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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1:47 minutes

Problem 18

Textbook Question

Explain how 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 biological systems.

Learn the components of a buffer system: A chemical buffer system typically consists of a weak acid and its conjugate base (or a weak base and its conjugate acid). These components can donate or accept H⁺ ions to resist changes in pH.

Explore the mechanism of buffering: When the pH decreases (becomes more acidic), the conjugate base in the buffer system reacts with excess H⁺ ions to form the weak acid, reducing the impact of the added H⁺ ions. Conversely, when the pH increases (becomes more basic), the weak acid releases H⁺ ions to counteract the excess OH⁻ ions.

Examine an example: The bicarbonate buffer system in the blood is a key example. It involves carbonic acid (H₂CO₃) and bicarbonate (HCO₃⁻). The reaction can be represented as:

H ₂ CO ₃ \leftrightarrow H ⁺ + H CO ₃ ⁻

. This system helps maintain blood pH around 7.4.

Understand the importance of buffer systems: Buffer systems are crucial for maintaining homeostasis in the body. Without them, even small changes in pH could disrupt enzyme function, cellular processes, and overall physiological balance.

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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. A pH less than 7 indicates acidity, while a pH greater than 7 indicates basicity. Understanding the pH scale is crucial for comprehending how buffers function, as they are designed to maintain pH levels within a specific range, essential for many biochemical processes.

Equilibrium Reactions

Equilibrium reactions are chemical reactions where the forward and reverse processes occur at the same rate, leading to a stable concentration of reactants and products. In the context of buffer systems, the equilibrium between a weak acid and its conjugate base allows the system to absorb excess H+ or OH- ions, thus minimizing changes in pH. This dynamic balance is key to the effectiveness of buffers in resisting pH fluctuations.

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Related Practice

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 the 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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Textbook Question

Explain how emphysema and congestive heart failure can lead to acid-base imbalance.

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