Acid-Base Balance in Human Physiology
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Questions and Answers

What is the normal H+ concentration in mEq/L in the body?

  • 0.00003 mEq/L
  • 0.00004 mEq/L (correct)
  • 0.0001 mEq/L
  • 0.00005 mEq/L

    • What happens to the pH when the H+ concentration increases?

  • pH decreases (correct)
  • pH increases
  • pH remains the same
  • pH becomes neutral

    • At what pH value is a person considered to have acidosis?

  • 7.0
  • 7.4
  • 7.2
  • 6.8 (correct)

    • What is the estimated pH range of intracellular fluid?

    <p>6.0 to 7.4</p> Signup and view all the answers

    What is the normal range of pH for venous blood?

    <p>7.35 to 7.40</p> Signup and view all the answers

    Which of the following is a weak acid involved in acid-base regulation?

    <p>H2CO3</p> Signup and view all the answers

    What can cause acid accumulation and decreased intracellular pH?

    <p>Hypoxia of the tissues</p> Signup and view all the answers

    What is the major role of the kidneys in acid-base regulation?

    <p>Excreting acids or bases at variable rates</p> Signup and view all the answers

    What is the primary role of the chemical acid-base buffer systems in body fluids?

    <p>To immediately combine with acids or bases</p> Signup and view all the answers

    What is the primary role of the kidneys in acid-base regulation?

    <p>To remove hydrogen ions from the body.</p> Signup and view all the answers

    Which system acts as the first line of defense against changes in H+ concentration?

    <p>Buffering system</p> Signup and view all the answers

    How do the kidneys contribute to regulating H+ concentration in the body?

    <p>They can excrete acid or alkaline urine</p> Signup and view all the answers

    Which of the following statements accurately describes alkalosis?

    <p>It refers to a deficiency of H+ in body fluids.</p> Signup and view all the answers

    Which substance is classified as a strong acid?

    <p>Hydrochloric acid (HCl)</p> Signup and view all the answers

    What happens when H+ concentration increases in the body fluids?

    <p>Buffers bind H+, forming weak acids</p> Signup and view all the answers

    What defines a base in the context of acid-base chemistry?

    <p>A substance that binds with H+ ions.</p> Signup and view all the answers

    Why are the kidneys considered the most powerful acid-base regulatory system?

    <p>They operate over hours to days to adjust H+ levels</p> Signup and view all the answers

    Which of the following is a weak base?

    <p>Bicarbonate (HCO3−)</p> Signup and view all the answers

    What is the general form of the buffering reaction in the body fluids?

    <p>H+ + buffer ↔ H buffer</p> Signup and view all the answers

    How quickly does the respiratory system respond to changes in H+ concentration?

    <p>Within minutes</p> Signup and view all the answers

    How does a strong base behave in an acid-base reaction?

    <p>It quickly removes H+ ions from a solution.</p> Signup and view all the answers

    What happens to the buffering reaction when H+ concentration decreases?

    <p>The reaction shifts to the left and releases H+ from the buffer</p> Signup and view all the answers

    Which of the following mechanisms is important for regulating acid-base balance in the body?

    <p>Buffers in the blood, cells, and lungs are crucial.</p> Signup and view all the answers

    Hydrogen ions (H+) are primarily associated with which type of solution?

    <p>Acidic solutions with a higher concentration of H+.</p> Signup and view all the answers

    What is the primary weak acid in the bicarbonate buffer system?

    <p>H2CO3</p> Signup and view all the answers

    What happens to H2CO3 in the bicarbonate buffer system?

    <p>It weakly dissociates to release small amounts of H+.</p> Signup and view all the answers

    What role does carbonic anhydrase play in the bicarbonate buffer system?

    <p>It speeds up the conversion of CO2 and H2O to H2CO3.</p> Signup and view all the answers

    How does the body respond when a strong acid, such as HCl, is added to the bicarbonate buffer solution?

    <p>HCO3− reacts with the strong acid to form H2CO3.</p> Signup and view all the answers

    What is the function of the bicarbonate salt in the bicarbonate buffer system?

