A solution contains 0.036 M Cu2+ and 0.044 M Fe2+. 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? Ksp(CuS) = 1.3 × 10-36, Ksp(FES) = 6.3 × 10-18 O 3.6 x 10-35 M, FeS О 3.6 x O 10-35 M, CuS 1.4 × 10-16 M. CUS 1.4 × 10-16 M. FeS No precipitate will form at any concentration of sulfide ion.
A solution contains 0.036 M Cu2+ and 0.044 M Fe2+. 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? Ksp(CuS) = 1.3 × 10-36, Ksp(FES) = 6.3 × 10-18 O 3.6 x 10-35 M, FeS О 3.6 x O 10-35 M, CuS 1.4 × 10-16 M. CUS 1.4 × 10-16 M. FeS No precipitate will form at any concentration of sulfide ion.
Chapter16: Solubility And Complex Ion Equilibria
Section: Chapter Questions
Problem 60E: A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly...
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