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Standard XII

Chemistry

Osmotic Pressure

Determine the...

Question

Determine the osmotic pressure of a solution prepared by dissolving 2.5 $\times 10^{- 2}$ of $K_{2} {S O}_{4}$ in 2L of water at $25^{o} C$ , assuming that it is completely dissociated.
( $R =$ 0.0821 L atm $K^{- 1} {m o l e}^{- 1}$ , Molar mass $K_{2} {S O}_{4}$ =174 g ${m o l e}^{- 1}$ )

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Solution

Concentration of solution $(C) = \frac{M o l e s}{V o l u m e} = \frac{\frac{2.5 \times 10^{- 2} \times 10^{3}}{174}}{2} = 0.07 M$
$∴$ Osmotic pressure $(π) = C R T = 0.07 \times 0.0821 \times 298 = 1.75 a t m$

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Q. Determine the osmotic pressure of a solution prepared by dissolving

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Determine the osmotic pressure of a solution prepared by dissolving 250 g of $K_{2} S O_{4}$ in 2L of water at $25^{o} C$ , assuming that it is completely dissociated.( $R = 0.0821 L a t m K^{- 1} m o l^{- 1}$ , Molar mass of $K_{2} S O_{4}$ = 174 g $m o l^{- 1})$

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Determine the osmotic pressure of a solution prepared by dissolving 2.5×10−2 of K2SO4 in 2L of water at 25 o C, assuming that it is completely dissociated. (R= 0.0821 L atm K−1mole−1, Molar mass K2SO4=174 g mole−1)

Concentration of solution (C)=MolesVolume=2.5×10−2×1031742=0.07M∴ Osmotic pressure (π)=CRT=0.07×0.0821×298=1.75atm

Determine the osmotic pressure of a solution prepared by dissolving 2.5 $\times 10^{- 2}$ of $K_{2} {S O}_{4}$ in 2L of water at $25^{o} C$ , assuming that it is completely dissociated.
( $R =$ 0.0821 L atm $K^{- 1} {m o l e}^{- 1}$ , Molar mass $K_{2} {S O}_{4}$ =174 g ${m o l e}^{- 1}$ )

Concentration of solution $(C) = \frac{M o l e s}{V o l u m e} = \frac{\frac{2.5 \times 10^{- 2} \times 10^{3}}{174}}{2} = 0.07 M$
$∴$ Osmotic pressure $(π) = C R T = 0.07 \times 0.0821 \times 298 = 1.75 a t m$