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AP Chemistry · Chapter 8 of 9

Acids and Bases

Analyze acid-base behavior with Bronsted-Lowry theory, pH relationships, and equilibrium constants for weak acids and bases.

Why this chapter matters

Acid-base systems appear across chemistry, from environmental chemistry to biochemical pathways and industrial processes.

What you will learn

  • Classify acids and bases and identify conjugate pairs in reactions.
  • Compute pH, pOH, and related concentrations in strong-acid or strong-base contexts.
  • Use Ka, Kb, and pKa ideas to compare weak-acid and weak-base behavior, including buffers.

Lessons in this chapter

  1. Bronsted-Lowry frameworkTrack proton transfer and identify conjugate acid-base pairs.
  2. pH and pOH calculationsConvert among [H+], [OH-], pH, and pOH with logarithmic definitions.
  3. Weak-acid and weak-base equilibriaUse Ka or Kb to estimate dissociation and relative strength.
  4. Buffers and titration curvesInterpret buffer regions, half-equivalence points, and indicator choice.

Study task

Solve a set of acid-base items including strong-acid pH, weak-acid comparison by Ka, and buffer interpretation at half-equivalence.

Chapter checkpoint

If [H3O+] = 2.0 x 10^-3 M, what is the pH?

pH = -log(2.0 x 10^-3) = 2.70 (to two decimal places).