Lesson 3.1.12.5

3.1.12.5 pH curves, titrations and indicators Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.12.5, pH curves, titrations and indicators: 20 multiple choice questions for the AQA Chemistry (7405), Unit 1: Physical chemistry, written with Revision Ninja.

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The 20 questions

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

    • 9
    • 7
    • 4
    • 14

  2. What is the pH at the equivalence point when titrating a weak acid with a strong base?

    • Exactly 7
    • Less than 7
    • Greater than 7
    • Exactly 0

  3. What is the pH at the equivalence point when titrating a strong acid with a weak base?

    • Exactly 14
    • Exactly 7
    • Greater than 7
    • Less than 7

  4. What feature on a titration pH curve corresponds to the equivalence point?

    • Flat buffer region
    • Steep vertical section
    • Horizontal plateau
    • Initial start point

  5. Which indicator is suitable for a weak acid and strong base titration?

    • Methyl red
    • Phenolphthalein
    • Bromophenol blue
    • Methyl orange

  6. Which indicator is suitable for a strong acid and weak base titration?

    • Thymolphthalein
    • Litmus paper
    • Methyl orange
    • Phenolphthalein

  7. 25.0 cm^3 of 0.100 mol dm^-3 NaOH is titrated with 0.0500 mol dm^-3 HCl. What volume of HCl is needed to reach the equivalence point?

    • 50.0 cm^3
    • 100 cm^3
    • 25.0 cm^3
    • 12.5 cm^3

  8. 20.0 cm^3 of 0.200 mol dm^-3 HCl is neutralised by 0.100 mol dm^-3 NaOH. What volume of NaOH is needed?

    • 40.0 cm^3
    • 80.0 cm^3
    • 10.0 cm^3
    • 20.0 cm^3

  9. 25.0 cm^3 of ethanoic acid is titrated with 0.100 mol dm^-3 NaOH, and 22.5 cm^3 is needed to reach the equivalence point. What is the concentration of the acid?

    • 0.100 mol dm^-3
    • 0.0900 mol dm^-3
    • 0.0450 mol dm^-3
    • 0.225 mol dm^-3

  10. What is the pH of a 0.10 mol dm^-3 strong acid at the start of its titration with a strong base?

    • 0.10
    • 13.0
    • 1.0
    • 7.0

  11. Why does a weak acid have a higher initial pH than a strong acid of equal concentration?

    • Complete dissociation
    • Higher concentration
    • Neutralisation
    • Partial dissociation

  12. Which ion reaction causes the equivalence point pH of a weak acid titration to be above 7?

    • Conjugate acid protonation
    • Conjugate base hydrolysis
    • Complete ionisation
    • Strong base precipitation

  13. A monoprotic acid solution of 25.0 cm^3 requires 20.0 cm^3 of 0.0250 mol dm^-3 NaOH to reach the equivalence point. What is the concentration of the acid?

    • 0.0250 mol dm^-3
    • 0.0400 mol dm^-3
    • 0.0100 mol dm^-3
    • 0.0200 mol dm^-3

  14. What volume of 0.10 mol dm^-3 NaOH neutralises 10.0 cm^3 of 0.050 mol dm^-3 nitric acid?

    • 20.0 cm^3
    • 10.0 cm^3
    • 2.5 cm^3
    • 5.0 cm^3

  15. Which type of titration curve has the steepest vertical section at the equivalence point?

    • Strong acid-strong base
    • Strong acid-weak base
    • Weak acid-weak base
    • Weak acid-strong base

  16. Where must an indicator colour change range lie on a pH titration curve?

    • Within steep section
    • In buffer region
    • At initial pH
    • After equivalence point

  17. Which acid-base titration combination results in an equivalence point at pH 7?

    • Weak acid-strong base
    • Weak acid-weak base
    • Strong acid-weak base
    • Strong acid-strong base

  18. What key feature of a pH curve allows selection of a suitable indicator?

    • Vertical section pH
    • Final buffer pH
    • Half-neutralisation volume
    • Initial acid pH

  19. On a weak acid-strong base pH curve, what does pH equal at half-neutralisation?

    • Ka
    • pKa
    • pH 7
    • pKw

  20. Where is the equivalence point located on a typical pH titration curve?

    • Upper flat region
    • Curve starting point
    • Vertical section midpoint
    • Half-equivalence point

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