Chemistry Paper 3 Questions and Answers with Confidential - Kangundo Subcounty Pre Mock Exams 2021/2022

Instructions to candidates:

1. Answer all questions in the spaces provided in the question paper.
2. KNEC mathematical tables and electronic calculators may be used for calculations.
3. All working MUST be clearly shown where necessary.
4. Candidates should answer the questions in English.

1. You are provided with:
   Solid P – 3.6 g of hydrated oxalic acid with the formula H₂C₂O₄. X H₂O. Solution W – 0.2 M sodium hydroxide solution.
   You are required to determine:
   1. Solubility of solid P.
   2. The value of X in H₂C₂O₄. X H₂O.

Procedure I:

1. Fill the burette with distilled water.
2. Transfer 4 cm³ of distilled water from the burette in to a boiling tube containing solid P.
3. Heat the mixture while stirring carefully with a thermometer until all the solid dissolves.
4. Cool the mixture by dipping it in cold water contained in a beaker while stirring with the thermometer. Record the temperature at which crystals start to form in table 1 below.
5. Add a further 2 cm³ of distilled water from a burette to the mixture. Repeat step (iii) and (iv) above and record the crystallization temperature. Complete table 1 below.
   (RETAIN THE CONTENTS OF THE BOILING TUBE FOR USE IN PROCEDURE II)

1. Table 1
   

   Volume of distilled water in boiling tube.	Crystallization temperature.	Solubility of solid A in g/100g of water.
   4
   6
   8
   10
   12

   (5marks)
2. On the grid provided, plot a graph of solubility of solid P against crystallization temperature. (3marks)
   
3. From the graph, determine:
   1. The solubility of solid P at 60ºC. (1mark)
   2. The temperature at which 40 g of solid P would dissolve in 50 g of water. (2marks)

Procedure II:
Transfer all the contents of the boiling tube in procedure I into a clean 250 ml volumetric flask. Rinse the boiling tube and the thermometer with distilled water and add the contents into the volumetric flask. Add 100 cm³ of distilled water to the volumetric flask; shake until all the solid dissolves. Add more distilled water to the mark. Label this as solution Q. Drain the burette of any distilled water and then fill it with solution Q. Pipette 25 cm³ of solution W into a clean conical flask, add 3 drops of phenolphthalein indicator. Titrate solution Q against solution W. Record your reading in table 2 below. Repeat the titration two more times and complete the table below.

1. Table 2
   

   	I	II	III
   Final burette reading (cm3)
   Initial burette reading (cm3)
   Volume of solution Q used (cm3)

   (4marks)
2. Calculate the average volume of solution Q used. (1mark)
3. Calculate the:
   1. Number of moles of solution W used. (1mark)
   2. Number of moles of solution Q used given the equation below. (1mark)
      2NaOH_(aq) + H₂C₂O₄. X H₂O (aq) Na₂C₂O₄.XH₂O_(aq)+ H₂O (l)
   3. Concentration of solution Q in moles per litre. (1mark)
4. Determine the value of X in the formula H₂C₂O₄. X H₂O.(C = 12, H = 1, O = 16).(2mks)

2. You are provided with solid E. Carry out the tests below. Write your observations and inferences in the spaces provided. Place all solid E in a boiling tube. Add about 10 cm³ of distilled water and shake until all the solid dissolves. Use about 2 cm³ portions of the solution in a test tube for the tests below.
   1. To the first portion, add sodium hydroxide solution dropwise till in excess.
      

      Observations	Inferences

   2. To the second portion, add aqueous ammonia dropwise till in excess.
      

      Observations	Inferences

   3. To the third portion, add 3 drops of sodium chloride solution.
      

      Observations	Inferences

   4. To the fourth portion, add 3 drops of barium nitrate solution.
      

      Observations	Inferences

   5. To the fifth portion, add 3 drops of acidified lead (II) nitrate solution.
      

      Observations	Inferences

3. You are provided with solid F. Carry out the tests below. Write your observations and inferences in the spaces provided.
   1. Place half of solid F on a metallic spatula and ignite it over a Bunsen burner.
      

