The measured osmotic pressure of a solution p | vedclass

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(B) Given: Osmotic pressure $\pi = 3.735 	imes 10^{-3} \ bar$,mass of $K_2SO_4$ $(\omega) = 17.4 \ mg = 17.4 	imes 10^{-3} \ g$,volume $(V) = 2 \ L$

Vedclass · Accepted Answer

$3$

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(B) Given: Osmotic pressure $\pi = 3.735 	imes 10^{-3} \ bar$,mass of $K_2SO_4$ $(\omega) = 17.4 \ mg = 17.4 	imes 10^{-3} \ g$,volume $(V) = 2 \ L$,temperature $(T) = 27^{\circ} C = 300 \ K$.Molar mass $(M)$ of $K_2SO_4 = (2 	imes 39) + 32 + (4 	imes 16) = 174 \ g \ mol^{-1}$.Using the formula $\pi = iCRT$,where $C = \frac{\omega}{M 	imes V}$,we get $i = \frac{\pi 	imes M 	imes V}{\omega 	imes R 	imes T}$.Substituting the values: $i = \frac{3.735 	imes 10^{-3} 	imes 174 	imes 2}{17.4 	imes 10^{-3} 	imes 0.083 	imes 300} = \frac{1.30038}{0.43326} = 3.0$.Thus,the van't Hoff factor is $3$.

The measured osmotic pressure of a solution prepared by dissolving $17.4 \ mg$ of $K_2SO_4$ in $2 \ L$ of water at $27^{\circ} C$ is $3.735 \times 10^{-3} \ bar$. The van't Hoff factor is $(R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$; atomic weights $K = 39, S = 32, O = 16)$.

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