Question 1

Which of the following best describes the role of the carbonic acid-bicarbonate buffer system depicted in the image?

Accepted Answer

It maintains blood pH by converting strong acids and bases into weak ones, minimizing changes in pH.

Question 2

If a patient experiences a sudden drop in blood pH, which direction will the equilibrium in the buffer system shift according to Le Chatelier's principle?

Accepted Answer

Toward the formation of more $$\mathrm{H_2CO_3} to $$consume excess $$\mathrm{H^+}.$$

Question 3

What would happen if the concentration of $$\mathrm{$$HCO_3$$^-} in $$the blood decreased significantly?

Accepted Answer

The blood would become more acidic, as there would be less buffer to neutralize excess $$\mathrm{H^+}.$$

Question 4

Which of the following equations correctly represents the dissociation of carbonic acid in the buffer system?

Accepted Answer

$$\mathrm{H_2CO_3 \rightarrow $$HCO_3$$^- + H^+}$$

Question 5

A patient is hyperventilating, causing excessive loss of $$\mathrm{CO_2$}. $$How does this affect the buffer system?

Accepted Answer

It shifts the equilibrium to the left, decreasing $$\mathrm{H^+}$$ concentration and increasing blood pH.

Question 6

Which component in the buffer system acts as a weak acid?

Accepted Answer

$$\mathrm{H_2CO_3}$$

Question 7

If a patient’s blood pH rises above normal, what is the immediate response of the buffer system?

Accepted Answer

$$\mathrm{H_2CO_3}$$ dissociates to release $$\mathrm{H^+}$$, lowering the pH.

Question 8

Which organ systems are primarily responsible for regulating the components of the carbonic acid-bicarbonate buffer system?

Accepted Answer

The respiratory and urinary systems

Question 9

Why is the carbonic acid-bicarbonate buffer system considered an effective buffer in blood?

Accepted Answer

Because it can both donate and accept $$\mathrm{H^+}$$ ions, minimizing pH changes.

Question 10

Which of the following best explains what happens during a neutralization reaction involving this buffer system?

Accepted Answer

$$\mathrm{H^+}$$ from a strong acid combines with $$\mathrm{$$HCO_3$$^-} to $$form $$\mathrm{H_2CO_3}$$, which then dissociates into $$\mathrm{CO_2$}$$ and $$\mathrm{H_2O}.$$

Biochemistry: Chemistry Comes Alive (Anatomy & Physiology Study Notes)

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