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DELHI PUBLIC SCHOOL

Nacharam
Cambridge International Education
AY 2024 - 2025
Worksheet Worksheet No.: DPSNH/45

Chemistry Subject Code: 0620

Paper: 6 Month: April
Paper Type: Alternative to practical (Summer Break WS) Duration: 1 hour

Candidate Name: Grade: 10 Section:A&B

Centre Number: Candidate Number:

Chapter: 12 Experimental techniques and chemical analysis

Sub Unit& Concept in Focus:

12.1 Experimental design

12.2 Acid–base titrations

12.3 Chromatography

12.4 Separation and purification

12.5 Identification of ions and gases

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1 Silver chloride is an ionic compound and is insoluble in water. Molten silver chloride breaks down
during electrolysis. The products are chlorine and silver.
Chlorine gas is soluble in water and toxic.

A student suggests using the apparatus shown to break down silver chloride.

power
supply

silver chloride

(a) Draw an arrow on the diagram to show where heat must be applied so that the silver chloride
can break down. [1]

(b) Complete the diagram to show how chlorine gas can be collected and the volume of the
chlorine measured. Label any apparatus you have drawn. [2]

(c) Give two observations that are made as the silver chloride breaks down.

1 ..................................................................................................................................................

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

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(d) The person doing the experiment followed all normal laboratory safety rules.

State one additional safety precaution that should be taken when doing this experiment. Give
a reason for your answer.

safety precaution ........................................................................................................................

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

(e) Suggest one reason why zinc is not a suitable material to use as the electrodes.

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

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

(f) The chlorine gas was bubbled into an aqueous solution of a sodium salt. The colour of the
solution changed from colourless to orange.

Identify the sodium salt and explain what has happened to cause the colour change.

sodium salt .................................................................................................................................

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

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

 [Total: 10]

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2 A student investigated the reaction between aqueous potassium hydroxide and two different
aqueous solutions of hydrochloric acid labelled solution A and solution B.

Two experiments were done.

(a) 
Experiment 1
● A burette was filled with solution A. Some of solution A was run out of the burette so that
the level of solution A was on the burette scale.
● A measuring cylinder was used to measure 25 cm3 of the aqueous potassium hydroxide.
● The aqueous potassium hydroxide was poured into a conical flask.
● Five drops of methyl orange indicator were added to the conical flask.
● Solution A was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.

Use the burette diagrams to complete the table for Experiment 1.

7 16

8 17

9 18

initial reading final reading

Experiment 1

final burette reading / cm3

initial burette reading / cm3

volume of solution A added / cm3


Experiment 2
● The conical flask was emptied and rinsed with distilled water.
● The burette was emptied and rinsed with distilled water.
● The burette was rinsed with solution B.
● The burette was filled with solution B. Some of solution B was run out of the burette so that
the level of solution B was on the burette scale.
● A measuring cylinder was used to measure 25 cm3 of the aqueous potassium hydroxide.
● The aqueous potassium hydroxide was poured into the conical flask.
● Five drops of methyl orange indicator were added to the conical flask.
● Solution B was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.

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Use the burette diagrams to complete the table for Experiment 2.

7 26

8 27

9 28

initial reading final reading

Experiment 2

final burette reading / cm3

initial burette reading / cm3

volume of solution B added / cm3

[4]

(b) State the colour change observed in the conical flask at the end-point in Experiment 2.

from ................................................................ to ................................................................. [1]

(c) Before starting the titration in Experiment 2 the conical flask was rinsed with water.

(i) Explain why the conical flask was rinsed with water.

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

(ii) The conical flask was not then rinsed with aqueous potassium hydroxide.

State how rinsing the conical flask with aqueous potassium hydroxide would change the
volume of solution B needed. Explain your answer.

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

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

(d) (i) Deduce which aqueous solution of hydrochloric acid, A or B, was more concentrated.
Explain your answer.

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

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

(ii) Deduce how many times more concentrated this solution of hydrochloric acid was than the
other solution of hydrochloric acid.

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

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(e) Explain why Experiment 1 and Experiment 2 should be repeated.

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

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

(f) Deduce the volume of solution B required if Experiment 2 is carried out with 50 cm3 of aqueous
potassium hydroxide.

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

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

(g) Describe one change that could be made to the apparatus to improve the accuracy of the
results.

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

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

(h) Describe what effect using a larger conical flask would have on the results obtained.

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

 [Total: 15]

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3 Two solids, solid C and solid D, were analysed.

Tests were done on each solid.

tests on solid C


Tests were carried out and the following observations were made.

tests observations
test 1

A flame test was carried out on solid C. a red flame was seen

Solid C was dissolved in distilled water to

produce solution C.

test 2

About 5 cm3 of aqueous sodium hydroxide was no change

added to solution C.

test 3

A piece of aluminium foil was added to the effervescence was seen;

mixture formed in test 2.The mixture was damp red litmus paper turned blue
warmed gently and any gas produced was
tested.

(a) Name the gas that turned the damp red litmus paper blue in test 3.

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

(b) Identify solid C.

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

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

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tests on solid D

Solid D was aluminium sulfate.

Complete the expected observations.

Solid D was dissolved in water to form solution D. Solution D was divided into four approximately
equal portions in four test-tubes.

(c) A
 queous sodium hydroxide was added dropwise and then in excess to the first portion of
solution D.

observations ...............................................................................................................................

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

(d) Aqueous ammonia was added dropwise and then in excess to the second portion of solution D.

observations ...............................................................................................................................

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

(e) About 1 cm3 of dilute nitric acid and a few drops of aqueous silver nitrate were added to the
third portion of solution D.

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

(f) About 1 cm3 of dilute nitric acid and a few drops of aqueous barium nitrate were added to the
fourth portion of solution D.

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

 [Total: 9]

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4 Old concrete contains calcium carbonate. Calcium carbonate reacts with dilute hydrochloric acid.

CaCO3(s) + 2HCl (aq) → CaCl 2(aq) + H2O(l) + CO2(g)

Plan an investigation to find which of two lumps of concrete contains the larger percentage of
calcium carbonate. Your plan should include how you will use your results to determine which one
of the two lumps has the larger percentage of calcium carbonate.

You have access to all common laboratory materials and a supply of dilute hydrochloric acid.

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...................................................................................................................................................... [6]

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