The following chemical reaction takes place in aqueous solution: 2 AgNO3(aq)+K₂CO3(aq) - → Ag₂CO3(s)+2 KNO3(aq) Write the net ionic equation for this reaction.
The following chemical reaction takes place in aqueous solution: 2 AgNO3(aq)+K₂CO3(aq) - → Ag₂CO3(s)+2 KNO3(aq) Write the net ionic equation for this reaction.
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
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![### Net Ionic Equation for the Reaction
**Chemical Reaction:**
\[ 2 \text{AgNO}_3(\text{aq}) + \text{K}_2\text{CO}_3(\text{aq}) \rightarrow \text{Ag}_2\text{CO}_3(\text{s}) + 2 \text{KNO}_3(\text{aq}) \]
**Task:**
Write the net ionic equation for this reaction.
**Explanation:**
When writing the net ionic equation, we follow these steps:
1. **Write the Balanced Molecular Equation:**
\[ 2 \text{AgNO}_3(\text{aq}) + \text{K}_2\text{CO}_3(\text{aq}) \rightarrow \text{Ag}_2\text{CO}_3(\text{s}) + 2 \text{KNO}_3(\text{aq}) \]
2. **Dissociate All Strong Electrolytes into Their Ions:**
- \( 2 \text{AgNO}_3(\text{aq}) \) dissociates into \( 2 \text{Ag}^+(\text{aq}) + 2 \text{NO}_3^-(\text{aq}) \)
- \( \text{K}_2\text{CO}_3(\text{aq}) \) dissociates into \( 2 \text{K}^+(\text{aq}) + \text{CO}_3^{2-}(\text{aq}) \)
- \( 2 \text{KNO}_3(\text{aq}) \) dissociates into \( 2 \text{K}^+(\text{aq}) + 2 \text{NO}_3^-(\text{aq}) \)
3. **Identify the Spectator Ions:**
Spectator ions are those that do not participate in the reaction. They appear unchanged on both the reactant and product sides.
- In this case, the spectator ions are \( 2 \text{K}^+ \) and \( 2 \text{NO}_3^- \).
4. **Write the Net Ionic Equation:**
Remove the spectator ions, and write only the ions and compounds directly involved in the reaction.
- The net ionic equation is:
\[ 2 \text{Ag}^+(\text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F621954ed-ec20-4c07-b25b-e8811e0f0e49%2F1662adcb-355f-4b88-9ac2-07f80b22999b%2Fdhagrpl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Net Ionic Equation for the Reaction
**Chemical Reaction:**
\[ 2 \text{AgNO}_3(\text{aq}) + \text{K}_2\text{CO}_3(\text{aq}) \rightarrow \text{Ag}_2\text{CO}_3(\text{s}) + 2 \text{KNO}_3(\text{aq}) \]
**Task:**
Write the net ionic equation for this reaction.
**Explanation:**
When writing the net ionic equation, we follow these steps:
1. **Write the Balanced Molecular Equation:**
\[ 2 \text{AgNO}_3(\text{aq}) + \text{K}_2\text{CO}_3(\text{aq}) \rightarrow \text{Ag}_2\text{CO}_3(\text{s}) + 2 \text{KNO}_3(\text{aq}) \]
2. **Dissociate All Strong Electrolytes into Their Ions:**
- \( 2 \text{AgNO}_3(\text{aq}) \) dissociates into \( 2 \text{Ag}^+(\text{aq}) + 2 \text{NO}_3^-(\text{aq}) \)
- \( \text{K}_2\text{CO}_3(\text{aq}) \) dissociates into \( 2 \text{K}^+(\text{aq}) + \text{CO}_3^{2-}(\text{aq}) \)
- \( 2 \text{KNO}_3(\text{aq}) \) dissociates into \( 2 \text{K}^+(\text{aq}) + 2 \text{NO}_3^-(\text{aq}) \)
3. **Identify the Spectator Ions:**
Spectator ions are those that do not participate in the reaction. They appear unchanged on both the reactant and product sides.
- In this case, the spectator ions are \( 2 \text{K}^+ \) and \( 2 \text{NO}_3^- \).
4. **Write the Net Ionic Equation:**
Remove the spectator ions, and write only the ions and compounds directly involved in the reaction.
- The net ionic equation is:
\[ 2 \text{Ag}^+(\text{
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