• Polyprotic Acids
  • Acids that can give up more than one hydrogen ion in a solution.
  • Amphoteric
  • Substances that can either act as an acid or a base.
  • Equivalence Point
  • Point in titration when exactly enough base has been added to neutralize all of the acid (or vice-versa).
  • Strong Acids
  • HCl, HBr, HI, HNO3, HClO4, HClO3, H2SO4.
  • Strong Bases
  • LiOH, NaOH, KOH, Ba(OH)2, Sr(OH)2.
  • Arrhenius Acid/Base
  • Substance that ionizes in water and produces hydrogen/hydroxide ions.
  • Bronsted-Lowry Acid/Base
  • Substance that is capable of donating/accepting a hydrogen ion.
  • Lewis Acid/Base
  • Substance that is an electron pair acceptor/donor.
  • Common Ion Effect
  • A weak acid and its conjugate base (or vice-versa) can remain in solution together without neutralizing each other.
  • Buffer
  • Solution with a very stable pH.