The osmotic pressure of a solution of $\mathrm{NaCl}$ is $0.10$ $\mathrm{atm}$ and that of a glucose solution is $0.20 \mathrm{~atm}$. The osmotic pressure of a solution formed by mixing $1 \mathrm{~L}$ of the sodium chloride solution with $2 \mathrm{~L}$ of the glucose solution is $x \times 10^{-3}$ atm. $x$ is
Osmotic pressure $=\pi=\mathrm{i} \times \mathrm{C} \times \mathrm{RT}$
For $\mathrm{NaCl} \mathrm{i}=2$ so
$\pi_{\mathrm{NaCl}}=\mathrm{i} \times \mathrm{C}_{\mathrm{NaCl}} \times \mathrm{RT} \quad \mathrm{C}_{\mathrm{NaCl}}=$ conc. of $\mathrm{NaCl}$
$0.1=2 \times \mathrm{C}_{\mathrm{NaCl}} \times \mathrm{RT}$
$\mathrm{C}_{\text {Glucose }}=\frac{0.2}{\mathrm{RT}}$ $\eta_{\mathrm{NaCl}}=$ No. of moles $\mathrm{NaCl}$
$\eta_{\mathrm{NaCl}}$ in $1 \mathrm{~L}=\mathrm{C}_{\mathrm{NaCl}} \times \mathrm{V}_{\mathrm{Litre}}$
$=\frac{0.05}{\mathrm{RT}} \quad \eta_{\mathrm{glucose}}=$ No. of moles glucose
$\eta_{\text {glucose }}$ in $2 \mathrm{~L}=\mathrm{C}_{\text {glucose }} \times \mathrm{V}_{\text {Litre }}$
$=\frac{0.4}{\mathrm{RT}}$
$\mathrm{V}_{\text {Total }}=1+2=3 \mathrm{~L}$
so Final conc. $\mathrm{NaCl}=\frac{0.05}{3 \mathrm{RT}}$
$\pi_{\text {Total }}=\pi_{\mathrm{NaCl}}+\pi_{\text {glucose }}$
$=\left[\mathrm{i} \times \mathrm{C}_{\mathrm{NaCl}}+\mathrm{C}_{\text {glucose }}\right] \times \mathrm{RT}$
$=\left(\frac{2 \times 0.05}{3 \mathrm{RT}}+\frac{0.4}{3 \mathrm{RT}}\right) \times \mathrm{RT}$
$=\frac{0.5}{3} \mathrm{~atm}$
$=0.1666 \mathrm{~atm}$
$=166.6 \times 10^{-3} \mathrm{~atm}$
$\Rightarrow 167.00 \times 10^{-3} \mathrm{~atm}$
so $x=167.00$
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