What would be the pH needed to initiate precipitation for a solution that contains 8.22 x...

What would be the pH needed to initiate precipitation for a solution that contains 8.22 x 10-6 M Pb(NO3)2? Ksp of Pb(OH)2 is 1.2 x10-15.?

Expert Solution

Pb(OH)2 --------------> Pb⁺² + 2OH^-

x 2x

8.22*10^-6

x+8.22*10^-6 2x

KsP = [Pb⁺²][OH^-]²

1.2*10^-15 = (x+0.00000822)(2x)^2

x = 4.8*10^-6M

[OH-] = 2x = 2*4.8*10^-6

= 9.6*10^-6M

POH = -log[OH-]

= -log0.0000096 = 5.0177

PH = 14-POH

= 14-5.0177 = 8.9823

queen_honey_blossom answered 2 years ago

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