What does Le Chatelier's principle describe?

Le Chatelier's principle describes how a system at equilibrium responds to changes in external conditions. When an equilibrium system experiences a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium state. This principle is essential for understanding how equilibrium shifts occur in chemical reactions.

For example, if a reactant concentration is increased, the system will favor the forward reaction to use up that added reactant, shifting the equilibrium position. Similarly, if the temperature of an exothermic reaction is increased, the equilibrium will shift towards the reactants to absorb that extra heat. This principle is fundamental in predicting the direction of a shift in a chemical reaction when conditions change, making it a cornerstone of chemical equilibrium studies.

The other options focus on specific topics—such as reaction rates, properties of acids, and electrolyte dissociation—which do not encompass the broader implications of Le Chatelier's principle concerning equilibrium systems.