A solution contains one or more of the following ions: Ag⁺ , Ca²⁺ , and Cu²⁺ . When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Write net ionic equations for the formation of each of the precipitates observed.

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Identify the ions present in the solution: Ag^{+}, Ca^{2+}, and Cu^{2+}.

Determine the solubility rules for the ions with the added reagents: NaCl, Na_2SO_4, and Na_2CO_3.

Since no precipitate forms with NaCl, AgCl is not formed, indicating Ag^{+} is not present.

When Na_2SO_4 is added, a white precipitate forms, indicating the formation of CaSO_4. Write the net ionic equation: Ca^{2+} (aq) + SO_4^{2-} (aq) \rightarrow CaSO_4 (s).

After filtering, adding Na_2CO_3 results in another precipitate, indicating the formation of CuCO_3. Write the net ionic equation: Cu^{2+} (aq) + CO_3^{2-} (aq) \rightarrow CuCO_3 (s).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility Rules

Solubility rules are guidelines that help predict whether a compound will dissolve in water. For example, most chlorides are soluble, except for those of silver, lead, and mercury. In contrast, sulfates are generally soluble, but barium, lead, and calcium sulfates are exceptions. Understanding these rules is crucial for determining which ions will precipitate when mixed.

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble compound, known as a precipitate. This process can be represented by net ionic equations, which focus on the ions that participate in the formation of the precipitate. Identifying the ions involved and their solubility is essential for writing accurate equations.

Net Ionic Equations

Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions that do not change during the reaction. To write a net ionic equation, one must first identify the reactants, determine the products, and then eliminate the ions that remain unchanged. This simplification helps clarify the essential chemical changes occurring in the solution.

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Net Ionic Equations

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