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Titrations of Diprotic and Polyprotic Acids definitions

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Terms in this set (15)

  • Diprotic Acid
    An acid with two acidic hydrogens, requiring two Ka values for buffer calculations.
  • Polyprotic Acid
    An acid with more than one acidic hydrogen, involving multiple Ka values.
  • Monoprotic Acid
    An acid with a single acidic hydrogen, using one Ka value in buffer equations.
  • Henderson Hasselbalch Equation
    A formula used to calculate pH of a buffer solution, involving pKa and concentrations of acid and base.
  • Conjugate Base
    The species formed when an acid donates a proton, typically with one less hydrogen.
  • Ka Value
    The acid dissociation constant, indicating the strength of an acid in solution.
  • pKa
    The negative logarithm of the Ka value, used in pH calculations for buffers.
  • Acidic Form
    The form of an acid with all its acidic hydrogens intact.
  • Intermediate Form
    The form of a diprotic or polyprotic acid after losing one or more acidic hydrogens.
  • Basic Form
    The form of an acid after losing all its acidic hydrogens.
  • Carbonic Acid
    A diprotic acid example, with two acidic hydrogens, used in buffer solutions.
  • Phosphoric Acid
    A triprotic acid example, with three acidic hydrogens, used in buffer solutions.
  • Molarity
    A concentration unit, moles of solute per liter of solution, used in buffer calculations.
  • Sodium Bicarbonate
    A compound used as a conjugate base in diprotic buffer solutions.
  • Sodium Carbonate
    A compound representing the basic form in diprotic buffer solutions.