      Observations	Inferences

   2. Place the remaining portion of solid F in a boiling tube. Add 5 cm³ of distilled water and shake. Preserve the resulting mixture for test (i) and (ii) below.
      

      Observations	Inferences

   3. To about 2 cm³ of the solution in a test tube, add 3 drops of acidified potassium manganate (VII) solution.
      

      Observations	Inferences

   4. To another 2 cm³ portion of the solution, add 3 drops of acidified potassium dichromate (VI) solution.
      

      Observations	Inferences

CONFIDENTIAL
The information contained here is to help the teacher in charge of chemistry and head of the institution to prepare adequately before the start of the practical. This information should therefore not be disclosed to anyone else, as that will constitute an exam irregularity.
In addition to the other apparatus found in the laboratory, each candidate should have the following:

1. Complete stand and clamp.
2. 50 ml burette.
3. 25 ml pipette.
4. A white tile.
5. A spatula.
6. Means of heating.
7. 2 boiling tubes.
8. 100 cm³ of solution W.
9. 3.6 g of accurately weighed solid P.
10. A conical flask.
11. 500 ml distilled water in a wash bottle.
12. 100 ml beaker.
13. Means of labeling.
14. 250ml volumetric flask.
15. 6 dry test tubes.
16. About 0.5 g of solid E.
17. One thermometer (-10ºC to 110ºC).
18. About 0.5 g of solid F.

Access to each of the following solutions:
NB: Each solution to be supplied with a dropper.

1. 2 M aqueous ammonia.
2. 2 M sodium hydroxide solution.
3. Sodium chloride solution.
4. Barium nitrate solution.
5. Acidified lead (II) nitrate solution.
6. Acidified potassium manganate (VII).
7. Acidified potassium dichromate (VI).
8. Phenolphthalein indicator.

Preparations.
Solid P is hydrated oxalic acid.
Solution W is 0.2 M sodium hydroxide solution.
Solid E is hydrated aluminium sulphate.
Solid F is maleic acid.

MARKNG SCHEME

Instructions to candidates:

1. Answer all questions in the spaces provided in the question paper.
2. KNEC mathematical tables and electronic calculators may be used for calculations.
3. All working MUST be clearly shown where necessary.
4. Candidates should answer the questions in English.

1. You are provided with:
   Solid P – 3.6 g of hydrated oxalic acid with the formula H₂C₂O₄. X H₂O. Solution W – 0.2 M sodium hydroxide solution.
   You are required to determine:
   1. Solubility of solid P.
   2. The value of X in H₂C₂O₄. X H₂O.

Procedure I:

1. Fill the burette with distilled water.
2. Transfer 4 cm³ of distilled water from the burette in to a boiling tube containing solid P.
3. Heat the mixture while stirring carefully with a thermometer until all the solid dissolves.
4. Cool the mixture by dipping it in cold water contained in a beaker while stirring with the thermometer. Record the temperature at which crystals start to form in table 1 below.
5. Add a further 2 cm³ of distilled water from a burette to the mixture. Repeat step (iii) and (iv) above and record the crystallization temperature. Complete table 1 below. 

(RETAIN THE CONTENTS OF THE BOILING TUBE FOR USE IN PROCEDURE II)

1. Table 1
   

   Volume of distilled water in boiling tube.	Crystallization temperature.	Solubility of solid A in g/100g of water.
   4
   6
   8
   10
   12

   10×½ = 5 mks
   Complete table: (1 Mark) Conditions:
   5 readings (1 mark)
   3-4 readings (½mark)
   Less than 3 readings (0mark)
   Penalties:
   Penalize ½ mark once for unrealistic temperature readings of above 100ºC. and below 10ºC.
   Decimals (1 mark)
   Accept temperature readings given as whole numbers, 1 d.p (.0 or .5) or 2 d.p of .00, .25, .50, .75
   Trend (1 mark).
   Accept only a decreasing trend of temperature, otherwise penalize fully. Solubility calculations in column II (2 marks):
   5 correctly worked out solubility values (2 marks)
   3-4 correctly worked out solubility values (1 mark)
   Less than 3 correctly worked out solubility values (0mark)
2. On the grid provided, plot a graph of solubility of solid P against crystallization temperature. (3marks)
   Graph (3 marks)
   
