Chemistry Paper 3 Questions and Answers - Maranda High School Mock Exams 2023

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Instructions to Candidates

  • Answer ALL the questions in the spaces provided below each question.
  • You are NOT allowed to start working with the apparatus for the first 15 minutes of the 2¼ hours allowed for this paper. This time is to enable you to read the question paper and make sure you have all the apparatus and chemicals that you may need.
  • All working MUST be clearly shown where necessary
  • Mathematical tables and silent non-programmed electronic calculators may be used.
  1. You are provided with:
    • Solution A – 2M Hydrochloric acid.
    • Solution B – 0.2M sodium hydroxide solution.
    • 6 pieces of 2cm length of magnesium ribbon
      You are required to;
    • Determine the mass of magnesium ribbon that reacted with hydrochloric acid
      Procedure I
      1. Using a clean measuring cylinder, measure 50 cm3 of solution A into a 100 ml glass beaker.
      2. Cut the magnesium into six (6) pieces each of 2 cm long.
      3. Put one piece of magnesium ribbon into the solution A in the 100ml glass beaker and simultaneously start the stop watch.
      4. Record the time taken by magnesium ribbon to get completely finished in table I.
      5. Record procedure (iii) and (iv) using the same solution in procedure (i) adding each piece of magnesium ribbon up to the 6th piece and complete the table I below. Label the resultant solution as M and retain it for procedure II.
        Table I
         Magnesium ribbon Number  1st  2nd  3rd  4th  5th 6th 
         Time taken (s)            
           1   (S−1)
         time
                   
        (5 marks)
        1. Plot a graph of 1time (vertical axis) against the magnesium ribbon number. (3 marks)
        2. From the graph, determine the time that would be taken for 5 cm piece of the ribbon to get completely finished. (2 marks)
          Procedure II
          Transfer all the solution M from procedure I into a 250ml volumetric flask. Top up the flask to the mark with distilled water and shake. Label as solution N.
          • Fill the burette with solution N.
          • Using a pipette filler, place 25cm3 of solution B in a 250ml conical flask. Add 2 drops of phenolphthalein indicator and titrate with solution N.
          • Record your results in table II. Repeat the titration two more times to complete table II.
            Table II
               1  2  3
             Final burette reading      
             Initial burette reading      
             Volume of Solution N used (cm³)      
            (4 marks)
            Calculate the:
            1. average volume of solution N (1 mark)
            2. moles of sodium hydroxide, solution B used. (1 mark)
            3. moles of hydrochloric acid, in solution N used. (1 mark)
            4. moles of hydrochloric acid in 250cm3 of solution N. (1 mark)
            5. moles of hydrochloric acid in 50cm3 of solution A. (1 mark)
            6. moles of hydrochloric acid in solution A that reacted with all pieces of magnesium ribbon. (1 mark)
            7. mass of magnesium ribbon used in the reaction. (Mg = 24) (2 marks)
  2. You are provided with solid P. Carry out the tests below and record your observations and inferences in the spaces provided.
    Place solid P in a clean boiling tube, add 10cm3 of distilled water and shake well. Use about 2cm3 portions of the mixture for the tests below.
    1. Add aqueous ammonia dropwise until in excess.
       Observations  Inferences
                                                 (1 mark)                                         ( 1mark)        
    2. Add 2M sodium hydroxide solution dropwise until in excess.
       Observations  Inferences
                                                 (1 mark)                                         ( 1mark)     
    3. Add 4 drops of 2M sulphuric (VI) acid.
       Observations  Inferences
                                                 (1 mark)                                         ( 2marks)     
    4. Add 3 drops of lead (II) nitrate solution
       Observations  Inferences
                                                 (½ mark)                                         ( 1mark)     
    5. Add 3 drops of barium nitrate solution
       Observations  Inferences
                                                 (½ mark)                                         ( 1mark)     
  3. You are provided with an organic substance Q. Carry out the tests below and record your observations and inferences in the spaces provided.
    1. To about 2cm3 of substance Q in a test tube, add 2 drops of acidified potassium manganate (VII) solution.
       Observations  Inferences
                                                 (1 mark)                                         ( 1mark)     
    2. Place 3 drops of substance Q on a watch glass and ignite.
       Observations  Inferences
                                                 (1 mark)                                         ( 1mark)     
    3. To about 2cm3 of substance Q, add 2cm3 of ethanoic acid followed by 5 drops of 2M sulphuric (VI) acid and heat.
       Observations  Inferences
                                                 (1 mark)                                         ( 1mark)     
    4. To another 2cm3 of substance Q, add 2 drops of acidified potassium dichromate (VI) solution.
       Observations  Inferences
                                                 (1 mark)                                         ( 1mark)     

