Non-Bicarbonate Buffer Systems — MCQs
Which of the following methods cannot be used to precipitate proteins?
What is the most important extracellular buffer?
The pH of body fluids is stabilized by buffer systems. Which of the following compounds is the most effective buffer at physiologic pH?
Hyperkalemia and metabolic acidosis are commonly associated with which type of renal tubular acidosis?
Assertion: In a patient with chronic kidney disease (CKD) and metabolic acidosis, sodium bicarbonate should be initiated to correct acidosis. Reason: Sodium bicarbonate therapy reduces the progression of kidney disease by decreasing tubular injury and slowing fibrosis.
A person with type 1 diabetes ran out of her prescription insulin and has not been able to inject insulin for the past 3 days. The patient is hyperventilating to compensate for her metabolic acidosis. Which of the following reactions explains this respiratory compensation for metabolic acidosis?
HCO3/H2CO3 is the best buffer because it is:
The transport of CO2 in the blood is primarily influenced by which of the following factors?
A hyperventilating patient has the following ABG values: pH=7.53, pCO2=20 mmHg, HCO3= 26 mEq/L. What is the most likely diagnosis?
What is the primary mechanism for maintaining acid-base balance during prolonged vomiting?
Non-Bicarbonate Buffer Systems Indian Medical PG Practice Questions and MCQs
Question 1: Which of the following methods cannot be used to precipitate proteins?
- A. Add alcohol and acetone
- B. Using heavy metal ions
- C. Adding trichloroacetic acid
- D. Moving pH away from isoelectric pH (Correct Answer)
Explanation: ***Moving pH away from isoelectric pH*** - Proteins are **least soluble** at their **isoelectric point (pI)**, where their net charge is zero, causing them to aggregate and precipitate. - Moving the pH **away from the isoelectric point** increases the net charge on the protein, enhancing its solubility and preventing precipitation. *Add alcohol and acetone* - **Organic solvents** like alcohol and acetone reduce the dielectric constant of water, weakening the **hydrophobic interactions** that maintain protein solubility. - This leads to increased protein-protein interactions and **precipitation** as the protein unfolds or aggregates. *Using heavy metal ions* - **Heavy metal ions** (e.g., lead, mercury) are positively charged and bind strongly to the negatively charged groups on proteins, such as **carboxylates** and **sulfhydryl groups**. - This binding can disrupt protein structure, lead to aggregation, and cause **precipitation**. *Adding trichloroacetic acid* - **Trichloroacetic acid (TCA)** is a strong acid that significantly lowers the pH of the solution, causing proteins to become **protonated**. - This change in charge and the disruption of **salt bridges** and hydrogen bonds lead to protein denaturation and **precipitation**.
Question 2: What is the most important extracellular buffer?
- A. Bicarbonates (Correct Answer)
- B. Phosphate buffer
- C. Plasma protein buffer
- D. Ammonium buffer
Explanation: ***Bicarbonates*** - The **bicarbonate buffer system** is the most important extracellular buffer because its components (carbonic acid and bicarbonate) are present in high concentrations and their levels can be regulated by both the lungs (CO2 excretion) and the kidneys (bicarbonate reabsorption/secretion). - Its pKa (6.1) makes it an effective buffer against metabolically produced acids, which frequently challenge blood pH. *Phosphate buffer* - The **phosphate buffer system** is more important as an intracellular buffer and in renal tubular fluid due to its higher concentration in these compartments. - Its concentration in the extracellular fluid is relatively low compared to bicarbonate, limiting its capacity as the primary extracellular buffer. *Plasma protein buffer* - **Plasma proteins**, particularly albumin, have numerous ionizable groups and contribute to buffering in the extracellular fluid. - However, their overall buffering capacity is less significant than that of the bicarbonate system due to lower concentration compared to bicarbonate and less dynamic regulation. *Ammonium buffer* - The **ammonium buffer system** (ammonia/ammonium) is primarily important for acid-base regulation by the kidneys, where it plays a critical role in excreting excess acid, particularly in chronic acidosis. - It is not a major extracellular fluid buffer in the systemic circulation under normal physiological conditions.
Question 3: The pH of body fluids is stabilized by buffer systems. Which of the following compounds is the most effective buffer at physiologic pH?
