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Acids, bases and titrations

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OCR AS and A-level Chemistry past-paper questions since 2016 · 90 parts · mark schemes follow the questions · www.chemistryaleveltutor.com · Questions and mark schemes © OCR

1. June 2025 · Paper 1 · Q4 · 1 marks ·
4 What volume, in cm3, of 0.250 mol dm–3 barium hydroxide solution is required to exactly neutralise 25.0 cm3 of 0.115 mol dm–3 hydrochloric acid? Ba(OH)2(aq) + 2HCl (aq) BaCl 2(aq) + 2H2O(l) A 5.75 B 11.50 C 23.00 D 54.35 Your answer [1]
2. June 2025 · AS Paper 1 · Q7 · 1 marks ·
7 Which of the following is not a redox reaction? A CH4(g) + 2O2(g) CO2(g) + 2H2O(l) B NaOH(aq) + HCl (aq) NaCl (aq) + H2O(l) C 2KCl O3(s) 2KCl (s) + 3O2(g) D Fe(s) + H2SO4(aq) FeSO4(aq) + H2(g) Your answer [1]
3. June 2025 · Paper 1 · Q19(b)(i) · 2 marks ·
(b) (i) Nitrous acid, HNO2, is a weak monobasic acid. Predict whether the pH of 0.150 mol dm–3 HNO2 is higher, lower or the same as the pH of 0.150 mol dm–3 nitric acid, HNO3. Explain your answer. Prediction ........................................................ Explanation ...................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... ..................................................................................................................................................... [2]
4. June 2025 · AS Paper 2 · Q1(a) · 1 marks ·
1 A student is investigating the enthalpy change of neutralisation for a strong acid and a strong alkali. (a) Explain what is meant by an alkali. .......................................................................................................................................................... ..................................................................................................................................................... [1]
5. June 2025 · AS Paper 2 · Q1(b) · 1 marks ·
(b) Write the ionic equation for the neutralisation reaction between an acid and an alkali. ..................................................................................................................................................... [1]
6. June 2025 · AS Paper 2 · Q3(a)(i) · 1 marks ·
3 Malic acid tablets are sold as a health supplement. A student carries out a titration to determine the mass of malic acid, C4H6O5, in one tablet. The student follows the method below: Step 1 Crush three tablets, transfer the powder into a beaker and dissolve in distilled water. Step 2 Transfer the solution into a 250.0 cm3 volumetric flask and make up to the mark with distilled water. Step 3 Pipette 25.0 cm3 of the solution from Step 2 into a conical flask and add a few drops of indicator. Step 4 Titrate this solution with 0.0800 mol dm–3 sodium hydroxide, NaOH, in the burette. The equation for the neutralisation reaction is: C4H6O5 + 2NaOH C4H4O5Na2 + 2H2O (a) The student takes burette readings to the nearest 0.05 cm3. The student’s readings are shown in the table. The rough titre has been omitted. (i) Complete the table below. Titration 1 2 3 Final reading / cm3 23.60 46.70 25.65 Initial reading / cm3 0.30 23.65 2.50 Titre / cm3 ................................ ................................ ................................ [1]
7. June 2025 · AS Paper 2 · Q3(a)(ii) · 1 marks ·
(ii) Calculate the mean titre of NaOH that the student should use to analyse the results. Mean titre = ................................................. cm3 [1]
8. June 2025 · AS Paper 2 · Q3(a)(iii) · 5 marks ·
(iii) Calculate the mass, in mg, of malic acid in one tablet. Assume that malic acid (molar mass 134.0 g mol–1) is the only acid in the tablets. Give your answer to 3 significant figures. Mass of malic acid ................................................... mg [5]
9. June 2025 · AS Paper 2 · Q3(b) · 2 marks ·
(b) Another student carries out the same experiment. Instead of rinsing the burette used in Step 4 with 0.0800 mol dm–3 NaOH, the student rinses with water before filling it up with 0.0800 mol dm–3 NaOH. State and explain how this error would affect the titre. .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... ..................................................................................................................................................... [2]
10. June 2024 · Paper 1 · Q19(b)(i) · 5 marks ·
(b) A student titrates a 10.0 cm3 sample of ethanoic acid, CH3COOH, against an aqueous solution of 0.0560 mol dm–3 Ba(OH)2. 2CH3COOH + Ba(OH)2 Ba(CH3COO)2 + 2H2O The student used a pH meter to measure the pH of the mixture after every addition of Ba(OH)2 throughout the titration. The student’s results are shown below. 12 11 10 9 8 7 pH 6 5 4 3 2 1 0 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 volume of Ba(OH)2 / cm3 (i) Draw a best-fit curve on the graph and calculate the concentration of the CH3COOH solution. CH3COOH concentration = .......................................... mol dm–3 [5]
11. June 2024 · Paper 1 · Q21(a) · 3 marks ·
21 This question is about redox reactions and electrode potentials. (a) The flowchart shows some reactions of barium and its compounds. Barium Reaction 1 Barium oxide Reaction 2 Barium hydroxide Reaction 3 Barium chloride • Write balanced equations for Reaction 1 and Reaction 2. • Identify the type of reaction in Reaction 3. Reaction 1: equation ....................................................................................................................... Reaction 2: equation ....................................................................................................................... Reaction 3: type of reaction ............................................................................................................ [3]
12. June 2024 · AS Paper 1 · Q22(a) · 1 marks ·
22 This question is about the reactions of acids. (a) What is the difference between a strong acid and a weak acid? .......................................................................................................................................................... ..................................................................................................................................................... [1]
13. June 2024 · AS Paper 1 · Q22(b)(i) · 1 marks ·
(b) Ethanoic acid, CH3COOH, is found in some descalers to soften hard water. A student carries out a titration with a standard solution of sodium carbonate, Na2CO3, to determine the percentage composition by mass of CH3COOH in a descaler. The equation is shown below. 2CH3COOH + Na2CO3 2CH3COONa + CO2 + H2O (i) The method is outlined below: • Dissolve 6.50 g of the descaler in distilled water. • Transfer the solution into a 250.0 cm3 volumetric flask. • Make up to the mark with distilled water and invert several times. • Pipette 25.0 cm3 of this solution into a conical flask and add a few drops of indicator. • Titrate this solution with 0.200 mol dm–3 Na2CO3(aq), in the burette. The student carries out a trial titration, followed by further titrations. The results are shown in the table below. The trial titration has been omitted. Titration 1 2 3 Final reading / cm3 48.95 24.15 48.35 Initial reading / cm3 24.55 0.00 24.10 Titre / cm3 Complete the table by adding the titres. [1]
