activity resources (teacher's edition) - 2 years
TRANSCRIPT
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SPN 21SPN 21CHEMISTRY
ACTIVITY RESOURCES
CHEMISTRY
ACTIVITY RESOURCES
Teachers Edition
OH SING SENG
GOH SIAH CHING
N RAZIMI HJ MUDA
ROSLENA HJ MUNEL
SRI YANI HEPNIE
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Page
INTRODUCTION TO CHEMISTRY 3
KINETIC PARTICLE THEORY 4 8
CHEMICAL FORMULA 9
TYPES OF COMMON CHEMICAL REACTIONS 10 25
STOICHIOMETRY AND MOLE CONCEPT 26 29
EXPERIMENTAL CHEMISTRY 30 33
ACIDS, BASES AND NEUTRALIZATION 34 38
SALTS 39 46
QUALITATIVE ANALYSIS 47 55
METAL AND EXTRACTION 56 64
THE PERIODIC TABLE 65 66
ENERGY FROM CHEMICALS 67 70
ELECTROLYSIS 71 76
SPEED OF REACTIONS 77 83
REVERSIBLE REACTIONS 84 86
REDOX 87 88
ATMOSPHERE AND ENVIRONMENT 89
ORGANIC CHEMISTRY 90 99
REFERENCES 100
CCoonntteennttss
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Activity 1.4
INTRODUCTION TO CHEMISTRY
Aim: Use mnemonics to familiarize with name and symbol of first row of common transition
metals.
Example:Use mnemonics to memorise the first row of the common transition metals.Scandium, Titanium, Vanadium, Chromium, Manganese, Iron, Cobalt, Nickel, Copper, and Zinc
ScaryTimVeryCrookedManICallNickCorporalZee
- Scandium- Titanium- Vanadium- Chromium- Manganese- Iron- Cobalt- Nickel- Copper- Zinc
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Activity 2.2
KINETIC PARTICLE THEORY
Aim: Using role play to demonstrate the movement of particles in solid, liquid and gas.
Procedure:1. A group of students (6- 9), stand at the front of the room acting as atoms.
2. Standing next to each other in 2 or 3 rows with arms linked they represent a solid- particles
closed together, moving slightly (vibrating) at their fixed position.
3. As heat energy is applied the students move further away from each other and eventually the
links break.
4. Allowing students to move randomly passing each other but still remain close together.
5. Further heating the students move freely away from each other at high speed.
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Activity 2.3
KINETIC PARTICLE THEORY
Aim: To determine the melting point of naphthalene using cooling curve.
Apparatus:ThermometerRetort standBoiling tube
Conical flaskBunsen burnerStopwatch
Materials:Solid naphthalene
Procedure:1. Clamp boiling tube on retort stand.
2. Add 3 spatulas of powdered naphthalene into a boiling tube and insert a thermometer.
3. Heat the naphthalene until all has melted (about 85 C ).
4. Then, leave it to cool in a conical flask.
5. Record the temperature for every 20 seconds until it falls to about 60 C .
6. Record the results in a table.
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Results:Cooling of naphthalene
Time (s) Temperature ( C ) Time (s) Temperature ( C )
0 16020 180
40 200
60 220
80 240
100 260
120 280
140 300
Analysis of data:
1. Plot a graph of temperature against time for the cooling of naphthalene.
2. From the graph deduce the melting point of naphthalene.
3. The melting point of naphthalene is C
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Activity 2.4
KINETIC PARTICLE THEORY
Aim: To determine the purity of ethanol by determining its boiling point.
Apparatus:Thermometer
Beaker 250 3cmRetort standBoiling tubeStirrer or glass rod
Tripod standWire gauzeBunsen burnerStopwatchPorcelain chip
Materials:WaterEthanol sample (Caution: ethanol is flammable)
Procedure:1. Quarter fill the boiling tube with your ethanol sample.
2. Add a porcelain chip to the boiling tube to ensure it does not froth up too much on boiling.
3. Set up apparatus as shown below.
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4. Heat the water gently and stir continuously to ensure an even temperature around the boiling
tube.
5. Continue heating until the ethanol boil. This is when the bubbles start to appear from the
porcelain chip.
Results:
1. Record the highest reading on the thermometer. .. C
2. Allow the ethanol to boil for one minute to see if the temperature change. Record this
temperature. C
Questions:1. The boiling point of ethanol is 78 C . Is your ethanol sample pure?
2. What effect does an impurity have on the boiling point of a substance?
3. Why must we heat the ethanol in a water bath and not heat it directly with a Bunsen flame?
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Activity 5.1
CHEMICAL FORMULA
Aim: To work out the formula of ionic compound using card games.
Materials:A set of cards representing common anions and cations. Each card has the symbol of the ionwritten on it.
Procedure:1. Group the students (2 to 3 students in a group).
2. Give each group a set of cards.
3. To get a correct formula, join the shapes to form a rectangle.
4. The formula can then be read or copied from the card.
For example, to find the formula of copper(II) chloride, a complete rectangle is formed by joiningone copper(II) ion card and two chloride ion cards (see below). Hence the formula of copper(II)
chloride is 2CuCl .
Questions:Now use the card to work out the chemical formulae of the following ionic compounds
(a) Potassium chloride(b) Zinc chloride(c) Copper(II) oxide(d) Potassium sulphate
(e) Potassium manganate(VII)(f) Sodium hydrogencarbonate(g) Potassium dichromate(VI)(h) Magnesium hydroxide(i) Sodium hydroxide
(j) Iron(II) sulphide(k) Sodium sulphate(l) Iron(III) hydroxide(m) Ammonium nitrate
(n) Iron(II) nitrate(o) Iron(II) sulphate(p) Iron(III) sulphate(q) Ammonium sulphate
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Activity 6.2
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show relative reactivity of metals with water.
Apparatus:Test tubes with rackPair of forcepsKnife or scalpel
White tileWater trough (for sodium only)
Materials:Sodium (store in oil) teachers demonstrationCalciumMagnesiumIron
CopperDistilled water
Procedure:1. Place distilled water in four test tubes to a depth of 5 cm.
2. Drop a piece of calcium into a test tube filled with water.
3. Observe the reaction carefully and answer the following questions:
(a) Does the metal float or sink in water?
(b) Does the metal react vigorously?
4. Test the gas given out using lighted splint
5. Dip a piece of red litmus to the solution in the test tube. Is there a colour change?
6. Repeat step 1, 2, 3, and 4 for the other metals.
7. Record all your observations in a table provided under the Results section.
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Results:
ObservationsElement
Float or SinkVigorous or
Not vigorous
Lighted splint testEffect on redlitmus paper
Magnesium
Copper
Calcium
Sodium
Iron
From the results arranged the five metals in the order of decreasing reactivity.
