What is the solubility of zinc hydroxide in a buffer with pH=10
use:
pH = -log [H+]
10 = -log [H+]
[H+] = 1*10^-10 M
use:
[OH-] = Kw/[H+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H+]
[OH-] = (1.0*10^-14)/(1*10^-10)
[OH-] = 1*10^-4 M
At equilibrium:
Zn(OH)2 <----> Zn2+ + 2 OH-
s 1*10^-4 + 2s
Ksp = [Zn2+][OH-]^2
5*10^-17=(s)*(1*10^-4+ 2s)^2
Since Ksp is small, s can be ignored as compared to 1*10^-4
Above expression thus becomes:
5*10^-17=(s)*(1*10^-4)^2
5*10^-17= (s) * 10^-8
s = 5.0*10^-9 M
Answer: 5.0*10^-9 M
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