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2 marksIdentification of Cations and Anions

CAPE Chemistry Unit 1 · May/June 2023 · Paper 2 · Question 1(f)(i)

Testing for halide ions using acidified silver nitrate solution.

Write the simplest ionic equation for the formation of the yellow precipitate when silver nitrate solution acidified with dilute nitric acid is added to an aqueous solution containing iodide ions.

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  1. 1(a)(i)State Boyle's law.[1 mark]
  2. 1(a)(ii)State Charles' law.[1 mark]
  3. 1(b)List FOUR assumptions made about gas molecules in the kinetic molecular theory with reference to ideal gases.[4 marks]
  4. 1(c)A flask has a mass of 47.392 g when empty, and 47.816 g when filled with acetone vapor at 100 °C and 745 mm Hg. If the volume of the flask is 247.3 mL,…[4 marks]
  5. 1(d)(i)State Hess' law.[2 marks]
  6. 1(d)(ii)Construct a Born–Haber cycle for the formation of lead (II) fluoride, PbF₂(s), showing clearly, using equations, the steps of the enthalpy changes involved.[6 marks]
  7. 1(d)(iii)Using the data in Table 1, calculate the lattice energy of PbF₂(s).[3 marks]
  8. 1(e)(i)State the effect of ionic charge on the magnitude of the lattice energy.[1 mark]
  9. 1(e)(ii)State the effect of ionic radius on the magnitude of the lattice energy.[1 mark]
  10. 1(f)(ii)State the result observed when concentrated ammonia solution is added to this yellow precipitate.[1 mark]
  11. 1(f)(iii)State why the silver nitrate solution is acidified when testing for iodide ions.[1 mark]
  12. 1(f)(iv)Explain why dilute hydrochloric acid is not used to acidify the silver nitrate solution in this test for iodide ions.[1 mark]
  13. 1(g)Describe the result observed when chlorine water is added to a solution of potassium bromide, followed by aqueous silver nitrate.[2 marks]

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