The solubility of in water is at 298 K. The value of its solubility product will be (Given molar mass of ) [2018]

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Q.
The solubility of ${BaSO}_{4}$ in water is $2.42 \times 10^{- 3}$ $g$ $L^{- 1}$ at 298 K. The value of its solubility product $(K_{s p})$ will be (Given molar mass of ${BaSO}_{4} = 233$ $g$ ${mol}^{- 1}$ ) [2018]

1 $1.08 \times 10^{- 10}$ ${mol}^{2}$ $L^{- 2}$

2 $1.08 \times 10^{- 12}$ ${mol}^{2}$ $L^{- 2}$

3 $1.08 \times 10^{- 14}$ ${mol}^{2}$ $L^{- 2}$

4 $1.08 \times 10^{- 8}$ ${mol}^{2}$ $L^{- 2}$

Ans.
(1)

Solubility of ${BaSO}_{4}$

$s = \frac{2.42 \times 10^{- 3}}{233}$ $mol$ $L^{- 1} = 1.04 \times 10^{- 5}$ $mol$ $L^{- 1}$

${BaSO}_{4}$ ionizes completely in the solution as: ${BaSO}_{4 (s)} ⇌ {Ba}_{(a q)}^{2 +} + {SO}_{4}_{(a q)}^{2 -}$

$K_{s p} = [{Ba}^{2 +}] [{SO}_{4}^{2 -}] = s^{2}$

$= {(1.04 \times 10^{- 5})}^{2} = 1.08 \times 10^{- 10}$ ${mol}^{2}$ $L^{- 2}$

Solution

Q.
The solubility of ${BaSO}_{4}$ in water is $2.42 \times 10^{- 3}$ $g$ $L^{- 1}$ at 298 K. The value of its solubility product $(K_{s p})$ will be (Given molar mass of ${BaSO}_{4} = 233$ $g$ ${mol}^{- 1}$ ) [2018]

1 $1.08 \times 10^{- 10}$ ${mol}^{2}$ $L^{- 2}$

2 $1.08 \times 10^{- 12}$ ${mol}^{2}$ $L^{- 2}$

3 $1.08 \times 10^{- 14}$ ${mol}^{2}$ $L^{- 2}$

4 $1.08 \times 10^{- 8}$ ${mol}^{2}$ $L^{- 2}$

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Solution

Q. The solubility of BaSO4 in water is 2.42×10-3 g L-1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO4=233 g mol-1) [2018]

1 1.08×10-10 mol2 L-2

2 1.08×10-12 mol2 L-2

3 1.08×10-14 mol2 L-2

4 1.08×10-8 mol2 L-2

Ans. (1) Solubility of BaSO4 s=2.42×10-3233 mol L-1=1.04×10-5 mol L-1 BaSO4 ionizes completely in the solution as: BaSO4(s)⇌Ba(aq)2++SO4(aq)2- Ksp=[Ba2+][SO42-]=s2 =(1.04×10-5)2=1.08×10-10 mol2 L-2

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Q.
The solubility of ${BaSO}_{4}$ in water is $2.42 \times 10^{- 3}$ $g$ $L^{- 1}$ at 298 K. The value of its solubility product $(K_{s p})$ will be (Given molar mass of ${BaSO}_{4} = 233$ $g$ ${mol}^{- 1}$ ) [2018]

1 $1.08 \times 10^{- 10}$ ${mol}^{2}$ $L^{- 2}$

2 $1.08 \times 10^{- 12}$ ${mol}^{2}$ $L^{- 2}$

3 $1.08 \times 10^{- 14}$ ${mol}^{2}$ $L^{- 2}$

4 $1.08 \times 10^{- 8}$ ${mol}^{2}$ $L^{- 2}$