A solution contains 0.036 M Cu$^{2+}$ and 0.044 M Fe$^{2+}$. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? $K_{sp}(CuS) = 1.3 \times 10^{-36}$, $K_{sp}(FeS) = 6.3 \times 10^{-18}$.
1.4 × 10$^{-16}$ M, FeS
3.6 × 10$^{-35}$ M, CuS
3.6 × 10$^{-35}$ M, FeS
1.4 × 10$^{-16}$ M, CuS
No precipitate will form at any concentration of sulfide ion.