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Answer the following.
Calculate the osmotic pressure of a solution prepared by dissolving of in of water at assuming that…
Calculate the osmotic pressure of a solution prepared by dissolving $0\cdot025\text{ g}$ of $\text{K}_2\text{SO}_4$ in $2\cdot0\text{ litres}$ of water at $25^\circ\text{C}$ assuming that $\text{K}_2\text{SO}_4$ is completely dissociated. (mol. wt. of $\text{K}_2\text{SO}_4 = 174\text{ g mol}^{-1}$)
Answer
Answer
AIFormula used: Osmotic pressure: pi = i*C*R*T with R = 0.0821 L atm K^-1 mol^-1, T = 298 K, V = 2.0 L, i = 3, M2 = 174 g mol^-1, w2 = 0.025 g, so pi = 0.00527 atm
Formula: $\pi = iCRT$
$C = \dfrac{0\cdot025\text{ g}}{174\text{ g mol}^{-1}\times 2\cdot0\text{ L}} = 7\cdot18\times10^{-5}\text{ mol L}^{-1}$
$i = 3$ (complete dissociation into $2\mathrm{K^+}$ and $\mathrm{SO_4^{2-}}$), $T = 298\text{ K}$
$\pi = 3\times 7\cdot18\times10^{-5}\text{ mol L}^{-1}\times 0\cdot0821\text{ L atm K}^{-1}\text{mol}^{-1}\times 298\text{ K} = 5\cdot27\times10^{-3}\text{ atm}$
Final answer: 0.00527 atm
From ISC 2018 Chemistry Paper 1, question 1(d)(iii).
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