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CAIE A-Level Chemistry AS 11.3.1 Reactivity of Halide Ions As Reducing Agents Questions

Practise ranking chloride, bromide and iodide reducing strength and using it to explain redox outcomes.

Syllabus
2028–2030
Course
Chemistry 9701
Level
AS

Exam points

  • state that reducing strength increases from Cl− to Br− to I− down Group 17
  • identify oxidation of a halide ion by its electron loss and formation of the corresponding halogen
  • explain why chloride gives the highest HX yield with concentrated H2SO4 while bromide and iodide reduce it

CAIE A-Level Chemistry AS 11.3.1 Reactivity of Halide Ions As Reducing Agents Questions question 1

[Maximum number: 1]

The solids sodium chloride and sodium iodide both react with concentrated sulfuric acid at room temperature.

With NaCl , the products are NaHSO4\mathrm{NaHSO}_{4} and HCl .
With NaI , the products are NaHSO4,HI,I2,SO2,H2O,S\mathrm{NaHSO}_{4}, \mathrm{HI}, \mathrm{I}_{2}, \mathrm{SO}_{2}, \mathrm{H}_{2} \mathrm{O}, \mathrm{S} and H2 S\mathrm{H}_{2} \mathrm{~S}.
What is the explanation for this difference in products?

A

Chloride ions will displace iodine from the solution.

B

Hydrogen chloride is more volatile than hydrogen iodide.

C

lodide ions are better reducing agents than chloride ions.

D

Sulfuric acid is able to act as a dehydrating agent with NaI .

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