INSTRUCTIONS TO CANDIDATES
- Write your name and index number in the spaces provided above.
- Sign and write the date of examination in the spaces provided.
- Answer ALL the questions in the spaces provided in the question paper
- Mathematical tables and electronic calculators may be used.
- All working MUST be clearly shown where necessary.
FOR EXAMINER'S USE ONLY
Question |
Maximum marks |
Candidate's score |
1 |
22 |
|
2 |
12 |
|
3 |
6 |
|
Total score |
40 |
QUESTIONS
-
- You are provided with
- 2.0M sodium hydroxide solution labelled solution B
- Solution C containing 12.25 g per litre of a mineral acid C
You are required to- Prepare a dilute solution of sodium hydroxide, solution B.
- Determine the
Relative Formula mass of the acid C
Molar Enthalpy change of reaction between acid C and sodium hydroxide solution B.
- You are provided with
Procedure 1.
Using a pipette and a pipette filler place 25.0cm³ of solution B in a 250.0ml volumetric flask. Add to
it about 150cm³ of distilled water. Shake well. Add more distilled water to make upto the mark. Label this solution D.
Fill a burette with solution C. Using a clean pipette and a pipette filler, place 25.0cm³ of solution D into a 250ml conical flask. Add two drops of phenolphthalein indicator and titrate with solution C. Record your results in table 1. Repeat the titration two more times and complete the table. (4 marks)
1 |
2 |
3 |
|
Final burette reading (cm³) |
|||
Initial burette reading (cm³) |
|||
Volume of solution C used (cm³) |
Calculate:
- Average volume of solution C used. (1 mark)
- Moles of solution D used. (2 marks)
- Concentration in moles per litre of acid in solution C given that the number of moles of acid C used are half the moles of D used. (2 marks)
- Relative formula mass (RFM) of solution C. (1 mark)
b) PROCEDURE II.
- Using a clean burette, place 5.0cm³ of solution C into each of six (6) test-tubes.
- Using a 100ml measuring cylinder, place 20cm³ of solution D, sodium hydroxide solution in a 100ml plastic beaker. Measure the temperature of solution D and record it in table 2 below.
- To solution D in the beaker, add acid C, solution C from one of the test-tubes. Stir the mixture with the thermometer and record in Table 2, the maximum temperature reached. Continue with step (iv) IMMEDIATE
- Add the acid C, solution C from another test-tube to the mixture obtained in (iii) above, stir and record the maximum temperature reached in Table 2. Continue adding the acid C, solution C from each of the other four test-tubes, stirring the mixture and recording the maximum temperature each time and complete Table 2.
TABLE 2 (4 marks)
Volume of solution C |
0 |
5 |
10 |
15 |
20 |
25 |
30 |
Maximum temperature (°C) |
c) On the grid provided, plot a graph of temperature (vertical axis) against volume of acid C solution C added. (3 marks)
d) Using the graph
- Determine the volume of solution C which gave the maximum change in temperature. (1 mark)
- Determine the temperature change for the reaction. (1 mark)
e) Using your answer in parts d (i) and d(ii), calculate the molar enthalpy change of the neutralisation reaction between acid C and sodium hydroxide solution.
(Heat capacity = 4.2J g-1 k-1; density of the mixture = 1.0gcm-3) (3 marks)
2.
- You are provided with solid F carry out the following tests write your observations and inferences in the spaces provided.
i) Place a half spatula and full of solid F in a dry test tube and heat strongly. Test the gases produced with litmus paper
Observations |
Inferences |
(1mark) |
(1 mark) |
ii) Place the remaining solid F in a boiling tube and add 10cm3 of distilled water. Divide the resulting solution into five portions
Observations |
Inferences |
(1 mark) |
(1 mark) |
iii) To the first portion, add sodium hydroxide solution drop wise until in excess.
Observations |
Inferences |
(1mark) |
( 1 mark) |
iv) To the second portion, add 5 drops of the hydrogen peroxide and then add ammonia solution drop wise until in excess.
Observations |
Inferences |
(1 ½ mark) |
( ½ mark) |
v) To the third portion, add three drops of acidified lead (II) nitrate solution.
Observations |
Inferences |
( 1 mark) |
(1mark) |
vi) To the fourth portion, add three drops of barium nitrate solution.
