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Diprotic Buffers definitions

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  • Diprotic Acid
    A molecule containing two acidic hydrogens, each capable of dissociating in solution, leading to two distinct ionization steps.
  • Acidic Hydrogen
    A proton within a molecule that can be released during dissociation, contributing to the molecule's acidic properties.
  • Ka1
    The equilibrium constant describing the dissociation of the first acidic hydrogen from a molecule with more than one acidic proton.
  • Ka2
    The equilibrium constant for the removal of the second acidic hydrogen in a molecule with two acidic protons.
  • pKa1
    The negative logarithm of the first dissociation constant, indicating the strength of the initial proton release.
  • pKa2
    The negative logarithm of the second dissociation constant, reflecting the ease of losing the second proton.
  • Conjugate Base
    The species formed when an acid donates a proton, possessing one fewer hydrogen than the original acid.
  • Intermediate Form
    The partially deprotonated species in a diprotic system, having lost only one acidic hydrogen.
  • Base Form
    The fully deprotonated species in a diprotic system, with both acidic hydrogens removed.
  • Henderson-Hasselbalch Equation
    A formula relating pH, pKa, and the ratio of conjugate base to acid, adapted for each dissociation step in diprotic systems.
  • Buffer System
    A solution that resists pH changes by containing a weak acid and its conjugate base, or their equivalents in diprotic cases.
  • Sulfurous Acid
    A diprotic acid, H2SO3, used as an example for illustrating sequential proton loss and buffer calculations.
  • Hydrogen Sulfite
    The intermediate form of sulfurous acid after losing one proton, also known as bisulfite.
  • Sulfite Ion
    The base form of sulfurous acid, resulting from the loss of both acidic hydrogens.
  • Polyprotic Acid
    A molecule containing more than one acidic hydrogen, capable of undergoing multiple dissociation steps.