Acid Base Equilibria

These flashcards cover key terms related to acid-base equilibria, their definitions, and related concepts.

Henderson-Hasselbalch equation

A formula that relates the pH of a buffer solution to the concentrations of the acid and its conjugate base.

Bronsted-Lowry Theory

A theory that defines acids as proton donors and bases as proton acceptors.

Lewis Theory

A theory that defines acids as electron pair acceptors and bases as electron pair donors.

Conjugate Acid/Base

A pair of compounds that differ by one proton (H+).

Auto-ionization of Water

The process by which water spontaneously breaks down into H+ and OH- ions.

pH

The negative logarithm of the hydrogen ion concentration, given by the formula pH = -log[H+].

Dissociation Constant (Ka)

A constant that measures the strength of an acid in solution; higher Ka indicates a stronger acid.

Weak Acid

An acid that only partially ionizes in solution.

Strong Acid

An acid that fully dissociates in solution.

pOH

The negative logarithm of the hydroxide ion concentration, given by the formula pOH = -log[OH-].

Equilibrium Constant (K)

A constant that expresses the ratio of the concentration of products to reactants at equilibrium.

Acid Dissociation Constant (Ka)

A numerical value that indicates the strength of an acid in solution.

Base Dissociation Constant (Kb)

A numerical value that indicates the strength of a base in solution.