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Buffer

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Intro to Chemistry

Definition

A buffer is a solution that resists significant changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid.

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5 Must Know Facts For Your Next Test

  1. Buffers maintain pH stability by neutralizing added acids (H+ ions) or bases (OH- ions).
  2. The Henderson-Hasselbalch equation, $pH = pK_a + \log \left( \frac{[A^-]}{[HA]} \right)$, is used to calculate the pH of buffer solutions.
  3. Buffers are most effective when the pH is close to the $pK_a$ value of the weak acid in the solution.
  4. Biological systems heavily rely on buffers; for example, human blood maintains its pH around 7.4 using bicarbonate buffering.
  5. Buffer capacity depends on the concentrations of the buffering agents; higher concentrations provide greater resistance to pH change.

Review Questions

  • What components make up a typical buffer solution?
  • How does the Henderson-Hasselbalch equation relate to buffers?
  • Why are buffers important in biological systems?
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