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Weak Base Strong Acid Titrations quiz #1

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Terms in this set (10)

  • What is the relative pH at the equivalence point during the titration of a weak base with a strong acid?
    At the equivalence point of a weak base–strong acid titration, all the weak base has reacted with the strong acid, producing only the conjugate acid (a weak acid) in solution. The pH at this point will be less than 7 (acidic), because the weak acid partially ionizes, increasing the concentration of H3O+ in solution.
  • What is the purpose of using an ICF chart during a weak base–strong acid titration?
    An ICF chart helps track the moles of reactants and products at each stage of the titration, allowing you to determine which species remain and in what amounts.
  • Which equation is used to calculate pH before the equivalence point in a weak base–strong acid titration?
    The Henderson-Hasselbalch equation is used before the equivalence point because a buffer system is present.
  • What species are present in solution before the equivalence point during a weak base–strong acid titration?
    Before the equivalence point, both the weak base (conjugate base) and its conjugate acid (weak acid) are present, forming a buffer.
  • How do you determine the pH after the equivalence point in a weak base–strong acid titration?
    After the equivalence point, the pH is determined by the concentration of the excess strong acid, using its molarity and taking the negative log to find pH.
  • What happens to the weak base and strong acid at the equivalence point in a titration?
    At the equivalence point, all the weak base and strong acid have reacted completely, leaving only the conjugate acid (weak acid) in solution.
  • Why do you use an ICE chart at the equivalence point in a weak base–strong acid titration?
    An ICE chart is used to calculate the concentration of H3O+ produced by the weak acid formed at the equivalence point, which is needed to find the pH.
  • What is the role of the strong acid after the equivalence point in a titration?
    After the equivalence point, the strong acid is in excess and determines the pH of the solution because it dominates the concentration of H3O+.
  • How do you find the molarity of the strong acid after the equivalence point?
    Divide the moles of strong acid remaining by the total volume of solution to get its molarity.
  • What is the relationship between the terms 'conjugate acid' and 'weak acid' in the context of weak base–strong acid titrations?
    In this context, the conjugate acid formed from the weak base is also considered a weak acid, and the terms are interchangeable.