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What does acid-base balance primarily regulate in body fluids?
What does acid-base balance primarily regulate in body fluids?
Which of the following factors is NOT directly involved in the regulation of acid-base balance?
Which of the following factors is NOT directly involved in the regulation of acid-base balance?
What effect does acidosis have on K+ secretion in the body?
What effect does acidosis have on K+ secretion in the body?
Which process is a source of hydrogen ions (H+) in the body?
Which process is a source of hydrogen ions (H+) in the body?
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What is a major consequence of altered acid-base balance?
What is a major consequence of altered acid-base balance?
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In which compartment are body fluids primarily found?
In which compartment are body fluids primarily found?
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How does alkalosis affect potassium ion levels in the body?
How does alkalosis affect potassium ion levels in the body?
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What is one of the primary functions of maintaining acid-base balance?
What is one of the primary functions of maintaining acid-base balance?
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What is a significant effect of TRIS buffer on biological systems?
What is a significant effect of TRIS buffer on biological systems?
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How does temperature affect TRIS buffer's behavior?
How does temperature affect TRIS buffer's behavior?
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When does a buffer function optimally?
When does a buffer function optimally?
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What is indicated when the pH of a solution equals the pK of the buffer?
What is indicated when the pH of a solution equals the pK of the buffer?
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What role does electron transport play in biological systems, especially as affected by TRIS buffer?
What role does electron transport play in biological systems, especially as affected by TRIS buffer?
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Why is lipid solubility relevant to the function of TRIS buffer?
Why is lipid solubility relevant to the function of TRIS buffer?
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Which of the following statements regarding the Henderson-Hasselbalch equation is incorrect?
Which of the following statements regarding the Henderson-Hasselbalch equation is incorrect?
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What happens to the concentration of acid and base forms of a buffer when pH equals pK?
What happens to the concentration of acid and base forms of a buffer when pH equals pK?
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Which of the following best describes the behavior of TRIS buffer at elevated temperatures?
Which of the following best describes the behavior of TRIS buffer at elevated temperatures?
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What is the primary consequence of TRIS buffer's ability to uncouple electron transport reactions?
What is the primary consequence of TRIS buffer's ability to uncouple electron transport reactions?
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Which process occurs primarily in α-intercalated cells of the late distal tubule and collecting duct?
Which process occurs primarily in α-intercalated cells of the late distal tubule and collecting duct?
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What does a high Ka indicate about an acid?
What does a high Ka indicate about an acid?
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What bicarbonate ion level range indicates a normal metabolic acid-base balance?
What bicarbonate ion level range indicates a normal metabolic acid-base balance?
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What indicates metabolic acidosis in terms of blood pH and HCO3− levels?
What indicates metabolic acidosis in terms of blood pH and HCO3− levels?
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Which components are typically included in a buffer solution?
Which components are typically included in a buffer solution?
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What is the typical fluctuation range of PCO2 when respiratory function is normal?
What is the typical fluctuation range of PCO2 when respiratory function is normal?
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In the context of the Henderson-Hasselbalch equation, what does the pKa represent?
In the context of the Henderson-Hasselbalch equation, what does the pKa represent?
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How effective is buffering capacity in relation to the pKa of a buffer?
How effective is buffering capacity in relation to the pKa of a buffer?
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Which of the following processes contributes to the generation of new HCO3−?
Which of the following processes contributes to the generation of new HCO3−?
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What is typically recognized as a metabolic acid-base imbalance?
What is typically recognized as a metabolic acid-base imbalance?
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Why is the Henderson-Hasselbalch equation significant in biological systems?
Why is the Henderson-Hasselbalch equation significant in biological systems?
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Which cellular mechanism is primarily responsible for bicarbonate secretion and H+ ion reabsorption in the distal tubule?
Which cellular mechanism is primarily responsible for bicarbonate secretion and H+ ion reabsorption in the distal tubule?
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What characterizes a weak acid in terms of Ka and pKa?
What characterizes a weak acid in terms of Ka and pKa?
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Which equation is specifically used for calculating the pH of a solution containing a buffer?
Which equation is specifically used for calculating the pH of a solution containing a buffer?
