Key Terms Definition Arrhenius Acids acid-base reactions are characterized by acids, which dissociate in aqueous solution to form hydrogen ions (H+) and bases, which form hydroxide (OH−) ions. Acids are defined as a compound or element that releases hydrogen (H+) ions into the solution. Amphoteric (of a compound, especially a metal oxide or hydroxide) able to react both as a base and as an acid. Strong Acid one that completely ionizes (dissociates) in a solution (provided there is sufficient solvent). In water, one mole of a strong acid HA dissolves yielding one mole of H+ (as hydronium ion H3O+) and one mole of the conjugate base, A−. Essentially, none of the non-ionized acid HA remains. Monoprotic an acid that donates only one proton or hydrogen atom per molecule to an aqueous solution. This contrasts with acids capable of donating more than one proton or hydrogen, which are called polyprotic acids. Diprotic a class of Arrhenius acids which can donate two protons or hydrogen cations per molecule when dissociating in aqueous solutions.
- Summer '17