14. June 2024 · AS Paper 1 · Q22(b)(ii) · 1 marks ·
(ii) Calculate the mean titre, to the nearest 0.05 cm3, that the student should use for analysing these results. mean titre = ................................................... cm3 [1]
15. June 2024 · AS Paper 1 · Q22(b)(iii) · 5 marks ·
(iii) Calculate the percentage composition by mass of CH3COOH in the descaler. Assume that CH3COOH is the only acid in the descaler. Give your answer to 3 significant figures. percentage composition by mass = ..................................................... % [5]
16. June 2024 · Paper 2 · Q23(b)(i) · 3 marks ·
(b) (i) In Step 2, Na2CO3(aq) removes the sulfuric acid catalyst and any unreacted compound G from the mixture. Write equations for this removal. Removal of sulfuric acid .......................................................................................................................................................... Removal of unreacted compound G O OH OH Compound G [3]
17. June 2024 · Paper 3 · Q1(d) · 5 marks ·
(d) A student is provided with hydrated copper(II) nitrate, Cu(NO3)2•3H2O. The student needs to prepare a standard solution of Cu(NO3)2•3H2O with a concentration of 0.200 mol dm–3. The student has access to usual laboratory apparatus and equipment. Describe how the student would prepare 100.0 cm3 of this solution, giving quantities, apparatus and method. .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .......................................................................................................................................................... .................................................................................................................................................... [5]
18. June 2023 · Paper 1 · Q4 · 1 marks · AO2
4 40.0 cm3 of 0.200 mol dm–3 HCl is added to 60.0 cm3 of 0.100 mol dm–3 NaOH. What is the concentration of the resulting solution? A 0.0200 mol dm–3 HCl and 0.0200 mol dm–3 NaCl B 0.0200 mol dm–3 HCl and 0.0400 mol dm–3 NaCl C 0.0200 mol dm–3 HCl and 0.0600 mol dm–3 NaCl D 0.0600 mol dm–3 HCl and 0.0200 mol dm–3 NaCl Your answer [1]
19. June 2023 · Paper 1 · Q20(c)(i) · 1 marks · AO2
(c) A student reacts 1.00 g of strontium carbonate, SrCO3, with an excess of dilute nitric acid, HNO3. A gas is produced. (i) Construct the equation for this reaction. ...................................................................................................................................... [1]
20. June 2023 · Paper 1 · Q20(d)(ii) · 3 marks · AO1, 3
(ii) Explain why these two reactions of magnesium produce the same volume of gas but at different rates. ........................................................................................................................................... ........................................................................................................................................... ........................................................................................................................................... ........................................................................................................................................... ...................................................................................................................................... [3]
21. June 2023 · AS Paper 1 · Q22(a) · 1 marks · AO1
22 This question is about reactions involving acids. (a) Hydrochloric acid and nitric acid are classified as strong acids. What is meant by a strong acid? ................................................................................................................................................... .............................................................................................................................................. [1]
22. June 2023 · AS Paper 1 · Q22(b)(i) · 1 marks · AO2
(b) Write equations for the reactions below. State symbols are not required. (i) The reaction of copper(II) oxide with dilute hydrochloric acid. ...................................................................................................................................... [1]
23. June 2023 · AS Paper 1 · Q22(b)(ii) · 2 marks · AO2
(ii) The reaction of ammonium carbonate with dilute nitric acid. ...................................................................................................................................... [2]
24. June 2023 · AS Paper 1 · Q22(c)(i) · 1 marks · AO1
(c) A student carries out an investigation to identify an unknown Group 1 metal M. • The student reacts 2.62 g of the Group 1 metal, M, with water. A solution of the alkali, MOH(aq), is formed. • The student makes this solution of MOH(aq) up to 250.0 cm3 with water. • The student pipettes 25.0 cm3 of this MOH(aq) solution into a conical flask. • The student titrates this 25.0 cm3 volume of MOH(aq) with 0.165 mol dm–3 H2SO4(aq). The equation is shown below. 2MOH(aq) + H2SO4(aq) M2SO4(aq) + 2H2O(l) (i) Name the type of flask that the student should use to make up the 250.0 cm3 solution of MOH(aq). ...................................... flask [1]
25. June 2023 · AS Paper 1 · Q22(c)(ii) · 1 marks · AO1
(ii) The student takes burette readings to the nearest 0.05 cm3. The student’s readings are shown in the table. The rough titre has been omitted. Complete the table below. Final reading 20.25 40.85 25.85 / cm3 Initial reading 0.00 20.25 5.50 / cm3 Titre / cm3 ................................ ................................ ................................ [1]
26. June 2023 · AS Paper 1 · Q22(c)(iii) · 1 marks · AO2
(iii) Calculate the mean titre of H2SO4, to the nearest 0.05 cm3, that the student should use to analyse the results. mean titre = ................................................... cm3 [1]
27. June 2023 · AS Paper 1 · Q22(c)(iv) · 4 marks · AO3
(iv) Calculate the amount, in mol, of MOH in 25.0 cm3 of solution and determine the identity of the Group 1 metal M. metal M = .......................................................... [4]
28. June 2023 · Paper 3 · Q5(a) · 6 marks · AO2