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What is the relationship between pKa and acid strength?
What is the relationship between pKa and acid strength?
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What is a conjugate base?
What is a conjugate base?
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What impact does a buffer have on pH during a titration?
What impact does a buffer have on pH during a titration?
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What is the primary function of the bicarbonate buffer system in regulating pH?
What is the primary function of the bicarbonate buffer system in regulating pH?
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Which of the following describes the action of strong acid on the phosphate buffer system?
Which of the following describes the action of strong acid on the phosphate buffer system?
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What occurs when a strong base is added to the bicarbonate buffer system?
What occurs when a strong base is added to the bicarbonate buffer system?
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What component of the phosphate buffer system acts as a weak base?
What component of the phosphate buffer system acts as a weak base?
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Which type of buffer system is characterized by its ability to resist changes in pH when strong acids or bases are added?
Which type of buffer system is characterized by its ability to resist changes in pH when strong acids or bases are added?
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When a strong acid is added to a buffer system, what happens chemically?
When a strong acid is added to a buffer system, what happens chemically?
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In the context of pH regulation, the presence of sodium bicarbonate mainly functions to:
In the context of pH regulation, the presence of sodium bicarbonate mainly functions to:
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What factor is essential for a buffer system to effectively neutralize both acids and bases?
What factor is essential for a buffer system to effectively neutralize both acids and bases?
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The phosphate buffer system primarily regulates pH in which biological context?
The phosphate buffer system primarily regulates pH in which biological context?
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Study Notes
Acid-Base Balance
- Acid-base balance refers to precise regulation of free hydrogen ion (H+) concentration in body fluids.
- Total body water = 40 Liters, 60% of body weight.
- Major fluid compartments: Intracellular fluid (ICF) - 25 L (40% body weight), Interstitial fluid (IF) - 12 L (80% of ECF), Extracellular fluid (ECF) - 15 L (20% body weight)
- Plasma (3 L, 20% ECF), comprises primarily Na+, Cl-, and HCO3-.
- ICF (25 L) contains high amounts of K+ and PO43-.
- Body fluids consist of water and solutes in three main compartments.
Homeostasis
- Homeostasis of the body is regulated by water intake and output, Na+, K+, and Ca2+ regulation, and pH (acid-base balance) regulation.
Importance of Acid-Base Balance
- Changes in nerve & muscle cell excitability are influenced by acid-base balance.
- Enzyme activity is influenced by acid-base balance.
- Acid-base balance influences K+ levels in the body; acidosis decreases K+ secretion, while alkalosis increases it.
Sources of H+ Ions in the Body
- Carbonic acid formation during metabolic processes.
- Inorganic acids produced during breakdown of nutrients.
- Organic acids from intermediary metabolism.
Acid Dissociation Constant
- Acid dissociation constant (Ka) shows acid strength.
- HA ⇌ H⁺ + A⁻
- pKa = -log10Ka
Henderson-Hasselbalch Equation
- pH of a solution containing an acid or base can be calculated using the Henderson-Hasselbalch equation.
- This equation is derived from the behavior of weak acids (and bases) in solution, and uses the kinetics of reversible reactions.
- pH = pKa + log ([A⁻]/[HA])
Buffer
- A buffer is a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid.
- Key buffer systems in the body include bicarbonate, phosphate, and protein.
- pH = pKa + log [conjugate base]/[acid]
Buffering Capacity
- Effectiveness of a buffer depends on concentration and pKa value.
- Effective buffering occurs when the solution pH is within ±1 pH unit of the buffer pKa.
- Buffers only work ±1 unit on either side of their pKa values.
Kₐ and pKₐ Values for Weak Acids
- A table of various weak acids and their Kₐ and pKₐ values.
pH Values of Some Common Substances
- A table of various substances and their corresponding pH values.
Ideal Buffer Characteristics for Biological Purposes
- Impermeability to biological membranes.
- Biological stability and lack of interference with metabolic and biological processes.
- Minimal absorption of ultraviolet or visible light.
- Minimal formation of insoluble complexes with cations.
- Minimal effect of ionic composition or salt concentration.
