Free until 14 Nov · 80% off for the first 100 · Pricing

Get started

Chemistry 9701/33 October/November 2023: question paper and mark scheme

Cambridge AS & A Level Chemistry (9701), Paper 3 Advanced Practical Skills 1, October/November 2023. Read both free below, or download them. Done the paper? Get it marked by AI against this mark scheme.

9701_w23_qp_339701_w23_ms_339701/33/O/N/23

Mark my answers with AIRead the paper and scheme
Paper
Paper 3 Advanced Practical Skills 1
Total marks
40
Time
2 hours
Questions
3
Code on the paper
9701/33/O/N/23
9701_w23_ms_33.pdf

9701/33 mark scheme, question by question

Each question as it's printed, and the mark scheme's points for it, as text. Diagrams, tables and graphs are in the PDFs above.

Question 114 marks

Question

You will carry out a titration to determine the concentration of a solution of potassium manganate(VII), KMnO4. Potassium manganate(VII) reacts with excess acidified potassium iodide to produce iodine. This iodine is titrated with aqueous sodium thiosulfate. FA 1 is aqueous potassium manganate(VII), KMnO4. FA 2 is 0.500 mol dm–3 potassium iodide, KI. FA 3 is 0.120 mol dm–3 sodium thiosulfate, Na2S2O3. FA 4 is dilute sulfuric acid, H2SO4. FA 5 is starch indicator. (a) Method Titration ● Fill the burette with FA 3. ● Pipette 25.0 cm3 of FA 1 into a conical flask. ● Use the 25 cm3 measuring cylinder to add 10.0 cm3 of FA 2 to the conical flask. ● Use the 50 cm3 measuring cylinder to add 15.0 cm3 of FA 4 to the conical flask. ● Perform a rough titration by adding FA 3 from the burette to the conical flask until the solution is yellow. ● Then add several drops of FA 5. Continue the titration until the mixture in the flask becomes colourless. This is the end-point. ● Record the initial and final burette readings in the space below. The rough titre is …… cm3. ● Carry out as many accurate titrations as you think necessary to obtain consistent results. ● Make sure any recorded results show the precision of your practical work. ● Record, in a suitable form below, all your burette readings and the volume of FA 3 added in each accurate titration. Keep FA 2 and FA 5 for use in Question 3(b). I II III IV V VI VII [7] (b) From your accurate titration results, calculate a suitable mean value to be used in your calculations. Show clearly how you obtained the mean value. The iodine produced by FA 1 required …… cm3 of FA 3. [1] (c) Calculations (i) Give your answers to (c)(ii), (c)(iii) and (c)(iv) to the appropriate number of significant figures. [1] (ii) Calculate the amount, in mol, of sodium thiosulfate in the volume of FA 3 calculated in (b). amount of Na2S2O3 = …… mol [1] (iii) The reaction by which iodine is produced is shown. 2KMnO4(aq) + 10KI(aq) + 8H2SO4(aq) 6K2SO4(aq) + 2MnSO4(aq) + 5I2(aq) + 8H2O(l) During the titration, sodium thiosulfate reacts with the iodine produced. 2Na2S2O3(aq) + I2(aq) 2NaI(aq) + Na2S4O6(aq) Calculate the concentration of potassium manganate(VII), in mol dm–3, in FA 1. concentration of KMnO4 = …… mol dm–3 [2] (iv) A laboratory technician purchased a bottle containing 50.00 g of potassium manganate(VII), KMnO4, for this practical examination. Using your answer to (c)(iii), calculate the maximum volume of FA 1, in dm3, that the technician can prepare using the contents of this bottle. volume of FA 1 = …… dm3 [1] (d) A student suggested that the accuracy of the experiment would be increased by using a 10 cm3 pipette to measure FA 2. State whether the student is correct. Explain your answer. …… [1] [Total: 14]

