Lesson 5.3.2

5.3.2 Ionic equations, observations and hazards Quiz: Pearson Edexcel Chemistry, Unit 5

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 5.3.2, Ionic equations, observations and hazards: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 5: Formulae, Equations and Amounts of Substance, written with Revision Ninja.

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The 20 questions

  1. In the reaction NaCl(aq) + AgNO3(aq) -> AgCl(s) + NaNO3(aq), which species are spectator ions?

    • Na+(aq) and NO3-(aq)
    • Na+(aq) and Cl-(aq)
    • AgCl(s) and NaNO3(aq)
    • Ag+(aq) and Cl-(aq)

  2. Which is the correct ionic equation for the precipitation of silver chloride from aqueous silver ions and aqueous chloride ions?

    • Ag(s) + Cl2(g) -> AgCl(s)
    • Ag+(aq) + Cl-(aq) -> AgCl(s)
    • Ag+(aq) + Cl-(s) -> AgCl(s)
    • Ag+(aq) + Cl-(aq) -> AgCl(aq)

  3. What is the ionic equation for the neutralisation of hydrochloric acid by sodium hydroxide solution, including state symbols?

    • H+(aq) + OH-(aq) -> H2O(l)
    • H+(aq) + Cl-(aq) -> HCl(aq)
    • Na+(aq) + OH-(aq) -> NaOH(s)
    • H2(g) + O2(g) -> H2O(l)

  4. Dilute hydrochloric acid is added to solid sodium carbonate. Which observation is expected?

    • A white precipitate forms immediately
    • A brown solid is deposited on the carbonate
    • Effervescence, as carbon dioxide gas is given off
    • The solution turns blue and a gas with a pungent smell is released

  5. Which observation is expected when acidified barium chloride solution is added to a solution containing sulfate ions?

    • A white precipitate of barium sulfate forms
    • A blue precipitate of copper hydroxide forms
    • A yellow precipitate of barium iodide forms
    • A green solution and a colourless gas form

  6. A sample is warmed with sodium hydroxide solution and a gas is produced that turns damp red litmus paper blue. Which ion is most likely present?

    • Chloride, Cl-
    • Sulfate, SO4 2-
    • Carbonate, CO3 2-
    • Ammonium, NH4+

  7. When heating a flammable organic liquid in a school laboratory, which precaution is most appropriate?

    • Heat it directly over a Bunsen flame with the tube open
    • Heat it on a hotplate with the flask stoppered and the lid left on
    • Heat it in a sealed flask on a gas ring next to other experiments
    • Heat it with a water bath or electric heater, away from naked flames

  8. What mass of silver chloride (Mr = 143.5) is precipitated when excess chloride ions react with 0.0200 mol of silver ions?

    • 2.87 g
    • 1.44 g
    • 0.287 g
    • 28.7 g

  9. How many moles of hydrochloric acid are present in 25.0 cm3 of a 0.200 mol dm-3 solution?

    • 0.00125 mol
    • 0.0500 mol
    • 0.00500 mol
    • 0.0200 mol

  10. What mass of calcium carbonate (Mr = 100.1) reacts completely with 50.0 cm3 of 0.500 mol dm-3 hydrochloric acid? CaCO3 + 2HCl -> CaCl2 + H2O + CO2

    • 0.125 g
    • 2.50 g
    • 0.625 g
    • 1.25 g

  11. A reaction should give 5.00 g of product but 3.80 g is collected. What is the percentage yield?

    • 76%
    • 132%
    • 13%
    • 24%

  12. Calculate the atom economy for making ethene by the reaction C2H5OH -> C2H4 + H2O. (Mr: C2H5OH = 46.0, C2H4 = 28.0, H2O = 18.0)

    • 100%
    • 39%
    • 28%
    • 61%

  13. A burette reading has an uncertainty of +/- 0.05 cm3. A titre uses two readings and is 20.00 cm3. What is the percentage uncertainty in the titre?

    • 0.05%
    • 0.5%
    • 5%
    • 0.25%

  14. A student wants to reduce the percentage uncertainty caused by a burette reading in a titration. Which change is most effective?

    • Use a larger titre volume so the fixed reading error is a smaller fraction
    • Round each reading to the nearest whole cm3 before subtracting
    • Read the burette more quickly to save time between readings
    • Use a burette with a smaller number of graduations per cm3

  15. When zinc metal is added to aqueous copper(II) sulfate, what would be observed?

    • A white precipitate forms and the solution turns green
    • The blue solution fades and a brown-red solid deposits on the zinc
    • A black solid dissolves and the solution turns yellow
    • Bubbles of hydrogen form and the solution turns colourless immediately

  16. Which is the correct ionic equation for magnesium reacting with dilute hydrochloric acid?

    • Mg2+(aq) + 2OH-(aq) -> Mg(OH)2(s)
    • Mg(s) + 2HCl(aq) -> Mg2+(aq) + H2(g)
    • Mg(s) + 2H+(aq) -> Mg2+(aq) + H2(g)
    • Mg(s) + 2Cl-(aq) -> MgCl2(aq)

  17. 25.0 cm3 of 0.100 mol dm-3 lead(II) nitrate is added to excess sodium chloride solution. What mass of lead(II) chloride (Mr = 278.2) precipitates?

    • 1.39 g
    • 0.696 g
    • 0.0278 g
    • 0.348 g

  18. 25.0 cm3 of 2.00 mol dm-3 hydrochloric acid reacts with excess magnesium. What volume of hydrogen gas is produced at room conditions, where molar volume is 24.0 dm3 mol-1?

    • 300 cm3
    • 24 cm3
    • 600 cm3
    • 1200 cm3

  19. Why is methyl orange often preferred over phenolphthalein for titrating a strong acid with a weak base?

    • Methyl orange changes colour only in strongly alkaline solutions above pH 12
    • Phenolphthalein cannot be used with any acid because it reacts with hydrogen ions
    • Methyl orange gives a colour change at exactly pH 7 for every titration
    • Methyl orange changes colour in the acidic pH range, matching the lower pH of the equivalence point

  20. What is the ionic equation for the precipitation of calcium carbonate when aqueous calcium chloride is mixed with aqueous sodium carbonate?

    • Ca2+(aq) + 2Cl-(aq) -> CaCl2(s)
    • Ca2+(aq) + CO3 2-(aq) -> CaCO3(aq)
    • Ca2+(aq) + CO3 2-(aq) -> CaCO3(s)
    • Ca(s) + CO3 2-(aq) -> CaCO3(s)

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