Question 1

Which of the following variables are computed by the H-H equation?
I.pK
II.pH
III.HCO3-
IV.PCO2

Accepted Answer

A)  I, II 
B)  III, IV 
C)  II, IV 
D)  II, III, IV 
A)  I, II 
B)  III, IV 
C)  II, IV 
D)  II, III, IV D

Question 2

Which of the following systems has the greatest buffering capacity?

Accepted Answer

A)  Hb 
B)  HCO3- 
C)  Organic phosphates 
D)  Plasma proteins 
A)  Hb 
B)  HCO3- 
C)  Organic phosphates 
D)  Plasma proteins B

Question 3

Which of the following are examples of a fixed acid?
I.Carbonic acid
II.Lactic acid
III.Phosphoric acid
IV.Sulfuric acid

Accepted Answer

A)  I, II 
B)  III, IV 
C)  II, IV 
D)  II, III, IV 
A)  I, II 
B)  III, IV 
C)  II, IV 
D)  II, III, IV D

Question 4

Which of the following nonbicarbonate buffers is the most important?

Accepted Answer

A)  Hb 
B)  HCO3- 
C)  Organic phosphates 
D)  Plasma proteins 
A)  Hb 
B)  HCO3- 
C)  Organic phosphates 
D)  Plasma proteins

Question 5

Which of the following is considered a rapid compensatory mechanism to restore the pH back to normal levels in the presence of a metabolic acidosis?

Accepted Answer

A)  CO2 retention 
B)  CO2 elimination 
C)  HCO3- retention 
D)  HCO3- elimination 
A)  CO2 retention 
B)  CO2 elimination 
C)  HCO3- retention 
D)  HCO3- elimination

Question 6

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO2 rise to a level of 60 mm Hg will be associated with which of the following changes in the [HCO3-]?

Accepted Answer

A)  [HCO3-] rises to approximately 34 mEq/L. 
B)  [HCO3-] rises to approximately 31 mEq/L. 
C)  [HCO3-] rises to approximately 26 mEq/L. 
D)  [HCO3-] rises to approximately 25 mEq/L. 
A)  [HCO3-] rises to approximately 34 mEq/L. 
B)  [HCO3-] rises to approximately 31 mEq/L. 
C)  [HCO3-] rises to approximately 26 mEq/L. 
D)  [HCO3-] rises to approximately 25 mEq/L.

Question 7

A young, previously healthy drug overdose victim with severely depressed ventilation enters the emergency room with the following arterial blood gases: pH = 7.22, PaCO2 = 70 mm Hg, HCO3-= 28 mEq/L.What is the acid-base disturbance of this victim?

Accepted Answer

A)  Uncompensated respiratory acidosis 
B)  Compensated respiratory acidosis 
C)  Uncompensated respiratory alkalosis 
D)  Uncompensated metabolic acidosis 
A)  Uncompensated respiratory acidosis 
B)  Compensated respiratory acidosis 
C)  Uncompensated respiratory alkalosis 
D)  Uncompensated metabolic acidosis

Question 8

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO2 rise of 10 mm Hg will be associated with which of the following changes?

Accepted Answer

A)  [HCO3-] rises by approximately 10 mEq/L. 
B)  [HCO3-] rises by approximately 5 mEq/L. 
C)  [HCO3-] rises by approximately 2 mEq/L. 
D)  [HCO3-] rises by approximately 1 mEq/L. 
A)  [HCO3-] rises by approximately 10 mEq/L. 
B)  [HCO3-] rises by approximately 5 mEq/L. 
C)  [HCO3-] rises by approximately 2 mEq/L. 
D)  [HCO3-] rises by approximately 1 mEq/L.

Question 9

Which of the following is the only volatile acid of physiological significance in the body?

Accepted Answer

A)  Carbonic acid 
B)  Lactic acid 
C)  Phosphoric acid 
D)  Sulfuric acid 
A)  Carbonic acid 
B)  Lactic acid 
C)  Phosphoric acid 
D)  Sulfuric acid

Question 10

Which of the following disturbances in the pH may potentially occur in patients with nasogastric suction catheters?

Accepted Answer

A)  Respiratory alkalosis 
B)  Metabolic alkalosis 
C)  Respiratory acidosis 
D)  Metabolic acidosis 
A)  Respiratory alkalosis 
B)  Metabolic alkalosis 
C)  Respiratory acidosis 
D)  Metabolic acidosis

Question 11

Which of the following statements are true of acid excretion?
I.The lungs excrete only volatile acid.
II.The lungs can excrete large quantities of CO2 in minutes.
III.The kidneys excrete primarily fixed acids.
IV.The kidneys remove fixed acids at a much slower pace (hours to days).

