Chemical Equilibrium and Acid-Base Concepts

These flashcards cover key vocabulary and concepts related to chemical equilibrium and acid-base theories, which are crucial for understanding the course material in chemistry.

Chemical Equilibrium

The state in which the rates of forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.

Non-Reversible Reaction

A reaction that proceeds in only one direction and cannot revert to recreate reactants.

Reversible Reaction

A reaction that can proceed in both the forward and backward directions, allowing reactants to form products and products to reform reactants.

Equilibrium Constant (K)

A numerical value that expresses the ratio of conditions at equilibrium for a chemical reaction, defined as products over reactants.

Le Chatelier’s Principle

A principle stating that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance.

Dynamic System

A system characterized by constant movement and activity, here referring to the ongoing reactions in both forward and backward directions at equilibrium.

Concentration

The amount of substance (in moles) per unit volume (usually in liters) in a solution.

pH

A measure of the acidity or basicity of a solution, defined as the negative base 10 logarithm of the concentration of hydronium ions.

Strong Acid

An acid that completely dissociates in water, resulting in a high concentration of hydrogen ions.

Equilibrium Shift

The change in the position of equilibrium in response to changes in concentration, pressure, or temperature, as predicted by Le Chatelier’s Principle.

Dissociation

The process by which compounds break apart into smaller components, such as ions, in a solution.

Arrhenius Definition of Acid

An Arrhenius acid is a substance that increases the concentration of H+ ions in aqueous solution.