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(B) The osmotic pressure $(\pi)$ is a colligative property given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar c

Vedclass · Accepted Answer

Solutions of non-electrolytes only

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(B) The osmotic pressure $(\pi)$ is a colligative property 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 equimolal solutions,$C$ is the same.
However,for the osmotic pressure to be equal,the van't Hoff factor $(i)$ must also be the same.
Non-electrolytes have $i = 1$,whereas electrolytes dissociate into ions,resulting in $i > 1$.
Therefore,the statement is true only for non-electrolyte solutions.

At low concentrations,the statement that equimolal solutions under a given set of experimental conditions have equal osmotic pressure is true for:

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