Chem 111 Exam 3: Aqueous Equilibria (from prof notes)

Flashcards covering key concepts from Gen Chem II on Aqueous Equilibria.

Common Ion Effect

A phenomenon where the solubility of a weak electrolyte is reduced in a solution that already contains a common ion.

Buffer Solutions

Solutions that resist drastic changes in pH when small amounts of strong acid or strong base are added.

Acid-Dissociation Constant (Ka)

The equilibrium constant for the ionization of a weak acid, indicating its strength as an acid.

Buffer Capacity

The amount of acid or base a buffer can neutralize before the pH begins to change appreciably.

Henderson-Hasselbalch Equation

pH = pKa + log([conjugate base]/[acid]), used to calculate the pH of buffer solutions.

Solubility Product Constant (Ksp)

An equilibrium constant that expresses the solubility of a sparingly soluble ionic compound.

Selective Precipitation

The process of separating cations in a mixture by forming precipitates selectively.

Amphoterism

The ability of a substance to act as both an acid and a base.

Complex Ion

An assembly of a metal ion and one or more Lewis bases bonded to it.

Equivalence Point

The point in a titration at which the amount of titrant added is stoichiometrically equivalent to the amount of substance being titrated.