Mark scheme

1(a) I All the following data are recorded • two burette readings and titre for the rough titration • initial and final burette readings for two (or more) accurate titrations II Appropriate headings and units shown in the accurate titration table and titre values recorded for accurate titrations. • initial / start and (burette) reading/volume • final / end and (burette) reading/volume • titre or volume / FA 3 and used / added • unit: / cm3 or (cm3) or in cm3 (for each heading) or cm3 unit given for each volume recorded Ill All accurate burette readings are recorded to the nearest 0.05 cm3. The requirement to record to 0.05 applies to burette readings, including 0.00 cm3 (if this was the initial reading), but it does not apply to the titre. lV The final accurate titre recorded is within 0.10 cm3 of any other accurate titre. Do not include a reading if it is labelled ‘rough’. For assessment of accuracy (Q) marks, the Examiner should round all burette readings to the nearest 0.05 cm3. Check and correct subtractions. Then select the ‘best’ titres using the hierarchy: • two (or more) accurate identical titres (ignoring any that are labelled ‘rough’), then • two (or more) accurate titres within 0.05 cm3, then • two (or more) accurate titres within 0.10 cm3, etc. These ‘best’ titres should be used to calculate the mean titre, expressed to nearest 0.01 cm3. Calculate the difference (δ) between the candidate’s mean titre and the supervisor’s. Award three accuracy (Q) marks as shown below. Award V if δ ⩽ 0.60 (cm3) 7 Award VI if δ ⩽ 0.40 Award VII if δ ⩽ 0.20 Tolerances for low titres: If supervisor’s titre is ⩽ 10.00 cm3, tolerances are 0.30, 0.20, 0.10 cm3. If supervisor’s titre is ⩽ 5.00 cm3 then tolerances are 0.15, 0.10, 0.05 cm3. 1(b) Correctly calculates the mean titre. 1 • Candidate must take the average of two (or more) titres that are within a total spread of not more than 0.20 cm3. • Working/explanation must be shown or ticks must be shown next to the two (or more) accurate readings selected. • The mean should be quoted to 2 dp, and be rounded correctly to nearest 0.01 cm3. (e.g. 26.625 cm3 must be rounded to 26.63 cm3) • Allow a mean expressed to 1 dp, if all accurate burette readings were given to 1 dp and the mean is exactly correct. (e.g. mean of 26.0 and 26.2 = 26.1 is allowed) (e.g. mean of 26.0 and 26.1 = 26.1 is wrong: it should be 26.05) 1(c)(i) All answers to parts (c)(ii), (c)(iii) and (c)(iv) quoted to 3 or 4 significant figures (sf). 1 1(c)(ii) Correct calculation of no of moles of Na2S2O3 1 No of moles = 0.120 × mean titre/1000 1(c)(iii) Correct use of 1(c)(ii) 2 M1: amount of KMnO4 in 25 cm3 FA 1 = 0.2 × (c)(ii) mol M2: Concn of KMnO4 = 40 × 0.2 × (c)(ii) = 8 × (c)(ii) mol dm–3 1(c)(iv) Correct use of (c)(iii) to calculate volume of FA 1 1 Volume of FA 1 = 50/158 × 1/(c)(iii) 1(d) No and FA 2 is used in excess (so exact volume is not important) 1