    <p>It provides a source of HCO3− that can neutralize excess H+.</p> Signup and view all the answers

    What occurs when a strong base, like sodium hydroxide (NaOH), is added to the bicarbonate buffer solution?

    <p>HCO3− reacts with the base to form more NaHCO3.</p> Signup and view all the answers

    What is the typical concentration of H+ in body fluids?

    <p>0.00004 mEq/L</p> Signup and view all the answers

    What effect does increased CO2 production have on respiration?

    <p>It stimulates respiration to eliminate CO2.</p> Signup and view all the answers

    Study Notes

    Acid-Base Balance

    • Definition: The mechanisms the body uses to keep fluids close to neutral pH, allowing for normal function.
    • Regulation: Maintaining a balance between H+ intake/production and its removal, with kidneys playing a key role in elimination.
    • Buffering Systems: Blood, cells, and lungs help maintain normal H+ concentrations in extracellular and intracellular fluids.

    Acidosis and Alkalosis

    • Alkalosis: Excess removal of H+ from body fluids.
    • Acidosis: Excess addition of H+ to body fluids.

    Acids and Bases

    • Acids: Molecules that release H+ in solutions.
    • Examples of Acids: Hydrochloric acid (HCl) and carbonic acid (H2CO3).
    • Bases: Ions or molecules that can accept H+.
    • Examples of Bases: Bicarbonate (HCO3-) and phosphate (HPO4-) ions.
    • Body Proteins as Bases: Amino acids in proteins have negative charges that readily accept H+.

    Strong and Weak Acids and Bases

    • Strong Acids: Rapidly dissociate in solution and release large amounts of H+ (e.g., HCl).
    • Weak Acids: Less likely to dissociate, releasing fewer H+ (e.g., H2CO3).
    • Strong Bases: React quickly and strongly with H+ to remove it from solution (e.g., OH-).
    • Weak Bases: Bind with H+ weakly (e.g., HCO3-).

    Normal Concentration and pH of Body Fluids

    • Normal Blood H+ Concentration: Around 0.00004 mEq/L (40 nEq/L).
    • Normal pH Range: Arterial blood: 7.4; Venous blood & interstitial fluids: 7.35; Intracellular fluid: 6.0-7.4; Urine: 4.5-8.0.
    • Acidosis: pH below 7.4.
    • Alkalosis: pH above 7.4.

    Defending Against Changes in H+ Concentration

    • Three Main Systems:
      • Chemical acid-base buffer systems (immediate reaction).
      • Respiratory center (regulation of CO2 removal; minutes).
      • Kidneys (excretion of acid or alkaline urine; hours to days).

    Buffering System

    • Definition: Substances that reversibly bind H+ to minimize changes in H+ concentration.
    • Role: Bind H+ temporarily until balance is restored.

    The Respiratory System

    • Role: Eliminates CO2 (and, therefore, H2CO3) from the body.

    The Kidney System

    • Role: Excrete excess acid or base from the body.
    • Most Powerful Regulatory System: Acts slowly but effectively over a prolonged period.

    Buffering of H+ in the Body Fluids

    • Buffering Reaction (General Form): H + + Buffer → H Buffer
    • Mechanism: Buffers bind with H+ when concentrations increase, and release H+ when concentrations decrease.

    Bicarbonate Buffer System

    • Components:
      • Weak acid: H2CO3 (formed by CO2 and H2O).
      • Bicarbonate salt: NaHCO3.
    • Role: Maintains pH by buffering H+ from strong acids like HCl, forming weak acid H2CO3, which then decomposes into CO2 and H2O.
    • CO2 Excretion: Increased CO2 production stimulates respiration, removing CO2 from the body.
    • Alkaline Reaction: When a strong base (e.g., NaOH) is added, HCO3- reacts to form H2CO3, which then releases CO2 and H2O.

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    Acid-Base Balance PDF

    Description

    This quiz explores the concepts of acid-base balance, including the definitions of alkalosis and acidosis, and the roles of various buffers in the body. Understand the mechanisms that maintain neutral pH levels for normal bodily function and how strong and weak acids and bases interact in physiological processes.

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