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

2. Cell Chemistry & Cell Components

pH Scale

Anatomy & Physiology

2. Cell Chemistry & Cell Components

pH Scale

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Problem L3.4

Textbook Question

Explain how buffer systems in the body work if the pH of body fluids increases. Is this an example of a negative or a positive feedback loop? Explain.

Verified step by step guidance

Understand the concept of pH: pH is a measure of hydrogen ion (H⁺) concentration in a solution. A higher pH indicates a decrease in H⁺ concentration, making the solution more basic (alkaline). The normal pH range of body fluids, such as blood, is tightly regulated around 7.35–7.45.

Identify the role of buffer systems: Buffer systems in the body, such as the bicarbonate buffer system, help maintain pH homeostasis by resisting changes in pH. They do this by either releasing H⁺ ions when the pH increases (becomes more basic) or binding H⁺ ions when the pH decreases (becomes more acidic).

Describe the bicarbonate buffer system: The bicarbonate buffer system is the primary buffer in the blood. It involves the reversible reaction: \( \text{H}_2\text{CO}_3 \leftrightarrow \text{H}^+ + \text{HCO}_3^- \). When the pH increases, carbonic acid (\( \text{H}_2\text{CO}_3 \)) dissociates to release H⁺ ions, which helps lower the pH back to normal.

Explain the feedback mechanism: This process is an example of a negative feedback loop. Negative feedback loops work to counteract changes and restore balance. In this case, the buffer system acts to decrease the pH when it rises, maintaining homeostasis.

Summarize the importance: Buffer systems are critical for maintaining the stability of the body's internal environment. Without these systems, even small changes in pH could disrupt cellular processes and lead to severe physiological consequences.

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Key Concepts

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

Buffer Systems

Buffer systems in the body are chemical solutions that resist changes in pH when acids or bases are added. They work by neutralizing excess hydrogen ions (H+) or hydroxide ions (OH-), maintaining a stable pH in body fluids. Key buffers include bicarbonate, phosphate, and proteins, which play crucial roles in physiological processes.

pH Regulation

pH regulation is essential for maintaining homeostasis in the body, as enzymes and biochemical reactions are highly sensitive to pH changes. When the pH of body fluids increases (becomes more alkaline), buffer systems help to restore balance by releasing H+ ions to lower the pH back to normal levels, ensuring optimal functioning of cellular processes.

Negative Feedback Loop

A negative feedback loop is a biological mechanism that counteracts a change in a system to maintain stability. In the context of increased pH, the buffer systems act to lower the pH, demonstrating a negative feedback response. This process helps to return the body to its desired state, contrasting with positive feedback, which amplifies changes.

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Related Practice

Textbook Question

A can of cola consists mostly of sugar dissolved in water, with some carbon dioxide gas that makes it fizzy and makes the pH less than 7. In chemical terms, you could say that cola is an aqueous solution where water is the _________ , sugar is a _________ , and carbon dioxide makes the solution _________ .a. solvent . . . solute . . . basicb. solute . . . solvent . . . basicc. solvent . . . solute . . . acidicd. solute . . . solvent . . . acidic

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Textbook Question

If you were given a solution that has a pH of 8.5, what would be its concentration of protons? What is the difference in proton concentration between this solution and one that has a pH of 7?

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Textbook Question

A recent experimental study looked at the combined effects of ocean acidification and increased ocean temperatures, both aspects of climate change, on the growth of polyps, juvenile coral animals. Researchers reported the average polyp biomass (in μg/polyp) after 42 days of growth under four treatments: a control with pH and temperature maintained close to normal reef conditions, a pH lowered by 0.2 units, a temperature raised by 1°C, and a combined lower pH and higher temperature. The results showed that polyp biomass was reduced somewhat in both the low-pH and high-temperature treatments, but the combined treatment resulted in a reduction in growth by almost a third—a statistically significant result. Experiments often look at the effects of changing one variable at a time, while keeping all other variables constant. Explain why this experiment considered two variables—both a higher temperature and a lower pH—at the same time.

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Multiple Choice

Buffers are substances that help resist shifts in pH by:

Mark the following statements as true or false. If a statement is false, correct it to make a true statement.

As a solution's pH rises, it becomes more acidic.

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Textbook Question

Some claim that the pH of your blood can be affected by eating acidic foods such as citrus. Do you believe this to be true? Explain your answer. (Hint: What happens when extra hydrogen ions are added to the blood?)

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Multiple Choice

What is the relationship between pH and hemoglobin saturation in erythrocytes?

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Multiple Choice

In a neutral solution, the concentration of __________.