Textbook Question
Explain the difference between an ionic and a covalent bond.
Ch. 2 The Chemistry of Life
Amerman2nd EditionHuman Anatomy & PhysiologyISBN: 9780136873822
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Table of contents
- Ch. 1 Introduction to Anatomy and Physiology26
- Ch. 2 The Chemistry of Life38
- Ch. 3 The Cell55
- Ch. 4 Histology47
- Ch. 5 The Integumentary System30
- Ch. 6 Bones and Bone Tissue36
- Ch. 7 The Skeletal System40
- Ch. 8 Articulations19
- Ch. 9 The Muscular System36
- Ch. 10 Muscle Tissue and Physiology29
- Ch. 11 Introduction to the Nervous System and Nervous Tissue28
- Ch. 12 The Central Nervous System42
- Ch. 13 The Peripheral Nervous System41
- Ch. 14 The Autonomic Nervous System and Homeostasis31
- Ch. 15 The Special Senses39
- Ch. 16 The Endocrine System42
- Ch. 17 The Cardiovascular System I: The Heart30
- Ch. 18 The Cardiovascular System II: The Blood Vessels43
- Ch. 19 Blood32
- Ch. 20 The Lymphatic System and Immunity45
- Ch. 21 The Respiratory System27
- Ch. 22 The Digestive System27
- Ch. 23 Metabolism and Nutrition7
- Ch. 24 The Urinary System39
- Ch. 25 Fluid, Electrolyte, and Acid-Base Homeostasis39
- Ch. 26 The Reproductive System10
- Ch. 27 Development and Heredity5
Chapter 2, Problem L3.2
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?)
Verified step by step guidance1
Understand the concept of pH: pH is a measure of hydrogen ion (H⁺) concentration in a solution. A lower pH indicates higher acidity (more H⁺ ions), while a higher pH indicates alkalinity (fewer H⁺ ions). Normal blood pH is tightly regulated between 7.35 and 7.45, which is slightly alkaline.
Learn about the body's buffering systems: The body has mechanisms, such as the bicarbonate buffer system, to maintain blood pH within its narrow range. The bicarbonate buffer system involves the equilibrium: \( \text{HCO}_3^- + \text{H}^+ \leftrightarrow \text{H}_2\text{CO}_3 \leftrightarrow \text{CO}_2 + \text{H}_2\text{O} \). This system helps neutralize excess H⁺ ions or hydroxide ions (OH⁻).
Consider the digestion process: When you eat acidic foods like citrus, the acids are neutralized in the stomach by gastric acid (which is already highly acidic, with a pH of around 1.5-3.5). The acidic food does not directly enter the bloodstream in its original form.
Examine the role of homeostasis: The kidneys and lungs work together to regulate blood pH. For example, the lungs can expel more CO₂ (a byproduct of the bicarbonate buffer system) to reduce acidity, while the kidneys can excrete H⁺ ions or reabsorb bicarbonate ions to maintain pH balance.
Conclude based on physiology: Eating acidic foods like citrus does not significantly affect blood pH because of the body's robust buffering systems and homeostatic mechanisms. Any minor changes in H⁺ ion concentration are quickly corrected to maintain the blood's pH within its normal range.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH and Hydrogen Ions
pH is a measure of the acidity or alkalinity of a solution, determined by the concentration of hydrogen ions (H+) present. A lower pH indicates higher acidity, while a higher pH indicates alkalinity. The addition of hydrogen ions to the blood can lower its pH, making it more acidic, which can disrupt normal physiological functions.
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pH Scale
Homeostasis in Blood pH
The body maintains blood pH within a narrow range (approximately 7.35 to 7.45) through homeostatic mechanisms. This regulation is crucial because even slight deviations can lead to acidosis or alkalosis, which can have serious health implications. The body employs buffers, respiratory control, and renal function to stabilize pH levels despite dietary changes.
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03:46Homeostasis Example 1
Dietary Impact on Blood pH
While certain foods, like citrus, are acidic, their effect on blood pH is minimal due to the body's regulatory systems. The digestion of food can produce metabolic byproducts that influence pH, but the body effectively neutralizes these changes. Therefore, the claim that eating acidic foods significantly alters blood pH is largely unfounded, as the body prioritizes maintaining homeostasis.
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Related Practice
Textbook Question
Identify each of the following molecules or compounds as ionic, polar covalent, or nonpolar covalent.
a. H2O _________
b. LiI _________
c. C10H22 _________
d. N2 _________
e. MgBr2 _________
f. H2S _________
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Textbook Question
The drug methotrexate is used to treat several different types of cancer and diseases of the immune system. It works by inhibiting an enzyme in the cell necessary for folic acid synthesis. Without folic acid, the cell cannot make nucleotides. What, specifically, does an enzyme do in the cell? Why would inhibiting this enzyme disrupt folic acid synthesis? What effect would a disruption in folic acid synthesis have on the cell as a whole? (Hint: Think about the role that folic acid plays in the cell.) (Connects to Chapter 2)
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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.
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Textbook Question
Many drugs and poisons exert their effects by blocking one or more enzymes. How could blocking an enzyme lead to the death of a cell?
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Textbook Question
What are hydrogen bonds, and how do they form?
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