Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). d. H₂CO₃

Key Concepts

Strong vs. Weak Acids

Strong acids completely dissociate in water, releasing all their protons (H+), while weak acids only partially dissociate. This distinction is crucial for understanding acid behavior in solution, as it affects pH and reactivity. Common strong acids include HCl and HNO3, whereas weak acids include acetic acid and carbonic acid (H2CO3).

Acid Ionization Constant (Ka)

The acid ionization constant (Ka) quantifies the strength of a weak acid by measuring the extent of its dissociation in water. It is defined by the equilibrium expression: Ka = [H+][A-]/[HA], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the undissociated acid. A larger Ka value indicates a stronger weak acid.

Carbonic Acid (H2CO3)

Carbonic acid (H2CO3) is a weak acid formed in solution when carbon dioxide (CO2) dissolves in water. It partially dissociates into bicarbonate (HCO3-) and hydrogen ions (H+), making it an important component in biological systems and buffering processes. Its ionization can be represented by the equation: H2CO3 ⇌ H+ + HCO3-, illustrating its weak acid nature.