When an iron nail is dipped into copper sulfate (CuSO4) solution, a chemical reaction occurs. Here’s what happens in detail:
Reaction Overview
- When the iron nail is placed in the CuSO4 solution, a displacement reaction takes place.
- This is because iron is more reactive than copper.
Displacement Reaction
- Iron (Fe) displaces copper (Cu) from copper sulfate (CuSO4).
- The reaction can be represented as:
Fe + CuSO4 → FeSO4 + Cu
Visual Changes
- The solution changes color from blue to pale green.
- Blue color indicates the presence of copper sulfate.
- Pale green color indicates the formation of iron(II) sulfate (FeSO4).
Precipitation of Copper
- Copper metal starts to deposit on the surface of the iron nail.
- This deposition is visible as a reddish-brown coating.
Conclusion
- The iron nail undergoes oxidation, losing electrons and forming iron ions (Fe²⁺).
- Copper ions (Cu²⁺) in the solution gain electrons and are reduced to form solid copper.
Key Points to Remember
- Iron is more reactive than copper.
- A displacement reaction results in a color change.
- Copper is deposited on the iron nail.
This simple experiment illustrates key concepts in chemistry, such as reactivity series and displacement reactions, making it a fascinating topic for students.