General Chemistry II - Acids and Bases

This set of flashcards covers key vocabulary terms and definitions related to acids and bases as taught in General Chemistry II.

Acid

A substance that produces H+ ions in aqueous solution (Arrhenius definition).

Base

A substance that produces OH- ions in aqueous solution (Arrhenius definition).

Brønsted-Lowry Acid

A substance that donates H+ ions.

Brønsted-Lowry Base

A substance that accepts H+ ions.

Amphoteric Species

A molecule that can act as either an acid or a base.

Lewis Acid

Any species that accepts a lone pair of electrons.

Lewis Base

Any species that donates a lone pair of electrons.

Strong Acid

An acid that completely dissociates in water.

Weak Acid

An acid that does not fully dissociate in water.

Ionization Constant (Ka)

A measure of the strength of an acid in solution.

Superacids

Substances that are more efficient H+ donors than 100% H2SO4.

Hydronium Ion (H3O+)

The ion formed when H+ interacts with water.

Autoionization of Water

Water acts as both an acid and a base, represented by the equilibrium Kw = [H3O+][OH-].

pH Scale

A logarithmic scale used to specify the acidity or basicity of a solution.

pKa

The negative logarithm of the acid dissociation constant (Ka), indicating acid strength.

Conjugate Acid

The species formed when a base accepts a proton.

Conjugate Base

The species that remains after an acid donates a proton.

Hydrolysis

A reaction between an ion and water in which the ion acts as an acid or a base.

Percent Ionization

The percentage of a weak acid or base that ionizes in solution.

Hydrolysis of Salts

The process by which salt ions interact with water, affecting the pH of the solution.

Inductive Effect

The electronic effect transmitted through σ-bonds in a molecule due to electronegativity.

Oxyacids

Acids that contain oxygen, often characterized by their acidic properties.