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CHEMISTRY 0620/61
Paper 6 Alternative to Practical October/November 2024

1 hour

You must answer on the question paper.

No additional materials are needed.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name, centre number and candidate number in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● Do not write on any bar codes.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 40.
● The number of marks for each question or part question is shown in brackets [ ].
● Notes for use in qualitative analysis are provided in the question paper.

This document has 16 pages. Any blank pages are indicated.

IB24 11_0620_61/4RP
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1 A student has a mixture of copper(II) carbonate powder and crystals of sodium sulfate.
Copper(II) carbonate is insoluble in water. Sodium sulfate is soluble in water.

The student tries to obtain pure copper(II) carbonate and crystals of pure sodium sulfate from the
mixture. Fig. 1.1 shows four of the steps the student carries out.

step 1 step 2
Add distilled water to Filter the mixture.
the mixture and stir.
residue

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filtrate

step 3 step 4
Heat the filtrate from step 2 Leave the residue on the filter paper
until crystals start to form. from step 2 in a warm place to dry.

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residue

heat filter paper

Fig. 1.1

(a) State what happens to the sodium sulfate in step 1.

.............................................................................................................................................. [1]

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(b) State what is removed from the filtrate in step 3.

.............................................................................................................................................. [1]

(c) Describe what must be done after the filtrate has been heated in step 3 to obtain a larger
amount of sodium sulfate crystals.

....................................................................................................................................................

.............................................................................................................................................. [1]
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(d) (i) State what must be done to the residue before it is allowed to dry in step 4 to obtain pure
copper(II) carbonate.

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Identify the substance removed from the copper(II) carbonate in (d)(i).

....................................................................................................................................... [1]
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[Total: 5]
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BLANK PAGE

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2 A student investigates the reaction between aqueous magnesium sulfate and aqueous barium
nitrate.
A precipitate of barium sulfate forms in the reaction.

The student does eight experiments.

Experiment 1

● Fill a burette with aqueous magnesium sulfate. Run some of the aqueous magnesium sulfate
out of the burette so that the level of the aqueous magnesium sulfate is on the burette scale.
● Fill a second burette with aqueous barium nitrate. Run some of the aqueous barium nitrate out
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of the burette so that the level of the aqueous barium nitrate is on the burette scale.
● Add 4.0 cm3 of aqueous magnesium sulfate from the first burette into a 10 cm3 measuring
cylinder.
● Add 1.0 cm3 of aqueous barium nitrate from the second burette into the same measuring
cylinder.
● Place a stopper in the top of the measuring cylinder and invert the measuring cylinder several
times.
● Leave the measuring cylinder to stand for 15 minutes.
● Record the level of the precipitate on the measuring cylinder scale.
● Rinse the measuring cylinder with distilled water.

Experiment 2
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● Repeat Experiment 1 using 1.5 cm3 of aqueous barium nitrate instead of 1.0 cm3.

Experiment 3

● Repeat Experiment 1 using 2.5 cm3 of aqueous barium nitrate instead of 1.0 cm3.

Experiment 4

● Repeat Experiment 1 using 3.0 cm3 of aqueous barium nitrate instead of 1.0 cm3.

Experiment 5
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● Repeat Experiment 1 using 3.5 cm3 of aqueous barium nitrate instead of 1.0 cm3.

Experiment 6

● Repeat Experiment 1 using 4.5 cm3 of aqueous barium nitrate instead of 1.0 cm3.

Experiment 7

● Repeat Experiment 1 using 5.0 cm3 of aqueous barium nitrate instead of 1.0 cm3.

Experiment 8

● Repeat Experiment 1 using 5.5 cm3 of aqueous barium nitrate instead of 1.0 cm3.
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(a) Use the information in the description of the experiments and the measuring cylinder diagrams
to complete Table 2.1.

Table 2.1

experiment 1 2 3 4 5 6 7 8
volume of
aqueous 4.0
magnesium
sulfate / cm3

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volume of
aqueous
1.0
barium nitrate
/ cm3

cm3 cm3 cm3 cm3 cm3 cm3 cm3 cm3

10 10 10 10 10 10 10 10

9 9 9 9 9 9 9 9

8 8 8 8 8 8 8 8

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7 7 7 7 7 7 7 7

measuring 6 6 6 6 6 6 6 6
cylinder
diagram 5 5 5 5 5 5 5 5

4 4 4 4 4 4 4 4

3 3 3 3 3 3 3 3
solution
2 2 2 2 2 2 2 2

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1 1 1 1 1 1 1 1
precipitate

level of
precipitate on
the measuring 1.2
cylinder scale
/ cm3

[4]
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(b) Complete a suitable scale on the y-axis and plot the results from Experiments 1 to 8 on Fig. 2.1.
Draw two straight lines of best fit through your points. The first straight line should be for the
first five experiments and must be extended to pass through (0,0). The second straight line
should be for the last three experiments and must be horizontal. Extend the straight lines so
that they cross each other.
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level of precipitate
on the measuring
cylinder scale / cm3
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0.0
0.0 1.0 2.0 3.0 4.0 5.0 6.0
volume of aqueous barium nitrate / cm3

Fig. 2.1
[5]

(c) Use Fig. 2.1 to deduce the level of precipitate on the measuring cylinder scale when the
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experiment is repeated using 2.8 cm3 of aqueous barium nitrate.

Show clearly on Fig. 2.1 how you worked out your answer.

level of precipitate = .............................. cm3 [2]

(d) The student repeats the experiment using 6.5 cm3 of aqueous barium nitrate.

Predict the level of precipitate on the measuring cylinder scale.

Explain your answer.

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prediction ...................................................................................................................................

explanation ................................................................................................................................

