Question

Ketoacidosis is relieved by rapid breathing, which converts hydrogen carbonate ions and hydrogen ions in the blood to gaseous carbon dioxide and water, as shown in this equation. $$ \mathrm{H}^{+}+\mathrm{HCO}_{3}^{-} \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2}(\text { Exhaled }) $$ (a) Assuming that these reactions can go in either direction, how does a state of acidosis help to increase the generation of carbon dioxide? (b) What principle describes the effect of added reactants and products on an equilibrium?

Name: Problem 16, Chapter 22: Fundamentals of General, Organic, and Biological Chemistry
Uploaded: 2022-01-11T16:46:44-08:00
Duration: 2 min 9 s
Channel: Shahina -

   Ketoacidosis is relieved by rapid breathing, which converts hydrogen carbonate ions and hydrogen ions in the blood to gaseous carbon dioxide and water, as shown in this equation.
$$
\mathrm{H}^{+}+\mathrm{HCO}_{3}^{-} \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2}(\text { Exhaled })
$$
(a) Assuming that these reactions can go in either direction, how does a state of acidosis help to increase the generation of carbon dioxide?
(b) What principle describes the effect of added reactants and products on an equilibrium?

Fundamentals of General, Organic, and Biological Chemistry

John McMurry, David… 1st Edition

Chapter 22, Problem 16

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Solved by Expert Shahina -

01/11/2022

Step 1

Step 1: The given reaction is: $$ \mathrm{H}^{+}+\mathrm{HCO}_{3}^{-} \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2}(\text { Exhaled }) $$ This reaction can go in either direction, meaning it can proceed Show more…

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Ketoacidosis is relieved by rapid breathing, which converts hydrogen carbonate ions and hydrogen ions in the blood to gaseous carbon dioxide and water, as shown in this equation. $$ \mathrm{H}^{+}+\mathrm{HCO}_{3}^{-} \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2}(\text { Exhaled }) $$ (a) Assuming that these reactions can go in either direction, how does a state of acidosis help to increase the generation of carbon dioxide? (b) What principle describes the effect of added reactants and products on an equilibrium?

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Key Concepts

Bicarbonate Buffer System

The bicarbonate buffer system is the primary mechanism for regulating blood pH. It operates through the reversible reaction where hydrogen ions (H+) combine with bicarbonate ions (HCO3-) to form carbonic acid (H2CO3), which then decomposes into water and carbon dioxide. This equilibrium helps to maintain a stable pH in the blood by shifting in response to changes in hydrogen ion concentration.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system adjusts to partially counteract the disturbance and a new equilibrium is established. In the context of acid-base chemistry, an increase in hydrogen ion concentration (acidosis) shifts the equilibrium towards the production of carbonic acid, which then decomposes to water and carbon dioxide, thereby helping to alleviate the acidosis.

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