This concept covers the three progressively broader definitions of acids and bases in chemistry. The Arrhenius definition classifies an acid as a substance that increases hydrogen ion concentration in aqueous solution and a base as one that increases hydroxide ion concentration; the Bronsted-Lowry definition generalizes this to any solvent, defining an acid as a proton donor and a base as a proton acceptor; the Lewis definition is broadest still, defining an acid as an electron-pair acceptor and a base as an electron-pair donor. These frameworks belong to acid-base chemistry within general/inorganic chemistry and build on equilibrium concepts such as water's autoionization and Le Chatelier's Principle, describing how added acids or bases shift the hydrogen/hydroxide equilibrium.
This concept covers the three progressively broader definitions of acids and bases in chemistry. The Arrhenius definition classifies an acid as a substance that increases hydrogen ion concentration i…