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. c. Fe(NO3)2(𝑎𝑞)+KOH(𝑎𝑞)⟶

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Write the balanced molecular equation for the reaction: \[ \text{Fe(NO}_3\text{)}_2(\text{aq}) + 2\text{KOH}(\text{aq}) \rightarrow \text{Fe(OH)}_2(\text{s}) + 2\text{KNO}_3(\text{aq}) \]

Identify the states of matter for each compound: Fe(NO3)2 and KOH are aqueous, Fe(OH)2 is a solid (precipitate), and KNO3 is aqueous.

Write the complete ionic equation by separating all aqueous compounds into their ions: \[ \text{Fe}^{2+}(\text{aq}) + 2\text{NO}_3^{-}(\text{aq}) + 2\text{K}^+(\text{aq}) + 2\text{OH}^-(\text{aq}) \rightarrow \text{Fe(OH)}_2(\text{s}) + 2\text{K}^+(\text{aq}) + 2\text{NO}_3^{-}(\text{aq}) \]

Identify and cancel out the spectator ions, which are ions that appear on both sides of the equation without undergoing any change. In this case, the spectator ions are \( \text{K}^+ \) and \( \text{NO}_3^- \).

Write the net ionic equation by removing the spectator ions: \[ \text{Fe}^{2+}(\text{aq}) + 2\text{OH}^-(\text{aq}) \rightarrow \text{Fe(OH)}_2(\text{s}) \]

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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 omitted when writing net ionic equations. 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. Understanding solubility is essential for determining the states of reactants and products in a reaction, which is necessary for writing balanced equations.

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Solubility Rules

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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)⟶

Textbook Question

Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?

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Textbook Question

You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3,CaCl2, or Al2(SO4)3. You take a portion of the solution and add an aqueous solution of Ba(NO3)2 to it, and observe that a white solid precipitates Then you take another portion of the unlabeled solution and add an aqueous solution of NaCl to it; nothing appears to happen. What is the most likely identity of the solution in the unlabeled bottle: silver nitrate, calcium chloride, aluminum sulfate?