* Copper sulfate solution (CuSO₄): This solution is initially blue due to the presence of copper(II) ions (Cu²⁺).
* Iron filings (Fe): Iron is more reactive than copper in the reactivity series of metals.
* Reaction: When iron filings are added to the copper sulfate solution, the iron atoms displace the copper ions from the solution, forming iron(II) sulfate (FeSO₄) and depositing copper metal.
The chemical equation for this reaction is:
Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)
* Iron(II) sulfate solution (FeSO₄): The resulting solution contains iron(II) ions (Fe²⁺) which have a light green color.
* Copper metal (Cu): The reddish-brown copper metal is deposited out of the solution, often appearing as a coating on the iron filings.
In summary:
The blue copper sulfate solution turns light green because the copper ions (Cu²⁺) are replaced by iron(II) ions (Fe²⁺), which give the solution its characteristic light green color. This reaction is a good demonstration of the reactivity of metals and the concept of single displacement reactions.
