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Weak Base-Strong Acid Titrations definitions

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Termini in questo insieme (15)

  • Weak Base
    A substance that partially accepts protons in water, resulting in a basic solution with a pH above 7 before titration.
  • Strong Acid
    A substance that completely donates protons in water, causing a rapid decrease in pH when added to a base.
  • Titrant
    A solution of known concentration added during titration to react with the analyte and determine its quantity.
  • Analyte
    The substance in a titration whose concentration is being determined by reaction with a titrant.
  • ICF Chart
    A table tracking moles of reactants and products at initial, change, and final stages during titration.
  • ICE Chart
    A table using molarity to monitor concentrations at initial, change, and equilibrium for weak species.
  • Equivalence Point
    The stage in titration where moles of acid equal moles of base, resulting in complete neutralization.
  • Buffer
    A solution containing a weak acid and its conjugate base, resisting pH changes upon small additions of acid or base.
  • Henderson-Hasselbalch Equation
    A formula relating pH to pKa and the ratio of conjugate base to acid in a buffer system.
  • Conjugate Acid
    The species formed when a base accepts a proton, often influencing pH after neutralization.
  • Conjugate Base
    The species remaining after an acid donates a proton, often acting as a weak base in solution.
  • Base Dissociation Constant
    A value (Kb) expressing the extent to which a base dissociates in water, crucial for pH calculations.
  • Acid Dissociation Constant
    A value (Ka) indicating the degree to which an acid dissociates in water, derived from Kb for conjugate pairs.
  • pOH
    A measure of hydroxide ion concentration, calculated as the negative logarithm of [OH−], used to find pH.
  • 5% Approximation
    A shortcut for simplifying equilibrium calculations by neglecting small changes when the initial concentration greatly exceeds Kb.