Question 212 marks

Question

You will determine the enthalpy change for the reaction of magnesium oxide with water to form magnesium hydroxide. MgO(s) + H2O(l) Mg(OH)2(s) The procedure will involve two experiments, one with magnesium oxide and the other with magnesium hydroxide. In each case you will react the solid with hydrochloric acid. FA 6 is magnesium oxide, MgO. FA 7 is 2.0 mol dm–3 hydrochloric acid, HCl. FA 8 is magnesium hydroxide, Mg(OH)2. (a) Experiment 1 is the determination of the enthalpy change of reaction, ΔH1, of magnesium oxide with hydrochloric acid. MgO(s) + 2HCl (aq) MgCl 2(aq) + H2O(l) (i) Method ● Support a cup in the 250 cm3 beaker. ● Use the 50 cm3 measuring cylinder to transfer 30.0 cm3 of FA 7 into the cup. ● Measure and record the temperature of the solution in the cup. ● Weigh the container with FA 6. Record the mass. ● Tip all of FA 6 into the cup containing FA 7. FA 7 is in excess. ● Stir the mixture until the maximum temperature is obtained. Record the maximum temperature. ● Weigh the container with any residual FA 6. Record the mass. ● Calculate and record the mass of FA 6 used. ● Calculate and record the temperature rise. I II III [3] (ii) Calculate the energy released in your experiment. energy released = …… J [1] (iii) Calculate the enthalpy change of reaction, ΔH1, in kJ mol–1 of MgO(s), for the reaction of magnesium oxide with hydrochloric acid. Show your working. ΔH1 = …… …… kJ mol–1 sign value [2] (b) Experiment 2 is the determination of the enthalpy change of the reaction, ΔH2, of magnesium hydroxide with hydrochloric acid. Mg(OH)2(s) + 2HCl (aq) MgCl 2(aq) + 2H2O(l) (i) Method ● Place the other cup in the beaker. ● Use the 50 cm3 measuring cylinder to transfer 30.0 cm3 of FA 7 into the cup. ● Measure and record the temperature of the solution in the cup. ● Weigh the container with magnesium hydroxide, FA 8. Record the mass. ● Tip all of FA 8 into the cup containing FA 7. FA 8 is in excess. ● Stir the mixture until the maximum temperature is obtained. Record the maximum temperature. ● Weigh the container with any residual FA 8. Record the mass. ● Calculate and record the mass of FA 8 used. ● Calculate and record the temperature rise. I II III [3] (ii) Calculate the enthalpy change of reaction, ΔH2, in kJ mol–1 of Mg(OH)2(s), for the reaction of magnesium hydroxide with hydrochloric acid. Show your working. ΔH2 = …… …… kJ mol–1 sign value [2] (c) Use your answers to (a)(iii) and (b)(ii) to calculate the enthalpy change, ΔHr, in kJ mol–1, for the reaction between magnesium oxide and water. The equation for the reaction is shown. MgO(s) + H2O(l) Mg(OH)2(s) Show your working. ΔHr = …… …… kJ mol–1 sign value [1] [Total: 12] Qualitative Analysis For each test you should record all your observations in the spaces provided. Examples of observations include: ● colour changes seen ● the formation of any precipitate and its solubility (where appropriate) in an excess of the reagent added ● the formation of any gas and its identification (where appropriate) by a suitable test. You should record clearly at what stage in a test an observation is made. Where no change is observed, you should write ‘no change’. Where reagents are selected for use in a test, the name or correct formula of the element or compound must be given. If any solution is warmed, a boiling tube must be used. Rinse and reuse test-tubes and boiling tubes where possible. No additional tests should be attempted.

