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DP IB Chemistry: HL

Topic Questions

Home / IB / Chemistry: HL / DP / Topic Questions / 18. Acids & Bases (HL only) / 18.2 Calculations Involving Acids & Bases / Structured Questions: Paper 2


18.2 Calculations Involving Acids & Bases

Question 1a

Marks: 1
a)
Hydrocyanic acid, HCN, is used in the synthesis of polymers and pharmaceuticals. It is a weak acid.
Write an equation to show the dissociation of hydrocyanic acid.

[1]

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    Question 1b

    Marks: 1
    b)
    Pyridine is an organic compound with the chemical formula C5H5N. It is a weak base.
    Write an equation to show how pyridine acts as a base.

    [1]

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      Question 1c

      Marks: 2
      c)
      Write an equation to show the reaction between hydrocyanic acid and pyridine and identify two conjugate acid-base pairs.

      [2]

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        Question 1d

        Marks: 2
        d)
        The pKa of hydrocyanic acid, HCN, is 9.2 at 298 K. Using section 21 of the Data booklet, deduce which of the two acids, ethanoic, CH3COOH, or hydrocyanic is the stronger acid.

        [2]

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          Question 2a

          Marks: 4
          a)
          Using section 21 of the Data booklet, determine the Ka of chloroethanoic acid, dichloroethanoic acid and trichloroethanoic acid and state which is the stronger acid.

          [4]

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            Question 2b

            Marks: 1
            b)
            Write the Ka expression for dichloroethanoic acid, CHCl2COOH.

            [1]

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              Question 2c

              Marks: 1
              c)
              Methylamine, CH3NH2, is a substance used to synthesise many commercially available compounds. State the Kb expression for methylamine.

              [1]

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                Question 2d

                Marks: 1
                d)
                State the relationship between Ka and Kb for an acid and its conjugate base.

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                  Key Concepts
                  Relating Kw to Ka

                  Question 3a

                  Marks: 4
                  a)
                  A solution of 0.01 mol dm-3 ethanoic acid has a pH of 3.37 at 298 K. Determine the Ka of ethanoic acid.

                  [4]

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                    Question 3b

                    Marks: 5
                    b)
                    A solution of 0.10 mol dm-3 methylamine, CH3NH2, has a pH of 11.80 at 298 K. Determine the Kb at this temperature.

                    [5]

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                      Question 3c

                      Marks: 2
                      c)
                      Determine the [H+] in a 0.10 mol dm-3 solution whose Ka = 1.00 x 10-8 at 298 K.

                      [2]

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                        Question 3d

                        Marks: 2
                        d)
                        Determine the pOH of the solution in part c).

                        [2]

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                          Question 4a

                          Marks: 3
                          a)
                          Use section 12 of the Data booklet to answer this question.

                          i)
                          Write the formula of the conjugate base of methanoic acid.

                          [1]

                          ii)
                          Determine the pKb of the conjugate base

                          [2]

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                            Question 4b

                            Marks: 1
                            b)
                            The pKa of ethanoic acid is 4.76. Determine whether the conjugate base of methanoic acid is weaker or stronger than the conjugate base of ethanoic acid.

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                              Question 4c

                              Marks: 1
                              c)
                              At 283 K the pKw of pure water is 14.54. Determine the pH at this temperature.

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                                Question 4d

                                Marks: 2
                                d)
                                Comment on the acid-base nature of water at 283 K in part c).

                                [2]

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