Ka (Acid Dissociation Constant):

• • Measures the strength of an acid in solution.

  • Specifically, it quantifies the extent to which an acid donates protons (H⁺) to water.

Kb (Base Dissociation Constant):

• • Measures the strength of a base in solution.

  • Specifically, it quantifies the extent to which a base accepts protons or produces hydroxide ions (OH⁻) in water.

Understanding Acid-Base Dissociation

Dissociation: The process in which molecules (or ionic compounds) break apart in solution to form ions.

• For Acids (HA):   HA⇌H++A−

• For Bases (B):   B+H2O⇌BH++OH−

Interpreting Ka and Kb Values

• Stronger Acids: Higher Ka values; they dissociate more in solution, producing more H⁺ ions.

• Weaker Acids: Lower Ka values; they dissociate less.

• Stronger Bases: Higher Kb values; they dissociate more in solution, producing more OH⁻ ions.

• Weaker Bases: Lower Kb values; they dissociate less.