   1. Axis (2 correctly labelled) = ½ mk.
      Only one axis labelled or axes completely unlabeled = 0 mk.
   2. Scale (½mk)
      Penalize fully for nonlinear / inconsistent interval on any of the axis. Penalize fully if plotting is on less than half of the grid space provided.
   3. Plotting (1 mark)
      All five points correctly plotted = 1 mark. 3 – 4 correctly plotted points = ½mk
      Less than 3 correctly plotted points = 0 mks
   4. Curve (1 mark).
      Accept a smooth curve passing through atleast 3 correctly plotted points, otherwise penalize fully.
3. From the graph, determine:
   1. The solubility of solid P at 60ºC. (1mark)
      Award 1 mark for correctly read solubility value. 
   2. The temperature at which 40 g of solid P would dissolve in 50 g of water. (2marks)
      40 g dissolve in 50 g of water
      ? dissolve in 100g of water.
      40 × 100
          50
      = 80 g√1mark
      Then read the temperature that gives a solubility of 80g/100g of water. √1mark

Procedure II:

Transfer all the contents of the boiling tube in procedure I into a clean 250 ml volumetric flask. Rinse the boiling tube and the thermometer with distilled water and add the contents into the volumetric flask. Add 100 cm³ of distilled water to the volumetric flask; shake until all the solid dissolves. Add more distilled water to the mark. Label this as solution Q. Drain the burette of any distilled water and then fill it with solution Q. Pipette 25 cm³ of solution W into a clean conical flask, add 3 drops of phenolphthalein indicator. Titrate solution Q against solution W. Record your reading in table 2 below. Repeat the titration two more times and complete the table below.

1. Table 2
   

   	I	II	III
   Final burette reading (cm3)
   Initial burette reading (cm3)
   Volume of solution Q used (cm3)

   1. Complete table = 1 mark.
      Complete table with three titrations = 1 mark.
      Incomplete table with two titrations = ½mark.
      Incomplete table with one titration = 0 mark.
      Penalties.
      1. Wrong arithmetic.
      2. Inverted table.
      3. Burette readings beyond 50 ml and below 1.0 ml.
         For any of the above penalties, penalize ½mark each upto a maximum of ½mark.
   2. Use of decimals = 1 mark
      1. 1 d.p used consistently.
      2. If 2 decimal places are used, the second decimal place MUST be a 0 or 5.
         Penalize FULLY for any other use of decimal place.
   3. Accuracy = 1 mark.
      • Compare any of the candidates reading with the school value.
      • If atleast one titre value is within ±0.1 cm³ of the school value = 1 mark.
      • If none is within ±0.1 cm³ of s.v but within ±0.2 cm³ of s.v = ½mark.
      • If none is within ±0.2 cm³ of the s.v, award 0 mark.
      • In case of wrong arithmetic in the table, cored the correct titre with the s.v and award accordingly.
   4. Principles of averaging = 1 mark.
      • 3 consistent values averaged = 1 mark.
      • 3 titrations done, only two consistent and averaged = 1 mark.
      • Only two titrations done, are consistent and averaged = ½mark.
   5. Final answer = 1 mark.
      • Compare the school value with the candidate’s averaged titre.
        • If within ± 0.1 cm³ of the s.v award 1 mark.
        • If not within ± 0.1 cm3 but within ±0.2 cm³ of the s.v award ½mark.
        • If beyond, ±0.2 cm3 award 0 mark.
2. Calculate the average volume of solution Q used. (1mark)
   • Tied to (V) above.
3. Calculate the:
   1. Number of moles of solution W used. (1mark)
      0.2×25 √½mk
       1000
      = 0.005 moles. √½mk
      The above expression MUST be given as it is, otherwise penalize fully for any strange value used.
   2. Number of moles of solution Q used given the equation below. (1mark)
      2NaOH (aq) + H₂C₂O_4. X H₂O (aq) Na₂C₂O₄.X H₂O (aq) + H₂O (l)
      From the equation, mole ratio is 2:1
      0.005 √½mark 
         2
      = 0.0025 moles. √½mark
   3. Concentration of solution Q in moles per litre. (1mark)
      Answer in c(ii) above ×1000 √½mark
              Average titre.
      Correct answer √½mark
4. Determine the value of X in the formula H₂C₂O₄. X H₂O. (C = 12, H = 1, O = 16).(2mks)
   Molarity = Concentration (g/l)
                            RFM
   Conc in g/l = 3.6 ×1000
                                 250
   = 14.4 g/l. √½mark
   RFM =     14.4 (g/l)      √½mark
             Answer in c(iii)
   90 + 18X =     14.4 (g/l)      √½mark
                    Answer in c(iii)
   X =  (14.4 – 90)   ÷ 18√½mark
        Answer in c(iii)

