Ni(OH)2(s) ⇌ Ni2+(aq) + 2 OH–(aq)
Calculate the OH– concentration in the solution:
pOH = 3.7
[OH–] = 1.995x10–4 M
Notice that there is a common ion present, OH–.
We can construct an ICE table for the dissociation of Ni(OH)2.
The Ksp expression for Ni(OH)2 is:
We can now plug in the equilibrium concentrations and solve for x, which is the molar solubility of Ni(OH)2 in M or mol/L.
Calculate the molar solubility of Ni(OH)2 when buffered at pH = 10.3.
Express your answer using one significant figure.
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