Write the missing names and molecular formulas for the following reactions between the carbonic acid–bicarbonate buffer system and the bicarbonate reserve.
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a. ___
b. ___
c. ___

Verified step by step guidance

1. Step 1: Understand the carbonic acid–bicarbonate buffer system, which involves the equilibrium between carbonic acid (H2CO3), bicarbonate ion (HCO3\^-), and carbon dioxide (CO2). The system helps maintain blood pH by reversible reactions.
2. Step 2: Identify the missing names and molecular formulas by recalling the key reactions: (a) the formation of carbonic acid from CO2 and water, (b) the dissociation of carbonic acid into bicarbonate and hydrogen ions, and (c) the conversion of bicarbonate back to CO2 and water.
3. Step 3: For reaction (a), write the hydration of carbon dioxide: CO2 + H2O \leftrightarrow H2CO3. Name: Carbon dioxide hydration. Molecular formula: CO2 + H2O \rightarrow H2CO3.
4. Step 4: For reaction (b), write the dissociation of carbonic acid: H2CO3 \leftrightarrow HCO3\^- + H\^+. Name: Carbonic acid dissociation. Molecular formula: H2CO3 \rightarrow HCO3\^- + H\^+.
5. Step 5: For reaction (c), write the reverse reaction where bicarbonate combines with hydrogen ions to form carbonic acid, which then decomposes to CO2 and water: HCO3\^- + H\^+ \leftrightarrow H2CO3 \leftrightarrow CO2 + H2O. Name: Bicarbonate buffering and CO2 release.

Key Concepts

Carbonic Acid–Bicarbonate Buffer System

This buffer system maintains blood pH by balancing carbonic acid (H2CO3) and bicarbonate ions (HCO3-). It regulates acidity through reversible reactions involving CO2, helping to neutralize excess acids or bases in the body.

Bicarbonate Reserve

The bicarbonate reserve refers to the pool of bicarbonate ions available in the blood to neutralize acids. It acts as a buffer capacity, replenishing bicarbonate ions when they are consumed during acid-base reactions to maintain pH stability.

Chemical Equations of the Buffer Reactions

Understanding the specific chemical reactions, including the formation and dissociation of carbonic acid and bicarbonate ions, is essential. These equations show how CO2, H2CO3, HCO3-, and H+ interact to maintain acid-base balance.