Lesson 14.3.1

14.3.1 Redox titration calculations Quiz: Pearson Edexcel Chemistry, Unit 14

20 questions

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Lesson 14.3.1, Redox titration calculations: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 14: Redox II, written with Revision Ninja.

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The 20 questions

  1. In the titration of Fe2+ with MnO4- in acid, what is the mole ratio of MnO4- to Fe2+?

    • 1:8
    • 1:1
    • 1:5
    • 5:1

  2. What type of reaction occurs between the titrant and analyte in a redox titration?

    • Proton transfer
    • Precipitation
    • Neutralisation
    • Electron transfer

  3. Why does a potassium manganate(VII) titration not require an added indicator?

    • It is colourless
    • It changes colour
    • It forms a precipitate
    • It produces gas

  4. What colour complex does starch indicator form in the presence of iodine?

    • Bright yellow
    • Deep orange
    • Faint pink
    • Blue-black

  5. What is the mole ratio of I2 to S2O3^2- in the iodine-thiosulfate titration?

    • 1:2
    • 1:4
    • 1:1
    • 2:1

  6. Why is hydrochloric acid unsuitable for acidifying potassium manganate(VII) titrations?

    • Acid is neutralised
    • Chloride is oxidised
    • Chloride is reduced
    • Manganate is oxidised

  7. What is calculated first when processing data from a titration?

    • Moles of analyte
    • Mass of analyte
    • Concentration of analyte
    • Moles of titrant

  8. What colour change is observed at the end point when titrating iron(II) ions with manganate(VII)?

    • Pink to colourless
    • Yellow to green
    • Colourless to pink
    • Blue to black

  9. 25.0 cm3 of Fe2+ solution needs 22.50 cm3 of 0.0200 mol dm-3 MnO4- for complete reaction. What is the concentration of Fe2+?

    • 0.00900 mol dm-3
    • 0.0180 mol dm-3
    • 0.0900 mol dm-3
    • 0.450 mol dm-3

  10. 20.0 cm3 of 0.100 mol dm-3 Na2S2O3 is needed to titrate iodine. How many moles of iodine react?

    • 5.00 x 10^-4 mol
    • 2.00 x 10^-3 mol
    • 1.00 x 10^-3 mol
    • 4.00 x 10^-3 mol

  11. What is the mass of Fe2+ in 25.0 cm3 of a solution of concentration 0.0900 mol dm-3? (Ar Fe = 55.8)

    • 1.26 g
    • 0.126 g
    • 0.0126 g
    • 0.0403 g

  12. A 25.0 cm3 aliquot of Fe2+ solution needs 18.60 cm3 of 0.0200 mol dm-3 MnO4-. How many moles of Fe2+ are in the aliquot?

    • 1.86 x 10^-3 mol
    • 9.30 x 10^-3 mol
    • 7.44 x 10^-4 mol
    • 3.72 x 10^-4 mol

  13. How many electrons are gained by one manganate(VII) ion when reduced to manganese(II) in acid?

    • 3
    • 7
    • 5
    • 2

  14. How many electrons are lost by one thiosulfate ion when oxidised to tetrathionate?

    • 1
    • 6
    • 2
    • 4

  15. A 0.300 g sample containing Fe2+ needs 22.00 cm3 of 0.0200 mol dm-3 MnO4- for titration. What is the percentage of iron by mass? (Ar Fe = 55.8)

    • 40.9%
    • 81.8%
    • 4.09%
    • 12.3%

  16. If an iron(II) sample is partially oxidised by air before titration, how is the calculated concentration affected?

    • Too low
    • Too high
    • Zero
    • Unchanged

  17. Why is starch added only near the end point in an iodine-thiosulfate titration?

    • Prevents slow dissociation
    • Prevents iodine evaporation
    • Oxidises the thiosulfate
    • Increases the rate

  18. What are the moles of H+ needed to react with 15.00 cm3 of 0.0200 mol dm-3 MnO4- in acid?

    • 2.40 x 10^-3 mol
    • 1.50 x 10^-3 mol
    • 5.00 x 10^-3 mol
    • 3.00 x 10^-4 mol

  19. 25.00 cm3 of Fe2+ is titrated with 30.00 cm3 of 0.0100 mol dm-3 MnO4-. What is the concentration of Fe2+?

    • 0.0600 mol dm-3
    • 0.0120 mol dm-3
    • 0.0300 mol dm-3
    • 0.300 mol dm-3

  20. Why does using hydrochloric acid in a permanganate titration increase the titre?

    • Chloride is reduced
    • Chloride is oxidised
    • Hydrochloric acid neutralises
    • Manganate is oxidised

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