- A. NH4OH, pKa = 9.24
- B. Na2HPO4, pKa = 12.32
- C. NaH2PO4, pKa = 7.21 (Correct Answer)
- D. CH3CO2H, pKa = 4.75
Explanation: ***NaH2PO4, pKa = 7.21*** - A buffer's maximum effectiveness is typically within 1 pH unit of its **pKa value**. - With a **pKa of 7.21**, the H2PO4⁻/HPO4²⁻ buffer system (phosphate buffer) is optimally positioned to buffer fluctuations around the physiologic pH of **7.35-7.45**. - This makes the phosphate buffer system highly effective in intracellular and urinary pH regulation. *NH4OH, pKa = 9.24* - This compound is a **weak base** with a pKa of 9.24, meaning it would be effective at a pH much higher than the physiologic range. - Its buffering capacity would be minimal at **pH 7.4**, as the system would be predominantly in one form, reducing its ability to resist pH changes. *Na2HPO4, pKa = 12.32* - This represents the **second dissociation** of phosphoric acid (HPO4²⁻ ⇌ PO4³⁻ + H⁺) with a very high **pKa of 12.32**. - This dissociation occurs at extremely alkaline pH levels, far above the physiological range. - At physiologic pH, this equilibrium would be almost entirely shifted to HPO4²⁻, providing no buffering capacity. *CH3CO2H, pKa = 4.75* - **Acetic acid** has a pKa of 4.75, making it an effective buffer in the acidic range (around pH 3.75-5.75). - It would be almost entirely dissociated at **physiologic pH**, offering very little buffering capacity against pH changes in body fluids.
Question 4: Hyperkalemia and metabolic acidosis are commonly associated with which type of renal tubular acidosis?
- A. Type II renal tubular acidosis
- B. Type I renal tubular acidosis
- C. Type IV renal tubular acidosis (Correct Answer)
- D. Type III renal tubular acidosis
Explanation: ***Type IV renal tubular acidosis*** - This type is characterized by **hypoaldosteronism** or **aldosterone resistance**, leading to impaired potassium excretion and bicarbonate reabsorption [2]. - The resulting **hyperkalemia** inhibits ammonium excretion, contributing to a **non-anion gap metabolic acidosis** [1]. *Type I renal tubular acidosis* - This is a **distal RTA** caused by a defect in acid secretion in the collecting duct, leading to an inability to acidify urine [1]. - It typically presents with **hypokalemia**, **nephrolithiasis** (kidney stones), and an alkaline urine pH. *Type II renal tubular acidosis* - This is a **proximal RTA** due to impaired bicarbonate reabsorption in the proximal tubule. - It is typically associated with **hypokalemia**, and the urine can be acidified when systemic acidosis is severe. *Type III renal tubular acidosis* - This is a rare, historically used term, sometimes referring to a combination of features from Type I and Type II RTA. - It is not routinely used in current classification systems and does not specifically or primarily feature hyperkalemia and metabolic acidosis as its defining characteristics.
Question 5: Assertion: In a patient with chronic kidney disease (CKD) and metabolic acidosis, sodium bicarbonate should be initiated to correct acidosis. Reason: Sodium bicarbonate therapy reduces the progression of kidney disease by decreasing tubular injury and slowing fibrosis.
- A. Assertion is false, but Reason is true
- B. Both Assertion and Reason are true, and Reason is the correct explanation of Assertion
- C. Assertion is true, but Reason is false
- D. Both Assertion and Reason are true, but Reason is NOT the correct explanation of Assertion (Correct Answer)
Explanation: The **Assertion** is true: **KDIGO guidelines** recommend sodium bicarbonate therapy for CKD patients when serum bicarbonate falls below **22 mEq/L** to correct metabolic acidosis [2]. - The **Reason** is also true: studies demonstrate that bicarbonate therapy has **nephroprotective effects**, reducing CKD progression through decreased **tubular injury** and **interstitial fibrosis**. However, this describes a secondary benefit rather than the primary indication for initiating therapy. *Both Assertion and Reason are true, and Reason is the correct explanation of Assertion* - While both statements are medically accurate, the Reason does not explain the primary indication for bicarbonate initiation in CKD patients. - The main purpose is **acid-base correction** and prevention of acidosis complications like **bone disease**, **muscle wasting**, and **cardiovascular effects**, not primarily nephroprotection [1], [2]. *Assertion is false, but Reason is true* - The Assertion is medically correct: sodium bicarbonate is **standard therapy** for metabolic acidosis in CKD according to nephrology guidelines. - CKD patients develop acidosis due to impaired **renal acid excretion** and reduced **bicarbonate regeneration**, making correction clinically necessary [2]. *Assertion is true, but Reason is false* - The Reason is actually supported by **clinical evidence**: randomized controlled trials show bicarbonate therapy slows CKD progression. - Mechanisms include reduced **complement activation**, decreased **endothelin production**, and preservation of **residual kidney function**.
