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Questions and Answers
What is the normal pH range of blood that is crucial for enzyme function?
What is the normal pH range of blood that is crucial for enzyme function?
What is the main role of protein buffers in the body?
What is the main role of protein buffers in the body?
What type of acid dissociates completely in solution?
What type of acid dissociates completely in solution?
Which of the following statements about the hemoglobin buffer system is true?
Which of the following statements about the hemoglobin buffer system is true?
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Which of the following is considered a conjugate base of a weak acid?
Which of the following is considered a conjugate base of a weak acid?
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How do the lungs contribute to acid-base balance?
How do the lungs contribute to acid-base balance?
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Which statement is true regarding buffers?
Which statement is true regarding buffers?
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What occurs during acidosis regarding the respiratory system?
What occurs during acidosis regarding the respiratory system?
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What is the logarithmic scale of pH and what is the typical pH of pure water?
What is the logarithmic scale of pH and what is the typical pH of pure water?
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What is a disadvantage of the respiratory mechanism in maintaining pH balance?
What is a disadvantage of the respiratory mechanism in maintaining pH balance?
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What is the relationship between hydrogen ion concentration and pH?
What is the relationship between hydrogen ion concentration and pH?
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What happens to the bicarbonate buffer ratio during alkalosis?
What happens to the bicarbonate buffer ratio during alkalosis?
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Which combination represents a buffer system?
Which combination represents a buffer system?
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What happens to OH- concentration when the concentration of H+ increases?
What happens to OH- concentration when the concentration of H+ increases?
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Why is the buffer capacity of plasma proteins considered less than that of hemoglobin?
Why is the buffer capacity of plasma proteins considered less than that of hemoglobin?
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What is the consequence of the lungs failing to excrete CO2 effectively?
What is the consequence of the lungs failing to excrete CO2 effectively?
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What happens to the pH of a buffer when the ratio of salt to acid is 10:1?
What happens to the pH of a buffer when the ratio of salt to acid is 10:1?
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Which condition defines the maximum buffering capacity of a buffer?
Which condition defines the maximum buffering capacity of a buffer?
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Which buffer has a pKa that is closest to the blood pH of 7.4?
Which buffer has a pKa that is closest to the blood pH of 7.4?
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What is a major disadvantage of the bicarbonate buffer system in plasma?
What is a major disadvantage of the bicarbonate buffer system in plasma?
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Which components are regulated by the kidneys and lungs in relation to acid-base balance?
Which components are regulated by the kidneys and lungs in relation to acid-base balance?
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What is an accurate description of intracellular buffers?
What is an accurate description of intracellular buffers?
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What does a ratio of salt to acid concentrations determine in a buffer?
What does a ratio of salt to acid concentrations determine in a buffer?
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Which of the following describes a characteristic of the phosphate buffer?
Which of the following describes a characteristic of the phosphate buffer?
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Study Notes
Acid-Base Balance
- Blood pH is maintained within a narrow range (7.35-7.45) for optimal enzyme function.
- Metabolic reactions produce acids (volatile and non-volatile).
- Bicarbonate is generated from organic acids, which can significantly affect pH.
- Understanding acids, bases, and pH is crucial for comprehending acid-base balance.
Bronsted-Lowry Theory
- Acids are proton donors.
- Bases are proton acceptors.
- Examples: HCl → H+ + Cl-; H₂CO₃ ↔ H⁺ + HCO₃⁻;
Strong vs. Weak Acids & Bases
- Strong acids dissociate completely in solution, producing high H+ concentrations. (e.g., HCl, HNO₃, H₂SO₄)
- Weak acids do not completely ionize, resulting in lower H+ concentrations. (e.g., H₂CO₃, CH₃COOH)
- Conjugate bases of strong acids are weak bases, while conjugate bases of weak acids are strong bases.
Dissociation of Water
- The degree of dissociation increases with temperature.
- Water's H+ concentration is 1/100,000,000 gram moles per liter at 25°C.
- This applies to all solutions.
Buffers
- Resist changes in pH upon the addition of small amounts of acid or alkali.
- Composed of a weak acid and its conjugate base, or a weak base and its conjugate acid.
- Examples: CH₃COOH/CH₃COONa; H₂CO₃/HCO₃⁻.
- Effectiveness is highest at pH = pKa
Factors Affecting Buffer pH
- pKa value: Lower pKa = lower buffer pH
- Ratio of salt to acid: Ration remains the same with no change in pH.
Buffering Capacity
- Measures the ability to resist changes in pH when acids or bases are added.
- Determined by the absolute concentration of salt and acid.
- Most effective when salt:acid = 10:1 or 1:10.
Maintenance of Acid-Base Balance
- Three mechanisms: buffers, respiration, and kidneys.
Buffer Types
- Bicarbonate buffer (major extracellular buffer).
- Phosphate buffer (major intracellular buffer).
- Protein buffer (important in RBCs and plasma)
- Hemoglobin Buffer
Bicarbonate Buffer
- A critical plasma buffer system (HCO₃⁻ and H₂CO₃)
- Ratio of HCO₃⁻ to H₂CO₃ should be 20:1 to maintain pH 7.4.
- Bicarbonate concentration is higher (20 times).
- Controlled by kidneys (metabolic component).
- Controlled by lungs (respiratory component)
Phosphate Buffer
- Primary intracellular buffer
- pKa = 6.8 (close to blood pH)
- Less efficient if plasma pH is 7.4 due to low concentrations
Protein Buffers
- Important in plasma and intracellular fluids
- Plasma proteins (Pr-/HPr) act as buffers at pH 7.4
- Hemoglobin (important in RBCs).
Respiratory Mechanisms
- Controls H₂CO₃ (carbonic acid) levels in plasma.
- Hyperventilation (excretion of CO₂) or hypoventilation (accumulation of CO₂) adjusts pH.
- Rapid response mechanism (2-3 minutes)
- Not sufficient for complete pH restoration.
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Description
This quiz explores the fundamental concepts of acid-base balance, the Bronsted-Lowry theory, and the differences between strong and weak acids and bases. Questions will cover pH maintenance, dissociation of water, and the role of bicarbonates. Test your understanding of these key aspects in chemistry!