CONFIDENTIAL

  1. Each candidate
    1. About 60 cm3 of solution A
    2. About 100cm3 of solution B
    3. One burette 0 – 50 ml
    4. One pipette 25.0ml and a pipette filler
    5. One Filter funnel
    6. 100ml glass beaker
    7. Watch glass
    8. 13cm long of Magnesium ribbon
    9. Two clean dry 250 ml conical flasks
    10. Five (5) clean and dry test tubes on a test tube rack
    11. One boiling tube
    12. 10ml measuring cylinder
    13. Stopwatch
    14. 5cm3 of ethanoic acid supplied in a stoppered test tube
    15. About 500cm3 of distilled water supplied in a wash bottle
    16. One 250ml volumetric flask
    17. One 50ml measuring cylinder or 100ml measuring cylinder
    18. Two (2) labels
    19. One metallic spatula
    20. One test tube holder
    21. A white tile
    22. A wooden splint
    23. About 0.5g of solid P supplied in a stoppered container
    24. About 10ml of substance Q supplied in a syringe
    25. A scarpel
  2. Access to:
    1. Phenolphthalein indicator supplied with a dropper
    2. Bunsen burner
    3. 2.0M aqueous ammonia supplied with a dropper
    4. 2.0M sodium hydroxide solution supplied with a dropper
    5. 2.0 M sulphuric (VI) acid
    6. Acidified potasium dichromate (VI) solution supplied with a dropper
    7. Acidified potassium manganate (VII) solution supplied with a dropper 
    8. 0.5M Barium (II) nitrate solution supplied with a dropper
    9. 0.5M Lead (II) nitrate solution supplied with a dropper
  3. Preparation of solutions and solids
    1. Solution A (2.0M Hydrochloric acid) prepared by 172cm3 of concentrated hydrochloric acid diluted with distilled water to make a litre of solution.
    2. Solution B (0.2M Sodium Hydroxide) is prepared by dissolving 8.0g of sodium hydroxide in 700cm3 of distilled water and diluting it to one litre.
    3. Solid P is Aluminium sulphate
    4. Substance Q is Absolute Ethanol
    5. 13 cm long Magnesium ribbon

