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- $$K_a = \frac{\alpha^2 \cdot C}{1 - \alpha} \approx \alpha^2 \cdot C \text{ (if } \alpha < 0.05\text{)}$$
- Concept: Relates the dissociation constant of a weak electrolyte to its degree of ionization and molar concentration.
- Notation:
- $$\alpha$$ = Degree of ionization;
- $$C$$ = Molar concentration of weak acid;
- $$K_a$$ = Acid dissociation constant.
