Please, help Determine the molar solubility of Mg(OH)2 in a solution buffered at a pH of 7. KSP=1.2*10^-11
use:
pH = -log [H+]
7 = -log [H+]
[H+] = 1*10^-7 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^-7)
[OH-] = 1*10^-7 M
At equilibrium:
Mg(OH)2 <----> Mg2+ + 2 OH-
s 1*10^-7
Ksp = [Mg2+][OH-]^2
1.2*10^-11=(s)*(1*10^-7)^2
1.2*10^-11= (s) * 10^-14
s = 1.2*10^3 M
Answer: 1.2*10^3 M
Please, help Determine the molar solubility of Mg(OH)2 in a solution buffered at a pH of...
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