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### The osmotic pressure of CaCl2 and urea solutions of the same concentration at the same temperature are respectively 0.605 atm and 0.245 atm, calculate van’t Hoff factor for CaCl2. - Chemistry

Exercise | Q 3.4 | Page 46

## The osmotic pressure of CaCl2 and urea solutions of the same concentration at the same temperature are respectively 0.605 atm and 0.245 atm, calculate van’t Hoff factor for CaCl2.

### Solution:

Given: Osmotic pressure of CaCl2 solution = 0.605 atm

Osmotic pressure of urea solution = 0.245 atm

To find: The value of van’t Hoff factor

Formulae: π = MRT, π = iMRT

Calculation: For urea solution

π = MRT

0.245 atm = MRT       ....(i)

For CaCl2 solution

π = iMRT

0.602 atm = iMRT       ....(ii)

From equations (i) and (ii),

$\frac{0.605}{0.245}=\frac{\text{iMRT}}{\text{MRT}}$

∴ i = 2.47

The value of van’t Hoff factor is 2.47.