Answer:
After keeping a copper sulfate solution in an iron pot for a few days, you would likely find a number of reddish-brown deposits on the iron pot. These deposits are most likely copper (Cu) metal.
Here's why:
Copper sulfate (CuSO₄) is a salt composed of copper (Cu²⁺) and sulfate (SO₄²⁻) ions.
Iron (Fe) is more reactive than copper in this situation. This means it has a greater tendency to lose electrons and become oxidized.
When the iron pot comes in contact with the copper sulfate solution, a spontaneous redox reaction occurs.
Iron atoms donate electrons to copper ions, causing them to be reduced to metallic copper:
Fe(s) → Fe²⁺(aq) + 2e⁻
Cu²⁺(aq) + 2e⁻ → Cu(s)
The dissolved iron ions (Fe²⁺) remain in the solution, while the newly formed copper metal deposits onto the iron pot surface.
This reaction is known as a displacement reaction because the more reactive iron displaces the copper from the copper sulfate solution.
Therefore, the iron pot would exhibit reddish-brown deposits of copper metal due to the displacement reaction between iron and copper sulfate.
In addition to the copper deposits, the solution might also exhibit a greenish tint due to the formation of iron sulfate (FeSO₄), a byproduct of the reaction. However, the most visible change would be the presence of the copper metal on the iron pot.
