# Q5 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, the concentration of $XY\left ( in \; mol\; L\; ^{-1} \right )$ in solution is :

Given that

$\Pi_{X Y}=4 \times \Pi_{B a C l_{2}}$

since both are ionic solute, i.e.
$\begin{array}{l} X Y \longrightarrow X^{+}+Y^{-} \Rightarrow i=2 \\ B a C l_{2} \longrightarrow B a^{2+}+2 C l^{-} \Rightarrow i=3 \end{array}$
Now using the law,

$\Pi=i \times C R T\\ \Rightarrow 2 \times[X Y]=4 \times 3 \times 0.01 (\text{Assuming the same temperature})\\ [X Y]=0.06 M$

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