Explore: Acid Base Equilibrium

K_{a}} ⁠) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction HA ↽ − − ⇀ A − + H + {\displaystyle

In chemistry, an acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH via titration. Several

principle, applied to mixtures at equilibrium provides a definition of an equilibrium constant. Applications include acid–base, host–guest, metal–complex, solubility

there exists an equilibrium between the acid and its conjugate base. The equilibrium constant K is an expression of the equilibrium concentrations of

dissociation constant, Ka, of the acid, and the ratio of the concentrations of the acid and its conjugate base. Acid-base Equilibrium Reaction H A ( a c i d )

_{10}\left[{\mbox{OH}}^{-}\right]} If we multiply the equilibrium constants of a conjugate acid (such as NH4+) and a conjugate base (such as NH3) we obtain: K a × K b =

undissociated acid and its dissociation products being present, in solution, in equilibrium with each other. HA ⇌ H+ + A− Acetic acid (CH3COOH) is an

acid + base ⇌ conjugate base + conjugate acid. With an acid, HA, the equation can be written symbolically as: HA + B ⇌ A− + HB+ The equilibrium sign, ⇌

relatively small equilibrium constant values. The base is weaker when it has a lower equilibrium constant value. Bases react with acids to neutralize each

Dell, R. B.; Winters, R. W. (1967). "Quantitative Displacement of Acid-Base Equilibrium in Metabolic Acidosis". Annals of Internal Medicine. 66 (2): 312–322