The correct option is **C. zinc is more electropositive than copper**. ### Detailed Explanation: When excess zinc is added to a bluish-green solution of copper(II) sulfate (CuSO₄), a chemical reaction occurs. This reaction can be represented by the following equation: \[ \text{Zn (s)} + \text{CuSO}_4 (aq) \rightarrow \text{ZnSO}_4 (aq) + \text{Cu (s)} \] 1. **Understanding the Reaction**: - Zinc (Zn) is a more electropositive metal than copper (Cu). This means that zinc has a greater tendency to lose electrons and form positive ions compared to copper. - In this reaction, zinc displaces copper from copper(II) sulfate because it is more reactive. The zinc atoms lose electrons to form zinc ions (Zn²⁺), while copper ions (Cu²⁺) gain electrons to form solid copper (Cu). 2. **Color Change**: - The original solution of copper(II) sulfate is blue due to the presence of Cu²⁺ ions. When zinc is added, it reacts with the Cu²⁺ ions, reducing them to solid copper, which precipitates out of the solution. - As the reaction proceeds, the concentration of Cu²⁺ ions decreases, and eventually, the solution becomes colorless as all the copper ions are converted to solid copper and removed from the solution. 3. **Final Solution**: - After filtering off the excess zinc and the precipitated copper, the remaining solution contains zinc sulfate (ZnSO₄), which is colorless in solution. This is why the final solution appears colorless. ### Why Other Options Are Incorrect: - **A. both zinc and copper are metals**: - While it is true that both zinc and copper are metals, this statement does not explain why the solution becomes colorless. The key factor in the color change is the reactivity of zinc compared to copper, not merely their metallic nature. - **B. the sulphate radical and the zinc ion are divalent**: - This statement is misleading. While it is true that both the sulfate ion (SO₄²⁻) and the zinc ion (Zn²⁺) are divalent, this does not explain the color change of the solution. The color change is primarily due to the displacement reaction and the reduction of Cu²⁺ ions, not the charge of the ions involved. - **D. both zinc and copper form depositive ions in solution**: - This option is vague and does not accurately describe the process. While both metals can form positive ions, the critical point is that zinc is more electropositive and can displace copper from its compound. The formation of depositive ions does not directly relate to the color change observed in the solution. ### Summary of Key Points: - Zinc is more electropositive than copper, allowing it to displace copper from copper(II) sulfate. - The reaction results in the formation of solid copper and a colorless zinc sulfate solution. - The bluish-green color of the original copper(II) sulfate solution disappears as Cu²⁺ ions are reduced to solid copper. - Understanding the reactivity series of metals is crucial for predicting the outcomes of displacement reactions. This thorough understanding of the reaction and the properties of the involved substances will help you in similar questions regarding metal reactivity and displacement reactions in chemistry.