Most reactive Least reactive
............................., .............................., ............................., ..............................., ..............................
Questions:
1. Which group of the Periodic Table does sodium belong?.....
2. What is the common name for this group of metals?
.
3. Name the alkali formed when sodium reacts with water.
.
4. Name the gas produced when sodium reacts with water.
.....................................
5. Which other metals (listed above) will produce similar reaction with cold water?
.
6. Name this type of reaction.
.
7. Write a balanced equation for the above reaction.
.
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Activity 6.3
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show reaction between metals with dilute hydrochloric acid (Reactivity Series of Metals)
Apparatus:Test tubes with rack
Chemicals:Zinc foilMagnesium ribbonCopper foil
Iron wireDilute hydrochloric acid solution
Procedure:1. Place dilute hydrochloric acid in a test tube to a depth of 2 cm.
2. Drop a piece of zinc into the test tube.
3. Test the gas given out using a lighted splint.
4. Repeat step 1, 2 and 3 for magnesium, copper and iron.
5. Record all your observations in a table provided in the Results section.
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Results:
Metals Observations Lighted splint test
Copper
Zinc
Magnesium
Iron
From the results arranged the four metals in the order of decreasing reactivity.
Most reactive Least reactive
....................................., ......................................, ....................................., .......................................
Questions:1. Write the chemical formula for hydrochloric acid.
.
2. Name the gas given out when dilute acid reacts with a metal..................................................................................................................................................
3. Name the metals (listed above) other than zinc that produces similar reaction with acid.
.
4. What would you expect the reaction to be if potassium is used instead of zinc in the above
reaction?
.
5. Although copper is a metal, it does not react with dilute hydrochloric acid. Why?
.
6. Name the salt formed when zinc reacts with dilute hydrochloric acid.
.
7. Name this type of reaction
.
8. Write a balanced equation for the above reaction.
.
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Activity 6.4
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show reaction of carbonates with dilute hydrochloric acid.
Apparatus:Test tube with rackBoiling tube
Delivery tube (or plastic syringe)Spatula
Chemicals:Calcium carbonate powderCopper(II) carbonate powderDilute hydrochloric acid solutionLimewater
Procedure:1. The test tube is filled with dilute hydrochloric acid to a depth of 3 cm.
2. One spatula of powdered calcium carbonate is added to the dilute hydrochloric acid.
3. Pass the gas given out into limewater.
4. Repeat step 1 and 3 for powdered copper(II) carbonate.
5. Record all your observations in the table provided.
Dilute hydrochloric acid
Boiling tube
Calcium carbonate powder
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Results:
Observations Limewater test
Calcium carbonate
Copper(II) carbonate
Questions:Calcium carbonate
1. Name the gas given out in the reaction..
2. Is calcium carbonate soluble in water?
.
3. Name the salt formed when calcium carbonate reacts with dilute hydrochloric acid?
.
4. Is this salt soluble in water?
.
5. Name this type of reaction.
.
6. Write a balanced equation for the above reaction.
.
Copper(II) carbonate1. What is the colour of copper(II) carbonate?
........
2. Is copper(II) carbonate soluble in water?
.
3. Name the gas given out in the above reaction.
.
4. Write a balanced chemical reaction for the above reaction.
.
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Activity 6.5
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show precipitation reaction.
Apparatus:Test tubes
Materials:Potassium iodide solutionLead(II) nitrate solutionSilver nitrate solution
Sodium sulphate solutionBarium chloride solutionDilute hydrochloric acid solution
Procedure:1. Pour potassium iodide solution into a test tube (about 2 cm depth) and add an equal volume of
lead(II) nitrate solution and observe.
2. Leave the mixture to stand for a few minutes and observe.
3. Repeat step 1 and 2 for:
(a) silver nitrate and dilute hydrochloric acid solutions
(b) Sodium sulphate and barium chloride solutions
Results:
Reaction Initial observations When left to stand
(a) Potassium iodide +Lead(II) nitrate solution
(b) Silver nitrate + Dilutehydrochloric acid
(c) Sodium sulphate + bariumchloride
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Questions:1. Name the precipitate formed in experiment (a), (b) and (c).
Experiment (a): ..
Experiment (b): ..
Experiment (c): ..
2. Write the balanced chemical equations for experiment (a), (b) and (c).
Experiment (a): ...
Experiment (b): ...
Experiment (c):
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Activity 6.6
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show displacement reaction between metals.
Apparatus:
Beaker 50 3cmMeasuring cylinder
Sand paper
Materials:Magnesium ribbonLead(II) nitrate solutionZinc foilCopper(II) sulphate solution
Silver nitrate solutionMagnesium chloride solutionCopper foil
Procedure:1. Clean a strip of magnesium ribbon with a sand paper.
2. Pour about 20 3cm of lead(II) nitrate solution into a beaker.
3. Immerse the magnesium ribbon in the lead(II) nitrate solution.
4. Leave the mixture aside for few minutes, and observe.
5. Repeat the above experiment using the following:
(i) Zinc foil and copper(II) sulphate solution,
(ii) Magnesium ribbon and silver nitrate solution,(iii) Copper foil and magnesium chloride solution.
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Results:
Reaction Observations Conclusion
Magnesium+
lead(II) nitrate solution
Zinc+
copper(II) sulphate solution
Magnesium+
silver nitrate solution
Copper+
Magnesium chloride solution
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Activity 6.7
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show displacement reaction between halogens.
Apparatus:Test tubes
Materials:Chlorine waterBromine waterSodium bromide solution
Potassium iodide solutionIodineSodium chloride solution
Procedure:1. Pour potassium iodide solution into a test tube (about 2 cm depth).
2. Add an equal volume of chlorine water and observe.
3. Record your observations in the table provided.
4. Repeat the experiment for the following reaction:
(i) Chlorine water and sodium bromide solution,
(ii) Bromine water and sodium chloride solution,
(iii) Bromine water and potassium iodide solution,
(iv) Iodine and sodium chloride solution,
(v) Iodine and sodium bromide solution.
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Results:
HalidesHalogen
NaCl (aq) NaBr (aq) KI (aq)
Chlorine
Bromine
Iodine
Questions:1. From the results, arrange the three halogens in the order of decreasing reactivity.
Most reactive Least reactive
., ., ..
2. Write the balanced chemical equation for the following reactions:
(a) Chlorine and sodium bromide
..
(b) Chlorine and potassium iodide
..
(c) Bromine and potassium iodide
..