5 Aspirin tablets are used for pain relief. The structure of aspirin is shown below. O OH O O Aspirin (a) A student uses the reaction of aspirin with cold NaOH(aq) to determine the mass of aspirin in one tablet. In this reaction, 1 mol of aspirin reacts with 1 mol of cold NaOH(aq). The student’s method is outlined below. Step 1 The student reacts three aspirin tablets with 100 cm3 of 0.500 mol dm–3 NaOH(aq). The NaOH is in excess. A colourless solution forms. Step 2 The colourless solution from Step 1 is made up to 250.0 cm3 with distilled water. Step 3 A 25.00 cm3 sample of the diluted solution from Step 2 is titrated with 0.200 mol dm–3 HCl (aq) in the burette. The HCl (aq) reacts with excess NaOH(aq) that remains in Step 1: NaOH(aq) + HCl (aq) NaCl (aq) + H2O(l) The student repeats the titration to obtain concordant (consistent) titres. Titration results The trial titre has been omitted. The burette readings have been read to the nearest 0.05 cm3. 1 2 3 Final reading / cm3 23.10 45.40 27.40 Initial reading / cm3 0.00 23.10 5.00 Analysis of results From the results, the student can determine the following. 1. The amount, in mol, of excess NaOH(aq) that remains after the reaction of aspirin with NaOH(aq). 2. The amount, in mol, of NaOH(aq) that reacted with the aspirin. Use the results to determine the mass, in mg, of aspirin in one aspirin tablet. mass of aspirin in one tablet = ................................................... mg [6]
29. June 2023 · Paper 3 · Q6(b)(i) · 2 marks · AO2
(b) Dilute nitric acid reacts with aluminium oxide to form a solution of aluminium nitrate. (i) Write an equation for this reaction. ...................................................................................................................................... [2]
30. June 2022 · AS Paper 1 · Q3 · 1 marks · AO1
3 Which compound is an alkali? A CH3COOH B CH3OH C HNO3 D NH3 Your answer [1]
31. June 2022 · Paper 1 · Q19(a)(i) · 2 marks · AO1
19 This question is about acids and buffer solutions. (a) Succinic acid, HOOC(CH2)2COOH, is a weak dibasic acid that is used in tablet form in health supplements. A student plans to determine the mass of succinic acid in one tablet of a succinic acid health supplement. The student carries out a titration with potassium hydroxide. The end point occurs when both acidic protons in succinic acid have been replaced as shown in Equation 19.1. HOOC(CH2)2COOH + 2KOH KOOC(CH2)2COOK + 2H2O Equation 19.1 The student uses the following method. Stage 1 The student crushes four tablets of the health supplement and dissolves the powdered tablets in distilled water. Stage 2 The student makes up the solution from Stage 1 to 250.0 cm3 in a volumetric flask. Stage 3 The student titrates 10.0 cm3 portions of the solution obtained in Stage 2 with 0.0600 mol dm–3 potassium hydroxide, using phenolphthalein as the indicator. The student carries out a trial titration, followed by three further titrations. The results are shown below. Titration Trial 1 2 3 Final burette reading / cm3 25.25 23.75 25.35 25.75 Initial burette reading / cm3 2.50 1.30 2.65 3.20 Titre / cm3 (i) Complete the table and calculate the mean titre that the student should use for analysing the results. mean titre = .................................................. cm3 [2]
32. June 2022 · Paper 1 · Q19(a)(ii) · 5 marks · AO2, 3
(ii) Use the student’s results and Equation 19.1 to calculate the mass, in mg, of succinic acid in one tablet of the health supplement. Give you answer to 3 significant figures. mass = ................................................... mg [5]
33. June 2022 · Paper 1 · Q21(b)(ii) · 1 marks · AO3
(ii) 10 cm3 of dilute sulfuric acid is added to 10 cm3 of the colourless solution of Ba(OH)2. Write an ionic equation, including state symbols, for the reaction. ...................................................................................................................................... [1]
34. June 2022 · Paper 1 · Q21(c)(ii) · 2 marks · AO2
(ii) Huntite is a carbonate mineral with the chemical formula Mg3Ca(CO3)4. Huntite reacts with dilute hydrochloric acid to produce bubbles of a gas and a colourless solution. Construct the equation for the reaction. Include state symbols. ...................................................................................................................................... [2]
35. June 2022 · AS Paper 2 · Q1(a)(i) · 1 marks · AO1
1 Lime is a citrus fruit containing citric acid, C6H8O7. (a) Citric acid is a weak organic acid. (i) What is meant by an acid? ...................................................................................................................................... [1]
36. June 2022 · AS Paper 2 · Q1(a)(ii) · 1 marks · AO1
(ii) What is meant by an acid that is weak? ........................................................................................................................................... ...................................................................................................................................... [1]
37. June 2022 · AS Paper 2 · Q1(b)(i) · 4 marks · AO1
(b) A student carries out a titration to determine the mass of citric acid in a lime. The student follows the method below: • Squeeze the juice out of two limes. • Transfer the juice into a 250.0 cm3 volumetric flask and make up to the mark with distilled water. • Pipette 25.0 cm3 of the diluted lime juice into a conical flask and add a few drops of phenolphthalein indicator. • Titrate this solution with 0.800 mol dm–3 NaOH(aq). The student carries out a trial titration, followed by three further titrations. The diagram shows the burette readings for the three further titrations. Each reading is measured to the nearest 0.05 cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading 0 27 0 27 0 27 1 28 1 28 1 28 2 29 2 29 2 29 (i) Record the student’s burette readings in the table below. Calculate the mean titre, to the nearest 0.05 cm3, that the student should use to analyse the results. Titration 1 Titration 2 Titration 3 Final reading / cm3 Initial reading / cm3 Titre / cm3 mean titre .................................................. cm3 [4]
38. June 2022 · AS Paper 2 · Q1(b)(ii) · 5 marks · AO2
(ii) Citric acid, C6H8O7, is neutralised by NaOH as shown in the equation below. C6H8O7 + 3NaOH Na3C6H5O7 + 3H2O Calculate the mass, in g, of citric acid in one lime. Assume that citric acid (Mr = 192.0) is the only acid in lime juice. mass of citric acid in one lime = ...................................................... g [5]
39. June 2022 · AS Paper 2 · Q1(c) · 2 marks · AO3
(c) The student’s teacher thinks that there is an unnecessary safety risk in using a sodium hydroxide concentration of 0.800 mol dm–3 for the titration. Suggest how the student could modify the method using a sodium hydroxide concentration of 0.200 mol dm–3 instead of 0.800 mol dm–3. The student should aim to have the same titre as in the original method. Justify your answer. ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................. [2]
40. November 2021 · AS Paper 1 · Q3 · 1 marks · AO1
3 Which compound releases hydroxide ions when it dissolves in water? A CH3COOH B HNO3 C H2SO4 D NH3 Your answer [1]
41. November 2021 · AS Paper 1 · Q7 · 1 marks · AO2
