The osmotic pressure (O.P.) of equimolar solu | vedclass

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(A) The osmotic pressure $(\pi)$ is a colligative property,which depends on the number of particles in the solution. The formula is $\pi = iCRT$,where

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$AlCl_3 > BaCl_2 > Urea$

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(A) The osmotic pressure $(\pi)$ is a colligative property,which depends on the number of particles in the solution. The formula is $\pi = iCRT$,where $i$ is the van't Hoff factor.For equimolar solutions,the osmotic pressure is directly proportional to the van't Hoff factor $(i)$.$1$. $Urea$ is a non-electrolyte,so $i = 1$.$2$. $BaCl_2$ dissociates as $BaCl_2 	o Ba^{2 }   2Cl^{-}$,so $i = 3$.$3$. $AlCl_3$ dissociates as $AlCl_3 	o Al^{3 }   3Cl^{-}$,so $i = 4$.Since the number of particles follows the order $AlCl_3 (4) > BaCl_2 (3) > Urea (1)$,the osmotic pressure follows the same order: $AlCl_3 > BaCl_2 > Urea$.

The osmotic pressure $(O.P.)$ of equimolar solutions of $Urea$,$BaCl_2$,and $AlCl_3$ will be in the order:

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