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Activity 6.8
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show thermal decomposition of carbonates.
Apparatus:Pyrex glass test tubeTest tube with rackTest tube holder
Delivery tube (or plastic syringe)Bunsen burner
Materials:Copper(II) carbonate powder
Ammonium carbonate powderLimewaterZinc carbonate powder
Procedure:
1. Put some powdered copper(II) carbonate into a Pyrex test tube and heat it strongly.
2. Pass the gas given out through limewater and observe.
3. Record your observations in the table provided.
4. Repeat the experiment with ammonium carbonate and zinc carbonate.
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Results:
Reaction Observations Limewater test
(a) Copper(II) carbonate
(b) Zinc carbonate
(c) Ammonium carbonate
Questions:1. What is the colour of the residue in experiment (a)?
2. What is the colour of the residue in experiment (b)?
3. Do you see any residue in experiment (c)? Why?
4. Write the balanced chemical equation for all the reactions.
(i) Experiment (a): ..
(ii) Experiment (b): ..
(iii) Experiment (c): ..
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Activity 6.9
TYPES OF COMMON CHEMICAL REACTIONS
Aim: To show direct reactions by heating
Part 1: Heating iron with sulphur
Apparatus:CruciblePipeclay triangleTripod stand
TongSpatulaBunsen burner
Materials:Iron filingsSulphur powder
Procedure:1. Mix one spatula full sulphur powder with an equal amount of iron filing in a crucible.
2. Heat the mixture strongly and observe.
Results:
Observation: ...
Questions:1. Name the product of the reaction.
2. Write the equation for the reaction.
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Part 2: Heating sulphur with air (oxygen)
Apparatus:CruciblePipeclay triangle
Tripod stand
TongSpatula
Bunsen burner
Materials:Sulphur powderBlue litmus paper
Strip filter paperAcidified potassium dichromate(VI)
Procedure:1. Add one spatula full sulphur powder into a crucible.
2. Then, heat strongly and observe.
3. Test the gas given out using moist blue litmus paper and acidified potassium dichromate(VI)
paper.
4. Record your observations in the table
Results:
Test Observations
Using moist blue litmuspaper
Using acidified potassiumdichromate(VI) paper
Questions:1. Name the product of the reaction.
2. Write the equation for the reaction.
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Activity 7.1
STOICHIOMETRY AND MOLE CONCEPT
Aim: To prepare standard solution of copper(II) sulphate.
Part 1:
Preparation of 0.1 3dmmol copper(II) sulphate solution
Apparatus:
Volumetric flask 250 3cmBeakerBalance
Glass rod
Materials:
Distilled waterCopper(II) sulphate crystals
Procedure:1 Use the balance to weigh _______ g of copper(II) sulphate pentahydrate crystals.
2 Dissolve the copper(II) sulphate in distilled water inside a beaker.
3 Pour the solution into a 250 3cm volumetric flask.
4 Add distilled water until the graduation mark on the neck of the graduated flask.
Results:
The solution prepared is 0.1 3dmmol copper(II) sulphate solution.
The solution contains . mole OH5.CuSO 24 in 13dm solution.
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Part 2:
Preparation of 0.01 3dmmol copper(II) sulphate solution from 0.1 3dmmol copper(II) sulphate
solution.
Procedure:
1 Pipette 25 3cm of copper(II) sulphate solution from Part 1.
2 Pour the solution into a 250 3cm volumetric flask.
3 Add distilled water until the graduated mark on the neck of the graduated flask.
Results:
The solution prepared is 0.01 3dmmol copper(II) sulphate solution.
The solution contains mole OH5.CuSO 24 in 13dm solution.
Questions:
ionconcentratFinalionconcentratOriginalxfactorDilution
1. Calculate the dilution factor from the above equation?
X
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Activity 7.2
STOICHIOMETRY AND MOLE CONCEPT
Aim: To determine the percentage purity of sodium carbonate in a mixture of sodium carbonate
and ammonium carbonate.
Apparatus:Bunsen burner with matchesTripod standCrucible
Pipeclay triangleTongsSpatula
Materials:Sample of impure sodium carbonate (sodium carbonate mixed with ammonium carbonate)
Procedure:
1. Weigh the mass of the crucible.
2. Then add in sample of impure sodium carbonate and weigh.
3. Place the crucible on the tripod stand, and heat it strongly for five minutes.
4. Leave the crucible to cool and weigh the content again.
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Results:(a) Mass of the empty crucible = .. g
(b) Mass of the crucible + impure sample of sodium carbonate = .. g
(c) Mass of impure sample of sodium carbonate [(b) (a)] = .. g
(d) Mass of crucible after heating = .. g
(e) Mass of pure sodium carbonate [(d) (a)] = .. g
Formula to calculate percentage purity:
Questions:
Calculate the percentage purity of sodium carbonate.
%100mplemass of sa
lece in samptanre subsmass of pu=puritypercentage
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Activity 8.1
EXPERIMENTAL CHEMISTRY
Aim: To obtain copper(II) sulphate crystals from a mixture of copper(II) sulphate and sand.
Apparatus:
250 3cm beaker
250 3cm conical flaskFilter paperFilter funnel
Stirring rodEvaporating dishBunsen burnerTripod stand
Materials:A mixture of copper(II) sulphate with sand
Procedure:1. Put the mixture in a beaker
2. Add water to the mixture
3. Stir with a glass rod to make sure that copper(II) sulphate dissolved.
4. Filter the mixture; collect the filtrate in a conical flask.
5. Wash the residue on the filter paper with water.
6. Evaporate the filtrate until saturated, and leave it to crystallize.
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Results:1. The residue is
The filtrate is ...
The solvent is
2. Explain why the residue is washed with water.
3. Give an example of a mixture of two other substances that can be separated by this method.
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Activity 8.5
EXPERIMENTAL CHEMISTRY
Aim: To separate various dyes in food colouring and measure the R values.
Apparatus:Boiling tubeFilter paperRuler
Pair of scissorsDistilled water
Materials:Mixture of food colouring
Procedure:1. Cut a strip of filter paper such that it can fit neatly into a boiling tube. It should also be slightly
longer than the boiling tube.
2. Draw a baseline with a pencil, about 2 cm away from the bottom tip.
3. Mark a tiny spot on the middle of the baseline with food colouring.
4. Put about 1cm depth of distilled water into the boiling tube.
5. Mount the filter paper strip in the boiling tube.
6. Leave the apparatus to stand for a short while.
7. Observe the solvent front as the water travels up the paper.
8. Remove the piece of filter paper when the solvent front reaches just below (1cm) the top of the
paper. [DO NOT let the solvent front go beyond the top of the paper]
9. Allow the paper to dry.
spotbaseline
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Results:Attach your chromatogram in the space below.
