**Title: Understanding Ionic and Net Ionic Equations** **Complete Ionic and Net Ionic Equations for the Following Reaction** This exercise involves writing the complete ionic and net ionic equations for the given chemical reaction: \[ \text{Pb(NO}_3\text{)}_2\text{(aq)} + 2\text{KOH(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{KNO}_3\text{(aq)} \] ### Explanation: 1. **Reactants:** - **Pb(NO₃)₂(aq):** Lead (II) nitrate is in aqueous form, meaning it disassociates into ions in water. - **2KOH(aq):** Potassium hydroxide is also in aqueous form, disassociating into potassium (K⁺) and hydroxide (OH⁻) ions. 2. **Products:** - **Pb(OH)₂(s):** Lead (II) hydroxide is a solid, indicating a precipitate formation, which is a key part of identifying the net ionic equation. - **2KNO₃(aq):** Potassium nitrate remains in aqueous solution, disassociating into potassium (K⁺) and nitrate (NO₃⁻) ions. ### Writing the Equations: - **Complete Ionic Equation:** Break all aqueous compounds into their respective ions: \[ \text{Pb}^{2+}\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} + 2\text{K}^+\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{K}^+\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} \] - **Net Ionic Equation:** Remove the spectator ions (ions that appear on both sides of the equation) - potassium (K⁺) and nitrate (NO₃⁻): \[ \text{Pb}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} \] In the net
**Title: Understanding Ionic and Net Ionic Equations** **Complete Ionic and Net Ionic Equations for the Following Reaction** This exercise involves writing the complete ionic and net ionic equations for the given chemical reaction: \[ \text{Pb(NO}_3\text{)}_2\text{(aq)} + 2\text{KOH(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{KNO}_3\text{(aq)} \] ### Explanation: 1. **Reactants:** - **Pb(NO₃)₂(aq):** Lead (II) nitrate is in aqueous form, meaning it disassociates into ions in water. - **2KOH(aq):** Potassium hydroxide is also in aqueous form, disassociating into potassium (K⁺) and hydroxide (OH⁻) ions. 2. **Products:** - **Pb(OH)₂(s):** Lead (II) hydroxide is a solid, indicating a precipitate formation, which is a key part of identifying the net ionic equation. - **2KNO₃(aq):** Potassium nitrate remains in aqueous solution, disassociating into potassium (K⁺) and nitrate (NO₃⁻) ions. ### Writing the Equations: - **Complete Ionic Equation:** Break all aqueous compounds into their respective ions: \[ \text{Pb}^{2+}\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} + 2\text{K}^+\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{K}^+\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} \] - **Net Ionic Equation:** Remove the spectator ions (ions that appear on both sides of the equation) - potassium (K⁺) and nitrate (NO₃⁻): \[ \text{Pb}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} \] In the net
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Title: Understanding Ionic and Net Ionic Equations**
**Complete Ionic and Net Ionic Equations for the Following Reaction**
This exercise involves writing the complete ionic and net ionic equations for the given chemical reaction:
\[ \text{Pb(NO}_3\text{)}_2\text{(aq)} + 2\text{KOH(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{KNO}_3\text{(aq)} \]
### Explanation:
1. **Reactants:**
- **Pb(NO₃)₂(aq):** Lead (II) nitrate is in aqueous form, meaning it disassociates into ions in water.
- **2KOH(aq):** Potassium hydroxide is also in aqueous form, disassociating into potassium (K⁺) and hydroxide (OH⁻) ions.
2. **Products:**
- **Pb(OH)₂(s):** Lead (II) hydroxide is a solid, indicating a precipitate formation, which is a key part of identifying the net ionic equation.
- **2KNO₃(aq):** Potassium nitrate remains in aqueous solution, disassociating into potassium (K⁺) and nitrate (NO₃⁻) ions.
### Writing the Equations:
- **Complete Ionic Equation:**
Break all aqueous compounds into their respective ions:
\[ \text{Pb}^{2+}\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} + 2\text{K}^+\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{K}^+\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} \]
- **Net Ionic Equation:**
Remove the spectator ions (ions that appear on both sides of the equation) - potassium (K⁺) and nitrate (NO₃⁻):
\[ \text{Pb}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} \]
In the net](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F377a7caf-b074-415b-a7a2-489899521086%2F06589245-11da-420a-87a9-31cc0d3ca683%2F8xk02so.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Understanding Ionic and Net Ionic Equations**
**Complete Ionic and Net Ionic Equations for the Following Reaction**
This exercise involves writing the complete ionic and net ionic equations for the given chemical reaction:
\[ \text{Pb(NO}_3\text{)}_2\text{(aq)} + 2\text{KOH(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{KNO}_3\text{(aq)} \]
### Explanation:
1. **Reactants:**
- **Pb(NO₃)₂(aq):** Lead (II) nitrate is in aqueous form, meaning it disassociates into ions in water.
- **2KOH(aq):** Potassium hydroxide is also in aqueous form, disassociating into potassium (K⁺) and hydroxide (OH⁻) ions.
2. **Products:**
- **Pb(OH)₂(s):** Lead (II) hydroxide is a solid, indicating a precipitate formation, which is a key part of identifying the net ionic equation.
- **2KNO₃(aq):** Potassium nitrate remains in aqueous solution, disassociating into potassium (K⁺) and nitrate (NO₃⁻) ions.
### Writing the Equations:
- **Complete Ionic Equation:**
Break all aqueous compounds into their respective ions:
\[ \text{Pb}^{2+}\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} + 2\text{K}^+\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} + 2\text{K}^+\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} \]
- **Net Ionic Equation:**
Remove the spectator ions (ions that appear on both sides of the equation) - potassium (K⁺) and nitrate (NO₃⁻):
\[ \text{Pb}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Pb(OH)}_2\text{(s)} \]
In the net
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