7 After delivering a solution from a pipette, a droplet remains in the tip of the pipette. How should a student ensure that the pipette delivers the volume of solution stated on the pipette? A Fill the pipette just above the graduation line to compensate for the volume of the droplet that remains in the tip. B Leave the droplet in the tip. C Shake the pipette to force out the droplet left in the tip. D Use a pipette filler to force the droplet out of the tip. Your answer [1]
42. November 2021 · Paper 1 · Q18(a) · 2 marks · AO1, 2
18 A student carries out an experiment to determine the percentage by mass of copper in an ore containing copper in its +2 oxidation state. The student is provided with a sample of the copper ore, 1 mol dm–3 potassium iodide, KI(aq), and 0.0200 mol dm–3 sodium thiosulfate, Na2S2O3. The student’s method is outlined below. Step 1 Add an excess of warm nitric acid to 2.50 g of the ore. The copper(II) compounds in the ore react, forming aqueous copper(II) nitrate. Step 2 Filter the mixture to remove the unreacted rock. Neutralise the filtrate. Step 3 Add an excess of aqueous potassium iodide, KI(aq). A precipitate of copper(I) iodide and a solution of iodine, I2(aq), forms. Step 4 Titrate the mixture from Step 3 using 0.0200 mol dm–3 sodium thiosulfate, Na2S2O3 in the burette. I2(aq) + 2S2O3 2–(aq) → 2I–(aq) + S4O6 2–(aq) 26.55 cm3 of 0.0200 mol dm–3 Na2S2O3 are required to reach the end point. (a) In Step 1, the student observed that bubbles of gas were produced. Suggest the formula of the copper(II) compound which reacted with HNO3 to form the gas, and write a full equation for the reaction. Formula: .................................................................................................................................... Equation: .............................................................................................................................. [2]
43. November 2021 · Paper 1 · Q18(f) · 2 marks · AO3
(f) The student then modifies the method in order to obtain a more accurate value for the percentage by mass of copper in the ore. The student decides to use 25.00 g of the copper ore in Step 1. What further modifications should the student make to produce a more accurate value for the percentage by mass of copper in the ore? ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................. [2]
44. November 2021 · AS Paper 2 · Q3(a) · 1 marks · AO2
3 Glutaric acid is used in the production of polymers. The formula of glutaric acid can be represented as HOOC(CH2)nCOOH, where n is a whole number. A student carries out a titration to find the value of n. 1. The student dissolves 2.891 g of glutaric acid in water and makes up the solution to 250.0 cm3 in a volumetric flask. 2. The student transfers 25.0 cm3 of this solution into a conical flask. 3. The student titrates the solution with 0.240 mol dm–3 NaOH(aq) in the burette. Equation: HOOC(CH2)nCOOH(aq) + 2NaOH(aq) NaOOC(CH2)nCOONa(aq) + 2H2O(l) The student uses phenolphthalein as the indicator. Phenolphthalein is colourless in acid and pink in alkali. (a) State the colour change observed at the end point of the titration. Colour from ....................................................... to ....................................................... [1]
45. November 2021 · AS Paper 2 · Q3(b)(i) · 1 marks · AO2
(b) The student carries out a trial titration followed by three further titrations, 1, 2 and 3. The results are shown in the table below. Titration Trial 1 2 3 Final reading / cm3 18.70 36.55 18.30 36.60 Initial reading / cm3 0.20 18.50 0.10 18.30 Titre / cm3 (i) Complete the table to show the titre in each titration. [1]
46. November 2021 · AS Paper 2 · Q3(b)(ii) · 1 marks · AO2
(ii) Why does the student carry out a trial titration? ........................................................................................................................................... ...................................................................................................................................... [1]
47. November 2021 · AS Paper 2 · Q3(b)(iii) · 1 marks · AO2
(iii) Calculate the mean titre of NaOH(aq) that the student should use for analysing the results. mean titre = .................................................. cm3 [1]
48. November 2021 · AS Paper 2 · Q3(c) · 5 marks · AO2, 3
(c) Calculate the value of n in HOOC(CH2)nCOOH. Give your answer to the nearest whole number. n = .......................................................... [5]
49. November 2021 · AS Paper 2 · Q3(d) · 2 marks · AO3
(d) A 25.0 cm3 pipette was used to measure out the 25.0 cm3 of glutaric acid solution for each titration. Before use, one student washed the pipette out with water instead of the glutaric acid solution. State the effect of this mistake on the titre. Explain your answer. Effect ......................................................................................................................................... Explanation ............................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... [2]
50. November 2021 · Paper 3 · Q1(d) · 4 marks · AO1, 2
(d) Compound A has the following percentage composition by mass: Ca, 81.10%; N, 18.90%. A student reacts compound A with water to form alkaline gas B and alkali C. Identify A, B and C and write the equation for the reaction of compound A with water. ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................. [4]
51. November 2021 · Paper 3 · Q1(e) · 4 marks · AO2
(e) The structure of lactic acid is shown below. OH OH O lactic acid Complete and balance the equations for two reactions of lactic acid. Reaction with sodium carbonate CH3CH(OH)COOH + .................... ............................................................................................... Reaction with aluminium CH3CH(OH)COOH + .................... ............................................................................................... [4]
52. November 2021 · Paper 3 · Q3(a) · 5 marks · AO1, 2
3 This question is about carboxylic acids. Compound D is a cis stereoisomer of an unsaturated organic acid with the general formula CnH2n–1COOH. A student plans to analyse acid D by carrying out a titration. (a) A student first prepares 250.0 cm3 of a standard solution of 0.150 mol dm–3 Ba(OH)2 for the titration. The student is provided with solid Ba(OH)2 and usual laboratory apparatus and equipment. Describe how the student would prepare the standard solution, giving full details of quantities, apparatus and method. ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................. [5]
53. November 2021 · Paper 3 · Q3(b) · 7 marks · AO2, 3