Questions:
1. What is the principle behind paper chromatography?
2. Calculate theR for each colour.
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Activity 9.1
ACIDS, BASES AND NEUTRALIZATION
Aim: To neutralise hydrochloric acid by titrating with sodium hydroxide solution.
Apparatus:
Materials:Solution P is dilute hydrochloric acid of unknown concentration
Solution Q is 0.1 3dmmol sodium hydroxide solution
Methyl orange or screened methyl orange indicator.
Procedure:1. Fill the burette with solution P until 0 mark. Make sure that no air bubbles are trapped at the tip
of the burette.
2. Pipette a 25.0 3cm portion ofQ into a conical flask. Add a few drops of either screened methyl
orange or methyl orange indicator.
3. Titrate the solution Q with the solution P from the burette and record the results in the table,
repeating the titration as many times as you consider necessary to achieve consistent results.
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Results:
Titration number 1 2 3
Final burette reading / 3cm
Initial burette reading / 3cm
Volume ofP used / 3cm
Best titration results ()
Summary:Tick () the best titration results.
Using these results, the average volume ofP required was . 3cm .
Volume ofQ used was . 3cm
Hence,
. 3cm of NaOH required ................ cm3 of HCl
Questions:1. Calculate the number of moles of sodium hydroxide used in the titration.
2. Write a balanced equation for the neutralisation of HCl by NaOH.
3. How many moles of HCl would be used in neutralising NaOH in the titration?
4. Having known the number of moles of hydrochloric acid from (3) and also the volume of the
acid used in the titration, calculate the concentration in 3dmmol of the hydrochloric acid.
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Activity 9.2
ACIDS, BASES AND NEUTRALIZATION
Aim: To titrate sodium carbonate and hydrochloric acid and to find percentage purity of sodium
carbonate.
Materials:
Solution P is 0.2 3dmmol hydrochloric acid
Solution Q is made by dissolving 28 g of a mixture of sodium chloride and sodium carbonate in
water and made up to 1 3dm solution.
Procedure:You are required to find the percentage purity of sodium carbonate in the mixture.
1. Put solution P in a burette.2. Pipette a 25.0 3cm portion ofQ into a conical flask. Add a few drops of either screened methyl
orange or methyl orange indicator.
3. Titrate the solution Q with the solution P from the burette and record the results in the table,
repeating the titration as many times as you consider necessary to achieve consistent results.
Results:
Titration number 1 2 3Final burette reading / 3cm
Initial burette reading / 3cm
Volume ofP used / 3cm
Best titration results ()
Summary:In the above titration cm3 of solution P is required to exactly neutralise
... cm3
of solution Q.
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Questions:1. Write a chemical equation to show the reaction involved in the titration.
2. From the titration, calculate the concentration of sodium carbonate in solution Q in 3dmmol .
3. Given that the molecular mass of sodium carbonate, 32CONa is 106, calculate the
concentration of sodium carbonate in solution Q in 3dmg .
4. Calculate the percentage purity by mass of sodium carbonate in the original mixture used in
the preparation of solution Q.
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Activity 9.3
ACIDS, BASES AND NEUTRALIZATION
Aim: To show reaction between sodium hydroxide and ammonium chloride
Apparatus:Test tube with rackTest tube holder
Bunsen burnerSpatula
Materials:Sodium hydroxide solutionSolid ammonium chlorideLitmus paper
Procedure:
1. Put one spatula full solid ammonium chloride into a test tube and slowly pour in sodium
hydroxide solution. Smell the gas.
2. Warm the mixture gently by using a small Bunsen flame.
3. Test the gas by using moist red and blue litmus paper.
Results:
1. When aqueous sodium hydroxide is added to solid ammonium chloride and warmed gently a
gas is formed. Describe the smell of the gas.
2. Test the gas with moist blue litmus paper. Describe your observation.
3. Test the gas with moist red litmus paper. Describe your observation.
Conclusion:
1. When an ammonium salt reacts with an alkali gas is formed, which turnmoist .. litmus paper . .
2. Write an equation for the reaction between sodium hydroxide and ammonium chloride.
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Activity 10.1
SALTS
Aim: To prepare copper(II) sulphate crystals by reacting sulphuric acid with
copper(II) oxide or copper(II) carbonate
Apparatus:BeakerConical flaskStirrerFilter funnel
Filter paperEvaporating basinSpatula
Materials:Dilute sulphuric acidCopper(II) oxide or copper(II) carbonate
Procedure:1. Put about 100 cm3 of dilute sulphuric acid in a beaker and heat it gently.
2. Add copper(II) oxide or copper(II) carbonate to the hot sulphuric acid, a little at a time until in
excess.
3. Filter out the excess copper(II) oxide or copper(II) carbonate by using filter funnel and filter
paper.
4. Collect the filtrate in an evaporating basin and evaporate the filtrate until saturated.
5. Leave the saturated filtrate to cool and crystallise.
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Questions:1. Name the base or carbonate used in this reaction?
2. What is the formula of this compound?
3. Is this compound soluble or insoluble?
4. Name the above reaction.
5. Write chemical equation for the above reaction.
6. Name the salt formed from the above reaction.
7. Name the filtrate.
8. What is the residue left on the filter paper?
9. Why must the copper(II) oxide be added in excess?
10. Can the above reaction be carried out using titration method? Why?
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Activity 10.2
SALTS
Aim: To prepare insoluble salts
Apparatus:Test tubes with rack
Materials:Silver nitrate solutionPotassium iodide solution
Dilute hydrochloric acid solutionDilute nitric acid solution
Procedure:Carry out the following tests and record your observations in the table.
Testno.
Test observations
1 (a) To a portion of silver nitrate solution,add dilute hydrochloric acid until achange is seen.
(b) Leave the mixture to stand for a fewminutes and observe.
2 (a) To a portion of potassium iodidesolution, add lead(II) nitrate solutionuntil a change is seen.
(b) Leave the mixture to stand for a fewminutes and observe.
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Questions:1. Name the above reaction.
2. Write the symbol and ionic equations for the reactions between silver nitrate and hydrochloric
acid.
(a) Symbol equation
..
(b) Ionic equation
..
3. Write the symbol and ionic equations for the reactions between potassium iodide and lead(II)nitrate.
(a) Symbol equation
..
(b) Ionic equation
..
