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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In the following reaction, label the acid, base, conjugate acid, and conjugate base and state why that's the case.
![### Acid-Base Reaction: Interaction of Water and Acetate Ion
**Chemical Equation:**
\[ \mathrm{H_2O + CH_3COO^- \longrightarrow CH_3COOH + OH^-} \]
### Description:
This chemical equation represents the reaction between water (H₂O) and the acetate ion (CH₃COO⁻). In this reaction, the acetate ion reacts with water, yielding acetic acid (CH₃COOH) and hydroxide ion (OH⁻).
### Detailed Explanation:
1. **Reactants**:
- **Water (H₂O)**: A neutral molecule essential to many chemical reactions.
- **Acetate Ion (CH₃COO⁻)**: A negatively charged ion derived from acetic acid (CH₃COOH).
2. **Products**:
- **Acetic Acid (CH₃COOH)**: A weak organic acid commonly found in vinegar.
- **Hydroxide Ion (OH⁻)**: A negatively charged ion that makes solutions basic or alkaline.
### Reaction Dynamics:
This reaction is an example of a Bronsted-Lowry acid-base reaction where:
- Water (H₂O) acts as the acid, donating a proton (H⁺).
- The acetate ion (CH₃COO⁻) acts as the base, accepting a proton.
The equilibrium position of this reaction lies toward the left due to the weak acidity of acetic acid.
### Importance:
Understanding this reaction is crucial when analyzing the behavior of weak acids and bases in aqueous solutions. It exemplifies how conjugate acid-base pairs interact with water and highlights the concept of chemical equilibrium in acid-base chemistry.
### Visual Explanation:
**Equation Representation**:
\[ \mathrm{H_2O + CH_3COO^- \longrightarrow CH_3COOH + OH^-} \]
- **Left Side**: Reactants, including water and acetate ion.
- **Right Side**: Products, including acetic acid and hydroxide ion.
Such chemical equations are fundamental in understanding the nature of reactions, predicting product formation, and balancing chemical reactions in various fields of science and engineering.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F277d8e9e-796c-4923-a9a2-4c05d5ad95df%2F0e4ec6e1-4356-4c40-8e44-57f6e0f59102%2F177zsm8_processed.png&w=3840&q=75)
Transcribed Image Text:### Acid-Base Reaction: Interaction of Water and Acetate Ion
**Chemical Equation:**
\[ \mathrm{H_2O + CH_3COO^- \longrightarrow CH_3COOH + OH^-} \]
### Description:
This chemical equation represents the reaction between water (H₂O) and the acetate ion (CH₃COO⁻). In this reaction, the acetate ion reacts with water, yielding acetic acid (CH₃COOH) and hydroxide ion (OH⁻).
### Detailed Explanation:
1. **Reactants**:
- **Water (H₂O)**: A neutral molecule essential to many chemical reactions.
- **Acetate Ion (CH₃COO⁻)**: A negatively charged ion derived from acetic acid (CH₃COOH).
2. **Products**:
- **Acetic Acid (CH₃COOH)**: A weak organic acid commonly found in vinegar.
- **Hydroxide Ion (OH⁻)**: A negatively charged ion that makes solutions basic or alkaline.
### Reaction Dynamics:
This reaction is an example of a Bronsted-Lowry acid-base reaction where:
- Water (H₂O) acts as the acid, donating a proton (H⁺).
- The acetate ion (CH₃COO⁻) acts as the base, accepting a proton.
The equilibrium position of this reaction lies toward the left due to the weak acidity of acetic acid.
### Importance:
Understanding this reaction is crucial when analyzing the behavior of weak acids and bases in aqueous solutions. It exemplifies how conjugate acid-base pairs interact with water and highlights the concept of chemical equilibrium in acid-base chemistry.
### Visual Explanation:
**Equation Representation**:
\[ \mathrm{H_2O + CH_3COO^- \longrightarrow CH_3COOH + OH^-} \]
- **Left Side**: Reactants, including water and acetate ion.
- **Right Side**: Products, including acetic acid and hydroxide ion.
Such chemical equations are fundamental in understanding the nature of reactions, predicting product formation, and balancing chemical reactions in various fields of science and engineering.
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