Mark scheme

2(a)(i) I Six unambiguous headings recorded, with correctly displayed units and in the space provided. 3 • Units: (oC), / g, in g, or oC or g against each value • (Mass of) container + FA 6 / MgO / contents / solid / g • (Mass of) (empty) container (+ residue) / g • (Mass of) FA 6 / MgO (used) / g • (Initial) temperature / oC • Maximum / final temperature / oC • Temperature rise / change / ΔT / oC II Precision of readings in both experiments, 2(a) and 2(b). • Four weighings to same number of decimal places (2 or 3) • Four thermometer readings to .0 or .5 oC III Correct subtractions to calculate masses of FA 6 and FA 8 and for the temperature changes in both (a) and (b). 2(a)(ii) Correct calculation of energy change 1 Energy change = 30 × 4.18 × temp rise (= 125.4 × ΔT) AND answer correctly rounded to 2–4 sf Do not penalise inappropriate sf twice in question 2. 2(a)(iii) Correct use of (a)(ii) 2 M1: Correct display Amount of MgO = mass used/40.3 mol (no answer required) M2: Correctly uses Enthalpy change = (a)(ii)/mol MgO × 1/1000 kJ mol−1 and answer shows negative sign and is quoted to 2–4 sf 2(b)(i) I Six pieces of data recorded in the space provided (same readings are required as in (a)(i)) • Three temperatures • Three masses Accuracy marks in 2(b) • Round thermometer readings to 0.5 oC if necessary • Check supervisor’s and candidate’s subtractions for temp rise • Calculate difference (δ) between supervisor and candidate (to 0.5 oC). II + III: Accuracy marks in 2(b) 3 ΔTsup / ºC <5.0 5.0–9.5 10.0–19.5 20.0–29.5 ⩾ 30.0 1 mark ±1.0 ±1.5 2.0 2.5 3.0 2 marks ±0.5 ±1.0 1.0 1.5 2.0 2(b)(ii) Correct use of data in enthalpy calculation 2 M1: Amount Mg(OH)2 reacting = 0.5 × mol HCl (since Mg(OH)2 in excess) = 0.5 × 0.030 × 2.00 = 0.030 mol M2: Correct use of data in remainder of calculation (all three bullets correct) • Energy released = 30 × 4.18 × temp rise in (b) (J) • Enthalpy change = heat released/1000 x 0.030 kJ mol−1 • Answer has negative sign and is quoted to 2–4 sig fig. 2(c) Enthalpy change (correctly calculated, with correct sign) 1 ΔHr = (a)(iii) – (b)(ii) kJ mol−1 FA 9 is ZnCO3; FA 10 is ammonium iron(III) sulfate, NH4Fe(SO4)2