2. You are provided with solid E. Carry out the tests below. Write your observations and inferences in the spaces provided. Place all solid E in a boiling tube. Add about 10 cm³ of distilled water and shake until all the solid dissolves. Use about 2 cm³ portions of the solution in a test tube for the tests below.
   1. To the first portion, add sodium hydroxide solution dropwise till in excess.
      

      Observations	Inferences
      White precipitate√½mark soluble in excess√½mark	Pb2+, Al3+, Zn2+ present. All 3 mentioned = 1mk Any 2 correct mentioned = √½mk Only 1 correct mentioned = 0 mk.

   2. To the second portion, add aqueous ammonia dropwise till in excess.
      

      Observations	Inferences
      White precipitate√½mark insoluble in excess√½mark	Pb2+, Al3+ present. Penalize ½mk for any contradictory ion mentioned as present upto a maximum of 1 mark.

   3. To the third portion, add 3 drops of sodium chloride solution.
      

      Observations	Inferences
      No white precipitate.√1mark	Al3+ present.√1mark Award ½mk for Pb2+ mentioned as absent.

   4. To the fourth portion, add 3 drops of barium nitrate solution.
      

      Observations	Inferences
      White precipitate.√1mark	SO 2-, SO 2- , CO 2- present. (1mk) All 3 mentioned = 2mks Any 2 correct mentioned = 1mk Only 1 correct mentioned = 0 mk. Penalize ½mk for any contradictory ion mentioned as present upto a maximum of 2 marks.

   5. To the fifth portion, add 3 drops of acidified lead (II) nitrate solution.
      

      Observations	Inferences
      White prepitate.√1mark	SO 2- present.√1mark • Accept SO 2- , CO 2- mentioned as absent for ½mk. Penalize 1mk for any contradictory ion. (1mk) (1mk) NB: Penalize fully for any ion written with a wrong charge.

3. You are provided with solid F. Carry out the tests below. Write your observations and inferences in the spaces provided.
   1. Place half of solid F on a metallic spatula and ignite it over a Bunsen burner.
      

      Observations	Inferences
      Burns with a yellow / sooty flame. √1mark

   2. Place the remaining portion of solid F in a boiling tube. Add 5 cm³ of distilled water and shake. Preserve the resulting mixture for test (i) and (ii) below.
      

      Observations	Inferences
      Solid F dissolves or is soluble. √1mark	Polar compound or Q is polar. √1mark

      1. To about 2 cm³ of the solution in a test tube, add 3 drops of acidified potassium manganate (VII) solution.
         

         Observations	Inferences
         Purple color is decolorised changes from purple to colorless

      2. To another 2 cm³ portion of the solution, add 3 drops of acidified potassium dichromate (VI) solution.
         

         Observations	Inferences
         Orange colour changes to green.√1mark	R - OH present √1mark. (1mk)