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(C) 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 conce

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Osmotic pressure of $Na_2SO_4$ solution will be more than $NaCl$ solution

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(C) 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 $NaCl$,it dissociates as $NaCl \rightarrow Na^+ + Cl^-$,so the van't Hoff factor $i = 2$.For $Na_2SO_4$,it dissociates as $Na_2SO_4 \rightarrow 2Na^+ + SO_4^{2-}$,so the van't Hoff factor $i = 3$.Since both solutions have the same molar concentration $(C = 0.1 \ M)$ and are at the same temperature,the osmotic pressure depends directly on the van't Hoff factor $i$.Because $i$ for $Na_2SO_4$ $(i=3)$ is greater than $i$ for $NaCl$ $(i=2)$,the osmotic pressure of the $Na_2SO_4$ solution will be higher.

The osmotic pressure of a $0.1 \ M$ solution of $NaCl$ and $Na_2SO_4$ will be:

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