Cu2+ ions react with Fe2+ ions according to the following reaction.
Cu2+ + 2Fe2+ --> Cu + 2Fe3+
At equilibrium, the concentration of Cu2+ ions is not changed by the addition of
- A) Cu2++
- B) Fe2+
- C) Cu
- D) Fe3+.
The Attempt at a Solution
I chose A through elimination.
B won't work because the equilibrium will shift to the right if Fe2+ is added.
C and D won't work because the equilibrium will shift to the right.
Therefore A seems the most correct. However, if Cu2+ is added, then the equilibrium will also shift to the right. This means that it shifts to the right until the Cu2+ concentration is back to what it was before which seems impossible. Could someone shed some light on this?