Chemistry Lecture on Acid-Base Concepts and Titration

Flashcards covering key concepts related to acid-base chemistry, titration methods, buffer systems, and solubility equilibria.

Common Ion Effect

Ionization or dissociation of a weak acid is decreased by the addition of a compound that shares a common ion with the weak acid.

Le-Chatelier Principle

States that the equilibrium will shift to the left due to the common ion effect.

Buffers

Solutions of weak acid-base conjugate pairs that resist pH changes; weak acid neutralizes added base and conjugate base neutralizes added acid.

Buffer Capacity

The amount of acid or base that can be added to a buffer without destroying its effectiveness; increases with increasing concentration of acid-base conjugate pairs.

pH Range

The range of pH values over which a buffer system works effectively; optimal to choose an acid with pKa close to the target pH.

Acid-Base Titration

A process in which a solution of a base of known concentration is slowly added to a solution of acid.

Indicators

Substances (like a pH meter) that help determine when the solution has reached the equivalence point in titration.

Phenolphthalein

A common indicator used in acid-base titrations.

Solubility Equilibria

Heterogeneous equilibria involving the dissolution or precipitation of ionic compounds.

Amphoteric Metal Oxides and Hydroxides

Substances that are soluble in strong acids or bases.

solubility is affected by

 pH, temperature, common ions, formation of complex ions

weak base conjugates

HC2H3O2/C2H3O2, NH4+/NH3, HF/F