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Weak Acid Strong Base Titrations definitions

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Terms in this set (15)

  • ICE Chart
    A method used to calculate concentrations at equilibrium, using initial, change, and equilibrium values.
  • ICF Chart
    A method used to calculate moles in a reaction, using initial, change, and final values.
  • Molarity
    A measure of concentration, defined as moles of solute per liter of solution.
  • Equivalence Point
    The point in a titration where the amount of titrant added is stoichiometrically equal to the amount of substance in the sample.
  • Conjugate Base
    The species formed when an acid donates a proton during a chemical reaction.
  • Buffer
    A solution that resists changes in pH when small amounts of acid or base are added.
  • Henderson-Hasselbalch Equation
    An equation used to calculate the pH of a buffer solution, relating pH, pKa, and the ratio of conjugate base to acid.
  • pKa
    The negative logarithm of the acid dissociation constant, a measure of the strength of an acid.
  • pOH
    The negative logarithm of the hydroxide ion concentration, used to express the basicity of a solution.
  • Conservation of Mass
    A principle stating that mass is neither created nor destroyed in a chemical reaction.
  • Weak Acid
    An acid that partially dissociates in solution, resulting in a relatively low concentration of hydrogen ions.
  • Strong Base
    A base that completely dissociates in solution, resulting in a high concentration of hydroxide ions.
  • Sodium Nitrite
    A salt formed from the neutralization of nitrous acid by a strong base, acting as a conjugate base.
  • Kb
    The base dissociation constant, a measure of the strength of a base in solution.
  • Nitrous Acid
    A weak acid that partially dissociates in solution, forming nitrite ions and hydrogen ions.