When zinc pieces are placed into a blue copper sulfate solution, a series of observable chemical reactions occur. Below is a detailed explanation of the process and its outcomes.
Observation of Color Change
- Initially, the blue copper sulfate solution is vibrant blue due to the presence of copper (II) ions (Cu²⁺).
- Upon introducing zinc (Zn), the solution's color begins to fade, transitioning from blue to a lighter shade.
Reaction Process
- Zinc is more reactive than copper in the reactivity series, which allows it to displace copper from copper sulfate.
- The chemical reaction can be represented as follows:
\[
\text{Zn (s) + CuSO}_4 \text{(aq)} \rightarrow \text{ZnSO}_4 \text{(aq)} + \text{Cu (s)}
\]
- In this reaction, zinc sulfate (ZnSO₄) forms in solution, and solid copper precipitates out.
Formation of Copper
- As the reaction proceeds, you may observe reddish-brown copper deposits forming on the zinc pieces and settling at the bottom of the container.

Final Outcome
- The blue copper sulfate solution gradually loses its color, indicating a decrease in copper ions in the solution.
- Eventually, the solution may appear colorless or pale, depending on the concentration of zinc sulfate formed.
This reaction exemplifies a classic single displacement reaction, highlighting the differences in reactivity between metals and their ability to exchange places in compounds.