1. Tardigrade
  2. Question
  3. Chemistry
  4. The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, find the concentration of XY (in mol L-1) in solution.

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Q. The osmotic pressure of a dilute solution of an ionic 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, find the concentration of $XY$ (in mol $L^{-1}$) in solution.

Solutions

Solution:

We know, $\pi =iCRT; \pi_{xy} =4\pi_{BaCl_2}$
$\therefore 2{XY} = 4\times\left(0.01\right) \times3$
$\left[XY\right] = 0.06$
$= 6 \times 10^{-2}$mol/ $L = 0.06$ mol$/L$