(b) The student prepares a 100.0 cm3 solution containing 3.215 g of acid D. The student titrates 25.0 cm3 samples of the solution of D with 0.150 mol dm–3 Ba(OH)2(aq) in the burette. 1 mol Ba(OH)2 reacts with 2 mol of D. The mean titre of Ba(OH)2(aq) is 23.50 cm3. Analyse the titration results to determine two possible structures for the cis stereoisomer of organic acid D. Structures of 2 possible cis stereoisomers of acid D [7]
54. November 2020 · Paper 1 · Q1 · 1 marks · AO2
1 Several students titrate 25.00 cm3 of the same solution of sodium hydroxide, NaOH(aq) with hydrochloric acid, HCl (aq). One student obtains a smaller titre than the other students. Which procedure explains the smaller titre? A The burette readings are taken from the top of the meniscus instead of the bottom of the meniscus. B The conical flask is rinsed with water before carrying out the titration. C An air bubble is released from the jet of the burette during the titration. D The pipette is rinsed with water before filling with NaOH(aq). Your answer [1]
55. November 2020 · AS Paper 1 · Q23(a) · 3 marks · AO3
23 This question is about barium hydroxide. (a) Barium hydroxide is an alkali which releases hydroxide ions, OH−, in aqueous solution. A barium hydroxide solution contains 3.89 g of Ba(OH)2 in 100 cm3 at 20 °C. Calculate the concentration of hydroxide ions, OH−, in mol dm−3, of this solution at 20 °C. Give your answer to 3 significant figures. concentration of OH− ions = .......................................... mol dm−3 [3]
56. November 2020 · AS Paper 1 · Q23(b)(i) · 1 marks · AO2
(b) A student carries out a titration to determine the concentration of an aqueous solution of Ba(OH)2. The student adds 25.0 cm3 of the Ba(OH)2(aq) solution to a conical flask. The student titrates this solution by adding 0.160 mol dm−3 HNO3(aq) from the burette. The equation is shown below. Ba(OH)2(aq) + 2HNO3(aq) → Ba(NO3)2(aq) + 2H2O(l ) The student repeats the titration until concordant titres are obtained. The mean titre of 0.160 mol dm−3 HNO3(aq) is 26.75 cm3. (i) What is meant by concordant titres? ........................................................................................................................................... ...................................................................................................................................... [1]
57. November 2020 · AS Paper 1 · Q23(b)(ii) · 3 marks · AO2
(ii) Calculate the concentration, in mol dm−3, of the Ba(OH)2(aq) solution. concentration of Ba(OH)2(aq) = .......................................... mol dm−3 [3]
58. November 2020 · AS Paper 2 · Q1(c) · 6 marks · AO1, 2, 3
(c)* A student is provided with samples of three nickel compounds. One sample is nickel(II) bromide, another is nickel(II) sulfate and the third is nickel(II) carbonate. The student doesn’t know which sample is which. Describe the tests that the student could carry out to identify the anion (negative ion) in each sample, and write equations for any reactions. [6] ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... Additional answer space if required ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................
59. November 2020 · Paper 3 · Q4(a)(iii) · 1 marks · AO2
(iii) In Stage 3, write the ionic equation for the reaction taking place in the titration. ...................................................................................................................................... [1]
60. November 2020 · Paper 3 · Q4(a)(iv) · 6 marks · AO2, 3
(iv) Metal M can be identified following the steps below. 1. The amount, in mol, of excess HCl (aq) that remains after the reaction of M with HCl (aq). 2. The amount, in mol, of HCl (aq) that reacted with M. 3. The identity of metal M. Analyse the results to identify metal M. Metal M = .......................................................... [6]
61. November 2020 · Paper 3 · Q6(b) · 4 marks · AO2, 3
(b) Ethanoic acid, CH3COOH, and methanesulfonic acid, CH3SO2OH, are both monobasic acids. The pKa values are shown in the table. Acid pKa Ethanoic acid CH3COOH 4.76 Methanesulfonic acid CH3SO2OH –1.90 A student suggests that 1.0 mol dm−3 CH3SO2OH should have a lower pH value than 1.0 mol dm−3 CH3COOH. Write an equation, showing conjugate acid–base pairs, for the equilibrium of CH3SO2OH with water and explain, with reasons, whether the student is correct. Label the conjugate acid–base pairs: A1, B1 and A2, B2. ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................. [4]
62. June 2019 · Paper 1 · Q4 · 1 marks · AO2
4 In the laboratory, acid spills can be cleaned up and made safe by spreading anhydrous sodium carbonate over the spill to neutralise the acid. A student accidentally spills 50.0 cm3 of 2.00 mol dm−3 HCl (aq) on the bench. What is the minimum mass of anhydrous sodium carbonate required to neutralise the acid? A 4.15 g B 5.30 g C 8.30 g D 10.6 g Your answer [1]
63. June 2019 · Paper 1 · Q20(b)(i) · 1 marks · AO2
(b) A student adds a total of 45.0 cm3 of 0.100 mol dm−3 NaOH(aq) to 25.0 cm3 of 0.0800 mol dm−3 C2H5COOH(aq) and monitors the pH throughout. (i) Show by calculation that 20.0 cm3 of NaOH(aq) is required to reach the end point. [1]
64. June 2019 · AS Paper 1 · Q22(a)(i) · 1 marks · AO2
22 A student carries out a titration to determine the concentration of some hydrochloric acid. The student titrates the hydrochloric acid against a standard solution of sodium carbonate, Na2CO3. The equation is shown below. Na2CO3(aq) + 2HCl (aq) → 2NaCl (aq) + H2O(l) + CO2(g) • The student prepares 0.150 mol dm−3 Na2CO3 in a 250.0 cm3 volumetric flask. • The hydrochloric acid is added to a 50.0 cm3 burette. • The student pipettes the Na2CO3(aq) using a 25.0 cm3 pipette. (a) The student’s burette readings are shown in the table. The rough titre has been omitted. (i) Complete the table by adding the titres to the table. Final reading / cm3 24.60 48.45 34.30 Initial reading / cm3 0.40 24.60 10.00 Titre / cm3 ................... ................... ................... [1]
65. June 2019 · AS Paper 1 · Q22(a)(ii) · 1 marks · AO2
(ii) Calculate the mean titre of HCl , to the nearest 0.05 cm3, that the student should use for analysing the results. mean titre = .................................................. cm3 [1]
66. June 2019 · AS Paper 1 · Q22(b) · 3 marks · AO2
(b) Calculate the concentration, in mol dm−3, of the hydrochloric acid. Give your answer to 3 significant figures. concentration of HCl = .......................................... mol dm−3 [3]
67. June 2019 · AS Paper 2 · Q2(a) · 6 marks · AO2
2 Magnesium nitrate is used in fertilisers as a source of nitrogen. (a)* A student plans to prepare 250.0 cm3 of a 0.4000 mol dm–3 solution of magnesium nitrate, starting from magnesium nitrate crystals, Mg(NO3)2•6H2O. Describe how the student would prepare the solution, giving full details of quantities, apparatus and method. [6] ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... Additional answer space if required ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................
