The osmotic pressure of 253 mL of a solution dissolving 34.2 g of sugar at `27^@C` will be

Options

A. 7.12 atm
B. 5.26 atm
C. 3.96 atm
D. 9.73 atm

Answer

D

Explanation

Volume of the solution (V) = 253 mL = 0.253 litre, Weight of sugar `(W_B)= 34.2 g` and temperature `(T) = 27^@C = 300 K`
The molecular weight of sugar `(M_B) = 342 and R = 0.081 L atm K^(-1)`
Therefore, osmotic pressure, `pi = (W_B .RT)/(M_B.V) = (34.2 xx 0.0821xx 300)/(342xx0.253) = 9.73` atm