Kenya Certificate of Secondary Education
233/3- CHEMISTRY -Paper 3
(PRACTICAL)
2 ¼Hours
INSTRUCTIONS TO CANDIDATES
- Answer all the questions 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 time for the paper.
- Use 15 minutes to read through the question paper and make sure that you have all the chemicals and apparatus that you may require.
- Mathematical table and silent electronic calculators may be used.
- All workings must clearly be shown where necessary.
QUESTION 1 (17 MARKS)
You are provided with;
- Solution A containing 2g of sodium hydroxide in 250cm3 of solution
- Solution B which is sulphuric (vi) acid
- Solid C
You are required to;
- Standardize solution B.
- Determine the mass of solid C that reacts with the standardized solution B.
Procedure I
- Fill the burette with solution B
- Transfer 25cm3 of solution B into a 250cm3 volumetric flask. Add distilled water up to the mark. Shake the mixture. Label it solution as D.
- Drain the burette and rinse it thoroughly
- Fill the burette with solution A.
- Pipette 25cm3 of solution D into a conical flask
- Add 2-3 drops of phenolphthalein indicator.
- Titrate solution A against D until pink colour just appears.
- Repeat the above procedure and fill the table 1 below.
Table 1
Experiment | I | II | III |
Final burette reading (cm3) | |||
Initial burette reading (cm3) | |||
VOlume of solution A used (cm3) |
(3marks)
- Calculate the ;
- Average volume of solution A used (show your working) (1mark)
- Molarity of sodium hydroxide solution A (Na =23, O=16, H=1) (1mark)
- Number of moles of solution A used for titration. (1mark)
- Molarity of the original solution B. (2marks)
Procedure II
- Rinse the burette thoroughly and fill it with solution B.
- Transfer 50cm3 of solution into a 100 cm3 beaker.
- Add all the solid C provided to solution B.
- Swirl the mixture until there is no more effervescence.
- Label the mixture as solution E.
- Rise the burette thoroughly and fill it with solution E.
- Pipette 25.0cm3 of solution A into a conical flask.
- Add 2 or 3 drops of phenolphthalein indicator
- Titrate solution E against solution A until the solution turns just colourless.
- Repeat the titration and fill the table II below.
Table II
Experiment | I | II | III |
Final burette reading (cm3) | |||
Initial burette reading (cm3) | |||
Volume of solution E used (cm3) |
(3marks)
- Calculate the ;
- Average volume of solution E used (show your working) (1mark)
- Moles of sulphuric (vi) acid present in 50cm3 of solution B. (1mark)
- Number of moles of solution A used for the titration. (1mark)
- Moles of sulphuric (vi) acid in solution E used for the titration. (1mark)
- Number of moles of sulphuric (vi) acid that reacted with solid C. (1mark)
- Given that 1 mole of C reacts with 1 mole of Sulphuric (VI) acid and the relative formula mass of C is 106, calculate the mass of solid C used in this experiment. (1mark)
QUESTION 2 (7MKS)
You are provided with 3.0g of potassium nitrate labeled solid G. You are required to determine the enthalpy change of solution of solid G.
Procedure
Using a measuring cylinder, place 30cm3 of distilled water in 100cm3 plastic beaker. Stir the water gently with a thermometer and take the temperature after every half a minute. Record the readings in the table III below. At exactly 2 minutes add all solid G to water at once. Stir well and take the temperature of the mixture after every half a minute up to the 4th minute. Record your results in the table III below.
-
Time in Minutes 0 ½ 1 1½ 2 2½ 3 3½ 4 Temperature (oC) X - On the grid provided plot a graph of temperature against time. (2marks)
- On the graph show the change in temperature, ΔT (12mark)
- Calculate the molar enthalpy of solution (ΔHsoln). Assume density of solution= 1.0g/cm3, specific heat capacity of the solution = 4.2jg-K- , K=39.0, N=14.0, O=16.0) (21/2 marks)
QUESTION 3:- QUALITATIVE ANALYSIS (16MKS)
- You are provided with solid F.
You are required to identify the cations and anions in the solid.- Place all the solid F in a boiling tube and add about 10cm3 of distilled water. Shake thoroughly and then filter into a clean test tube. Retain both the filtrate and the residue for the subsequent steps
Observations Inferences 1 mark
1 mark
- Divide the filtrate into 4 portions.
- To the first portion, add aqueous ammonia dropwise till in excess.
Observations Inferences 1 mark
1 mark
- To the 2nd portion add 3 drops of sodium chloride solution.
Observations Inferences ½ mark
1 mark
- To the 3rd portion add about 2 drops of lead (II) nitrate solution and warm the mixture.
Observations Inferences 1 mark
½ mark
- To the first portion, add aqueous ammonia dropwise till in excess.
-
- Scrap the residue into a clean test tube, add dilute nitric (v) acid until the solid dissolves. Test for any gas produced using the wooden splint provided.
Observations Inferences 1 mark
1 mark
- To 2cm3 of the resultant mixture, add 2 drops of potassium iodide
Observations Inferences ½ mark
½ mark
- Scrap the residue into a clean test tube, add dilute nitric (v) acid until the solid dissolves. Test for any gas produced using the wooden splint provided.
- Place all the solid F in a boiling tube and add about 10cm3 of distilled water. Shake thoroughly and then filter into a clean test tube. Retain both the filtrate and the residue for the subsequent steps
- You are provided with solid Z. Carry out the tests below and record your observations and inferences in the spaces provided.
- Using a metallic spatula, ignite one half of solid Z in a Bunsen flame.
Observations Inferences ½ mark
1 mark
- Place the other half of solid Z in a boiling tube. Add about 15cm3 of distilled water and shake well. Use the solution for the following tests.
- Place 1cm3 of the solution in a test tube and determine its pH using universal indicator paper.
Observations Inferences ½ mark
½ mark
- To about 2cm3 of the solution in a test tube, add 3 drops of acidified potassium manganate (VII).
Observations Inferences 1 mark
1 mark
- To 2cm3 of the solution in a test tube, add 2 drops of bromine water.
Observations Inferences 1 mark
½ mark
- Place 1cm3 of the solution in a test tube and determine its pH using universal indicator paper.
- Using a metallic spatula, ignite one half of solid Z in a Bunsen flame.
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