68. June 2019 · Paper 2 · Q17(a)(ii) · 4 marks · AO2, 3
(ii) A student is provided with one of the four amino acids in Table 17.1. A student carries out a titration with a standard solution of hydrochloric acid to identify the amino acid. The student’s method is outlined below. • The student dissolves 5.766 g of the amino acid in water and makes the solution up to 250.0 cm3 in a volumetric flask. • The student titrates this solution with 25.0 cm3 of 0.150 mol dm−3 hydrochloric acid. • 21.30 cm3 of the amino acid solution were required for complete neutralisation of the hydrochloric acid. Determine which amino acid the student used. [4]
69. June 2018 · Paper 1 · Q4 · 1 marks · AO2
4 A student titrates a standard solution of barium hydroxide, Ba(OH)2, with nitric acid, HNO3. 25.00 cm3 of 0.0450 mol dm–3 Ba(OH)2 are needed to neutralise 23.35 cm3 of HNO3(aq). What is the concentration, in mol dm–3, of the nitric acid? A 0.0241 B 0.0482 C 0.0900 D 0.0964 Your answer [1]
70. June 2018 · AS Paper 1 · Q5 · 1 marks ·
5 Which equation does not represent a neutralisation reaction? A Zn + 2HCl → ZnCl 2 + H2 B 2NH3 + H2SO4 → (NH4)2SO4 C Na2CO3 + 2CH3COOH → 2CH3COONa + CO2 + H2O D CuO + 2HNO3 → Cu(NO3)2 + H2O Your answer [1]
71. June 2018 · Paper 1 · Q21(d) · 6 marks ·
(d)* Three different reactions of copper compounds are described below. Reaction 1: Aqueous copper(II) sulfate reacts with excess aqueous ammonia in a ligand substitution reaction. A deep-blue solution is formed, containing an octahedral complex ion, C, which is a trans isomer. Reaction 2: Copper(I) oxide reacts with hot dilute sulfuric acid in a disproportionation reaction. A blue solution, D, and a brown solid, E are formed. Reaction 3: Copper(II) oxide reacts with warm dilute nitric acid in a neutralisation reaction, to form a blue solution. Unreacted copper(II) oxide is filtered off, and the solution is left overnight in an evaporating basin. A hydrated salt, F, crystallises, with the percentage composition by mass: Cu, 26.29%; H, 2.48%; N, 11.59%; O, 59.63%. Identify C–F by formulae or structures, as appropriate. Include equations, any changes in oxidation number, and working. [6] ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... Additional answer space if required. ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................
72. June 2018 · AS Paper 1 · Q22(a)(iv) · 2 marks ·
(iv) Magnesium phosphate can also be prepared by reacting phosphoric acid with a compound of magnesium. Choose a suitable magnesium compound for this preparation and write the equation for the reaction. Formula of compound ............................. Equation ........................................................................................................................ [2]
73. June 2018 · AS Paper 2 · Q1(a) · 1 marks ·
1 A student carries out a titration to determine the molar mass and structure of a weak acid A. The student follows the method below. • Dissolve a weighed mass of A in 100 cm3 of distilled water and make the solution up to 250 cm3 in a beaker. • Add the solution of A to a burette. • Titrate the solution of A with a standard solution of sodium hydroxide, NaOH. (a) What is meant by the term standard solution? ................................................................................................................................................... .............................................................................................................................................. [1]
74. June 2018 · AS Paper 2 · Q1(b) · 1 marks ·
(b) Sodium hydroxide is an alkali. What is meant by the term alkali? ................................................................................................................................................... .............................................................................................................................................. [1]
75. June 2018 · AS Paper 2 · Q1(c)(i) · 4 marks ·
(c) The student carries out a trial, followed by three further titrations. The diagram shows the initial and final burette readings for the three further titrations. The student measures all burette readings to the nearest 0.05 cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading 0 27 0 27 0 27 1 28 1 28 1 28 2 29 2 29 2 29 (i) Record the student’s readings and the titres in the table below. Calculate the mean titre, to the nearest 0.05 cm3, that the student should use for analysing the results. Titration 1 Titration 2 Titration 3 Final reading/cm3 Initial reading/cm3 Titre/cm3 mean titre = .................................................. cm3 [4]
76. June 2018 · AS Paper 2 · Q1(c)(iii) · 1 marks ·
(iii) The student realised that the solution of A had not been prepared correctly. How should the student have made up the solution? ........................................................................................................................................... ........................................................................................................................................... ...................................................................................................................................... [1]
77. June 2018 · AS Paper 2 · Q1(d)(i) · 4 marks ·
(d) A student repeats the titration to determine the molar mass and structure of A. • The student prepares a 250.0 cm3 solution from 1.513 g of A. • The solution of A is added to the burette and titrated with 25.0 cm3 volumes of 0.112 mol dm–3 NaOH(aq). • 1 mol of A reacts with 2 mol of NaOH. • The student obtains a mean titre of 27.30 cm3. (i) Calculate the molar mass of A from these results. Give your answer to the nearest whole number. Show your working. molar mass of A = ............................................. g mol–1 [4]
78. June 2017 · Paper 1 · Q5 · 1 marks ·
5 0.0200 mol of calcium oxide is reacted completely with 2.00 mol dm–3 HCl. What is the volume, in cm3, of 2.00 mol dm–3 HCl required for this reaction? A 15 B 20 C 30 D 60 Your answer [1]
79. June 2017 · Paper 1 · Q17(a) · 1 marks ·
17 This question is about Group 2 and Group 17 (7). (a) Barium chloride can be prepared from barium hydroxide in a neutralisation reaction. Write the equation for this reaction. State symbols are not required. .............................................................................................................................................. [1]
80. June 2017 · AS Paper 1 · Q24(a) · 1 marks ·
24 Ethanoic acid, CH3COOH, is the main dissolved acid in vinegar. (a) Ethanoic acid is a weak acid. What is meant by acid and weak acid? ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................. [1]
