The osmotic pressure of equimolar solutions o | vedclass

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(A) Osmotic pressure $(\pi)$ is a colligative property,which depends on the van't Hoff factor $(i)$.$\pi = iCRT$.For equimolar solutions,$\pi \propto

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$AlCl_3 > BaCl_2 > Urea$

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(A) Osmotic pressure $(\pi)$ is a colligative property,which depends on the van't Hoff factor $(i)$.$\pi = iCRT$.For equimolar solutions,$\pi \propto i$.$Urea$ is a non-electrolyte,so $i = 1$.$BaCl_2$ dissociates as $BaCl_2 \rightarrow Ba^{2+} + 2Cl^-$,so $i = 3$.$AlCl_3$ dissociates as $AlCl_3 \rightarrow Al^{3+} + 3Cl^-$,so $i = 4$.Since the van't Hoff factor 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 of equimolar solutions of urea,$BaCl_2$,and $AlCl_3$ will be in the order:

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