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Activity 10.3
SALTS
Aim: To investigate solubility of salts in water
Apparatus:Test tubes with rackStoppersSpatula
Materials:Distilled WaterSolid salts:Silver chlorideSodium chloride
Lead(II) chlorideBarium sulphateCopper(II) sulphate
Lead(II) sulphateSodium carbonate
Calcium carbonatePotassium nitrateSilver nitrate
Procedure:1. Add half a spatula of a salt to a test tube.
2. Half-fill the test tube with distilled water. Then stopper the tube and shake well.
3. Record your observation in the table provided.
Results:
SaltSolubility
(soluble or insoluble)
Silver chloride
Sodium chloride
Lead(II) chloride
Barium sulphate
Copper(II) sulphateLead(II) sulphate
Sodium carbonate
Calcium carbonate
Potassium nitrate
Silver nitrate
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Questions:
State whether you think the following substances are soluble or insoluble in water:
(a) Zinc nitrate
(b) Potassium nitrate
(c) Copper(II) carbonate
(d) Sodium nitrate
(e) Ammonium chloride
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Activity 10.4
SALTS
Aim: To determine the solubility of salts in 3cmg .
Apparatus:BeakersGlass rodSpatulaBalance
Filter funnelFilter paperMeasuring cylinder
Materials:
Water
Solid salts: sodium chloride and copper(II) sulphate
Procedure:
1. Label each beaker with the name of the salts. Measure 100 3cm water into each beaker.
2. Record the mass of these beakers containing water.
3. Add a spatula of sodium chloride salt and stir till dissolved.
4. Repeat step 3 until no more salt can dissolve in the 100 3cm of water.
5. Filter this salt solution and collect the filtrate.
6. Record the mass of this salt solution (filtrate).7. Subtract this new mass with the previous mass.
8. The difference will represent the solubility of the salt in 3cm100g .
9. This solubility can then be converted to 3dmg .
10. Repeat the experiment with copper(II) sulphate salt.
11. Record your results in the table.
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Results:
Sodium chloride salt Copper(II) sulphate salt
Mass of beaker + 100 3cm water / g (a)
Mass of salt solution (filtrate) / g (b)
Solubility in 3cm100g (a) (b)
Solubility in 3dmg
Conclusion:
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Activity 11.1
QUALITATIVE ANALYSIS
Aim: To identify the following cations: 3 Al ,
4NH , 2Ca , 2Cu , 2Fe , 3Fe and 2Zn
Apparatus:Test tubes with rackTest tube holderBunsen burner
Materials:Aqueous sodium hydroxide solutionAqueous ammonia solution
Aqueous solution of the following salts:Aluminium sulphate AAmmonium chloride BCalcium chloride CCopper(II) sulphate D
Iron(II) sulphate EIron(III) chloride FZinc nitrate G
Procedure:A, B, C, D, E, F and G are unknown solutions containing different cations. Carry out the followingtest and record your observations in the table. You should test and name, where possible, anygases evolved.
Testno.
Test Observations
(a) To a portion ofA add aqueous sodiumhydroxide until a change is seen.
(b) Add an excess of aqueous sodiumhydroxide to the mixture from (a).
1
(c) To a portion ofA add aqueousammonia until a change is seen.
(d) Add an excess of aqueous ammonia tothe mixture from (c).
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Testno.
Test Observations
2 (a) To a portion ofB add equal volume ofaqueous sodium hydroxide.
(b) Then warm gently
(c) To a portion ofB add equal volume ofaqueous ammonia.
3 (a) To a portion ofC add aqueous sodium
hydroxide until a change is seen.
(b) Add an excess of aqueous sodiumhydroxide to the mixture from (a).
(c) To a portion ofC add equal volume ofaqueous ammonia.
(a) To a portion ofD add aqueous sodiumhydroxide until a change is seen.
(b) Add an excess of aqueous sodiumhydroxide to the mixture from (a).
4
(c) To a portion ofD add aqueousammonia until a change is seen.
(d) Add an excess of aqueous ammonia tothe mixture from (c).
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Testno.
Test Observations
(a) To a portion ofE add aqueous sodiumhydroxide until a change is seen.
(b) Add an excess of aqueous sodiumhydroxide to the mixture from (a).
5
(c) To a portion ofE add aqueousammonia until a change is seen.
(d) Add an excess of aqueous ammonia to
the mixture from (c).
(a) To a portion ofF add aqueous sodiumhydroxide until a change is seen.
(b) Add an excess of aqueous sodiumhydroxide to the mixture from (a).
6
(c) To a portion ofF add aqueousammonia until a change is seen.
(d) Add an excess of aqueous ammonia tothe mixture from (c).
(a) To a portion ofG add aqueous sodiumhydroxide until a change is seen.
(b) Add an excess of aqueous sodiumhydroxide to the mixture from (a).
7
(c) To a portion ofG add aqueousammonia until a change is seen.
(d) Add an excess of aqueous ammonia tothe mixture from (c).
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Questions:
Give the names and formulae of the cations present in:
Name Formula
Solution ASolution B
Solution C
Solution D
Solution E
Solution F
Solution G
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Activity 11.2
QUALITATIVE ANALYSIS
Aim: To identify the following anions: 2
3CO , Cl , I ,
3NO and 2
4SO
Apparatus:Test tubes with rackTest tube holderBunsen burner
Materials:Aqueous solution of the anions above:Sodium carbonate ASodium chloride B
Potassium iodide CSilver nitrate DSodium sulphate - E
Aqueous barium chlorideAqueous lead(II) nitrate
Aqueous sodium hydroxideAluminum foilDilute nitric acid
Students are required to carry out tests to identify the anions in solutions A, B, C, D and E.
State eitherpositive ( ) ornegative ( X ) for each test using the reagents belowSolution
Dilute nitric acid 3 AgNO (aq) 2BaCl (aq) 23 )NO(Pb (aq)NaOH + Al
and heat
A
B
C
D
E
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Anion
present
Observations
P
rocedure
Reagen
tgiving
positiv
etest
Writethepositivetestfo
rtheanions
A,
B,
C,
D
andE
inthespacesprovided
Solution
A B C DE
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Activity 11.3
QUALITATIVE ANALYSIS
Aim: To test for gases
Apparatus:Bunsen burnerLitmus paperSpatulaFilter paper
Test tube holderPlastic syringeTest tubes with rackWooden splint
Materials: Acidified potassium dichromate (VI) Dilute hydrochloric acidDistilled water
Ammonium chloride solution
Hydrogen peroxide solutionBleach solutionLimewater
Solid calcium hydroxideManganese(IV) oxide
Sodium sulphiteCalcium carbonateMagnesium ribbon
Procedure:1. Generate the gas as described in the table.