81. June 2017 · AS Paper 1 · Q24(c)(i) · 4 marks ·
(c) A student plans to determine the concentration, in mol dm–3, of CH3COOH in a bottle of vinegar. The student will carry out a titration with aqueous barium hydroxide, Ba(OH)2(aq). The student’s method is outlined below. • Dilute 10.0 cm3 of vinegar from the bottle with distilled water and make the solution up to 250.0 cm3. • Add the diluted vinegar to the burette. • Titrate 25.0 cm3 volumes of 0.0450 mol dm–3 Ba(OH)2 with the diluted vinegar. The mean titre of the diluted vinegar is 25.45 cm3. The reaction in the student’s titration is shown below. 2CH3COOH(aq) + Ba(OH)2(aq) → (CH3COO)2Ba(aq) + 2H2O(l) (i) Calculate the concentration, in mol dm–3, of CH3COOH in the original bottle of vinegar. Show your working. concentration of CH3COOH = .......................................... mol dm–3 [4]
82. June 2017 · AS Paper 2 · Q1(c)(ii) · 4 marks ·
(ii) Solid barium nitride is reacted with water, forming an alkaline solution A and an alkaline gas B. Identify A and B. Write an equation, including state symbols, for the reaction. A ......................................................................................................................................... B ......................................................................................................................................... ........................................................................................................................................... ........................................................................................................................................... ...................................................................................................................................... [4]
83. June 2017 · Paper 2 · Q10 · 1 marks ·
10 Equal amounts of the four compounds are added to the same volume of water. Which compound would produce the most acidic solution? A CH3CONH2 B CH3COOH C CH3COOCH3 D CH3COCl Your answer [1]
84. June 2017 · Paper 3 · Q4(a)(i) · 4 marks ·
4 This question is about weak acids. (a) Compound A is a weak monobasic acid. A student is supplied with a 250.0 cm3 solution prepared from 2.495 g of A. The student titrates 25.0 cm3 samples of this solution with 0.0840 mol dm−3 NaOH in the burette. The student carries out a trial, followed by the three further titrations. The diagrams show the initial burette readings and the final burette readings for the student’s three further titrations. All burette readings are measured to the nearest 0.05 cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading 0 23 23 45 9 32 1 24 24 46 10 33 2 25 25 47 11 34 (i) Record the student’s readings and the titres in an appropriate format. Calculate the mean titre that the student should use for analysing the results. mean titre = .................................................. cm3 [4]
85. June 2017 · Paper 3 · Q4(a)(ii) · 6 marks ·
(ii) The structure of compound A is shown below. O HO OH R compound A Compound A has four optical isomers. Using this information and the student’s results, answer the following. • Determine the molar mass of A and the formula of the alkyl group R. • Draw the structure of compound A and label any chiral carbon atoms with an asterisk*. Show all your working. [6]
86. June 2016 · AS Paper 1 · Q4 · 1 marks ·
3 4 Which equation is not a neutralisation reaction? A Ca(s) + 2HCl(aq) → CaCl2(aq) + H2(g) B H+(aq) + OH–(aq) → H2O(l) C K2CO3(s) + 2HNO3(aq) → 2KNO3(aq) + H2O(l) + CO2(g) D NH3(aq) + HCl(aq) → NH4Cl(aq) Your answer [1]
87. June 2016 · AS Paper 1 · Q11 · 1 marks ·
11 A student adds aqueous sodium carbonate to one test-tube and aqueous silver nitrate to a second test-tube. The student adds dilute sulfuric acid to each test-tube. Which row has the correct observations? Aqueous sodium carbonate Aqueous silver nitrate A no change precipitate B no change no change C effervescence no change D effervescence precipitate Your answer [1]
88. June 2016 · AS Paper 1 · Q21(c)(i) · 1 marks · AO1
(c) Nickel(II) nitrate, Ni(NO3)2, can be prepared by reacting nickel(II) oxide with dilute nitric acid. (i) Write the equation for this reaction. ...................................................................................................................................... [1]
89. June 2016 · AS Paper 1 · Q22(c) · 3 marks · AO2
16 (c) A student prepares a solution of sodium sulfate, Na2SO4, by adding 6.25 × 10–2 mol dm–3 sulfuric acid, H2SO4, from a burette to 25.0 cm3 of 0.124 mol dm–3 NaOH in a conical flask. 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) Calculate the minimum volume of the H2SO4 that the student would need to completely react with the NaOH present. volume of H2SO4 = .................................................. cm3 [3]
90. June 2016 · AS Paper 2 · Q5(a)(i) · 1 marks · AO3
12 5 A student investigates the reaction between strontium carbonate and dilute nitric acid. SrCO3 + 2HNO3 Sr(NO3)2 + CO2 + H2O The rate of reaction is determined from the loss in mass over a period of time. (a) (i) Explain why there is a loss in mass during the reaction. ........................................................................................................................................... ...................................................................................................................................... [1]

Mark schemes

1. June 2025 · Paper 1 · Q4
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2. June 2025 · AS Paper 1 · Q7
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3. June 2025 · Paper 1 · Q19(b)(i)
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4. June 2025 · AS Paper 2 · Q1(a)
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5. June 2025 · AS Paper 2 · Q1(b)
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6. June 2025 · AS Paper 2 · Q3(a)(i)
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7. June 2025 · AS Paper 2 · Q3(a)(ii)
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8. June 2025 · AS Paper 2 · Q3(a)(iii)
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9. June 2025 · AS Paper 2 · Q3(b)
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10. June 2024 · Paper 1 · Q19(b)(i)
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11. June 2024 · Paper 1 · Q21(a)
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12. June 2024 · AS Paper 1 · Q22(a)
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13. June 2024 · AS Paper 1 · Q22(b)(i)
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14. June 2024 · AS Paper 1 · Q22(b)(ii)
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15. June 2024 · AS Paper 1 · Q22(b)(iii)
