To understand the reaction between copper(II) sulfate (CuSO\(_4\)) and lead(II) nitrate (Pb(NO\(_3\))\(_2\)), let's break down the components and the expected outcomes step by step. ### Step 1: Identify the Reactants - **Copper(II) sulfate (CuSO\(_4\))**: This is a blue ionic compound that dissociates in water to form Cu\(^{2+}\) ions and SO\(_4^{2-}\) ions. - **Lead(II) nitrate (Pb(NO\(_3\))\(_2\))**: This is a colorless ionic compound that dissociates in water to form Pb\(^{2+}\) ions and NO\(_3^{-}\) ions. ### Step 2: Write the Dissociation Equations When these compounds are dissolved in water, they dissociate as follows: - CuSO\(_4\) (aq) → Cu\(^{2+}\) (aq) + SO\(_4^{2-}\) (aq) - Pb(NO\(_3\))\(_2\) (aq) → Pb\(^{2+}\) (aq) + 2 NO\(_3^{-}\) (aq) ### Step 3: Predict the Reaction When these two solutions are mixed, we need to consider the possible reactions between the ions present: - Cu\(^{2+}\) (aq) + Pb\(^{2+}\) (aq) + SO\(_4^{2-}\) (aq) + 2 NO\(_3^{-}\) (aq) In this case, we are looking for a possible precipitation reaction. The key is to identify if any of the combinations of ions will form an insoluble compound. ### Step 4: Identify Possible Products The potential products from the ions in solution are: 1. CuSO\(_4\) (remains in solution) 2. Pb(NO\(_3\))\(_2\) (remains in solution) 3. Cu(NO\(_3\))\(_2\) (remains in solution) 4. PbSO\(_4\) (potential precipitate) ### Step 5: Solubility Rules According to solubility rules: - Most sulfate salts are soluble, but lead(II) sulfate (PbSO\(_4\)) is an exception and is insoluble in water. Therefore, when Pb\(^{2+}\) ions react with SO\(_4^{2-}\) ions, they will form a white precipitate of PbSO\(_4\). ### Step 6: Conclusion When CuSO\(_4\) is added to Pb(NO\(_3\))\(_2\), a white precipitate of lead(II) sulfate (PbSO\(_4\)) is formed. Thus, the correct answer is **D. a white precipitate would be formed**. ### Explanation of Other Options - **A. There would be no visible change**: This is incorrect because a visible precipitate (PbSO\(_4\)) is formed. - **B. A blue precipitate would be formed**: This is incorrect. While CuSO\(_4\) is blue, it does not form a blue precipitate with Pb(NO\(_3\))\(_2\). The precipitate formed is white (PbSO\(_4\)). - **C. The resulting solution would become colorless**: This is misleading. While the solution may appear less colored due to the formation of a white precipitate, the remaining solution will still contain Cu\(^{2+}\) ions, which impart a blue color to the solution. ### Revision Summary - When CuSO\(_4\) is mixed with Pb(NO\(_3\))\(_2\), a white precipitate of PbSO\(_4\) forms. - Lead(II) sulfate (PbSO\(_4\)) is insoluble in water, leading to the formation of a precipitate. - The other options are incorrect due to the formation of a visible precipitate and the nature of the ions involved. - Understanding solubility rules is crucial for predicting the outcomes of ionic reactions in solution.