Question 6: A person with type 1 diabetes ran out of her prescription insulin and has not been able to inject insulin for the past 3 days. The patient is hyperventilating to compensate for her metabolic acidosis. Which of the following reactions explains this respiratory compensation for metabolic acidosis?
- A. H2O ⇌ H+ + OH-
- B. H+ + NH3 ⇌ NH4+
- C. CH3CHOHCH2COOH ⇌ CH3CHOHCH2COO- + H+
- D. CO2 + H2O ⇌ H2CO3 ⇌ H+ + HCO3- (Correct Answer)
Explanation: ***CO2 + H2O ⇌ H2CO3 ⇌ H+ + HCO3-*** - This reaction represents the **bicarbonate buffer system**, which is central to maintaining **pH balance** in the body. - In response to **metabolic acidosis**, the body hyperventilates to **decrease CO2** levels, shifting the equilibrium to the left and reducing H+ which compensates for the increased acidity. *H2O ⇌ H+ + OH-* - This reaction describes the **autoionization of water**, which is fundamental but does not directly explain the body's respiratory compensation mechanism for metabolic acidosis. - While it shows the presence of H+ ions, it doesn't illustrate how the respiratory system manipulates CO2 to influence pH. *H+ + NH3 ⇌ NH4+* - This reaction represents the **ammonia buffer system** primarily active in the **kidneys** for acid excretion. - It plays a role in renal compensation for pH imbalances, but it is not the mechanism for respiratory compensation. *CH3CHOHCH2COOH ⇌ CH3CHOHCH2COO- + H+* - This represents the **dissociation of beta-hydroxybutyric acid**, a **ketone body** produced in diabetic ketoacidosis (DKA). - While DKA is the cause of the metabolic acidosis in this patient, this specific reaction describes the *production* of H+ ions, not the *respiratory compensatory mechanism* to address it.
Question 7: HCO3/H2CO3 is the best buffer because it is:
- A. Its components can be increased or decreased in the body as needed (Correct Answer)
- B. Good acceptor and donor of H+ ions
- C. Combination of a weak acid and weak base
- D. pKa near physiological pH
Explanation: ***Its components can be increased or decreased in the body as needed*** - The **bicarbonate buffer system** is unique because its components, **bicarbonate (HCO3-)** and **carbon dioxide (CO2)**, are physiologically regulated by the kidneys and lungs, respectively. - This allows for dynamic adjustment of buffer concentrations to maintain **pH homeostasis**, making it highly effective even when its pKa is not perfectly matched to physiological pH. *Good acceptor and donor of H+ ions* - While bicarbonate acts as an **acceptor of H+ ions** and carbonic acid can donate H+ ions, this characteristic is true for all effective buffer systems. - This option does not highlight the unique advantage of the bicarbonate buffer over other physiological buffers. *Combination of a weak acid and weak base* - The bicarbonate buffer system indeed consists of **carbonic acid (H2CO3)**, a weak acid, and its conjugate base, **bicarbonate (HCO3-)**. - However, this is the definition of any buffer system and doesn't explain why it's the *best* physiological buffer compared to others. *pKa near physiological pH* - The **pKa of the bicarbonate buffer system is 6.1**, which is not exactly at the physiological pH of 7.4. - While buffers are generally most effective when their pKa is close to the pH they regulate, the **open nature and physiological regulation** of the bicarbonate system compensate for this difference.
Question 8: The transport of CO2 in the blood is primarily influenced by which of the following factors?
