The solubility of BaSO 4 in water is 2.42 × 10-3 gL -1 at 298 K. The value of its solubility product ( K sp ) will be (Given molar mass of BaSO 4=233 g mol -1 )

Question

The solubility of BaSO 4 in water is 2.42 × 10-3 gL -1 at 298 K. The value of its solubility product ( K sp ) will be (Given molar mass of BaSO 4=233 g mol -1 ) (A) 1.08 × 10-8 mol2 L-2 (B) 1.08 × 10-10 mol2 L-2 (C) 1.08 × 10-14 mol2 L-2 (D) 1.08 × 10-12 mol2 L-2

Tardigrade Admin · Accepted Answer

Sol. Solubility of BaSO 4, s =(2.42 × 10-3/233)( mol L -1) =1.04 × 10-5( mol L -1) BaSO 4( s ) leftharpoons undersets Ba 2+( aq )+ undersetsSO 4 2-( aq ) K sp =[ Ba 2+][ SO 42-]= s 2 =(1.04 × 10-5)2 =1.08 × 10-10 mol 2 L -2

Q. The solubility of $B a S O_{4}$ in water is $2.42 \times 1 0^{- 3} g L^{- 1}$ at $298 K$ . The value of its solubility product $(K_{s p})$ will be
(Given molar mass of $B a S O_{4} = 233 g m o l^{- 1}$ )

$1.08 \times 1 0^{- 8} m o l^{2} L^{- 2}$

$1.08 \times 1 0^{- 10} m o l^{2} L^{- 2}$

$1.08 \times 1 0^{- 14} m o l^{2} L^{- 2}$

$1.08 \times 1 0^{- 12} m o l^{2} L^{- 2}$

Q. The solubility of BaSO4​ in water is 2.42×10−3gL−1 at 298K. The value of its solubility product (Ksp​) will be (Given molar mass of BaSO4​=233gmol−1 )

1.08×10−8mol2L−2

1.08×10−10mol2L−2

1.08×10−14mol2L−2

1.08×10−12mol2L−2

Sol. Solubility of BaSO4​,s=2332.42×10−3​(molL−1) =1.04×10−5(molL−1) BaSO4​(s)⇌sBa2+​(aq)+sSO42−​​(aq) Ksp​=[Ba2+][SO42−​]=s2 =(1.04×10−5)2 =1.08×10−10mol2L−2

Q. The solubility of $B a S O_{4}$ in water is $2.42 \times 1 0^{- 3} g L^{- 1}$ at $298 K$ . The value of its solubility product $(K_{s p})$ will be
(Given molar mass of $B a S O_{4} = 233 g m o l^{- 1}$ )

$1.08 \times 1 0^{- 8} m o l^{2} L^{- 2}$

$1.08 \times 1 0^{- 10} m o l^{2} L^{- 2}$

$1.08 \times 1 0^{- 14} m o l^{2} L^{- 2}$

$1.08 \times 1 0^{- 12} m o l^{2} L^{- 2}$