The osmotic pressure values of 0.1 M solutio | vedclass

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Question

(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

$P_1 > P_2$

Vedclass · Answer

(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 $0.1 \ M$ $KNO_3$ (a strong electrolyte),it dissociates completely into $K^+$ and $NO_3^-$ ions,so $i \approx 2$.For $0.1 \ M$ $CH_3COOH$ (a weak electrolyte),it dissociates only partially,so $i$ is slightly greater than $1$.Since $C$,$R$,and $T$ are the same for both solutions,the osmotic pressure depends on the van't Hoff factor $i$.Because $i_{KNO_3} > i_{CH_3COOH}$,it follows that $P_1 > P_2$.

The osmotic pressure values of $0.1 \ M$ solutions of $KNO_3$ and $CH_3COOH$ are $P_1$ and $P_2$ respectively. Establish the relationship between them.

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