equilibrium constant, often denoted as K, is a fundamental concept in chemistry that quantitatively describes the state of equilibrium in a chemical reaction. It represents the ratio of the concentrations (or partial pressures) of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. The value of K remains constant for a specific reaction at a given temperature and pressure. The magnitude of K provides information about the position of equilibrium and the extent to which the reaction has proceeded. If K is large, it indicates that the products are favored at equilibrium, while a small K suggests that the reactants are favored.

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC2H3O2 (aq) C2H3O2G (aq) + H+ (aq) At equilibrium at 25eC a 0.100 M solution of acetic acid has the following concentrations: [HC2H3O2] = 0.0990 M, [C2H3O2G] = 1.33 ˛ 10-3 M, and [H+] = 1.33 ˛ 10-3 M. The equilibrium constant, Keq, for the ionization of acetic acid at 25eC is __________