2. Note its colour and odour and record your observations in the table
3. Carry out specific tests described in column 3 and record your observations.
Note: Use a test tube holder when heating anything in a test tube.
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TestNo.
Gas observations Specific Test and observations
1 HydrogenPut one magnesium ribbon
into a test tube.
Then add 2 3 3cm ofdilute hydrochloric acid intothe test tube.
Wooden splint testInsert a lighted wooden splint into the
mouth of the test tube.
2 Oxygen
Put 2 3 3cm of hydrogenperoxide into a test tube.
Then add a small amountof manganese(IV) oxideinto the test tube.
Wooden splint testInsert a glowing wooden splint into themouth of the test tube.
3 Carbon dioxidePut calcium carbonate intoa test tube.
Then add 2 3 3cm of
dilute hydrochloric acid intothe test tube.
Limewater testCollect the gas using plastic syringe thenpass the gas into test tube containinglimewater then shake.
4 Sulphur dioxidePut sodium sulphite into atest tube.
Then add 2 3 3cm ofdilute hydrochloric acid intothe test tube and heat.
Litmus testHold moist blue litmus paper in the gas.
Potassium dichromate(VI) testHold a piece of filter paper dipped inacidified potassium dichromate(VI) in the
gas.
Potassium manganate(VII) testHold a piece of filter paper dipped inacidified potassium manganate(VII) in thegas.
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TestNo.
Gas observations Specific Test and observations
5 Chlorine
Add about 2 3cm of dilute
hydrochloric acid into a testtube.
Then add about 2 3cm ofbleach solution.
Litmus testHold moist blue litmus paper in the gas.
6 AmmoniaPut ammonium chloridesolution into a test tube.
Then add one spatula ofsolid calcium hydroxide andwarm gently.
Litmus testHold moist red litmus paper in the gas.
7 Water vapourOne third fill a boiling tubewith water
Then heat gently.
Hold a piece of blue cobalt chloride paperin the gas.
8 Nitrogen dioxide(N 2006, P 3)
Put one spatula of sodiumnitrite in a test tube.
Then add about 2 3cm ofdilute hydrochloric acid.
Litmus testHold moist blue litmus paper in the gas.
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Activity 12.1
METALS AND EXTRACTION
Aim: To compare the reactivity of metals by displacement reaction.
Apparatus:Test tubes with rackSandpaperSpatula
Materials:Magnesium ribbonZinc foilsIron fillingsCopper foils
1 3dmmol Magnesium sulphate solution
1 3dmmol Zinc sulphate solution
1 3dmmol Iron (II) sulphate solution
1 3dmmol Copper (II) sulphate solution
Procedure:1. Clean a strip of magnesium ribbon with sandpaper.
2. Half fill a test tube with zinc sulphate solution.
3. Immerse the magnesium ribbon in the zinc sulphate solution.
4. Leave the mixture aside for a few minutes, and observe.
5. Repeat the experiment above using the materials stated in the table.
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Results:
Observations with
Magnesium Zinc Iron Copper
Magnesiumsulphate solution
Zinc sulphatesolution
Iron(II) sulphatesolution
Copper(II) sulphatesolution
Questions:
1. From your results arrange the four metals in order of decreasing reactivity.
Most reactive Least reactive
................................... , ................................... , ................................... , ................................... .
2. Complete these displacement equations:
CuSO4 (aq) + Fe (s) __________ + _________
FeSO4 (aq) + Zn (s) __________ + _________
ZnSO4 (aq) + Mg (s) __________ + _________
3. Aluminium is more reactive than zinc but less reactive than magnesium. Will aluminiumdisplace iron from a solution of iron (II) salt? Explain.
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Activity 12.2
METALS AND EXTRACTION
Aim: To show Thermit reaction (reduction of metal oxide) demonstration only.
Apparatus:Sand bathPaper cone made from filter paperSpatula
Materials:Iron(III) oxide
Aluminium powderMagnesium powder
Magnesium ribbonBarium peroxide (or potassium chlorate)
Procedure:1. Mix a few grams of iron(III) oxide powder with an equal amount of aluminium powder and put
the mixture in a paper cone mounted on a sand bath as shown in the diagram.
2. Mix a little barium peroxide or potassium chlorate with magnesium powder and pour the
mixture into the paper cone containing the mixture of iron(II) oxide and aluminium powder. This
mixture is to set off a preliminary reaction.
3. Using a long piece of clean magnesium ribbon as a fuse, stick one end into the base of the
paper cone and burn the other end.
[Caution: Immediately move far away from the burning magnesium ribbon.]
Sand bath
Paper cone
Mixture of
iron(III) oxide andaluminium powder
Mixture of barium peroxide and
magnesium powder
Magnesium ribbon
as fuse
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Results:
1. Describe the reaction.
2. Write the equation to show the reaction between iron(III) oxide and aluminium.
...
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Activity 12.3
METALS AND EXTRACTION
Aim: To show the action of heat on the carbonates.
Apparatus:Test tubes with rackTest tube holders
Bunsen burnerPlastic syringe (or delivery tube)
Materials:Zinc carbonateCopper(II) carbonateLime water
Procedure:
1. Put some powdered zinc carbonate into a test-tube and heat it strongly.
2. Pass the gas given out through lime water and observe for the formation of a new substance.
3. Repeat the experiment using copper(II) carbonate and observe for the colour change and the
formation of a new substance.
Results:(a) Zinc carbonate is (colour). When strongly heated zinc carbonate gives out a
(colour) gas which turns lime water
(b) The residue is (colour) when hot and (colour) when cold.
(c) The gas is and the residue is
(d) Write word equation for the above reaction.
(e) Write symbol equation for the above reaction.
(f) Copper(II) carbonate is (colour). When strongly heated copper(II) carbonate
gives out a (colour) gas which turns lime water
(g) The residue is (colour)
(h) The gas is and the residue is
(i) Write word equation for the above reaction.
(j) Write symbol equation for the above reaction.
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Activity 12.4
METALS AND EXTRACTION
Aim: To determine the conditions for rusting
Apparatus:Boiling tubesTest tube rack
Materials:Iron nailsBoiled water
Cooking oilTap water
Procedure:1. Prepare four boiling tubes in a rack, labelled them as A, B, C and D.
2. Into each boiling tube place a clean iron nail.
3. Pour water from the tap into boiling tube A until the nail is fully submerged.
4. Pour some hot water into boiling tube B until the nail is fully submerged and pour a layer of
cooking oil to cover the surface of the water.
5. Place a little anhydrous cobalt chloride into boiling tube C and cork the mouth of the boiling
tube with a rubber bung.
