The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of $0.01 \mathrm{M} \mathrm{BaCl}_{2}$ in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in $\mathrm{mol} \mathrm{L}^{-1}$ ) in solution is

JEE Main · 2019 · 09 Apr 2019 · Shift 1 · Solutions

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 (in

mol L^{- 1}

) in solution is

(A) $4 \times 1 0^{- 4}$
(B) $6 \times 1 0^{- 2}$ ✓ Correct
(C) $16 \times 1 0^{- 4}$
(D) $4 \times 1 0^{- 2}$

Answer: (B)

Solution

Osmotic pressure is

π = i C R T

. For

BaCl X_{2}

, which breaks into three ions,

i = 3

, so its

0.01

M solution gives

π = 0.03 R T

. The salt

XY

breaks into two ions,

i = 2

. We are told its osmotic pressure is four times that of the barium chloride,

4 \times 0.03 R T = 0.12 R T

, so

2 C_{X Y} R T = 0.12 R T

and

C_{X Y} = 0.06 = 6 \times 1 0^{- 2} mol L^{- 1}

JEE Main · 2019 · 09 Apr 2019 · Shift 1 · Single correct option

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