Questions
INSTRUCTIONS TO CANDIDATES
- Answer all the questions in the spaces provided in this question paper.
- You are NOT allowed to start working with the apparatus for the first 15 minutes of the 2 ¼ hours allowed for this paper.
- This time is to enable you to read the question paper and make sure you have all the chemicals and apparatus that you may need.
- All working MUST be clearly shown where necessary
- Mathematical tables and electronic calculators may be used.
- Candidates should answer questions in English.
- You are provided with:
- 0.1M Sodium hydroxide, Solution F
- Solution G made by dissolving 12.6g of dibasic acid, H2J2O4 ,in 250cm3 of distilled water.
- 0.02M acidified potassium manganate (vii), Solution N.
You are required to:- Dilute Solution G
- Standardize the resulting dilute solution using sodium hydroxide Solution F
- Determine the mass of J in the formula H2J2O4
- Determine the rate of reaction between solution G and solution N at various temperatures.
- Procedure I
- Using a measuring cylinder measure 20cm3 of solution G and transfer into a beaker.
- Measure 80cm3of distilled water and add it to the 20cm3 of solution G in the beaker.
- Label this solution H.
- Place solution H in a burette.
- Pipette 25cm3of solution F into a 250cm3 conical flask.
- Add 2 drops of phenolphthalein indicator and titrate with solution Record your results in table
- Repeat the titrations two more times and complete table 1.
- Table 1 ( 4 marks)
I II III Final burette reading(cm3) Initial burette reading (cm3) Volume of solution H used (cm3) - Calculate the average volume of solution H used ( 1 mark)
- Determine the number of moles of:
- Sodium hydroxide, Solution F used. (1 mark)
- The acid, solution H used ( 2 marks)
- Acid in 100cm3 of solution H ( 1 mark)
- Acid in 20cm3 of solution G ( 1 mark)
- Acid in 250cm3 of solution G (1 mark)
- Calculate the:
- Molar mass of acid H2J2O4 ( 2 marks)
- Mass of J in the formula given H2J2O4 that H=1 and O=16 (1 mark)
- Table 1 ( 4 marks)
- Procedure II
- Place 5cm3of solution N in a boiling tube.
- Place another 5cm3of solution G in a boiling tube
- Heat solution N on a Bunsen burner flame to 800C.Allow it to cool to 70°C.Note that care should be taken to prevent breaking of the thermometer.
- Add all solution G into solution N and immediately start a stopwatch.
- Stir the mixture using a thermometer and record the time taken for the purple colour to disappear.
- Clean the boiling tubes and repeat the procedure by allowing solution N to cool to 60°C,50°C,40°C and complete Table 2 below.
- Table II (5 marks)
Temperature,°C 70 60 50 40 Time taken for purple colour to disappear (s) Reciprocal of time, 1/time(s-1) - On the grid provided plot a graph of 1/time (y-axis) against temperature. (3 marks)
- From the graph determine the time taken for the purple colour to disappear at 450C. ( 1 mark)
- State the relationship between the rate of reaction and temperature at which purple colour disappears. ( 1 mark)
- Table II (5 marks)
- You are provided with solid P. Put all solid P in a clean boiling tube and add about 10cm3of distilled water and stir. Divide mixture into four portions.
Observation Inference
(1 mark)
(1 mark)- To the first portion, add sodium hydroxide dropwise until in excess.
Observation Inference
(1 mark)
(1 mark) - To the second portion, dip a glass rod and burn in a non-luminous flame
Observation Inference
(½ mark)
(1 mark) - To the third portion, add 2 drops of Barium nitrate
Observation Inference
(½ mark)
(1 mark) - To the fourth portion add 2 drops of acidified potassium manganate (vii)
[Solution N] using the dropper provided.
Observation Inference
(1 mark)
(1 mark)
- To the first portion, add sodium hydroxide dropwise until in excess.
- You are provided with Solid R. Carry out the following tests and record your observations and inferences in the tables below.
- Using a clean metallic spatula, burn about one third of solid R in a non-luminous flame
Observation Inference
(1 mark)
(1 mark) - Dissolve the remaining solid R in about 10cm3distilled water in a test tube and divide the solution into 3 portions.
To the first portion add 2 drops of potassium manganate (vii) [Solution N] using the dropper provided.
Observation Inference
(1 mark)
(1 mark) - To the second portion add two drops of bromine water.
Observation Inference
( ½mark)
(1 mark) - To the third portion add sodium carbonate provided.
Observation Inference
(½ mark)
(1 mark)
- Using a clean metallic spatula, burn about one third of solid R in a non-luminous flame
Confidential
In addition to the common laboratory apparatus and fittings, each candidate shall be supplied with the following:
- 80cm3 of solution F
- 80cm3 of solution G
- 30cm3 of solution N
- One 50cm3 burette
- One 25cm3 pipette
- Two 250cm3 conical flasks
- One 100cm3 measuring cylinder
- One 250cm3 empty beaker
- Distilled water in a wash bottle
- One thermometer
- Source of heat
- Six dry test tubes
- One glass rod
- Two boiling tubes
- One stopwatch
- One clean dropper
- One clean metallic spatula
- One test tube holder
- 0.5g of sodium carbonate
- 0.5g solid P
- 0.5g solid R
The students should have access to the following: - Phenolphthalein indicator supplied with a dropper
- Bromine water supplied with a dropper
- 2M sodium hydroxide supplied with a dropper
- 1M barium nitrate supplied with a dropper
NOTES- Bromine water is prepared by adding 1cm3 of liquid bromine to 100cm3 of distilled water and shaking thoroughly.
- Solution N is prepared by adding 3.16g of potassium manganate (vii) in 200cm3 of 2M sulphuric (vi) acid and adding water to make one litre.
- Solution F is prepared by dissolving 4g of sodium hydroxide in about 800cm3 of distilled water and making up to one litre solution.
- Solution G is prepared by dissolving 12.6g of oxalic acid in 400cm3 of distilled water and making the solution up to one litre.
- Solid P is sodium sulphite and solid R is oxalic acid.
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