Question 314 marks

Question

FA 9 contains one cation and one anion. The cation is one of calcium, magnesium, manganese(II) or zinc. The anion is oxide or carbonate. (a) Describe reactions to identify FA 9. You are advised to test for the anion first. State any conditions needed for these reactions. Carry out your reactions and record all your observations. Deduce the formula of FA 9. FA 9 is …… . [4] (b) (i) FA 10 is a solution of a double salt. It contains two cations and one anion, all of which are listed in the Qualitative analysis notes. Use a 1 cm depth of this solution of FA 10 in a test-tube for Tests 1–3. Table 3.1 test observations Test 1 Add an equal volume of FA 2, aqueous potassium iodide, then add FA 5, aqueous starch. Test 2 Add aqueous barium chloride (or barium nitrate), then add dilute hydrochloric acid (or nitric acid). Test 3 Add aqueous silver nitrate, then add aqueous ammonia. Test 4 In a boiling tube, add aqueous sodium hydroxide to a 1 cm depth of solution of FA 10, then warm gently and carefully, then remove from heat and add one piece of aluminium foil to the mixture. [5] (ii) Identify the three ions in FA 10 by writing the formula of each ion. The three ions are …… and …… and …… . [2] (iii) Identify the two tests in (b)(i) that involve redox reactions. Justify your answer for one of the tests. Tests …… and …… involve redox reactions. justification …… …… [2] (iv) Give an ionic equation for the reaction of one of the ions in FA 10 with sodium hydroxide in Test 4. Include state symbols. …… [1] [Total: 14] Qualitative analysis notes 1 Reactions of cations cation reaction with NaOH(aq) NH3(aq) aluminium, Al 3+(aq) white ppt. soluble in excess white ppt. insoluble in excess ammonium, NH4+(aq) no ppt. – ammonia produced on warming barium, Ba2+(aq) faint white ppt. is observed unless no ppt. [Ba2+(aq)] is very low calcium, Ca2+(aq) white ppt. unless [Ca2+(aq)] is very no ppt. low chromium(III), Cr3+(aq) grey-green ppt. soluble in excess grey-green ppt. insoluble in excess giving dark green solution copper(II), Cu2+(aq) pale blue ppt. insoluble in excess pale blue ppt. soluble in excess giving dark blue solution iron(II), Fe2+(aq) green ppt. turning brown on green ppt. turning brown on contact with air contact with air insoluble in excess insoluble in excess iron(III), Fe3+(aq) red-brown ppt. insoluble in excess red-brown ppt. insoluble in excess magnesium, Mg2+(aq) white ppt. insoluble in excess white ppt. insoluble in excess manganese(II), Mn2+(aq) off-white ppt. rapidly turning brown off-white ppt. rapidly turning brown on contact with air on contact with air insoluble in excess insoluble in excess zinc, Zn2+(aq) white ppt. soluble in excess white ppt. soluble in excess 2 Reactions of anions anion reaction carbonate, CO32– CO2 liberated by dilute acids chloride, Cl –(aq) gives white ppt. with Ag+(aq) (soluble in NH3(aq)) bromide, Br –(aq) gives cream / off-white ppt. with Ag+(aq) (partially soluble in NH3(aq)) iodide, I–(aq) gives pale yellow ppt. with Ag+(aq) (insoluble in NH3(aq)) nitrate, NO3–(aq) NH3 liberated on heating with OH–(aq) and Al foil nitrite, NO2–(aq) NH3 liberated on heating with OH–(aq) and Al foil; decolourises acidified aqueous KMnO4 sulfate, SO42–(aq) gives white ppt. with Ba2+(aq) (insoluble in excess dilute strong acids); gives white ppt. with high [Ca2+(aq)] sulfite, SO32–(aq) gives white ppt. with Ba2+(aq) (soluble in excess dilute strong acids); decolourises acidified aqueous KMnO4 thiosulfate, S2O32–(aq) gives off-white/pale yellow ppt. slowly with H+ 3 Tests for gases gas test and test result ammonia, NH3 turns damp red litmus paper blue carbon dioxide, CO2 gives a white ppt. with limewater hydrogen, H2 ‘pops’ with a lighted splint oxygen, O2 relights a glowing splint 4 Tests for elements element test and test result iodine, I2 gives blue-black colour on addition of starch solution Important values, constants and standards molar gas constant R = 8.31 J K–1 mol–1 Faraday constant F = 9.65 × 104 C mol–1 Avogadro constant L = 6.022 × 1023 mol–1 electronic charge e = –1.60 × 10–19 C molar volume of gas Vm = 22.4 dm3 mol–1 s.t.p. (101 kPa and 273 K) Vm = 24.0 dm3 mol–1 at room conditions ionic product of water Kw = 1.00 × 10–14 mol2 dm–6 (at 298 K (25 °C)) specific heat capacity of water c = 4.18 kJ kg–1 K–1 (4.18 J g–1 K–1) The Periodic Table of Elements Group 1 2 13 14 15 16 17 18 1 2 H He hydrogen helium Key 1.0 4.0 3 4 atomic number 5 6 7 8 9 10 Li Be atomic symbol B C N O F Ne lithium beryllium name boron carbon nitrogen oxygen fluorine neon 6.9 9.0 relative atomic mass 10.8 12.0 14.0 16.0 19.0 20.2 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar sodium magnesium aluminium silicon phosphorus sulfur chlorine argon 23.0 24.3 3 4 5 6 7 8 9 10 11 12 27.0 28.1 31.0 32.1 35.5 39.9 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton at www.cambridgeinternational.org after the live examination series. 39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon 85.5 87.6 88.9 91.2 92.9 95.9 – 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 12 55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 lanthanoids Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon 132.9 137.3 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 – – – 87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson – – – – – – – – – – – – – – – – – 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium 138.9 140.1 140.9 144.4 – 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.1 175.0 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium – 232.0 231.0 238.0 – – – – – – – – – – – Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge

