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CO,+H20+ HCO3 → H+ + HCO3

CO,+H20+ HCO3 → H+ + HCO3

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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What changes would you see in pH? 

The image presents a chemical equilibrium reaction involving carbon dioxide (CO₂) and water (H₂O), which interact to form carbonic acid (H₂CO₃). This reaction is in dynamic equilibrium, as indicated by the double arrows between the reactants and products. In the next step of the reaction, carbonic acid dissociates into hydrogen ions (H⁺) and bicarbonate ions (HCO₃⁻), also shown by double arrows indicating a state of equilibrium. This reaction is significant in many biological and environmental processes, such as respiratory gas exchange and the buffering of blood pH. Understanding this equilibrium is crucial for comprehending how carbon dioxide is transported in the bloodstream and how it affects the acid-base balance in various systems.
Transcribed Image Text:The image presents a chemical equilibrium reaction involving carbon dioxide (CO₂) and water (H₂O), which interact to form carbonic acid (H₂CO₃). This reaction is in dynamic equilibrium, as indicated by the double arrows between the reactants and products. In the next step of the reaction, carbonic acid dissociates into hydrogen ions (H⁺) and bicarbonate ions (HCO₃⁻), also shown by double arrows indicating a state of equilibrium. This reaction is significant in many biological and environmental processes, such as respiratory gas exchange and the buffering of blood pH. Understanding this equilibrium is crucial for comprehending how carbon dioxide is transported in the bloodstream and how it affects the acid-base balance in various systems.
Expert Solution
Step 1: The bicarbonate buffer

Here, we are given the reaction taking place in the bicarbonate buffer. Blood plasma is buffered mainly by this buffering system. The enzyme that catalyzes the reversible reaction of the bicarbonate buffer is carbonic anhydrase. The pH changes depending on which side of the reaction the equilibrium lies.

Remember, when H+ concentration increases, pH decreases and vice-versa.

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