Question

What happens when an iron nail is dipped in copper sulfate solution? Write with equation.

Hint:

Memorize the reactivity series to easily predict single displacement reactions: K, Na, Ca, Mg, Al, Zn, Fe, Pb, (H), Cu, Hg, Ag, Au.

Answer 1

Step 1: Understanding the Concept:
This is a single displacement reaction. A more reactive metal displaces a less reactive metal from its salt solution.

Step 2: Detailed Explanation:
Iron (\(\text{Fe}\)) is placed higher than Copper (\(\text{Cu}\)) in the reactivity series, meaning it is more reactive.
When an iron nail is placed in an aqueous solution of copper sulfate (\(\text{CuSO}_4\)), iron displaces copper from the solution to form iron(II) sulfate (\(\text{FeSO}_4\)).
Observations:
1. The blue color of the copper sulfate solution gradually fades and turns light green due to the formation of iron(II) sulfate.
2. A reddish-brown coating of metallic copper is deposited on the surface of the iron nail.
Chemical Equation:
\(\text{Fe}(s) + \text{CuSO}_4(aq) \rightarrow \text{FeSO}_4(aq) + \text{Cu}(s)\)

Step 3: Final Answer:
Iron displaces copper. The blue solution turns green, and brown copper coats the nail.