Concept of Acids and Bases
Start with the big picture
The lesson compares Arrhenius, Brønsted–Lowry, and Lewis definitions, then introduces broader frameworks such as Lux–Flood, Usanovich, and Pearson HSAB. It explains how Ka, Kb, pKa, and pKb describe strength; how conjugate pairs differ by one proton; and why amphoteric compounds can behave as acids or bases. You will also encounter stepwise dissociation of polyprotic acids, solvent-dependent strength and leveling, and factors that influence acidity and basicity. The topic connects these principles to pH, Kw, buffering, indicators, industrial uses, and biological relevance, providing a framework for interpreting acid–base behavior across chemical contexts.
What you'll learn
- Compare Arrhenius, Brønsted–Lowry, and Lewis acid–base definitions.
- Relate Ka, Kb, and conjugate pairs to acid and base strength.
- Describe amphoteric behavior and stepwise dissociation of polyprotic acids.
- Explain how solvents and molecular features influence acidity and basicity.
- Connect pH, Kw, buffering, indicators, and acid–base applications.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
