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

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$2.5 \ M AB_2$ type,$i=2.5$,temperature $= 57^{\circ} C$

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(D) The osmotic pressure 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 $(0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$,and $T$ is the temperature in Kelvin.$(a)$ For $5.0 \ M$ urea: $\pi = 1 	imes 5.0 	imes 0.0821 	imes (67 + 273) = 1 	imes 5.0 	imes 0.0821 	imes 340 = 139.57 \ atm$.$(b)$ For $1.5 \ M A_2 B_3$: $\pi = 4.1 	imes 1.5 	imes 0.0821 	imes (27 + 273) = 4.1 	imes 1.5 	imes 0.0821 	imes 300 = 151.47 \ atm$.$(c)$ For $3.0 \ M AB$: $\pi = 1.6 	imes 3.0 	imes 0.0821 	imes (27 + 273) = 1.6 	imes 3.0 	imes 0.0821 	imes 300 = 118.22 \ atm$.$(d)$ For $2.5 \ M AB_2$: $\pi = 2.5 	imes 2.5 	imes 0.0821 	imes (57 + 273) = 2.5 	imes 2.5 	imes 0.0821 	imes 330 = 169.33 \ atm$.Comparing the values,the solution with the highest osmotic pressure is $2.5 \ M AB_2$.

Which one of the following solutions of compounds shows the highest osmotic pressure? ($AB, AB_2$ and $A_2 B_3$ are ionic compounds)

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