Observations |
Inferences |
( 1 mark) |
( 1 mark) |
3. You are provided with an organic liquid P. Carry out the following tests and record you observations and inferences in the space provided.
a) Place about 4cm³ of liquid P in a boiling tube. Add to it 10cm³ of distilled water and shake well.
Label this solution G.
Observations |
Inferences |
( 1 mark) |
(1mark) |
b) Place 2cm³ of solution G in a test-tube. Add to it solid sodium hydrogen carbonate provided.
Observations |
Inferences |
( 1 mark) |
(1mark) |
c) To a second 2cm³ portion of solution G in a test-tube, add 2 to 3 drops of acidified potassium dichromate (VI) and warm.
Observations |
Inferences |
(1 mark) |
(1mark) |
MARKING SCHEME
- PROCEDURE 1
Table 1 . . . . . .(5 marks) Complete table . . . . . 1 mark
Complete table with 3 titration done - 1 mk
Incomplete table with 2 titrations done - ½mk
Incomplete table with 1 titration done - 0 mk
Penalties - Penalise ½ mk ONCE for
- Wrong arithmetic / subtraction
- Inverted table.
- Burette readings beyond 50cm³ unless explained.
- Unrealistic titre values e.g. below 1.00cm³ or in hundreds.
- If two d.ps used, the second decimal must be either a zero of five.
- If three consistent titrations done and averaged . . . 1 mark
- If three titrations done but only two are consistent and averaged . . .1 mark
- If two titrations done, consistent and averaged . . . 1 mark
- If three titrations are done, inconsistent but averaged = 0 mark
- Penalise ½ mk if no working is shown but answer given is correct.
Penalise fully if no working is shown and the answer is wrong. - Accept rounding off or trancating of the answer to 2d.p e.g. 25.666 ~ 25.66 or 25.67 otherwis4e penalise ½ mk for rounding off to 1 d.p
Accept the answer if it works out exactly to a whole no. or to 1.d.p and credit fully.
Final accuracy . . . 1 mark
Tied to correct averaged titre.
Compare the candidates correct averaged titre to the school value.
If within ± 0.10 cm³ of S.V. . . . 1 mark
If not within ± 0.10 cm³ of S.V but withint ±
0.20cm³ of S.V award . . . .½ mark
If beyond (outside) ± 0.20cm³ of S.V .0 mk
Calculations
Moles of solution D used
Moles of B used = 25.2 = 0.05 moles
2
= 1000 = 0.05 = 0.2 m
250
Hence moles of solution D used
= 0.005 moles
Molarity of solution C
Conditions.
- Ans must not have any unit otherwise penalise ½ mk for g or any other unit.
- Accept R.FM as :
88 ≤ RFM ≤ 108
Procedure II
TABLE
- Complete table . . . . 1 mark
Complete table with seven (7) readings and realistic values
Use of decimal . . . (1 mark)- If one decimal place is used, it can either be 0 or 5.
- If 2 d.p are used then they must be 0.00, 0.25, 0.50 or 0.75
- Decimal points must be used consistently as either whole numbers or 1d.p
Accuracy . . . .1 mark
Compare the candidates constant temperature readings with school value (S.V) S.V is the teachers reading at 0. If within ± 2.0°C of S.V award 1 mark.
Trend . . . 1 mark
Conditions.
- Award 1 mark for a continuous rise followed by a constant then a drop
Graph . . . . 3 marks
Award a total of 3 marks distributed as follows.
i). Labelling of axes . . . . ½ mark
If both axes are correctly labelled.
Penalties.
Penalise fully for inverted axes.
Penalise fully for wrong units used. Otherwise ignore if units are omitted.
Penalise fully (award 0) if only one axes is correctly labelled.
Scale . . . . ½ mark
Conditions.
- Area covered by plots should be at least ½ the grid provided i.e .7 big squares verti and 8 big square horizontally.
- Scale interval must be consistent on each axis.
- Scale chosen must be able to accommodate all the readings whether plotted or not.
Plotting . . . 1 mark
If 7 or 6 points are correctly plotted . . 1mk
If 4 or 5 points correctly plotted . . .½ mk
If less than 4 points correctly plotted . . . 0mk
NB
- Accept correct plots even if the axes are inverted and award accordingly.
