Chapter 16, Problem 89AE

a. Using the K_sp value for Cu(OH)₂ (1.6 × 10⁻¹⁹) and the overall formation constant for Cu(NH₃)₄²⁺ (1.0 × 10¹³), calculate the value for the equilibrium constant for the following reaction:

${\text{Cu(OH)}}_{\text{2}}\text{(}s\text{)}\text{+}{\text{4NH}}_{\text{3}}(aq)\rightleftharpoons Cu{(N{H}_3)}_4{}^{2+}(aq)+2O{H}^{-}(aq)$

b. Use the value of the equilibrium constant you calculated in part a to calculate the solubility (in mol/L) of Cu(OH)₂ in 5.0 M NH₃. In 5.0 M NH₃ the concentration of OH⁻ is 0.0095 M.