Mark scheme

3(a) Test for anion 4 EITHER Add specified mineral acid * Fizzing / effervescence / bubbling occurs * (Bubble) gas/CO2 through limewater * White ppt formed * Colourless solution formed or vigorous (owtte) reaction * OR Heat the solid * (Bubble) gas / CO2 through limewater * White ppt formed * Solid goes yellow / yellow-green (when hot) * Solid becomes paler on cooling / goes white (on cooling) * Test for cation To a solution * made using acid * Add (aqueous) sodium hydroxide or ammonia * White ppt formed * Soluble in excess alkali * [Maximum mark for observations above = 3] FA 9 is ZnCO3 * (formula required) 2 * = 1 mark. [Maximum mark for 3(a) = 4] 3(b)(i) Observations: 11 * available = 5 marks rounding down. 5 Test 1 (KI) (Solution) turns dark yellow / brown / red-brown / orange-brown / yellow-brown * (With starch) (goes) dark blue / blue-black / black * (Ignore state) Test 2 (Ba2+) White precipitate * (With acid) precipitate insoluble / no change * Test 3 (AgNO3) No change / no precipitate / no reaction / solution remains colourless/pale yellow * (with NH3) brown / red-brown / orange-brown / rust precipitate * Test 4 (NaOH etc.) Brown/red-brown/orange-brown/rust precipitate * Ppt is insoluble in excess NaOH * (with heat) Gas / ammonia turns (damp red) litmus blue * (with Al) effervescence / fizzing / bubbling occurs * Gas/H2 ‘pops’ with lighted splint or gas / ammonia turns (damp red) litmus blue * 3(b)(ii) Ions are NH4+ and Fe3+ and SO42– 2 3(b)(iii) M1: Tests 1 and 4 involve redox (both must be correct) 2 M2: Any one strand of explanation correct (from those listed below) • Iodide ion is oxidised to iodine (or 2I− → I2 + 2e−) • Fe3+ is reduced to Fe2+ (or Fe3+ + e− → Fe2+) • Fe3+ is the oxidising agent and I− is the reducing agent • Fe3+ is reduced and I– is oxidised • Iodine changes from oxidation state -1 to 0 • Aluminium is oxidised to aluminium ions (or Al → Al3+ + 3e−) • Water / hydroxide ions is / are reduced to hydrogen • Al is the reducing agent and water / OH− ions ions is / are the oxidising agent • Al is oxidised and water / OH− ions is / are reduced 3(b)(iv) Fe3+(aq) + 3OH−(aq) → Fe(OH)3(s) 1 OR NH4+(aq) + OH–(aq) → NH3(g) + H2O(l) or (g)

Checked your answers against these? Let AI mark the whole paper, on your own working.

Mark my 9701/33

How this paper is marked

Examiners follow the generic marking principles at the front of the scheme, then each question's points: method (M), accuracy (A) and independent (B) marks, error carried forward where the scheme allows it, and positive marking, so you're credited for what you got right.

Check your answers against it

Done this paper? Upload your script and CIE Buddy's AI marker marks it question by question against this exact scheme, puts the ticks on your own working and says what each lost mark needed.

Other variants, October/November 2023

9701/33 in other series

Find another Chemistry paper

Every AS & A Level Chemistry mark scheme

Question papers and mark schemes © Cambridge University Press & Assessment. CIE Buddy is independent and not connected to Cambridge.

9701/33 questions

Where can I find the 9701/33 October/November 2023 mark scheme?

On this page, free: the mark scheme for AS & A Level Chemistry 9701/33, October/November 2023 (9701_w23_ms_33), and the question paper (9701_w23_qp_33), to read or download, with each question's marking points written out underneath.

How many marks is 9701/33 out of?

Chemistry 9701/33 for October/November 2023 is out of 40 marks, with 2 hours to answer it, across 3 questions.

Can I get my 9701/33 answers marked?

Yes. Upload your answers to 9701/33/O/N/23 as a PDF or photos, and CIE Buddy marks every question against this paper's official mark scheme, using Cambridge's marking rules. You get your score, each lost mark explained on your own script, and the topics to revise. It's a guide, not an official Cambridge grade.