Q: Given the equation $$pH = -\log_{10}[H^+]$$, what is the hydrogen ion concentration $$[H^+] of a $$solution with a pH of 4?

$$[H^+] = 1 \times 10$$^{-4}$$ M

Question 1

Which of the following statements best describes the relationship between hydrogen ion concentration and pH, as shown in the pH scale image?

Accepted Answer

As [H+] increases, pH decreases.

Question 2

A solution with a pH of 3 is how many times more acidic than a solution with a pH of 6?

Accepted Answer

1000 times

Question 3

Given the equation $$pH = -\log_{10}[H^+]$$, what is the hydrogen ion concentration $$[H^+] of a $$solution with a pH of 4?

Accepted Answer

$$[H^+] = 1 	imes 10$$^{-4}$$ M

Question 4

If a patient’s blood pH drops from 7.4 to 7.1, what happens to the hydrogen ion concentration?

Accepted Answer

It increases by a factor of $$10^{0.3} ($$about 2 times)

Question 5

Which of the following best explains why strong acids have a greater effect on pH than weak acids at the same concentration?

Accepted Answer

Strong acids fully dissociate, releasing more $$H^+$$ ions.

Question 6

A buffer solution contains a weak acid and its conjugate base. What happens when a small amount of strong acid is added to this buffer?

Accepted Answer

The buffer neutralizes the added acid, so pH changes very little.

Question 7

Which equation correctly represents the dissociation of carbonic acid in the body’s buffer system?

Accepted Answer

$$H_2CO_3 \rightleftharpoons $$HCO_3$$^- + H^+$$

Question 8

A patient is experiencing respiratory alkalosis due to hyperventilation. Which of the following compensatory mechanisms would the kidneys use?

Accepted Answer

Retain more $$H^+$$ and excrete $$HCO_3$$^-$$

Question 9

If a buffer solution has a pKa of 6.35, what happens to its buffering capacity if the pH is raised to 8.0?

Accepted Answer

Buffering capacity decreases because the acid form is depleted

Question 10

Which of the following scenarios would most likely result in metabolic acidosis?

Accepted Answer

Strenuous exercise

Question 11

During rebreathing, $$CO_2$$ levels in the blood increase. According to the equilibrium $$CO_2 + H_2O$$ \rightleftharpoons H_2CO_3 \rightleftharpoons $$HCO_3^- + H$$^+$$, what is the effect on blood pH?

Accepted Answer

Blood pH decreases (becomes more acidic)

Question 12

Which of the following best describes the role of the respiratory system in acid-base balance?

Accepted Answer

It rapidly adjusts blood pH by altering $$CO_2$$ exhalation.

Question 13

A patient with metabolic alkalosis has a blood pH of 7.55. How would the lungs compensate for this condition?

Accepted Answer

Decrease breathing rate to retain more $$CO_2$$

Question 14

Which of the following is true regarding buffer capacity?

Accepted Answer

It increases with higher concentrations of buffer components.

Question 15

If a solution has a pH of 9, how would you classify it based on the pH scale image?

Accepted Answer

Weakly alkaline

Question 16

Which of the following best explains why the pH of a buffer solution remains relatively constant when small amounts of acid or base are added?

Accepted Answer

The buffer contains a weak acid and its conjugate base, which neutralize added acids or bases.

Question 17

A patient with ketoacidosis is likely to have which of the following acid-base imbalances?

Accepted Answer

Metabolic acidosis

Question 18

Which of the following equations correctly shows the relationship between pH and hydrogen ion concentration?

Accepted Answer

$$pH = -\log_{10}[H^+]$$

Question 19

If the concentration of $$H^+ in a $$solution is $$1 	imes 10$$^{-7}$$ M, what is the pH of the solution?

Accepted Answer

pH = 7

Question 20

Which of the following is a likely cause of metabolic alkalosis?

Accepted Answer

Antacid overdose

Acid-Base Balance and Buffer Systems in Human Physiology

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