The osmotic pressure of a dilute solution of a compound XY in water is four times that of a solution of 0.01 M `BaCl_(2)` in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in `"mol" L^(-1)`) in solution is:

Options

A. `4xx10^(-4)`
B. `4xx10^(-2)`
C. `6xx10^(-2)`
D. `16xx10^(-4)`

Explanation

For XY
`i=2` as complete dissociation takes place.
`pi_(XY)=2xxCRT`
For `BaCl_(2)`
`i=3`
`pi_(BaCl_(2)=3xx0.01xxRt=0.03RT`
As `pi_(XY)=4xxpi_(BaCl_(2))`
`(pi_(XY))/(pi_(BaCl_(2))=(2xxCxRT)/(0.03RT)`
`(4xpi_(BaCl_(2)))/(pi_(BaCl_(2)))=(2xxC)/0.03`
`C=(4xx0.03)/2=6xx10^(-2)`