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(D) The osmotic pressure is given by the formula $\pi = iMRT$,where $i$ is the van't Hoff factor,$M$ is the molarity,$R$ is the gas constant,and $T$ i

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(D) The osmotic pressure is given by the formula $\pi = iMRT$,where $i$ is the van't Hoff factor,$M$ is the molarity,$R$ is the gas constant,and $T$ is the temperature.For isotonic solutions,the osmotic pressure $\pi$ must be equal.$(A)$ For urea: $i = 1$,$\pi = 1 	imes 0.2 \ RT = 0.2 \ RT$$(B)$ For $NaCl$: $i = 2$,$\pi = 2 	imes 0.1 \ RT = 0.2 \ RT$$(C)$ For $BaCl_{2}$: $i = 3$,$\pi = 3 	imes 0.05 \ RT = 0.15 \ RT$$(D)$ For $AlCl_{3}$: $i = 4$,$\pi = 4 	imes 0.05 \ RT = 0.2 \ RT$Since the osmotic pressure of solution $C$ is $0.15 \ RT$ while others are $0.2 \ RT$,solution $C$ is not isotonic with the others.

Solutions $A, B, C$ and $D$ are respectively $0.2 \ M$ urea,$0.10 \ M$ $NaCl$,$0.05 \ M$ $BaCl_{2}$ and $0.05 \ M$ $AlCl_{3}$. All solutions are isotonic with each other except:

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