6. Pour some cooking oil into boiling tube D until the nail is fully submerged.
7. Leave the four boiling tubes in the rack for a few days and then observe.
Results:(a) Does the tap water in boiling tube A contain air? Why?
(b) Does the water in boiling tube B contain air? Why?
(c) Does the air in the boiling tube C contain water? Why?
(d) Does boiling tube D contain any air or water?
(e) Which iron nail becomes rusty?
(f) Why does the iron nail become rusty?
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Activity 12.5
METALS AND EXTRACTION
Aim: To show sacrificial protection of metal.Apparatus:3 Petri dishesCotton wool
Materials:Salt solutionIron nailsMagnesium ribbonCopper foil
Procedure:1. Fill the three Petri dishes with some salt solution and then make a cushion of cotton wool and
place it in each Petri dish so that it is soaked in the salt solution.
2. Label the Petri dishes as A, B, and C.
3. In Petri dish A, place a clean iron nail on the cushion of cotton wool. In Petri dish B, place a
clean iron nail wound with magnesium ribbon and in Petri dish C, place a clean iron nail wound
with copper strip.
4. Leave the three Petri dishes for a few days and then observe.
Copper foil
cotton wool soakedin salt solution
Magnesium ribbon
A B C
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Results:1. What happen to the iron nail in A?
...
2. Which iron nail shows no rusting? Why?
3. What is the difference between iron nail in A from that in C?
4. Explain your observation in 3.
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Activity 12.6
METALS AND EXTRACTION
Aim: To reduce lead(II) oxide by carbon.
Apparatus:Bunsen burnerBlow pipe
Materials:Lead(II) oxideCarbon block
Procedure:
1. Wet the middle of carbon block using tap water.2. Place a little amount of lead(II) oxide on a carbon block.3. Heat and blow air using blow pipe over the oxide.4. Observe any changes on the carbon block.
Observations:
...
...
lead(II) oxidecarbon block
blow pipe
Bunsen burner
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Activity 13.1
THE PERIODIC TABLE
Aim: To show reactivity of Group I metals with water.Apparatus:BeakerScalpel
Pair of forcepsWhite tile
Materials:LithiumPotassiumSodium
Litmus paperPhenolphthalein
Procedure:
1. Put a few drops of phenolphthalein in a 250 3cm beaker containing water.
2. Cut a very small piece of lithium and drop it in water, and observe.
3. Repeat the above experiment with the following metals: sodium and potassium.
4. Record your observations in the table.
Results:
Metal ObservationsEffect of solution on
red litmus paper
Effect onphenolphthalein
indicator
Lithium
Sodium
Potassium
Lumps of lithiumor sodium orpotassium
White tile
Lithium or sodiumor potassium
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Questions:
1. Place the three metals in the order of decreasing reactivity.
Most reactive Least reactive
, ,
From the results, it shows that when a metal reacts with water, the solution formed is
. The compound formed is an .
The gas given off in the reaction is
2. Write a balanced chemical equation for the reaction between lithium and water.
3. Write a balanced chemical equation for the reaction between sodium and water.
4. Write a balanced chemical equation for the reaction between potassium and water.
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Activity 14.1
ENERGY FROM CHEMICALS
Aim: To find H using 0.1 3dmmol HCl and 0.1 3dmmol NaOH solutions.
Apparatus:
Two 100 3cm measuring cylinders
250 3cm beakers
ThermometerPlastic cup
Materials:
0.1 3dmmol HCl solution Q
0.1 3dmmol NaOH solution P
Procedure:In this question you are required to determine the heat of neutralisation between a strong acid HY
and a strong alkali MOH.
You are provided with the following.
(a) Solution P is 0.1 3dmmol alkali MOH.
(b) Solution Q is 0.1 3dmmol acid HY.
1. Using a measuring cylinder measure 100 cm3 ofQ into a plastic cup and then measure the
temperature.
2. Using another measuring cylinder measure 100 cm3 ofP into a 250 cm3 beaker and similarly
measure the temperature.
3. Record the temperature of the two solutions and calculate the mean temperature.
4. Slowly pour the solution Q into the beaker containing solution P.
5. Stir the mixture with the thermometer and record the maximum temperature reached.
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Results:
Initial temperature of the acid Q = ...... )a(
Initial temperature of the alkali P = .. )b(
Mean initial temperature [ 2)ba( ] = .. )c(
Maximum final temperature of mixture = .. )d(
Temperature increase [d c] = .. )e(
(Assume that the density of HCl and NaOH is 1 3cmg )
Questions:1. Write an equation to show the neutralisation between P and Q.
2. Write an ionic equation for the above reaction.
3. Ignoring the heat lost to the plastic container and the beaker, calculate the heat given out by
the reaction. (The specific heat of solution is 4.2 gJ C).
[Hint: Use the formula H = m x c x ]
4. Calculate the number of mole of the acid HY or the alkali MOH involved in the reaction.
5. Calculate the heat of neutralisation, H, between MOH and HY.
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Activity 14.2
ENERGY FROM CHEMICALS
Aim: To investigate heat of solution of salts.
Apparatus:Plastic cupThermometerSpatula
Materials:Sodium hydroxide
Ammonium chloride
Procedure:
1. Measure out 50 cm3 of water in a measuring cylinder and pour it into a plastic cup.
2. Measure the initial temperature of the water.
3. Add a spatula full of solid sodium hydroxide into the water in the cup.
4. Stir to dissolve the solid.
5. Record the highest temperature obtained.
6. Repeat step 1- 4 with ammonium chloride and for step 5 record the lowest temperature
obtained.
[Repeat with other salts; nitrates, sulphates, carbonates etc.]
Result:
ReactionInitial
temperature/ CFinal
temperature/ CChange in
temperature/ C
Exothermicor
Endothermic
Sodium hydroxide +water
Ammonium chloride +water
Conclusion:
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Activity 14.3
ENERGY FROM CHEMICALS
Aim: To set up Daniel cell.
Apparatus:BeakerVoltmeter
Materials:Copper plateZinc plate
1.0 3dmmol zinc sulphate solution
1.0 3dmmol copper(II) sulphate solution
VoltmeterConnecting wires
Procedure:1. Set up copper metal as the positive terminal and zinc metal as the negative terminal.
2. Immerse the zinc metal in zinc sulphate solution and the copper metal in copper(II) sulphate
solution.
3. Connect the two solutions using a salt bridge as shown.
Or connect the two solutions using a porous pot as shown below.