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16. June 2024 · Paper 2 · Q23(b)(i)
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17. June 2024 · Paper 3 · Q1(d)
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18. June 2023 · Paper 1 · Q4
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19. June 2023 · Paper 1 · Q20(c)(i)
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20. June 2023 · Paper 1 · Q20(d)(ii)
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21. June 2023 · AS Paper 1 · Q22(a)
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22. June 2023 · AS Paper 1 · Q22(b)(i)
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23. June 2023 · AS Paper 1 · Q22(b)(ii)
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24. June 2023 · AS Paper 1 · Q22(c)(i)
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25. June 2023 · AS Paper 1 · Q22(c)(ii)
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26. June 2023 · AS Paper 1 · Q22(c)(iii)
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27. June 2023 · AS Paper 1 · Q22(c)(iv)
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28. June 2023 · Paper 3 · Q5(a)
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29. June 2023 · Paper 3 · Q6(b)(i)
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30. June 2022 · AS Paper 1 · Q3
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31. June 2022 · Paper 1 · Q19(a)(i)
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32. June 2022 · Paper 1 · Q19(a)(ii)
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33. June 2022 · Paper 1 · Q21(b)(ii)
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34. June 2022 · Paper 1 · Q21(c)(ii)
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35. June 2022 · AS Paper 2 · Q1(a)(i)
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36. June 2022 · AS Paper 2 · Q1(a)(ii)
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37. June 2022 · AS Paper 2 · Q1(b)(i)
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38. June 2022 · AS Paper 2 · Q1(b)(ii)
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39. June 2022 · AS Paper 2 · Q1(c)
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40. November 2021 · AS Paper 1 · Q3
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41. November 2021 · AS Paper 1 · Q7
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42. November 2021 · Paper 1 · Q18(a)
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43. November 2021 · Paper 1 · Q18(f)
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44. November 2021 · AS Paper 2 · Q3(a)
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45. November 2021 · AS Paper 2 · Q3(b)(i)
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46. November 2021 · AS Paper 2 · Q3(b)(ii)
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47. November 2021 · AS Paper 2 · Q3(b)(iii)
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48. November 2021 · AS Paper 2 · Q3(c)
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49. November 2021 · AS Paper 2 · Q3(d)
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50. November 2021 · Paper 3 · Q1(d)
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51. November 2021 · Paper 3 · Q1(e)
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52. November 2021 · Paper 3 · Q3(a)
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53. November 2021 · Paper 3 · Q3(b)
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54. November 2020 · Paper 1 · Q1
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55. November 2020 · AS Paper 1 · Q23(a)
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56. November 2020 · AS Paper 1 · Q23(b)(i)
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57. November 2020 · AS Paper 1 · Q23(b)(ii)
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58. November 2020 · AS Paper 2 · Q1(c)
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59. November 2020 · Paper 3 · Q4(a)(iii)
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60. November 2020 · Paper 3 · Q4(a)(iv)
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61. November 2020 · Paper 3 · Q6(b)
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62. June 2019 · Paper 1 · Q4
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63. June 2019 · Paper 1 · Q20(b)(i)
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64. June 2019 · AS Paper 1 · Q22(a)(i)
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65. June 2019 · AS Paper 1 · Q22(a)(ii)
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66. June 2019 · AS Paper 1 · Q22(b)
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67. June 2019 · AS Paper 2 · Q2(a)
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68. June 2019 · Paper 2 · Q17(a)(ii)
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69. June 2018 · Paper 1 · Q4
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70. June 2018 · AS Paper 1 · Q5
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71. June 2018 · Paper 1 · Q21(d)
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72. June 2018 · AS Paper 1 · Q22(a)(iv)
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73. June 2018 · AS Paper 2 · Q1(a)
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74. June 2018 · AS Paper 2 · Q1(b)
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75. June 2018 · AS Paper 2 · Q1(c)(i)
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76. June 2018 · AS Paper 2 · Q1(c)(iii)
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77. June 2018 · AS Paper 2 · Q1(d)(i)
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78. June 2017 · Paper 1 · Q5
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79. June 2017 · Paper 1 · Q17(a)
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80. June 2017 · AS Paper 1 · Q24(a)
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81. June 2017 · AS Paper 1 · Q24(c)(i)
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82. June 2017 · AS Paper 2 · Q1(c)(ii)
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83. June 2017 · Paper 2 · Q10
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84. June 2017 · Paper 3 · Q4(a)(i)
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85. June 2017 · Paper 3 · Q4(a)(ii)
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86. June 2016 · AS Paper 1 · Q4
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87. June 2016 · AS Paper 1 · Q11
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88. June 2016 · AS Paper 1 · Q21(c)(i)
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89. June 2016 · AS Paper 1 · Q22(c)
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90. June 2016 · AS Paper 2 · Q5(a)(i)
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