Chapter 16 Flashcards

Flashcards on Common Ion Effect and Buffer Solutions from Chapter 16.

Common Ion Effect

The presence of a common ion suppresses the ionization of a weak acid or weak base.

Le Chatelier’s Principle and Common Ion Effect

Adding CH3COONa to CH3COOH shifts the equilibrium, affecting H+ concentration.

Henderson-Hasselbalch Equation

Simplifies solutions involving the common ion effect, assuming [H+] is small.

Buffer Solutions

Chemical systems that resist pH changes by neutralizing added acid or base.

Components of a Buffer

Significant amounts of both a weak acid and its conjugate base (or a weak base and its conjugate acid).

Weak Acid in a Buffer

Neutralizes added base.

Conjugate Base in a Buffer

Neutralizes added acid.

Buffer Capacity

How much acid or base a buffer can effectively neutralize.

Optimal Buffer Capacity

Most effective when the concentrations of acid and conjugate base are equal and high.

Buffer Range

The pH range over which a particular acid and conjugate base can be effective.

Effective Buffer Range

Generally one pH unit on either side of the pKa.