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(A) 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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$CaCl_2$

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(A) 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.Since $C$,$R$,and $T$ are constant for all given solutions,the osmotic pressure depends directly on the van't Hoff factor $(i)$.For non-electrolytes like Glucose and Urea,$i = 1$.For $KCl$,it dissociates as $KCl \rightarrow K^+ + Cl^-$,so $i = 2$.For $CaCl_2$,it dissociates as $CaCl_2 \rightarrow Ca^{2+} + 2Cl^-$,so $i = 3$.Since $CaCl_2$ has the highest van't Hoff factor $(i=3)$,it will exhibit the maximum osmotic pressure.

Which of the following $0.1 \ M$ solutions has the maximum osmotic pressure at $25^o \ C$?

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