`x g` of non-electrolytic compound (molar mass =200) is dissolved in `1.0 L` of `0.05 M NaCl` solution. The osmotic pressure of this solution is found to be `4.92 atm` at `27^(@)C`. Calculate the value of `x`. Assume complete dissociation of `NaCl` and ideal behaviour of this solution.

Options

A. 16.52 gm
B. 24.032 gm
C. 19.959 gm
D. 12.35 gm

Answer

C

Explanation

`"(i) For "NaCl:pi=iCRT=2xx0.05xx0.0821xx300=2.463atm`
(ii) For unknown compound,
`pi=CRT=x/200xx0.0821xx300=0.1231" x atm"`
Total osmotic pressure `pi=pi_1+pi_2`
`4.92=2.463+0.1231"x "rArrx=19.959g`