Lesson 12.3.1

12.3.1 Titration curves and indicators Quiz: Pearson Edexcel Chemistry, Unit 12

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 12.3.1, Titration curves and indicators: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 12: Acid-base Equilibria, written with Revision Ninja.

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The 20 questions

  1. What is the pH at the equivalence point for a strong acid-strong base titration at 298 K?

    • 3.10
    • 8.70
    • 7.00
    • 14.00

  2. What is the pH at the equivalence point of a weak acid-strong base titration?

    • Greater than 7
    • Equal to 0
    • Exactly 7
    • Less than 7

  3. What is the pH at the equivalence point of a strong acid-weak base titration?

    • Greater than 7
    • Exactly 7
    • Equal to 14
    • Less than 7

  4. Where must an indicator's colour change occur on a titration curve?

    • High pH plateau
    • Zero volume point
    • Steep vertical section
    • Initial buffer region

  5. What relationship holds at the half-equivalence point during a weak acid titration?

    • pH = pKa
    • pH = Ka
    • pH = 7
    • pH = 14

  6. What feature on a titration curve signals the equivalence point?

    • Flat buffer region
    • Gradual initial rise
    • Zero pH value
    • Steep pH change

  7. What is the term for the point in a titration where an indicator changes colour?

    • Equivalence point
    • Neutral point
    • End point
    • Buffer point

  8. A 25.0 cm3 sample of 0.100 mol dm-3 hydrochloric acid is titrated, and no sodium hydroxide has been added. What is its pH?

    • 2.00
    • 13.00
    • 0.10
    • 1.00

  9. What is the pH after 10.0 cm3 of 0.100 mol dm-3 NaOH is added to 25.0 cm3 of 0.100 mol dm-3 HCl?

    • 7.00
    • 4.30
    • 1.37
    • 1.00

  10. What is the approximate pH at the equivalence point when 0.100 mol dm-3 ethanoic acid (Ka = 1.7 x 10^-5 mol dm-3) is titrated with 0.100 mol dm-3 NaOH?

    • About 8.7
    • About 3.0
    • Exactly 7.00
    • About 5.3

  11. What volume of 0.100 mol dm-3 NaOH is needed to reach the equivalence point with 25.0 cm3 of 0.200 mol dm-3 HCl?

    • 12.5 cm3
    • 25.0 cm3
    • 50.0 cm3
    • 100 cm3

  12. A weak acid is titrated with NaOH. At the half-equivalence point the pH is 4.76. What is the pKa of the acid?

    • 4.76
    • 2.38
    • 7.00
    • 9.52

  13. Which indicator is suitable for a weak acid-strong base titration with equivalence pH 8.7?

    • Bromophenol blue
    • Phenolphthalein
    • Methyl orange
    • Methyl red

  14. Using methyl orange for a weak acid-strong base titration causes what error in titre?

    • Titre too small
    • Titre too large
    • Titre doubled
    • No effect

  15. What is the pH of 25.0 cm3 of 0.100 mol dm-3 ethanoic acid (Ka = 1.7 x 10^-5 mol dm-3) before any NaOH is added?

    • 2.88
    • 4.76
    • 1.00
    • 7.00

  16. What type of mixture is formed before equivalence when titrating a weak acid with NaOH?

    • Neutral solution
    • Standard solution
    • Buffer solution
    • Saturated solution

  17. A 0.100 mol dm-3 weak acid HA with Ka = 2.0 x 10^-5 mol dm-3 is titrated with 0.100 mol dm-3 NaOH; 25.0 cm3 of acid is used. What volume of NaOH gives the half-equivalence point?

    • 6.25 cm3
    • 12.5 cm3
    • 25.0 cm3
    • 50.0 cm3

  18. What volume of 0.100 mol dm-3 NaOH neutralises 25.0 cm3 of 0.100 mol dm-3 weak monobasic acid?

    • 0.00 cm3
    • 25.0 cm3
    • 12.5 cm3
    • 50.0 cm3

  19. What is the pH after 30.0 cm3 of 0.100 mol dm-3 NaOH is added to 25.0 cm3 of 0.100 mol dm-3 HCl?

    • 7.00
    • 11.96
    • 12.50
    • 2.04

  20. Where must an indicator's colour change range fall on a titration curve?

    • Buffer region
    • Initial pH region
    • Vertical section
    • Final plateau

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