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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Question
Would this equation shift left or right?
![**Carbon Dioxide and Bicarbonate Equilibrium Reaction**
This equation illustrates the chemical equilibrium involving carbon dioxide, water, carbonic acid, protons, and bicarbonate ions. It is a crucial reaction in maintaining acid-base balance in biological systems.
**Equation:**
\[ \text{CO}_2 + \text{H}_2\text{O} \rightleftharpoons \text{H}_2\text{CO}_3 \rightleftharpoons \text{H}^+ + \text{HCO}_3^- \]
**Explanation:**
1. **Reactants:**
- \(\text{CO}_2\) (carbon dioxide) combines with \(\text{H}_2\text{O}\) (water).
2. **Intermediates and Products:**
- The combination forms \(\text{H}_2\text{CO}_3\) (carbonic acid), which is unstable.
- \(\text{H}_2\text{CO}_3\) dissociates into \(\text{H}^+\) (protons) and \(\text{HCO}_3^-\) (bicarbonate ions).
3. **Reversible Reaction:**
- The arrows indicate that this is a reversible reaction, where the products can revert to reactants. The system reaches equilibrium between the two sides, balancing the concentrations based on conditions like pH and CO₂ levels.
This reaction is integral to the physiological buffering system that manages the pH of blood and other fluids in the body.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc62819af-1f81-4d59-bfb3-1ca1702855ed%2Fd50b0271-a76f-493f-b0b6-e3347ec7ece0%2Fehqffn_processed.png&w=3840&q=75)
Transcribed Image Text:**Carbon Dioxide and Bicarbonate Equilibrium Reaction**
This equation illustrates the chemical equilibrium involving carbon dioxide, water, carbonic acid, protons, and bicarbonate ions. It is a crucial reaction in maintaining acid-base balance in biological systems.
**Equation:**
\[ \text{CO}_2 + \text{H}_2\text{O} \rightleftharpoons \text{H}_2\text{CO}_3 \rightleftharpoons \text{H}^+ + \text{HCO}_3^- \]
**Explanation:**
1. **Reactants:**
- \(\text{CO}_2\) (carbon dioxide) combines with \(\text{H}_2\text{O}\) (water).
2. **Intermediates and Products:**
- The combination forms \(\text{H}_2\text{CO}_3\) (carbonic acid), which is unstable.
- \(\text{H}_2\text{CO}_3\) dissociates into \(\text{H}^+\) (protons) and \(\text{HCO}_3^-\) (bicarbonate ions).
3. **Reversible Reaction:**
- The arrows indicate that this is a reversible reaction, where the products can revert to reactants. The system reaches equilibrium between the two sides, balancing the concentrations based on conditions like pH and CO₂ levels.
This reaction is integral to the physiological buffering system that manages the pH of blood and other fluids in the body.
Expert Solution
Step 1: Concept of Carbonic acid
We know an acid is a substance which dissociate to give H+ ion . Carbonic acid is a weak acid .
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