Table of contents

1. Introduction to Anatomy & Physiology5h 43m
2. Cell Chemistry & Cell Components12h 36m
3. Energy & Cell Processes10h 6m
4. Tissues & Histology10h 3m
5. Integumentary System2h 20m
6. Bones & Skeletal Tissue2h 16m
7. The Skeletal System2h 35m
8. Joints2h 17m
9. Muscle Tissue2h 33m
10. Muscles1h 11m
11. Nervous Tissue and Nervous System1h 35m
12. The Central Nervous System1h 6m
- Introduction to the Central Nervous System
  18m
- The Cerebrum
  48m
13. The Peripheral Nervous System1h 26m
14. The Autonomic Nervous System1h 38m
15. The Special Senses2h 41m
16. The Endocrine System2h 48m
17. The Blood3h 22m
18. The Heart3h 42m
19. The Blood Vessels3h 35m
20. The Lymphatic System3h 16m
21. The Immune System14h 37m
22. The Respiratory System3h 20m
23. The Digestive System2h 5m
24. Metabolism and Nutrition4h 0m
25. The Urinary System2h 39m
26. Fluid and Electrolyte Balance, Acid Base Balance37m
27. The Reproductive System2h 5m
28. Human Development1h 21m
29. Heredity3h 32m

26. Fluid and Electrolyte Balance, Acid Base Balance

Acid-Base Balance

Anatomy & Physiology

26. Fluid and Electrolyte Balance, Acid Base Balance

Acid-Base Balance

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1:30 minutes

Problem 18

Textbook Question

Explain how the chemical buffer systems resist changes in pH.

Verified step by step guidance

Understand the concept of pH: pH is a measure of the hydrogen ion (H⁺) concentration in a solution. A low pH indicates high acidity (more H⁺ ions), while a high pH indicates alkalinity (fewer H⁺ ions). Buffer systems help maintain a stable pH in the body.

Learn the role of buffer systems: Chemical buffer systems resist changes in pH by neutralizing excess acids (H⁺ ions) or bases (OH⁻ ions). They act as a first line of defense in maintaining homeostasis in the body's fluids.

Explore the components of buffer systems: Buffer systems typically consist of a weak acid and its conjugate base. For example, the bicarbonate buffer system includes carbonic acid (H₂CO₃) and bicarbonate (HCO₃⁻). These components work together to stabilize pH.

Understand the mechanism of action: When the pH drops (becomes more acidic), the conjugate base (e.g., HCO₃⁻) binds to excess H⁺ ions, forming the weak acid (e.g., H₂CO₃). Conversely, when the pH rises (becomes more basic), the weak acid releases H⁺ ions to neutralize excess OH⁻ ions.

Recognize key buffer systems in the body: The major buffer systems include the bicarbonate buffer system (important in blood plasma), the phosphate buffer system (active in intracellular fluids), and protein buffers (such as hemoglobin in red blood cells). Each system plays a specific role in maintaining pH balance in different compartments of the body.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Buffer Systems

Chemical buffer systems are solutions that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. This equilibrium allows buffers to neutralize added acids or bases, maintaining a relatively stable pH in biological and chemical systems.

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14, with 7 being neutral. Values below 7 indicate acidic solutions, while values above 7 indicate basic solutions. Understanding the pH scale is crucial for comprehending how buffer systems function, as they are designed to maintain pH within a specific range optimal for various biological processes.

Equilibrium and Le Chatelier's Principle

Equilibrium in chemical reactions refers to the state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. Le Chatelier's Principle states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance. This principle explains how buffer systems can adjust to changes in pH by shifting the equilibrium between the weak acid and its conjugate base.

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Related Practice

Textbook Question

More than one choice may apply.

In the carbonic acid–bicarbonate buffer system, strong acids are buffered by

a. Carbonic acid

b. Water

c. Bicarbonate ion

d. The salt of the strong acid

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Textbook Question

Two ions produced during catabolism of glutamine are:

a. Ammonium ions

b. Bicarbonate

c. Calcium

d. Chloride

e. Hydrogen ions

f. Magnesium

g. Phosphate

h. Potassium

i. Sodium

j. Water

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Textbook Question

In an individual with metabolic acidosis, a clue that the respiratory system is compensating is provided by:

a. High blood bicarbonate levels

b. Low blood bicarbonate levels

c. Rapid, deep breathing

d. Slow, shallow breathing

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Textbook Question

Describe the role of the respiratory system in controlling acid-base balance.

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Textbook Question

Explain how chemical buffer systems resist changes in pH.

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Textbook Question

Explain the relationship of the following to renal secretion and excretion of hydrogen ions:

Plasma carbon dioxide levels

Phosphate

Sodium bicarbonate reabsorption

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Textbook Question

Describe the role of the respiratory system in controlling acid-base balance.

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Textbook Question

For each of the following sets of blood values, name the acid-base imbalance (acidosis or alkalosis), determine its cause (metabolic or respiratory), decide whether the condition is being compensated, and cite at least one possible cause of the imbalance. Problem 1: pH 7.63; Pco₂ 19 mm Hg; Hco₃⁻ 19.5 mEq/L Problem 2: pH 7.22; Pco₂ 30 mm Hg; Hco₃⁻ 12.0 mEq/L

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