Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. a. Cr2(SO4)3(𝑎𝑞)+(NH4)2CO3(𝑎𝑞)⟶

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Identify the ions present in each compound: \( \text{Cr}_2(\text{SO}_4)_3 \) dissociates into \( 2\text{Cr}^{3+} \) and \( 3\text{SO}_4^{2-} \); \( (\text{NH}_4)_2\text{CO}_3 \) dissociates into \( 2\text{NH}_4^+ \) and \( \text{CO}_3^{2-} \).

Determine the possible products of the reaction: \( \text{Cr}_2(\text{CO}_3)_3 \) and \( \text{(NH}_4)_2\text{SO}_4 \).

Check the solubility of the products: \( \text{Cr}_2(\text{CO}_3)_3 \) is insoluble, forming a precipitate, while \( \text{(NH}_4)_2\text{SO}_4 \) is soluble.

Write the balanced molecular equation: \( \text{Cr}_2(\text{SO}_4)_3(\text{aq}) + 3(\text{NH}_4)_2\text{CO}_3(\text{aq}) \rightarrow \text{Cr}_2(\text{CO}_3)_3(\text{s}) + 3\text{(NH}_4)_2\text{SO}_4(\text{aq}) \).

Write the net ionic equation by removing spectator ions: \( 2\text{Cr}^{3+}(\text{aq}) + 3\text{CO}_3^{2-}(\text{aq}) \rightarrow \text{Cr}_2(\text{CO}_3)_3(\text{s}) \). Spectator ions are \( \text{NH}_4^+ \) and \( \text{SO}_4^{2-} \).

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Key Concepts

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

Net Ionic Equations

Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions. To write a net ionic equation, one must first write the balanced molecular equation, then dissociate all soluble ionic compounds into their constituent ions, and finally eliminate the spectator ions that do not change during the reaction.

Spectator Ions

Spectator ions are ions that exist in the same form on both the reactant and product sides of a chemical equation. They do not participate in the actual chemical reaction and can be removed from the net ionic equation. Identifying spectator ions is crucial for simplifying the equation to focus on the species that undergo a change.

Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. These rules indicate which ions are generally soluble or insoluble in aqueous solutions, which is essential for determining the reactants and products in a reaction, as well as for identifying the ions that will remain in solution versus those that will precipitate.

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Solubility Rules

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