Q. A solution of sucrose (Molar mass = 342 g/mol) is prepared by dissolving 68.4 g of it per litre of solution, what is its osmotic pressure (R=0.082 L atm $K^{- 1} \, mol^{- 1}$ ) at 273 K?

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A

4.48 atm

B

2 atm

C

1 atm

D

5 atm

Solution:

Sucrose is non ionisable so i = 1
$\text{\pi }=\text{i CRT}$
$= 1 \times \frac{\frac{68.4}{342}}{1} \left(0.082\right) \times 273$
$=4.477\text{atm}$
$\sim eq4.48\text{atm}$

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