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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 conce

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$CoCl_{2}$

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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 a given concentration and temperature,$\pi$ is directly proportional to the van't Hoff factor $(i)$.$1$. Urea: $i = 1$ (non-electrolyte)$2$. $CoCl_{2}$: $i = 3$ $(Co^{2+} + 2Cl^{-})$$3$. $KCl$: $i = 2$ $(K^{+} + Cl^{-})$$4$. Glucose: $i = 1$ (non-electrolyte)Since $CoCl_{2}$ has the highest van't Hoff factor $(i = 3)$,it will exhibit the highest osmotic pressure.

Which of the following $0.1 \ m$ aqueous solutions exhibits the highest osmotic pressure at $25^{\circ}C$?

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