Accepted Answer

A)  II, III, IV 
B)  I, II, III, IV 
C)  II, IV 
D)  I, II, III 
A)  II, III, IV 
B)  I, II, III, IV 
C)  II, IV 
D)  I, II, III

Question 12

What is the normal ratio of [HCO3-] to dissolved CO2 necessary to maintain a pH of 7.40?

Accepted Answer

A)  10:1 
B)  20:1 
C)  30:1 
D)  40:1 
A)  10:1 
B)  20:1 
C)  30:1 
D)  40:1

Question 13

Because pH is a logarithmic scale, it is anticipated that a change of one pH unit will result in what change in [H+]?

Accepted Answer

A)  Twofold change 
B)  Fivefold change 
C)  Tenfold change 
D)  Twentyfold change 
A)  Twofold change 
B)  Fivefold change 
C)  Tenfold change 
D)  Twentyfold change

Question 14

Which of the following are the major mechanisms responsible for maintaining a stable pH in the face of massive CO2 production?
I.Proteins
II.Ventilation
III.Isohydric buffering
IV.HCO3-

Accepted Answer

A)  I, II, III 
B)  III, IV 
C)  I, II, III, IV 
D)  II, III 
A)  I, II, III 
B)  III, IV 
C)  I, II, III, IV 
D)  II, III

Question 15

According to the widely accepted Brønsted-Lowry theory, what is an acid?

Accepted Answer

A)  Any substance that donates an electron (H+) to an aqueous solution 
B)  Any substance that donates a proton (H+) to an aqueous solution 
C)  Any substance that accepts a proton (H+), removing it from solution 
D)  Any substance that accepts an electron (H+), removing it from solution 
A)  Any substance that donates an electron (H+) to an aqueous solution 
B)  Any substance that donates a proton (H+) to an aqueous solution 
C)  Any substance that accepts a proton (H+), removing it from solution 
D)  Any substance that accepts an electron (H+), removing it from solution

Question 16

What is the function of buffers?

Accepted Answer

A)  They force H+ to go inside the cell. 
B)  They readily combine with HCO3-, removing H+ from solution. 
C)  They readily combine with H+ ions, removing them from solution. 
D)  They increase the HCO3- concentration in plasma. 
A)  They force H+ to go inside the cell. 
B)  They readily combine with HCO3-, removing H+ from solution. 
C)  They readily combine with H+ ions, removing them from solution. 
D)  They increase the HCO3- concentration in plasma.

Question 17

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO2 decrease of 10 mm Hg below 40 mm Hg will be associated with which of the following changes?

Accepted Answer

A)  [HCO3-] decreases by approximately 10 mEq/L. 
B)  [HCO3-] decreases by approximately 5 mEq/L. 
C)  [HCO3-] decreases by approximately 2 mEq/L. 
D)  [HCO3-] decreases by approximately 1 mEq/L. 
A)  [HCO3-] decreases by approximately 10 mEq/L. 
B)  [HCO3-] decreases by approximately 5 mEq/L. 
C)  [HCO3-] decreases by approximately 2 mEq/L. 
D)  [HCO3-] decreases by approximately 1 mEq/L.

Question 18

Which of the following organs is responsible for the physical removal of H+?

Accepted Answer

A)  Kidneys 
B)  Lungs 
C)  Intestine 
D)  Pancreas 
A)  Kidneys 
B)  Lungs 
C)  Intestine 
D)  Pancreas

Question 19

According to the widely accepted Brønsted-Lowry theory, what is a base?

Accepted Answer

A)  Any substance that donates an electron (H+) to an aqueous solution 
B)  Any substance that donates a proton (H+) to an aqueous solution 
C)  Any substance that accepts a proton (H+), removing it from solution 
D)  Any substance that accepts an electron (H+), removing it from solution 
A)  Any substance that donates an electron (H+) to an aqueous solution 
B)  Any substance that donates a proton (H+) to an aqueous solution 
C)  Any substance that accepts a proton (H+), removing it from solution 
D)  Any substance that accepts an electron (H+), removing it from solution

Question 20

What is the pH of a chemically neutral solution?

Accepted Answer

A)  6.5 
B)  7.0 
C)  7.5 
D)  8.0 
A)  6.5 
B)  7.0 
C)  7.5 
D)  8.0

Exam 10: Acid-Base Regulation

Which of the following variables are computed by the H-H equation? I.pK II.pH III.HCO3- IV.PCO2

Which of the following systems has the greatest buffering capacity?

