0620 Chemistry November 2025 Question Paper 62

1 Eggshells are made from a mixture of calcium carbonate and other insoluble substances.

Calcium carbonate reacts with dilute hydrochloric acid. The equation for the reaction is shown. CaCO3(s) + 2HCl (aq) CaCl 2(aq) + H2O(l) + CO2(g)

The other substances in eggshells do not react with dilute hydrochloric acid.

A student finds the percentage by mass of calcium carbonate in an eggshell.

Fig. 1.1 shows the first three steps of the method the student uses. step 1 Grind the eggshell into small pieces. step 2 Find the mass of the small pieces of eggshell. step 3 Add the small pieces of eggshell to excess dilute hydrochloric acid and warm the mixture while stirring it with a glass rod. small pieces of eggshell small pieces of eggshell balance pestle mortar eggshell dilute hydrochloric acid conical flask glass rod Fig. 1.1

(a) (i) Describe what is seen when the calcium carbonate in the eggshell reacts with dilute hydrochloric acid [1]

(ii) Describe what the student should do to make sure the acid is in excess and all of the calcium carbonate has reacted [2] , ,

(b) After step 3, the student filters the mixture to obtain the unreacted solid left from the eggshell.

(i) Draw a labelled diagram of the apparatus the student should use to filter the mixture.

[2]

(ii) After the filtration, the student washes the residue.

Identify the two substances removed from the residue by washing. substance 1 substance 2 [2]

(iii) After washing the residue, the student dries the residue in an oven.

The student then measures the mass of the dry residue.

The masses the student records are shown in Table 1.1. Table 1.1 mass of small pieces of eggshell / g 2.00 mass of dry residue after filtration / g 0.11

Use the data in Table 1.1 to calculate the percentage by mass of calcium carbonate in the eggshell.

percentage of calcium carbonate = [2]

[Total: 9] , ,

2 A student investigates the reaction between acidic solution B and two different solutions of aqueous sodium hydroxide, solution C and solution D, using two different indicators.

The student does two experiments.

Experiment 1 • Rinse a burette with distilled water and then with solution C. • Fill the burette with solution C. Run some of solution C out of the burette so that the level of the solution is on the burette scale. • Record the initial burette reading. • Use a measuring cylinder to pour 25 cm3 of solution B into a conical flask. • Add five drops of methyl orange indicator and five drops of thymolphthalein indicator to the conical flask. • Stand the conical flask on a white tile. • Slowly add solution C from the burette to the conical flask, while swirling the flask, until the solution changes colour from red to orange. This is the first end-point. • Record the burette reading at the first end-point. • Continue to add solution C from the burette to the conical flask while swirling the flask. The solution changes colour from orange to yellow. • Continue to add solution C, while swirling the flask, until the solution changes colour from yellow to green. This is the second end-point. • Record the burette reading at the second end-point.

Experiment 2 • Empty the conical flask and rinse it with distilled water. • Repeat Experiment 1 using solution D instead of solution C. , ,

(a) Use the burette diagrams in Fig. 2.1 and Fig. 2.2 to record the readings for Experiment 1 and Experiment 2 in Table 2.1. Complete Table 2.1. 1 2 initial burette reading burette reading at first end-point burette reading at second end-point 3 20 21 22 40 41 42 Experiment 1 Fig. 2.1 0 1 initial burette reading burette reading at first end-point burette reading at second end-point 2 10 11 12 20 21 22 Experiment 2 Fig. 2.2 Table 2.1 Experiment 1 using solution C Experiment 2 using solution D burette reading at first end-point / cm3 burette reading at second end-point / cm3 initial burette reading / cm3 volume added from burette to reach first end-point / cm3 total volume added from burette to reach second end-point / cm3

[5] , ,

(b) (i) Explain why the conical flask is rinsed with distilled water at the start of Experiment 2 [1]

(ii) At the start of Experiment 1, the burette is rinsed with distilled water and then with solution C.

Explain how the volume added from the burette to reach the first end-point would be different if the burette was not rinsed with solution C [2]

(iii) Explain why the conical flask is placed on a white tile during the titration [1]

(c) Compare the concentration of solution C used in Experiment 1 with the concentration of solution D used in Experiment 2.

Explain your answer [3]

(d) (i) Deduce the volume of solution C required to reach the first end-point if Experiment 1 is repeated using 50 cm3 of solution B instead of 25 cm3.

volume of solution C = [2]

(ii) State why using 50 cm3 of solution B would cause a problem when finding the volume of solution C needed to reach the second end-point in Experiment 1 [1] , ,

(e) A student repeats Experiment 2.

The student warms solution B in the conical flask before carrying out the titration.

State the effect, if any, on the volume of solution D required to reach the second end-point in Experiment 2.

Explain your answer. effect on volume of solution D explanation [2]

(f) State one change to the apparatus that will improve the accuracy of the results [1]

[Total: 18] , ,

3 A student tests two solids: solid E and solid F.

Tests on solid E

Solid E is ammonium sulfate.

Record the expected observations.

The student dissolves solid E in distilled water to form solution E. The student divides solution E into three approximately equal portions.

(a) (i) To the first portion of solution E, the student adds about 2 cm3 of aqueous sodium hydroxide. The student warms the mixture gently and tests any gas produced. observations [1]

(ii) Identify the gas given off in (a)(i) [1]

(b) To the second portion of solution E, the student adds about 1 cm3 of dilute nitric acid followed by a few drops of aqueous barium nitrate. observations [1]

(c) To the third portion of solution E, the student adds a few drops of acidified aqueous potassium manganate(VII). observations [1] , , Tests on solid F Table 3.1 shows the tests and the student’s observations for solid F. Table 3.1 tests observations test 1 Carry out a flame test on solid F. yellow flame test 2 Dissolve the remaining solid F in distilled water to form solution F. Divide solution F into three portions. To the first portion of solution F, add about 1 cm3 of dilute nitric acid followed by a few drops of aqueous silver nitrate. yellow precipitate forms test 3 To the second portion of solution F, add aqueous sodium hydroxide dropwise until in excess. white precipitate forms the precipitate dissolves in excess aqueous sodium hydroxide to form a colourless solution test 4 To the third portion of solution F, add aqueous ammonia dropwise until in excess. white precipitate forms the precipitate dissolves in excess aqueous ammonia to form a colourless solution

(d) Identify the three ions in solid F [3]

[Total: 7] , ,