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Chapter 10: Problem 60

Why would the pH of your blood plasma decrease if you hold your breath?

Short Answer

Expert verified
Holding breath increases CO2 in blood, producing more hydrogen ions, which decreases blood plasma pH.

Step by step solution

01

Identify the Components Involved

Understand that blood plasma pH is regulated by the concentration of carbon dioxide (CO2), bicarbonate (HCO3-), and hydrogen ions (H+).
02

Understand CO2 and pH Relationship

Recognize that CO2 reacts with water in the blood to form carbonic acid (H2CO3), which dissociates into bicarbonate (HCO3-) and hydrogen ions (H+): \( \text{CO}_2 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{CO}_3 \rightarrow \text{HCO}_3^- + \text{H}^+ \).
03

Analyze the Effect of Holding Breath

When you hold your breath, the level of CO2 in your blood increases because it is not being expelled through exhalation.
04

Relate Increased CO2 to pH

Increased CO2 leads to a higher concentration of carbonic acid, removing more bicarbonate ions and releasing more hydrogen ions, thereby decreasing the pH.
05

Conclusion

Therefore, holding your breath leads to an increase in CO2, which increases hydrogen ion concentration and results in a lower blood plasma pH.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Carbon Dioxide and Blood pH
Carbon dioxide (CO2) plays a key role in regulating the pH of your blood. When you breathe, CO2 is exchanged between your lungs and your blood. The amount of CO2 in your blood can affect its acidity or alkalinity.
  • CO2 combines with water (H2O) in your blood to form carbonic acid (H2CO3).
  • This carbonic acid quickly breaks down into bicarbonate ions (HCO3-) and hydrogen ions (H+).

The reaction can be summarized as: CO2 + H2O 鈫� H2CO3 鈫� HCO3- + H+

When you hold your breath, CO2 accumulates in your blood because it isn't being exhaled. This increase results in more carbonic acid and hydrogen ions being formed, thereby lowering the pH and making your blood more acidic.
Carbonic Acid-Bicarbonate Buffer System
The carbonic acid-bicarbonate buffer system is a crucial mechanism for maintaining a stable pH in your blood. It involves an equilibrium reaction that can

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Most popular questions from this chapter

Consider the buffer system of hydrofluoric acid, \(\mathrm{HF}\), and its salt, NaF. $$\mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{F}^{-}(a q)$$ a. The purpose of this buffer system is to: 1\. maintain [HF] 2\. maintain \(\left[\mathrm{F}^{-}\right]\) 3\. maintain \(\mathrm{pH}\) b. The salt of the weak acid is needed to: 1\. provide the conjugate base 2\. neutralize added \(\mathrm{H}_{3} \mathrm{O}^{+}\) 3\. provide the conjugate acid c. If \(\mathrm{OH}^{-}\) is added, it is neutralized by: 1\. the salt 2\. \(\mathrm{H}_{2} \mathrm{O}\) 3\. \(\mathrm{H}_{3} \mathrm{O}^{+}\) d. When \(\mathrm{H}_{3} \mathrm{O}^{+}\) is added, the equilibrium shifts in the direction of the: 1\. reactants 2\. products 3\. does not change

Which of the following are at equilibrium? a. The rate of the forward reaction is twice as fast as the rate of the reverse reaction. b. The concentrations of the reactants and the products do not change. c. The rate of the reverse reaction does not change.

Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting. (10.8) a. What changes occur in the blood pH during hyperventilation? b. How does breathing into a paper bag help return blood pH to normal?

Write formulas for each of the following acids and bases: a. barium hydroxide b. hydroiodic acid c. bromic acid d. strontium hydroxide e. acetic acid f. hypochlorous acid

State whether each of the following solutions is acidic, basic, or neutral: (10.6) a. saliva, \(\mathrm{pH} 6.8\) b. urine, pH 5.9 c. pancreatic juice, pH 8.0 d. bile, pH 8.4 e. blood, pH 7.45
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