Strong and Weak Acids and Bases

These flashcards cover key concepts related to strong and weak acids and bases, including definitions, examples, and the characteristics of their dissociation.

Strong Acids

Acids that completely dissociate in solution, examples include hydroiodic acid, hydrobromic acid, sulfuric acid, and nitric acid.

Weak Acids

Acids that do not fully dissociate in solution, forming an equilibrium; an example is acetic acid.

Equilibrium Arrow

Indicates a reversible reaction; if present, it suggests the substance is a weak acid or base.

Dissociation

The process by which an acid or base separates into ions in solution.

Ka

The acid dissociation constant, a measure of the strength of an acid in solution; larger Ka values indicate stronger acids.

HCl + Water Reaction

In the reaction of hydrochloric acid with water, HCl dissociates completely to form H3O+ and Cl-.

Strong Bases

Bases that completely dissociate in solution, for instance, sodium hydroxide (NaOH), leading to full ionization.

Ammonia

A common example of a weak base that does not fully dissociate in solution.

Indicator of Strong Acids/Bases

One directional arrow in a reaction indicates a strong acid or base, while an equilibrium arrow indicates a weak acid or base.

Product-favored Reaction

A reaction with a very large Ka, indicating that the products are favored at equilibrium.