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 is water, the concentration of XY ( $i n m o l L^{- 1}$ ) in solution is

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$4 \times 10^{- 4}$

$4 \times 10^{- 2}$

$6 \times 10^{- 2}$

$16 \times 10^{- 4}$

answer is D.

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Detailed Solution

$For xy i = 2 π_{xy} = 2 \times CRT For {BaCl}_{2} i = 3, π_{{BaCl}_{2}} = 3 \times 0.01 \times RT = 0.03 RT As, π_{xy} = 4 \times π_{{BaCl}_{2}} \frac{π_{xy}}{π_{{BaCl}_{2}}} = \frac{2 \times C \times RT}{0.03 RT}, \frac{4 \times π_{{BaCl}_{2}}}{π_{{BaCl}_{2}}} = \frac{2 \times C}{0.03} C = \frac{4 \times 0.03}{2 \times 100} = 6 \times 10^{- 2}$