Which of the following are examples of a fixed acid? I.Carbonic acid II.Lactic acid III.Phosphoric acid IV.Sulfuric acid

Which of the following nonbicarbonate buffers is the most important?

Which of the following is considered a rapid compensatory mechanism to restore the pH back to normal levels in the presence of a metabolic acidosis?

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO2 rise to a level of 60 mm Hg will be associated with which of the following changes in the [HCO3-]?

A young, previously healthy drug overdose victim with severely depressed ventilation enters the emergency room with the following arterial blood gases: pH = 7.22, PaCO2 = 70 mm Hg, HCO3-= 28 mEq/L.What is the acid-base disturbance of this victim?

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO2 rise of 10 mm Hg will be associated with which of the following changes?

Which of the following is the only volatile acid of physiological significance in the body?

Which of the following disturbances in the pH may potentially occur in patients with nasogastric suction catheters?

Which of the following statements are true of acid excretion? I.The lungs excrete only volatile acid. II.The lungs can excrete large quantities of CO2 in minutes. III.The kidneys excrete primarily fixed acids. IV.The kidneys remove fixed acids at a much slower pace (hours to days).

What is the normal ratio of [HCO3-] to dissolved CO2 necessary to maintain a pH of 7.40?

Because pH is a logarithmic scale, it is anticipated that a change of one pH unit will result in what change in [H+]?

Which of the following are the major mechanisms responsible for maintaining a stable pH in the face of massive CO2 production? I.Proteins II.Ventilation III.Isohydric buffering IV.HCO3-

According to the widely accepted Brønsted-Lowry theory, what is an acid?

What is the function of buffers?

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO2 decrease of 10 mm Hg below 40 mm Hg will be associated with which of the following changes?

Which of the following organs is responsible for the physical removal of H+?

According to the widely accepted Brønsted-Lowry theory, what is a base?

What is the pH of a chemically neutral solution?

The Airways and Alveoli

The Lungs and Chest Wall

Mechanics of Ventilation

Ventilation

Pulmonary Function Measurements

Pulmonary Blood Flow

Gas Diffusion

Oxygen Equilibrium and Transport

Carbon Dioxide Equilibrium and Transport

Control of Ventilation

Ventilation-Perfusion Relationships

Clinical Assessment of Acid-Base and Oxygenation Status

Physiological Basis for Oxygenation and Lung Protection Strategies

Physiology of Sleep Disordered Breathing

Fetal and Newborn Cardiopulmonary Physiology

Functional Anatomy of the Cardiovascular System

Cardiac Electrophysiology

The Electrocardiogram and Cardiac Arrhythmias In Adults

Control of Cardiac Output and Hemodynamic

Filtration, Urine Formation, and Fluid Regulation

Electrolyte and Acid-Base Regulation

Cardiopulmonary Response to Exercise in Health and Disease

Aging and the Cardiopulmonary System

Filters

Which of the following variables are computed by the H-H equation? I.pK II.pH III.HCO₃^- IV.PCO₂

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO₂ rise to a level of 60 mm Hg will be associated with which of the following changes in the [HCO3^-]?

A young, previously healthy drug overdose victim with severely depressed ventilation enters the emergency room with the following arterial blood gases: pH = 7.22, PaCO₂ = 70 mm Hg, HCO₃^-= 28 mEq/L.What is the acid-base disturbance of this victim?

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO₂ rise of 10 mm Hg will be associated with which of the following changes?

Which of the following statements are true of acid excretion? I.The lungs excrete only volatile acid. II.The lungs can excrete large quantities of CO₂ in minutes. III.The kidneys excrete primarily fixed acids. IV.The kidneys remove fixed acids at a much slower pace (hours to days).

What is the normal ratio of [HCO₃^-] to dissolved CO₂ necessary to maintain a pH of 7.40?

Because pH is a logarithmic scale, it is anticipated that a change of one pH unit will result in what change in [H⁺]?

Which of the following are the major mechanisms responsible for maintaining a stable pH in the face of massive CO₂production? I.Proteins II.Ventilation III.Isohydric buffering IV.HCO₃^-

In general, when the nonbicarbonate buffer concentration is normal, an acute PaCO₂ decrease of 10 mm Hg below 40 mm Hg will be associated with which of the following changes?

Which of the following organs is responsible for the physical removal of H⁺?