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(A) Osmotic pressure $(\pi)$ is a colligative property given by $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is

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Decimolar aluminium sulphate

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(A) Osmotic pressure $(\pi)$ is a colligative property given by $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.Since all solutions are decimolar $(C = 0.1 \ M)$,the osmotic pressure depends on the van't Hoff factor $(i = 1 + (n-1)\alpha)$.For $90\%$ dissociation,$\alpha = 0.9$.$(A)$ $Al_2(SO_4)_3 \rightarrow 2Al^{3+} + 3SO_4^{2-}$,$n = 5$,$i = 1 + (5-1)(0.9) = 4.6$.$(B)$ $BaCl_2 \rightarrow Ba^{2+} + 2Cl^-$,$n = 3$,$i = 1 + (3-1)(0.9) = 2.8$.$(C)$ $Na_2SO_4 \rightarrow 2Na^+ + SO_4^{2-}$,$n = 3$,$i = 1 + (3-1)(0.9) = 2.8$.$(D)$ Mixing $(B)$ and $(C)$ results in a solution with lower concentration of individual ions compared to $(A)$.Thus,$Al_2(SO_4)_3$ provides the maximum number of ions,resulting in the highest osmotic pressure.

Which of the following would have the highest osmotic pressure? (Assume that all salts are $90\%$ dissociated.)

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