- If scale intervals are inconsistent credit correct plots. If any, within the 1st scale interval and treat all other plots as wrong.
- Mark all the plots on the graph with either a tick or a cross (×)
2.
- You are provided with solid F carry out the following tests write your observations and inferences in the spaces provided.
i) Place a half spatula and full of solid F in a dry test tube and heat strongly. Test the gases produced with litmus paper
Observations |
Inferences |
Colourless gas turn blue litmus red and red litmus paper remain red Dissolve to form green solution Green precipitate insoluble in excess Brown precipitate formed White precipitate formed |
Acidic gas present Fe2+, Cu2+ Fe2+ present Fe2+ oxidized to Fe3+ SO 4 Cl-, Penalise ½mk for any contradictory ion |
ii) Place the remaining solid F in a boiling tube and add 10cm3 of distilled water. Divide the resulting solution into five portions
Observations |
Inferences |
White precipitate formed |
SO42- Present Reject any contradictory ion |
iii) To the first portion, add sodium hydroxide solution drop wise until in excess.
Observations |
Inferences |
(1mark) |
( 1 mark) |
iv) To the second portion, add 5 drops of the hydrogen peroxide and then add ammonia solution drop wise until in excess.
Observations |
Inferences |
(1 ½ mark) |
( ½ mark) |
v) To the third portion, add three drops of acidified lead (II) nitrate solution.
Observations |
Inferences |
( 1 mark) |
(1mark) |
vi) To the fourth portion, add three drops of barium nitrate solution.
Observations |
Inferences |
( 1 mark) |
( 1 mark) |
3. You are provided with an organic liquid P. Carry out the following tests and record you observations and inferences in the space provided.
a) Place about 4cm³ of liquid P in a boiling tube. Add to it 10cm³ of distilled water and shake well.
Label this solution G.
Observations |
Inferences |
Dissolves in water to form a colourless solution/miscible liquids |
Polar organic compound / Polar compound |
b) Place 2cm³ of solution G in a test-tube. Add to it solid sodium hydrogen carbonate provided.
Observations |
Inferences |
No bubbles / no effervescence. No fizzing |
R-COOH absent |
c) To a second 2cm³ portion of solution G in a test-tube, add 2 to 3 drops of acidified potassium dichromate (VI) and warm.
Observations |
Inferences |
Orange colour of H+ / K2 Cr2 O7 turn green |
R-OH Present |
- About 50cm3 of solution B
- About 150cm3 of solution C
- One pipette 25ml
- One pipette filler
- One burette 0 - 50ml
- Two conical flasks - 250ml
- One 10ml measuring cylinder
- One 100ml measuring cylinder
- 100ml empty beaker
- 250ml volumetric flask
- Six test tubes
- One thermometer -10ºC to 110ºC
- One boiling tube
- About 500cm3 of distilled water supplied in a wash bottle
- Two labels
- About 1g of solid F in a stoppered container
- About 0.2g of solid sodium hydrogen carbonate
- One blue and one red litmus paper
- About 6cm3 of liquid P
- Test tube holder
- Acidified lead (II) nitrate supplied with a dropper.
- Aqueous Barium (II) chloride supplied with a dropper.
- Phenolphthalein supplied with a dropper.
- Acidified potassium dichromate (VI) supplied with a dropper
- Bunsen burner
- Sodium hydroxide solution
- Hydrogen peroxide
- Solution C is prepared by dissolving 6.87cm3 of concentrated sulphuric (VI) acid in 200cm3 of distilled water and made up to 1000cm3 of solution with distilled water. Label this as solution C.
- Solution B is prepared by dissolving 80g of NaOH in about 600cm3 of distilled water and diluting to one litre of solution. Label this as solution B.
- Barium chloride is prepared by dissolving 30g of solid Barium chloride in about 600cm3 of distilled water and diluting to one litre of solution. Label thin as aqueous barium nitrate.
- Acidified potassium dichromate (VI) is prepared by dissolving 25g of potassium dichromate (VI) crystals in about 200cm3 of 2M sulphuric (VI) and diluting with distilled water to one litre of solution.
- Liquid P : Ethanol
- Solid F: iron (II) Sulphate
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