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Diprotic Acids and Bases definitions

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  • Diprotic Acid
    A molecule capable of donating two protons in two sequential steps, each with its own equilibrium constant.
  • Diprotic Base
    A species able to accept two protons, with each acceptance described by a separate equilibrium constant.
  • Ka1
    The equilibrium constant for the removal of the first proton from a diprotic acid, always larger than the second.
  • Ka2
    The equilibrium constant for the removal of the second proton from a diprotic acid, always smaller than the first.
  • Kb1
    The equilibrium constant for the acceptance of the first proton by a diprotic base.
  • Kb2
    The equilibrium constant for the acceptance of the second proton by a diprotic base.
  • Kw
    The ion-product constant for water, equal to 1.0 x 10^-14 at 25°C, linking acid and base equilibria.
  • Amphoteric Species
    An intermediate form that can act as either an acid or a base, depending on the reaction conditions.
  • Conjugate Base
    The form of an acid after it donates a proton, capable of further proton loss or gain.
  • Equilibrium Constant
    A value expressing the ratio of products to reactants at equilibrium for a reversible chemical reaction.
  • Fully Protonated Form
    The state of a diprotic acid containing both acidic hydrogens, behaving like a monoprotic acid.
  • Intermediate Form
    A species with one removable hydrogen, able to act as either an acid or a base in diprotic systems.
  • Hydrogen Sulfate
    A common amphoteric species that can donate or accept a proton, often used to illustrate acidic amphoterism.
  • Hydrogen Carbonate
    A basic amphoteric species, also known as bicarbonate, capable of both donating and accepting protons.
  • Polyprotic Species
    A molecule with more than one ionizable hydrogen, including diprotic and triprotic acids and bases.