MARKING SCHEME

  1. You are provided with:
    • Solution A – 2M Hydrochloric acid.
    • Solution B – 0.2M sodium hydroxide solution.
    • 6 pieces of 2cm length of magnesium ribbon
      You are required to;
    • Determine the mass of magnesium ribbon that reacted with hydrochloric acid
      Procedure I
      1. Using a clean measuring cylinder, measure 50 cm3 of solution A into a 100 ml glass beaker.
      2. Cut the magnesium into six (6) pieces each of 2 cm long.
      3. Put one piece of magnesium ribbon into the solution A in the 100ml glass beaker and simultaneously start the stop watch.
      4. Record the time taken by magnesium ribbon to get completely finished in table I.
      5. Record procedure (iii) and (iv) using the same solution in procedure (i) adding each piece of magnesium ribbon up to the 6th piece and complete the table I below. Label the resultant solution as M and retain it for procedure II.
        Table I
         Magnesium ribbon Number  1st  2nd  3rd  4th  5th 6th 
         Time taken (s)  35.62   40.00   47.62   55.56   66.69   83.41 
           1   (S−1)
         time
         0.028  0.025  0.021  0.018  0.015  0.012
        (5 marks)
        CT3
        DP½
        AC½
        TR1
        1. Plot a graph of 1time (vertical axis) against the magnesium ribbon number. (3 marks)
          F4ChemMarJMP32023Ans1a
        2. From the graph, determine the time that would be taken for 5 cm piece of the ribbon to get completely finished. (2 marks)
          1/t = 23 × 10−3 
          t = 1/23 × 103
            = 43.48sec
          showing ½✓
          Reading  ½✓
          Working  ½✓
          Correct ans  ½✓
          Procedure II
          Transfer all the solution M from procedure I into a 250ml volumetric flask. Top up the flask to the mark with distilled water and shake. Label as solution N.
          • Fill the burette with solution N.
          • Using a pipette filler, place 25cm3 of solution B in a 250ml conical flask. Add 2 drops of phenolphthalein indicator and titrate with solution N.
          • Record your results in table II. Repeat the titration two more times to complete table II.
            Table II
               1  2  3
             Final burette reading  20.5   20.6   20.7 
             Initial burette reading  0.0  0.0  0.0
             Volume of Solution N used (cm³)  20.5  20.6  20.7
            (4 marks)
            CT1
            DP1
            AC1
            PA1
            FA1
            Calculate the:
            1. average volume of solution N (1 mark)
              20.5 + 20.6 + 20.7 = 20.6
                              3
            2. moles of sodium hydroxide, solution B used. (1 mark)
              = 0.2 × 25 
                    1000
              = 0.005
            3. moles of hydrochloric acid, in solution N used. (1 mark)
              moles of HCl = moles of NaOH
                                   = 0.005
            4. moles of hydrochloric acid in 250cm3 of solution N. (1 mark)
              0.005 × 250 = 0.0607
                    20.6
            5. moles of hydrochloric acid in 50cm3 of solution A. (1 mark)
              2 × 50 = 0.1
               1000
            6. moles of hydrochloric acid in solution A that reacted with all pieces of magnesium ribbon. (1 mark)
              = 0.1 − 0.0607
              = 0.0393
            7. mass of magnesium ribbon used in the reaction. (Mg = 24) (2 marks)
              Moles of Mg used
              = 0.0393 
                       2
              = 0.01965
              mass = 0.01965 × 24
                        = 0.4716g
  2. You are provided with solid P. Carry out the tests below and record your observations and inferences in the spaces provided.
    Place solid P in a clean boiling tube, add 10cm3 of distilled water and shake well. Use about 2cm3 portions of the mixture for the tests below.
    1. Add aqueous ammonia dropwise until in excess.
       Observations  Inferences
        White ppt           
      Insoluble in excess      (1 mark)
       Mg2+, Al3+, Pb2+
       Present Accept Zn2+  absent          ( 1mark)        
    2. Add 2M sodium hydroxide solution dropwise until in excess.
       Observations  Inferences
        White ppt           
      Soluble in excess                                 (1 mark)
               Al3+, Pb2+ Present                          ( 1mark)     Penalise ½mk each for any contradictory ion to a max of 1mk
    3. Add 4 drops of 2M sulphuric (VI) acid.
       Observations  Inferences
       No white ppt
      No effervescence                                          (1 mark)
       Al3+, Present
       SO32−, CO32− absent                                      ( 2marks)     
    4. Add 3 drops of lead (II) nitrate solution
       Observations  Inferences
        white ppt                              (½ mark) SO42−,Cl/Br present                                        ( 1mark)     
    5. Add 3 drops of barium nitrate solution
       Observations  Inferences
      White ppt                     (½ mark)   SO42−   present                             ( 1mark)  Penalise FULLY for any contradicting ion.   
  3. You are provided with an organic substance Q. Carry out the tests below and record your observations and inferences in the spaces provided.
    1. To about 2cm3 of substance Q in a test tube, add 2 drops of acidified potassium manganate (VII) solution.
       Observations  Inferences
      Purple KMnO4
      Solution is decolourised                                           (1 mark)
      F4ChemMarJMP32023Ans3a                                        ( 1mark)     
    2. Place 3 drops of substance Q on a watch glass and ignite.
       Observations  Inferences
       Almost colourless/pale blue flame                                       (1 mark)  F4ChemMarJMP32023Ans3b                                       ( 1mark)     
    3. To about 2cm3 of substance Q, add 2cm3 of ethanoic acid followed by 5 drops of 2M sulphuric (VI) acid and heat.
       Observations  Inferences
       Pleasant/fruity smell
      reject: Sweet smell    (1 mark)
        R−OH present                   ( 1mark)     
    4. To another 2cm3 of substance Q, add 2 drops of acidified potassium dichromate (VI) solution.
       Observations  Inferences
      Orange K2Cr2O7                                      Solution changes to green     (1 mark)    R−OH present                       ( 1mark)     
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