Concepts of Acids, Bases, and Buffers
Start with the big picture
The lesson connects Brønsted–Lowry acid–base concepts with the chemistry of conjugate pairs and partial or near-complete dissociation. It introduces Ka, pKa, water ionization, and pH, then uses the Henderson–Hasselbalch relationship to explain buffer calculations. Buffer effectiveness depends on the balance between conjugate components, their total concentration, and proximity of pH to pKa. The topic also compares bicarbonate, phosphate, and protein buffers, including why bicarbonate functions as an open system. Special concepts include ampholytes and zwitterions, the isohydric principle, and temperature-related changes that affect pKa and Kw.
What you'll learn
- Distinguish Brønsted–Lowry acids, bases, and conjugate acid–base pairs.
- Relate acid strength to Ka and pKa, and interpret pH as a measure of hydrogen ion concentration.
- Explain how buffer composition and pH relative to pKa influence buffering effectiveness.
- Compare the physiological roles and open or closed characteristics of major buffer systems.
- Describe ampholytes, zwitterions, the isohydric principle, and temperature effects.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
