Chemistry Paper 3 Questions and Answers with Confidential - Form 3 End Term 3 Exams 2023

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Q1 = 11MKS
Q2 = 14MKS

Q1. You are provided with:

Solution A: Potassium Chromate VI
Solution B: 0.1mNa2SO3

You are required to determine the number of moles dichromate VI ions (Cr2O2-7) in one litre of solution.

PROCEDURE

Fill the burette with solution B. Pipette 25cm3 of solution A and transfer it into conical flask. Titrate until a permanent green colour is obtained. Record your results in table below and repeat the procedure to fill the table.

   I II  III 
 Find burette readings      
 Initial burette readings      
 Volume of solution B (cm3)      
  1. Determine the average volume of solution B. (5mks)
  2. Calculate the number of moles of solution B. (2mks)
  3. Given that the ionic equation for the reaction between dichromate ion and sulphate is;
    Cr2O2-7(aq) + 3SO2-3(aq) + 8H+(aq)  →  2Cr3+(aq) + SO2-4(aq) + 4H2O(l)
    Calculate;
    1. Number of moles of dichromate IV ion in 25cm3 (2mks)
    2. Moles of dichromate ion one litre of solution.

Q2. You are provided with substance E, carry out the tests below and write your observations and inferences in the space provided.

  1. Describe the appearance of substance E.
     Observation   inferences
       
     (1mk)                                                       (1mk)
  2. Place one third of substance E in the test tube. Heat it strongly.
     Observation   inferences
       
     (1mk)                                                       (1mk)
  3. Place remaining amount of E in boiling tube. Add about 10cm3 of distilled water and shake well. Retain the mixture for tests in d) below.
     Observation   inferences
       
     (1mk)                                                       (1mk)
  4. Use about 2cm3 potion of the mixture obtained in (c) for tests (i) to (iv)
    1. Add 2 to 3 drops of lead (ii) Nitrate to the mixture.
       Observation   inferences
         
       (1mk)                                                       (1mk)
    2. Add 2 to 3 drops of barium Nitrate to second portion of the mixture.
       Observation   inferences
         
       (1mk)                                                       (1mk)
    3. Add five drops of dilute nitric (v) acid to the mixture in (ii) above
       Observation   inferences
         
       (1mk)                                                       (1mk)
    4. To the last portion, add few then excess drops of sodium hydroxide.
       Observation   inferences
         
       (1mk)                                                       (1mk)
  5. Give the formula of cat ion and anion present in substance E.
    Cat ion
    Anion

CONFIDENTIAL

In addition of apparatus formed in lab, each student is expected to have;

  1. 100cm3 of solution A
  2. 100cm3 of solution B
  3. 0.5g of solid E
  4. Burette
  5. Pipette
  6. 2 conical flask
  7. test tubes in rack
  8. boiling tube holder
  9. Test tube holder
  10. Distilled water in wash bottle.

Access

  • 0.5 mBa (NO3)2 solution and dropper.
  • 2M NaOH solution and dropper.
  • Source of heat.
  • 0.1MPb (NO3)2 solution and dropper.
  • 2MHNO3 solution and dropper.
  • Solution A is acidified 0.01MK2CrO7.
  • Solution B is 0.1MNa2SO3.
  • Solution E is about 0.5g of MgSO4.H2O.

NOTE:

Solution A is prepared by dissolving 2.94g of K2CrO7 in 200cm3 of 2M H2SO4 then adding distilled water to 1l of solution.

 

 

MARKING SCHEME

Q1 = 11MKS
Q2 = 14MKS

Q1. You are provided with:

Solution A: Potassium Chromate Vi
Solution B : 0.1mNa2SO3

You are required to determine the number of moles dichromate VI ions (Cr2O2-7) in one litre of solution.

PROCEDURE

Fill the burette with solution B. Pipette 25cm3 of solution A and transfer it into conical flask. Titrate until a permanent green colour is obtained. Record your results in table below and repeat the procedure to fill the table.

   I II  III 
 Find burette readings  8.0 15.5  23.0 
 Initial burette readings  0.0  8.0 15.5 
 Volume of solution B (cm3)  8.0 7.5  7.5 
  1. Determine the average volume of solution B. (5mks)
    7.5 + 7.5 = 7.5cm3
            2
    CT√

    D√
    PA√
    A± 0.1√
    ±0.2√
    FA√
  2. Calculate the number of moles of solution B. (2mks)
    1.0 x 7.5
       1000
    = 0.00075moles
  3. Given that the ionic equation for the reaction between dichromate ion and sulphate is;
    Cr2O2-7(aq) + 3SO2-3(aq) + 8H+(aq)  →  2Cr3+(aq) + SO2-4(aq) + 4H2O(l)
    Calculate;
    1. Number of moles of dichromate IV ion in 25cm3 (2mks)
      0.00075
            3
      = 0.00025 moles
    2. Moles of dichromate ion one litre of solution.
      0.00025 x 1000
                   25
      = 0.01moles/litre

 Q2. You are provided with substance E, carry out the tests below and write your observations and inferences in the space provided.

  1. Describe the appearance of substance E.
    • White crystalline solid// colourless crystalline solid.
  2. Place one third of substance E in the test tube. Heat it strongly.
     Observation   inferences
     Colourless vapor on   condenses on cover plots   Hydrate salt// contains water   of crystallization
     (1mk)                                                       (1mk)
  3. Place remaining amount of E in boiling tube. Add about 10cm3 of distilled water and shake well. Retain the mixture for tests in d) below.
     Observation   inferences
     Solid dissolved forming   colorless   Solution soluble salt
      Absence of Fe2+,           Fe3+,Cu2+
     (1mk)                                                       (1mk)
  4. Use about 2cm3 potion of the mixture obtained in (c) for tests (i) to (iv)
    1. Add 2 to 3 drops of lead (ii) Nitrate to the mixture.
       Observation   inferences
       White precipitate   SO42-
        SO32- Present All=1√
        CO32- 3=√
        Cl-    2 or 1 = 0
       (1mk)                                                       (1mk)
    2. Add 2 to 3 drops of barium Nitrate to second portion of the mixture.
       Observation   inferences
       White precipitate   SO42-
        SO32- All=1√
        CO32- 2=√
        1 = 0
       (1mk)                                                       (1mk)
    3. Add five drops of dilute nitric (v) acid to the mixture in (ii) above
       Observation   inferences
       White precipitate present   SO42- confirmed
       (1mk)                                                       (1mk)
    4. To the last portion, add few then excess drops of sodium hydroxide.
       Observation   inferences
       Observation inferences
       White precipitate present 
       Insoluble in excess√
       Mg2+ √ present
       (1mk)                                                       (1mk)
  5. Give the formula of cation and anion present in substance E.
    Cat ion - Mg2+
    Anion - SO42
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