The osmotic pressures of 0.010 M solutions o | vedclass

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(A) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas

Vedclass · Accepted Answer

$1.80$

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(A) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.For sucrose (a non-electrolyte),the van't Hoff factor $i = 1$. Thus,$\pi_{	ext{sucrose}} = 1 	imes C 	imes R 	imes T = 0.24 \ atm$.For $KI$ (an electrolyte),$\pi_{KI} = i_{KI} 	imes C 	imes R 	imes T = 0.432 \ atm$.Dividing the two equations:$\frac{\pi_{KI}}{\pi_{	ext{sucrose}}} = \frac{i_{KI} 	imes C 	imes R 	imes T}{1 	imes C 	imes R 	imes T} = \frac{0.432}{0.24}$.$i_{KI} = 1.80$.

The osmotic pressures of $0.010 \ M$ solutions of $KI$ and of sucrose $(C_{12}H_{22}O_{11})$ are $0.432 \ atm$ and $0.24 \ atm$ respectively. The van't Hoff factor for $KI$ is

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