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(D) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas

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$0.03 \ M \ NaCl$ at $50 \ ^oC$

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(D) The osmotic pressure $(\pi)$ is 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 in Kelvin.For $0.011 \ M \ AlCl_3$ $(i=4)$: $\pi = 4 	imes 0.011 	imes R 	imes 323 = 0.014212 \ R$.For $0.03 \ M \ NaCl$ $(i=2)$: $\pi = 2 	imes 0.03 	imes R 	imes 298 = 0.01788 \ R$.For $0.012 \ M \ (NH_4)_2SO_4$ $(i=3)$: $\pi = 3 	imes 0.012 	imes R 	imes 298 = 0.010728 \ R$.For $0.03 \ M \ NaCl$ at $50 \ ^oC$ $(i=2)$: $\pi = 2 	imes 0.03 	imes R 	imes 323 = 0.01938 \ R$.Comparing the values,$0.03 \ M \ NaCl$ at $50 \ ^oC$ has the highest osmotic pressure.

Which of the following aqueous solutions should have the highest osmotic pressure?

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