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(B) Osmotic pressure is given by the formula $\Pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is molarity,$R$ is the gas constant,and $T$ is temper

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$P_1 > P_2$

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(B) Osmotic pressure is given by the formula $\Pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is molarity,$R$ is the gas constant,and $T$ is temperature.Since both solutions have the same molarity $(0.1 \ M)$ and are at the same temperature,the osmotic pressure depends on the van't Hoff factor $(i)$.$KNO_3$ is a strong electrolyte and dissociates completely into two ions ($K^+$ and $NO_3^-$),so its $i \approx 2$.$CH_3COOH$ is a weak electrolyte and dissociates only to a small extent,so its $i$ is slightly greater than $1$.Since $i_{KNO_3} > i_{CH_3COOH}$,it follows that $P_1 > P_2$.

Two solutions of $KNO_3$ and $CH_3COOH$ are prepared separately. Molarity of both is $0.1 \ M$ and osmotic pressures are $P_1$ and $P_2$ respectively. The correct relationship between the osmotic pressures is :-

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