Wht is the solubility of Ni(OH)2 in a solution buffêred at pH = 11.3? The Ksp of Ni(OH)2 at 25 oC is 6.0 × 10-16.
.................Ni(OH)2 ==> Ni^2+ + 2OH^-
I................solid..................0.............0
C...............solid..................x.............2x
E................solid..................x.............2x
Ksp = (Ni^2+)(OH^-)^2
You know Ksp. You can calculate OH^- from pH. Solve for (Ni^2+) which is the solubility. Post your work if you get stuck.