A solution contains one or more of the following ions: Hg₂²⁺, Ba²⁺, and Fe²⁺. When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Write net ionic equations for the formation of each of the precipitates observed.

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Identify the ions present in the solution: Hg_2^{2+}, Ba^{2+}, and Fe^{2+}.

Add potassium chloride (KCl) to the solution. The chloride ions (Cl^-) will react with Hg_2^{2+} to form a precipitate of mercury(I) chloride (Hg_2Cl_2). Write the net ionic equation: Hg_2^{2+} (aq) + 2Cl^- (aq) -> Hg_2Cl_2 (s).

Filter off the precipitate and add potassium sulfate (K_2SO_4) to the remaining solution. Since no precipitate forms, Ba^{2+} ions are not present in the solution, as barium sulfate (BaSO_4) would have precipitated.

Add potassium carbonate (K_2CO_3) to the remaining solution. The carbonate ions (CO_3^{2-}) will react with Fe^{2+} to form a precipitate of iron(II) carbonate (FeCO_3). Write the net ionic equation: Fe^{2+} (aq) + CO_3^{2-} (aq) -> FeCO_3 (s).

Summarize the net ionic equations for the precipitates: 1) Hg_2^{2+} (aq) + 2Cl^- (aq) -> Hg_2Cl_2 (s), 2) Fe^{2+} (aq) + CO_3^{2-} (aq) -> FeCO_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 sulfate is an exception. 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 reaction.

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Textbook Question

A solution contains one or more of the following ions: Hg₂²⁺ , Ba²⁺ , and Fe²⁺ . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Which ions were present in the original solution?

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