The following chemical reaction takes place in aqueous solution: Zn (NO3), (aq)+2KOH(aq) → Zn(OH),(s)+2 KNO3(aq) Write the net ionic equation for this reaction.
The following chemical reaction takes place in aqueous solution: Zn (NO3), (aq)+2KOH(aq) → Zn(OH),(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
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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![**The following chemical reaction takes place in aqueous solution:**
\[ \text{Zn(NO}_3\text{)}_2\text{(aq)} + 2\text{KOH(aq)} \rightarrow \text{Zn(OH)}_2\text{(s)} + 2\text{KNO}_3\text{(aq)} \]
Write the net ionic equation for this reaction.
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*Explanation:*
This image shows a chemical equation involving zinc nitrate \(\text{Zn(NO}_3\text{)}_2\), potassium hydroxide \(\text{KOH}\), zinc hydroxide \(\text{Zn(OH)}_2\), and potassium nitrate \(\text{KNO}_3\). The equation indicates that zinc nitrate reacts with potassium hydroxide in an aqueous solution to form solid zinc hydroxide and aqueous potassium nitrate.
*Key Points:*
- **\((aq)\)** indicates that the substances are in aqueous solution (dissolved in water).
- **\((s)\)** denotes a solid, indicating that a precipitate forms.
- The task is to write the net ionic equation, which involves identifying the ions that participate in the reaction and omitting the spectator ions.
*Net Ionic Equation:*
To write the net ionic equation:
1. Break down the aqueous compounds into their respective ions.
2. Identify and remove the spectator ions (ions that appear unchanged on both sides of the equation).
3. The net ionic equation shows only the particles that participate in the reaction.
For this reaction, the steps are:
- **Complete Ionic Equation:**
\[ \text{Zn}^{2+}\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} + 2\text{K}^+\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Zn(OH)}_2\text{(s)} + 2\text{K}^+\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} \]
- **Net Ionic Equation:**
\[ \text{Zn}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Zn(OH)}_2\text{(s)} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe7541ca2-3bda-4c25-af18-40a3b11b7637%2Fe3509a3d-2fff-4f34-9e9a-b3851fbd423f%2Fb7a6vmp_processed.png&w=3840&q=75)
Transcribed Image Text:**The following chemical reaction takes place in aqueous solution:**
\[ \text{Zn(NO}_3\text{)}_2\text{(aq)} + 2\text{KOH(aq)} \rightarrow \text{Zn(OH)}_2\text{(s)} + 2\text{KNO}_3\text{(aq)} \]
Write the net ionic equation for this reaction.
---
*Explanation:*
This image shows a chemical equation involving zinc nitrate \(\text{Zn(NO}_3\text{)}_2\), potassium hydroxide \(\text{KOH}\), zinc hydroxide \(\text{Zn(OH)}_2\), and potassium nitrate \(\text{KNO}_3\). The equation indicates that zinc nitrate reacts with potassium hydroxide in an aqueous solution to form solid zinc hydroxide and aqueous potassium nitrate.
*Key Points:*
- **\((aq)\)** indicates that the substances are in aqueous solution (dissolved in water).
- **\((s)\)** denotes a solid, indicating that a precipitate forms.
- The task is to write the net ionic equation, which involves identifying the ions that participate in the reaction and omitting the spectator ions.
*Net Ionic Equation:*
To write the net ionic equation:
1. Break down the aqueous compounds into their respective ions.
2. Identify and remove the spectator ions (ions that appear unchanged on both sides of the equation).
3. The net ionic equation shows only the particles that participate in the reaction.
For this reaction, the steps are:
- **Complete Ionic Equation:**
\[ \text{Zn}^{2+}\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} + 2\text{K}^+\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Zn(OH)}_2\text{(s)} + 2\text{K}^+\text{(aq)} + 2\text{NO}_3^{-}\text{(aq)} \]
- **Net Ionic Equation:**
\[ \text{Zn}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Zn(OH)}_2\text{(s)} \]
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