The solubility of Pb(OH)2 in water is 6.7 × 10 - 6 M. Calculate the solubility of Pb(OH)2 in a buffer solution of pH = 8.

Question

The solubility of Pb(OH)2 in water is 6.7 × 10 - 6 M. Calculate the solubility of Pb(OH)2 in a buffer solution of pH = 8. (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

In water, K sp = 4 S3 = 4 ( 6.2 × 10 - 4 )3 = 1.2 × 10 - 15 In buffer of pH = 8, pOH = 6, [ OH- ] = 10 - 6 K sp = S [ OH- ]2 S = ( 1.2 × 10 - 15 / 10 - 12) = 1.2 × 10 - 3 M

Q. The solubility of $P b (O H)_{2}$ in water is $6.7 \times 1 0^{- 6} M$ . Calculate the solubility of $P b (O H)_{2}$ in a buffer solution of $p H = 8$ .

In water, $K_{s p} = 4 S^{3} = 4 (6.2 \times 1 0^{- 4})^{3}$
$= 1.2 \times 1 0^{- 15}$
In buffer of $p H = 8, pO H = 6, [O H^{-}] = 1 0^{- 6}$
$K_{s p} = S [O H^{-}]^{2}$
$S = \frac{1.2 \times 1 0 ^{- 15}}{1 0 ^{- 12}} = 1.2 \times 1 0^{- 3} M$

Q. The solubility of Pb(OH)2​ in water is 6.7×10−6M. Calculate the solubility of Pb(OH)2​ in a buffer solution of pH=8.

In water, Ksp​=4S3=4(6.2×10−4)3 =1.2×10−15 In buffer of pH=8,pOH=6,[OH−]=10−6 Ksp​=S[OH−]2 S=10−121.2×10−15​=1.2×10−3M

Q. The solubility of $P b (O H)_{2}$ in water is $6.7 \times 1 0^{- 6} M$ . Calculate the solubility of $P b (O H)_{2}$ in a buffer solution of $p H = 8$ .

In water, $K_{s p} = 4 S^{3} = 4 (6.2 \times 1 0^{- 4})^{3}$
$= 1.2 \times 1 0^{- 15}$
In buffer of $p H = 8, pO H = 6, [O H^{-}] = 1 0^{- 6}$
$K_{s p} = S [O H^{-}]^{2}$
$S = \frac{1.2 \times 1 0 ^{- 15}}{1 0 ^{- 12}} = 1.2 \times 1 0^{- 3} M$