The pH of an aqueous solution of Ba ( OH )2 is 10 . If the K sp of Ba ( OH )2 is 1 × 10-9, then the concentration of Ba 2+ ions in the solution in mol L -1 is

Question

The pH of an aqueous solution of Ba ( OH )2 is 10 . If the K sp of Ba ( OH )2 is 1 × 10-9, then the concentration of Ba 2+ ions in the solution in mol L -1 is (A) 1 × 10-2 (B) 1 × 10-4 (C) 1 × 10-1 (D) 1 × 10-5

Tardigrade Admin · Accepted Answer

pH =10, pOH =4, stackrel ominus OH ]=10-4 M . Ba ( OH )2 longrightarrow Ba 2++2 overset ominus OH [ overset ominus OH ]=10-4 (Since total concentration of overset ominus O H =10-4 ) ∴ K sp =[ Ba 2+][ overset ominus OH ]2 10-9=x ×(10-4)2 ∴ x=10-1=[ Ba 2+]

Q. The $p H$ of an aqueous solution of $B a (O H)_{2}$ is $10$ . If the $K_{s p}$ of $B a (O H)_{2}$ is $1 \times 1 0^{- 9}$ , then the concentration of $B a^{2 +}$ ions in the solution in $m o l L^{- 1}$ is

$1 \times 1 0^{- 2}$

$1 \times 1 0^{- 4}$

$1 \times 1 0^{- 1}$

$1 \times 1 0^{- 5}$

$p H = 10, pO H = 4, O H ⊖] = 1 0^{- 4} M .$
$B a (O H)_{2} ⟶ B a^{2 +} + 2 O ⊖ H$
$[O ⊖ H] = 1 0^{- 4}$
(Since total concentration of $O ⊖ H = 1 0^{- 4}$ )
$∴ K_{s p} = [B a^{2 +}] [O ⊖ H]^{2}$
$1 0^{- 9} = x \times (1 0^{- 4})^{2}$
$∴ x = 1 0^{- 1} = [B a^{2 +}]$

Q. The pH of an aqueous solution of Ba(OH)2​ is 10 . If the Ksp​ of Ba(OH)2​ is 1×10−9, then the concentration of Ba2+ ions in the solution in molL−1 is

1×10−2

1×10−4

1×10−1

1×10−5