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A Level Chemistry Paper 1, 2 & 3 Chemistry Exam
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2022 Updated Version
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*9533612219*
a-level chemistry paper
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Cambridge InternationalAS &ALevel
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CHEMISTRY 9701/33
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Paper 3 Advanced Practical Skills 1 May/June 2021
2 hours
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You must answer on the question paper.
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You will need: The materials and apparatus listed in the confidential instructions
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INSTRUCTIONS
● Answer all questions.
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● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
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● Write your name, centre number and candidate number in the boxes at the top of the page.
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● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
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● Do not write on any bar codes.
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● You may use a calculator.
● You should show all your working, use appropriate units and use an appropriate number of significant
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figures.
● Give details of the practical session and laboratory, where appropriate,in
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the boxes provided. Session
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INFORMATION
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Laboratory
● The total mark for this paper is 40.
● The number of marks for each question or part question is shown
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in brackets [ ].
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● The Periodic Table is printed in the question paper.
● Notes for use in qualitative analysis are provided in the question paper. For Examiner’s Use
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A Level Chemistry Paper 1, 2 & 3 Chemistry Exam
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2022 Updated Version
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IB21 06_9701_33/3RP
© UCLES 2021
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10
Quantitative analysis
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Read through the whole method before starting any practical work. Where appropriate, prepare a tablefor
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your results in the space provided.
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Showiyourworkingandappropriatesignificantfiguresinthefinalanswertoeachstepofyourcalculations.
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Bleachismadebyreactingchlorinewithacoldsolutionofsodiumhydroxide.Thisreactionproduces
sodium chlorate(I), NaClO.
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Cl2(aq) + 2NaOH(aq) NaCl O(aq) + NaCl (aq) +
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H2O(l)
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In this experiment you will determine the concentration of sodium chlorate(I) in a sample of bleach,
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FA1.
To do this, you will react an acidified dilute solution of the bleach with iodide ions, I–. This reaction
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produces iodine, I2.
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ClO–(aq) + 2I–(aq) + 2H+(aq) I2(aq) + Cl–(aq) +
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H2O(l)
The amount of iodine produced will then be determined by titration with thiosulfate ions, S2O 2–.3
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I2(aq) + 2S2O3i 2–(aq) 2I–(aq) + S4O6 2–(aq)
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FA1 is a solution of bleach.
FA3 is dilute sulfuric acid, H2SO4.
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FA 4 is 0.500moldm–3 potassium iodide, KI.
FA 5 is 0.100im oldm–3 sodium thiosulfate, Na2S2O3.starch
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indicator
(a) Method la
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Dilution
● Pipette 25.0cm3 of FA 1 into the 250cm3 volumetric flask.
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Add distilled water to make 250cm3 of solution and shake the flask thoroughly.
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● Label this flask FA 2.
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Titration
● Fill a burette with FA 5.
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● Rinse the pipette thoroughly with distilled water and then with a little FA 2.
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● Pipette 25.0cm3 of FA 2 into a conical flask.
● Use the measuring cylinder to add 20cm3 of FA 3 to the conical flask.
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● Use the measuring cylinder to add 15icm3 of FA4 to the conical flask. The solution will turn
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brown as iodine is produced.
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● Add FA 5 from the burette until the solution has turned yellow.
● Add 10 drops of starch indicator to the conical flask. The solution will turnblue‑ black.
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● Continue to add more FA 5 from the burette until the blue‑ black colour just
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disappears. This is the end‑ point of the titration.
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● Carry out a rough titration and record your burette readings in the space provided.
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The rough titre = ............................... cm3.
© UCLES 2021 9701/33/M/J/21
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A Level Chemistry Paper 1, 2 & 3 Chemistry Exam
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2022 Updated Version
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la
tz
sh
Sp
ne
la
sh
Sp
*9533612219*
a-level chemistry paper
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la
tz
Cambridge InternationalAS &ALevel
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Sp
ne
la
sh
Sp
ne
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CHEMISTRY 9701/33
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Paper 3 Advanced Practical Skills 1 May/June 2021
2 hours
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You must answer on the question paper.
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sh
Sp
You will need: The materials and apparatus listed in the confidential instructions
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INSTRUCTIONS
● Answer all questions.
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● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
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● Write your name, centre number and candidate number in the boxes at the top of the page.
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● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
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● Do not write on any bar codes.
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● You may use a calculator.
● You should show all your working, use appropriate units and use an appropriate number of significant
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figures.
● Give details of the practical session and laboratory, where appropriate,in
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the boxes provided. Session
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INFORMATION
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Laboratory
● The total mark for this paper is 40.
● The number of marks for each question or part question is shown
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in brackets [ ].
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● The Periodic Table is printed in the question paper.
● Notes for use in qualitative analysis are provided in the question paper. For Examiner’s Use
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Sp
1
la
2
, Sp Sp Sp Sp Sp
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sh sh sh sh sh sh
ne ne ne ne ne ne
tz tz tz tz tz t
This document has 12 pages. Blank pages are indicated.
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la la la la la
sh sh sh sh sh
ne ne ne ne ne
, t
A Level Chemistry Paper 1, 2 & 3 Chemistry Exam
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2022 Updated Version
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ne
IB21 06_9701_33/3RP
© UCLES 2021
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10
Quantitative analysis
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Read through the whole method before starting any practical work. Where appropriate, prepare a tablefor
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your results in the space provided.
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Showiyourworkingandappropriatesignificantfiguresinthefinalanswertoeachstepofyourcalculations.
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Sp
1 ne
Bleachismadebyreactingchlorinewithacoldsolutionofsodiumhydroxide.Thisreactionproduces
sodium chlorate(I), NaClO.
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Cl2(aq) + 2NaOH(aq) NaCl O(aq) + NaCl (aq) +
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H2O(l)
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In this experiment you will determine the concentration of sodium chlorate(I) in a sample of bleach,
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FA1.
To do this, you will react an acidified dilute solution of the bleach with iodide ions, I–. This reaction
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produces iodine, I2.
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ClO–(aq) + 2I–(aq) + 2H+(aq) I2(aq) + Cl–(aq) +
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H2O(l)
The amount of iodine produced will then be determined by titration with thiosulfate ions, S2O 2–.3
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I2(aq) + 2S2O3i 2–(aq) 2I–(aq) + S4O6 2–(aq)
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FA1 is a solution of bleach.
FA3 is dilute sulfuric acid, H2SO4.
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FA 4 is 0.500moldm–3 potassium iodide, KI.
FA 5 is 0.100im oldm–3 sodium thiosulfate, Na2S2O3.starch
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indicator
(a) Method la
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Dilution
● Pipette 25.0cm3 of FA 1 into the 250cm3 volumetric flask.
●
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Add distilled water to make 250cm3 of solution and shake the flask thoroughly.
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● Label this flask FA 2.
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Titration
● Fill a burette with FA 5.
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● Rinse the pipette thoroughly with distilled water and then with a little FA 2.
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● Pipette 25.0cm3 of FA 2 into a conical flask.
● Use the measuring cylinder to add 20cm3 of FA 3 to the conical flask.
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● Use the measuring cylinder to add 15icm3 of FA4 to the conical flask. The solution will turn
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brown as iodine is produced.
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● Add FA 5 from the burette until the solution has turned yellow.
● Add 10 drops of starch indicator to the conical flask. The solution will turnblue‑ black.
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● Continue to add more FA 5 from the burette until the blue‑ black colour just
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disappears. This is the end‑ point of the titration.
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● Carry out a rough titration and record your burette readings in the space provided.
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The rough titre = ............................... cm3.
© UCLES 2021 9701/33/M/J/21
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