- A. Binding to hemoglobin as carbaminohemoglobin
- B. Conversion to bicarbonate ions by carbonic anhydrase (Correct Answer)
- C. Transport as carbonic acid in red blood cells
- D. Direct dissolution in blood plasma
Explanation: ***Conversion to bicarbonate ions by carbonic anhydrase*** - This is the **primary mechanism** for CO2 transport, accounting for approximately **70%** of total CO2 transport in blood. - Inside red blood cells, CO2 combines with water to form carbonic acid (H2CO3), catalyzed by the enzyme **carbonic anhydrase**. - Carbonic acid **immediately dissociates** into hydrogen ions (H+) and **bicarbonate ions (HCO3-)**. - Bicarbonate ions then diffuse into plasma in exchange for chloride ions (chloride shift), making this the most quantitatively significant transport mechanism. - **Carbonic anhydrase** is the key enzyme that influences this process by accelerating the reaction by approximately **5000-fold**. *Binding to hemoglobin as carbaminohemoglobin* - Approximately **20-23%** of CO2 is transported by directly binding to amino groups on hemoglobin to form **carbaminohemoglobin**. - This is significant but less than bicarbonate transport. - Deoxygenated hemoglobin binds CO2 more readily than oxygenated hemoglobin (Haldane effect). *Transport as carbonic acid in red blood cells* - This is **not correct** because carbonic acid (H2CO3) is only a **transient intermediate** that exists momentarily. - It immediately dissociates into H+ and HCO3-, so CO2 is not actually transported "as carbonic acid" but rather as **bicarbonate ions**. - The carbonic acid step is part of the mechanism, but bicarbonate is the actual transport form. *Direct dissolution in blood plasma* - Only about **7-10%** of CO2 is transported dissolved directly in plasma. - CO2 has limited solubility in plasma, making this the least significant mechanism. - This dissolved CO2 contributes to the partial pressure of CO2 (PCO2) in blood.
Question 9: A hyperventilating patient has the following ABG values: pH=7.53, pCO2=20 mmHg, HCO3= 26 mEq/L. What is the most likely diagnosis?
- A. Metabolic alkalosis
- B. Metabolic acidosis
- C. Respiratory alkalosis (Correct Answer)
- D. Respiratory acidosis
Explanation: ***Respiratory alkalosis*** - The pH of 7.53 indicates **alkalemia**, and the low pCO2 (20 mmHg) is the primary driver, signifying **respiratory alkalosis** - A hyperventilating patient exhales more CO2, leading to a decrease in its partial pressure in the blood and a subsequent rise in pH - The HCO3 is within normal range (26 mEq/L), indicating **uncompensated respiratory alkalosis** *Metabolic alkalosis* - This would be characterized by a high pH and an elevated **HCO3**, but the HCO3 is within the normal range (26 mEq/L) - While it causes alkalemia, the primary disturbance here is respiratory, not metabolic *Metabolic acidosis* - This would present with a **low pH** and a low **HCO3**, which is contrary to the given ABG values - The patient's pH is elevated, indicating an alkalotic state, not acidotic *Respiratory acidosis* - This would be defined by a **low pH** and an elevated **pCO2**, which is the exact opposite of the provided ABG results - The patient's high pH and low pCO2 rule out respiratory acidosis
Question 10: What is the primary mechanism for maintaining acid-base balance during prolonged vomiting?
- A. Increased chloride reabsorption
- B. Increased potassium excretion
- C. Increased bicarbonate excretion (Correct Answer)
- D. Decreased hydrogen secretion
Explanation: ***Increased bicarbonate excretion*** - Prolonged vomiting leads to the loss of **gastric acid (HCl)**, causing **metabolic alkalosis**. The kidneys compensate by increasing the excretion of **bicarbonate (HCO3-)** to restore acid-base balance. - This renal compensation is the primary mechanism to eliminate the excess alkali from the body. *Increased chloride reabsorption* - In **metabolic alkalosis** due to vomiting, the body tends to reabsorb less chloride, not more, in an attempt to excrete bicarbonate. - **Chloride depletion** can actually hinder bicarbonate excretion by promoting sodium reabsorption with bicarbonate. *Increased potassium excretion* - **Hypokalemia** can occur with prolonged vomiting due to increased aldosterone activity and direct renal loss associated with metabolic alkalosis. - However, increased potassium excretion itself is not the primary mechanism for correcting the acid-base disorder; rather, it is a consequence or a contributing factor to the imbalance. *Decreased hydrogen secretion* - In response to alkalosis, the kidneys would typically decrease, not increase, **hydrogen ion (H+) secretion** in an effort to retain H+ and normalize pH. - Decreased H+ secretion is a compensatory mechanism, but the direct excretion of bicarbonate is more crucial for correcting the metabolic alkalosis.
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