ${\mathrm{M}}_2=\frac{{\mathrm{K}}_{\mathrm{f}}\times {\mathrm{w}}_2\times 1000}{{\mathrm{\Delta T}}_{\mathrm{f}}\times {\mathrm{w}}_1}$

(iv) Osmotic pressure $\mathrm{\pi }=\mathrm{cRT}$ or $\mathrm{\pi }=\frac{\mathrm{n}}{\mathrm{V}}\mathrm{RT}$ and ${\mathrm{M}}_{\mathrm{2}}=\frac{{\mathrm{w}}_2\mathrm{RT}}{\mathrm{V\pi }}$

5. Van't Hoff factor:

(i)$\mathrm{i}=\frac{\text{Normal molar mass}}{\text{Abnormal molar mass}}=\frac{ \text{Observed colligative property} }{ \text{Calcluated colligative property} }$

(ii) Relative lowering in vapour pressure Δpp=i xsolute

(iii) Elevation in boiling point, ΔTb=i Kbm

(iv) Depression in freezing point, ΔTf=i Kfm

(v) Osmotic pressure, π=i nVRT