- Limited pH change in response to temperature.
pH Regulation by Respiration
- A rising plasma H+ concentration excites the respiratory center, stimulating deeper and faster respiration, removing CO2, and decreasing H+ concentration.
- When blood pH rises, the respiratory center is depressed, respiratory rate drops, CO2 accumulates, and H⁺ is increased.
Respiratory Adjustments to Acidosis and Alkalosis
- Provides a table of expected ventilation, CO2 removal rates, etc., in various physiological states.
Renal Mechanism of Acid-Base Balance
- Key functions include conservation and reabsorption of HCO3⁻, generation of new HCO3⁻, and excretion of HCO3⁻.
Altered Blood H⁺ Concentration
- Renal mechanisms adjust to changes in blood H⁺ concentration.
- Renal excretion of H⁺ depends on CO2 levels in the peritubular capillary blood.
Bicarbonate Reabsorption & H⁺ Ion Secretion in Distal Tubules
- Crucial process for maintaining acid-base balance. A detailed explanation of the mechanisms.
- Shows how different types of intercalated cells operate.
Renal Function to Regulate Acid-Base Balance
- Conservation of bicarbonate ions (HCO⁻₃)
- Generation of new bicarbonate ions (HCO⁻₃) through excretion of buffered H⁺ and NH₄⁺ excretion
- Excretion of HCO⁻₃
- Importance of peritubular capillary blood CO₂ concentration.
Buffer pairs
- Bicarbonate (e.g., NaHCO₃, KHCO₃), Plasma proteins, Hemoglobin, and Phosphate (e.g., Na₂HPO₄, NaH₂PO₄) are important buffer pairs in the body.
Regulation of pH by Buffers
- Bicarbonate Buffer System: This system involves the interaction of carbonic acid (H₂CO₃) and its salt, sodium bicarbonate (NaHCO₃) in the same solution. HCl (strong acid) reaction is demonstrated, and reactions with a strong base NaOH.
- Phosphate Buffer System: Operation and comparison to the bicarbonate system. Acids and bases' reactions in the buffer system are explained.
- Protein Buffer System: R-COOH ↔ R-COO⁻ + H⁺ and R-NH₂ + H⁺ ↔ R-NH₃⁺. Reactions in acid and alkaline mediums, buffering capacity is explained.
Intracellular pH Regulation
- Intracellular buffering plays a crucial role.
- Example: Buffering actions of proteins
- Erythrocyte buffering in acidosis and alkalosis is explicitly stated.
Response to Metabolic Acidosis and Alkalosis
- The response of the body's systems, particularly cells and the kidneys, to metabolic acidosis and alkalosis for pH control.
Causes of Acid-Base Disorders
- Explains the causes of Metabolic Acidosis and Metabolic Alkalosis, with various examples. Details are provided, such as overproduction of fixed H⁺ and loss of HCO₃.
Summary of Renal Responses to Acidosis and Alkalosis
- Comprehensive summary table of the renal responses.
Factors Influencing Increased H+ Secretion
- Key factors that increase H⁺ secretion are highlighted.
- Importance of aldosterone, K⁺ levels, and CO2 on secretion.
Control of Tubular H+ Secretion and HCO3⁻ Reabsorption
- Explanation of the body's mechanisms for regulating the secretion of H+ and reabsorption of HCO₃⁻ to keep up with cellular processes.
Respiratory and Metabolic Compensation
- Explanation of physiological compensation responses to maintain blood pH homeostasis.
Summary of Acid-Base Disorders
- Shows a summary regarding the imbalances of CO₂, H₂O, H⁺ and HCO₃⁻, explaining roles of respiratory and renal compensation.
Causes of Metabolic Acidosis and Alkalosis
- This section details causes and examples of metabolic acidosis and alkalosis.
Respiratory and Renal Compensation
- This section details how the respiratory system and kidney adjust to maintain balance.
Intracellular Acid-Base Balance
- Mechanisms for maintaining intracellular pH.
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Description
This quiz explores the concepts of acid-base balance and homeostasis, emphasizing the importance of hydrogen ion concentration in body fluids. You'll learn about fluid compartments, the influence of acid-base balance on nerve and muscle excitability, and how it affects enzyme activity and potassium levels in the body.
