AP Chem Unit 8 Acids and Bases

Acid

A substance that donates hydrogen ions (H+) to a solution.

Brønsted-Lowry acid

A substance that donates hydrogen ions (H+) to a solution.

Strong acid

An acid that completely ionizes in solution.

Weak acid

An acid that does not completely ionize in solution.

Hydronium ion (H3O+)

The ion formed when a hydrogen ion (H+) interacts with water.

pH scale

A scale used to measure the strength of acids and bases.

Strong base

A base that completely ionizes in solution.

Weak base

A base that does not completely ionize in solution.

Autoionization of water

The process by which water molecules ionize to produce H+ and OH-.

Percent Ionization

A measurement of the extent of ionization of an acid.

Henderson-Hasselbalch equation

An equation used to calculate the pH of a buffer solution.

Equivalence point

The point in a titration where the amount of acid equals the amount of base.

Buffer

A solution that can resist changes in pH when small amounts of acid or base are added.

Conjugate acid-base pair

A pair consisting of an acid and its corresponding base.

Ka

The acid dissociation constant, a measure of the strength of an acid.

Kb

The base dissociation constant, a measure of the strength of a base.

pKa

The negative logarithm of the Ka; indicates the strength of an acid.

Titration

A quantitative method used to determine the concentration of an unknown acid or base.

Electrolyte

A substance that dissolves in water to produce an electrically conducting solution.

Conjugate base

The species that remains after an acid donates a hydrogen ion.

Logarithmic scale

A scale in which each unit represents a tenfold change in magnitude.

pOH

A measure of the concentration of hydroxide ions (OH-) in a solution.

Autoionization constant of water (Kw)

The product of the concentrations of H3O+ and OH- in pure water, equal to 1.0 x 10^-14.

ICE table

A table used to calculate the concentrations of reactants and products at equilibrium.