....................................................................................................................................................
[2]

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(e) Sketch on Fig. 2.1 the graph obtained if all of the experiments are repeated using aqueous
barium nitrate of half the concentration used in Experiments 1 to 8. [2]

(f) Suggest why the measuring cylinder is inverted several times after the aqueous barium nitrate
is added.

....................................................................................................................................................

.............................................................................................................................................. [1]

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(g) Suggest why the measuring cylinder is left to stand before the level of the precipitate is
recorded.

....................................................................................................................................................

.............................................................................................................................................. [1]

(h) The volumes of both aqueous solutions are measured using burettes.

(i) Give a reason why burettes are used rather than measuring cylinders.

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.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Suggest why burettes are used rather than volumetric pipettes.

.............................................................................................................................................

....................................................................................................................................... [1]

[Total: 19]

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3 A student tests two solids: solid T and solid U.

Tests on solid T

Solid T is lithium sulfite.

Complete the expected observations.

(a) The student carries out a flame test on solid T.

observations ........................................................................................................................ [1]

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The student dissolves the remaining solid T in water to form solution T.

The student divides solution T into two portions.

(b) The student adds the first portion of solution T to a test-tube containing acidified aqueous
potassium manganate(VII).

State the colour change.

from ................................................................ to ................................................................ [2]

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(c) (i) To the second portion of solution T, the student adds excess dilute nitric acid.
The gas produced turns filter paper soaked in acidified aqueous potassium manganate(VII)
white.

Identify the gas produced.

....................................................................................................................................... [1]

(ii) To the solution produced in (c)(i), the student adds aqueous barium nitrate.

observations ................................................................................................................. [1]

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Tests on solid U

Solid U contains one cation and one anion.

Table 3.1 shows the tests and the student’s observations for solid U.

The student dissolves solid U in distilled water to form solution U. The student then divides solution U
into three portions.

Table 3.1

tests observations

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test 1

To the first portion of solution U, add a few green precipitate

drops of aqueous ammonia.

test 2

To the second portion of solution U, add 1 cm3 yellow precipitate

of dilute nitric acid followed by a few drops of
aqueous silver nitrate.

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test 3

To the third portion of solution U, add 1 cm3 of the solution turns brown
aqueous chlorine.

(d) Identify two cations that the tests and observations in Table 3.1 show could be in solid U.

....................................................................................................................................................

.............................................................................................................................................. [2]

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(e) Describe an additional test that the student could do to confirm which one of the two cations
identified in (d) is in solid U.
Give the expected result for one of the cations.

test .............................................................................................................................................

cation .........................................................................................................................................

result ..........................................................................................................................................
[2]

(f) Identify the anion in solid U.

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.............................................................................................................................................. [1]

[Total: 10]

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4 Beetroot is a coloured vegetable. The colour is caused by a mixture of water-soluble coloured

compounds.

Plan an experiment to find how many water-soluble coloured compounds there are in a beetroot.

Include in your plan:

● how to extract the coloured compounds from a beetroot
● how to separate the mixture of coloured compounds
● how the results show how many coloured compounds there are in a beetroot.

You are provided with a beetroot, distilled water and common laboratory apparatus.
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..................................................................................................................................................... [6]

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Notes for use in qualitative analysis

Tests for anions

anion test test result

carbonate, CO32– add dilute acid, then test for carbon effervescence, carbon dioxide
dioxide gas produced
chloride, Cl – acidify with dilute nitric acid, then white ppt.
[in solution] add aqueous silver nitrate
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bromide, Br – acidify with dilute nitric acid, then cream ppt.

[in solution] add aqueous silver nitrate
iodide, I– acidify with dilute nitric acid, then yellow ppt.
[in solution] add aqueous silver nitrate
nitrate, NO3– add aqueous sodium hydroxide, ammonia produced
[in solution] then aluminium foil; warm carefully
sulfate, SO42– acidify with dilute nitric acid, then white ppt.
[in solution] add aqueous barium nitrate
sulfite, SO32– add a small volume of acidified the acidified aqueous potassium
aqueous potassium manganate(VII) manganate(VII) changes colour
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from purple to colourless

Tests for aqueous cations

cation effect of aqueous sodium hydroxide effect of aqueous ammonia

aluminium, Al 3+ white ppt., soluble in excess, giving white ppt., insoluble in excess
a colourless solution
ammonium, NH4+ ammonia produced on warming –
calcium, Ca2+ white ppt., insoluble in excess no ppt. or very slight white ppt.
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chromium(III), Cr3+ green ppt., soluble in excess green ppt., insoluble in excess
copper(II), Cu2+ light blue ppt., insoluble in excess light blue ppt., soluble in excess,
giving a dark blue solution
iron(II), Fe2+ green ppt., insoluble in excess, green ppt., insoluble in excess,
ppt. turns brown near surface on ppt. turns brown near surface on
standing standing
iron(III), Fe3+ red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess
zinc, Zn2+ white ppt., soluble in excess, giving white ppt., soluble in excess, giving
a colourless solution a colourless solution
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Tests for gases

gas test and test result

ammonia, NH3 turns damp red litmus paper blue
carbon dioxide, CO2 turns limewater milky
chlorine, Cl 2 bleaches damp litmus paper
hydrogen, H2 ‘pops’ with a lighted splint
oxygen, O2 relights a glowing splint

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sulfur dioxide, SO2 turns acidified aqueous potassium manganate(VII) from purple to colourless

Flame tests for metal ions

metal ion flame colour

lithium, Li+ red
sodium, Na+ yellow
potassium, K+ lilac
calcium, Ca2+ orange-red

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barium, Ba2+ light green
copper(II), Cu2+ blue-green

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To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
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