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.

Question

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. (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

We know, π =iCRT; πxy =4πBaCl2 ∴ 2XY = 4×(0.01) ×3 [XY] = 0.06 = 6 × 10-2mol/ L = 0.06 mol/L

Q. The osmotic pressure of a dilute solution of an ionic compound $X Y$ in water is four times that of a solution of $0.01 M B a C l_{2}$ in water. Assuming complete dissociation of the given ionic compounds in water, find the concentration of $X Y$ (in mol $L^{- 1}$ ) in solution.

We know, $π = i CRT; π_{x y} = 4 π_{B a C l_{2}}$
$∴ 2 X Y = 4 \times (0.01) \times 3$
$[X Y] = 0.06$
$= 6 \times 1 0^{- 2}$ mol/ $L = 0.06$ mol $/ L$

Q. The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01MBaCl2​ in water. Assuming complete dissociation of the given ionic compounds in water, find the concentration of XY (in mol L−1) in solution.

We know, π=iCRT;πxy​=4πBaCl2​​ ∴2XY=4×(0.01)×3 [XY]=0.06 =6×10−2mol/ L=0.06 mol/L

Q. The osmotic pressure of a dilute solution of an ionic compound $X Y$ in water is four times that of a solution of $0.01 M B a C l_{2}$ in water. Assuming complete dissociation of the given ionic compounds in water, find the concentration of $X Y$ (in mol $L^{- 1}$ ) in solution.

We know, $π = i CRT; π_{x y} = 4 π_{B a C l_{2}}$
$∴ 2 X Y = 4 \times (0.01) \times 3$
$[X Y] = 0.06$
$= 6 \times 1 0^{- 2}$ mol/ $L = 0.06$ mol $/ L$