Chemistry: Examples
Arrhenius (restricted to aqueous solutions) Acids: substances that produce H+ ions in water Bases: substances that produce OH- ions in water HCl —> H+ + Cl- Bronsted-Lowry Acid-Base Reactions involve the transfer of H+ ions from one substance to another defined in terms of their ability to transfer protons Acid: substance (molecule/ion) that can transfer a proton to another substance must have H atom it can lose as H+ Base: substance that can accept a proton must have nonbonding pair of electrons to bind H+ HCl + H2O —> H3O+ + Cl- NH3 + H2O <==> NH4+ + OH- BLA BLB ammonia is arrhenius base because OH- ammonia is BLB because accepts proton Amphoteric- capable of acting as either an acid or a base (H2O) Conjugate acid-base pair: differ only in presence or absence of proton Every acid has a Conjugate Base formed by removal of proton from acid Every base has a Conjugate Acid formed by addition of proton to base **the stronger an acid, the weaker its conj.