Results:
The electrode potential of Daniel cell is . V
salt bridge
zinc platecopper plate
zinc sulphatesolution
copper(II) sulphatesolution
copper platezinc plate
zinc sulphatesolution
copper(II) sulphatesolution
porous pot copper can
copper(II)sulphate solution
zinc sulpha esolution
porous pot
voltmeter
zinc
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Activity 15.1
ELECTROLYSIS
Aim: To demonstrate electrolysis of molten lead(II) bromide.
Apparatus:CrucibleSpatulaGraphite electrodesPower pack
Crocodile clipsTripod standClay pipe triangleBunsen burner
Materials:
Lead(II) bromide
Procedure:1. A crucible is half filled with lead(II) bromide solid.
2. The solid lead(II) bromide is heated until it melts to a molten state.
3. Two carbon electrodes are dipped in the molten lead(II) bromide and are then connected to
power pack using crocodile clips.
4. Electric current is allowed to flow through for 15 minutes and the changes that occur at the
cathode and anode are recorded.
Results:
Observations Inference
At the anode
At the cathode
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Activity 15.2
ELECTROLYSIS
Aim: To demonstrate electrolysis of dilute sodium chloride solution.
Apparatus:Power packCarbon electrodesCrocodile clips
100 3cm beaker
Materials:
Aqueous 0.5 3dmmol sodium chloride solution
Procedure:
1. Aqueous sodium chloride is put into a beaker2. Insert two carbon electrodes into the aqueous sodium chloride and connect them to the power
pack.
3. The switch is turned on and electric current is allowed to flow for 15 minutes and observe.
4. Collect the gas and test.
5. Record your observations in the table.
Results:
Electrolyte Observations Test for the gas
At the cathode: Splint test
Dilute sodiumchloride solution At the anode: Splint test
aqueous sodium chloridecarbon electrodes
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Activity 15.3
ELECTROLYSIS
Title: To Demonstrate electrolysis of concentrated sodium chloride solution.
Apparatus:Power packCarbon electrodesCrocodile clips
100 3cm beaker
Materials:
Concentrated sodium chloride solution (1 3dmmol )
Procedure:
1. Concentrated sodium chloride is put into a beaker.
2. Insert two carbon electrodes into the concentrated sodium chloride solution and connect them
to the power pack.
3. The switch is turned on and electric current is allowed to flow for 15 minutes and observe.
4. Collect the gas and test.
5. Record your observations in the table.
Results:
Electrolyte Observations Test for the gas
At the cathode: Splint test
concentrated sodiumchloride solution At the anode: Litmus test
concentrated sodiumchloride solution
carbon electrodes
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Activity 15.4
ELECTROLYSIS
Aim: To demonstrate electrolysis of copper(II) sulphate using carbon electrodes.
Apparatus:Power packCarbon electrodesCrocodile clips
100 3cm beaker
Materials:
Aqueous 0.5 3dmmol copper(II) sulphate solution
Procedure:
1. Copper(II) sulphate solution is put into a beaker.2. Insert two carbon electrodes into the copper(II) sulphate solution and connect them to the
power pack.
3. The switch is turned on and electric current is allowed to flow for 15 minutes and observe.
4. Record your observations in the table.
Results:
Electrolyte Observations
At the cathode:
Copper(II) sulphatesolution At the anode:
Questions:1. What would you expect the colour of the copper(II) sulphate solution to be if the electrolysis is
carried out for a long period? Why?
2. Describe a test for the product formed at the anode.
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Activity 15.5
ELECTROLYSIS
Aim: To demonstrate electrolysis of copper(II) sulphate using copper electrodes.
Apparatus:Power packCopper electrodesCrocodile clips
100 3cm beaker
Materials:
Aqueous 1.0 3dmmol copper(II) sulphate solution
Procedure:1. Copper(II) sulphate solution is put into a beaker.
2. Insert copper electrodes into the copper(II) sulphate solution and connect them to the power
pack.
3. The switch is turned on and electric current is allowed to flow for 15 minutes and observe.
4. Record your observations in the table.
Results:
Electrode Observations
At the cathode:
Copper(II) sulphatesolution At the anode:
Questions:1. What would you expect the colour of the copper(II) sulphate solution to be if the electrolysis is
carried out for a long period? Why?
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Activity 15.6
ELECTROLYSIS
Aim: To demonstrate electroplating of spatula with copper.
Apparatus:Power pack
Beaker 250 3cmCrocodile clips
1.0 3dmmol copper(II) sulphate
Copper plateMetal spatula
Materials:
1.0 3dmmol copper(II) sulphate
Procedure:
1. Pour about 200 3cm of 1.0 3dmmol copper(II) sulphate solution into a beaker.
2. A piece of copper plate is connected to the positive terminal. This plate act as the anode.
3. The metal spatula is connected to the negative terminal. This metal spatula acts as the
cathode.
4. Immerse both the metal spatula and the copper plate in the copper(II) sulphate solution. (Make
sure that they do not come into contact)
5. The solution is electrolysed for 30 minutes using a small current (0.5A ).
Results:
Observations Half-equations
At the cathode: At the cathode:
At the anode: At the anode:
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Activity 16.1
SPEED OF REACTIONS
Aim: To show the effect of concentration on the speed of reaction.
Apparatus:BeakerStop-watch
Filter paper marked XMeasuring cylinders
Materials:
2.0 3dmmol hydrochloric acid
0.25 3dmmol sodium thiosulphate, 322 OSNa solution
Distilled water
Procedure
1. Measure 5 3cm of sodium thiosulphate solution into a 250 3cm beaker and add 45 3cm of
distilled water.
2. Place the beaker over the filter paper marked X.
3. By using a separate measuring cylinder, add 10 3cm of 2.0 3dmmol HCl and at once start the
stop-watch.
4. Swirl the beaker a few times and then put the beaker back on the paper over the mark X.
5. Observe the mark X from above through the solution mixture in the beaker.
6. As more precipitate is formed the mark X will eventually disappears from sight.
7. Stop the stop-watch when the mark X just disappears from sight. Record the time taken in the
table below.
8. Repeat the experiment by changing the volume of sodium thiosulphate and distilled water.
9. Record the time taken in the table provided.
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Results:
Volume of sodiumthiosulphate solution,
3cm
Volume of distilledwater
3cm
Volume ofhydrochloric acid
3cm
Reaction times
5
10
15
20
25
Draw the graph of volume of sodium thiosulphate in 3cm against time in seconds.
Conclusion:As the concentration of sodium thiosulphate increases ..
...
...
...
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Activity 16.2
SPEED OF REACTIONS
Aim: To show the effect of temperature on the speed of reaction.
Apparatus:BeakerStop-watchFilter paper marked X
Measuring cylinderThermometer
Materials:
2.0 3dmmol hydrochloric acid
Distilled water
0.25 3dmmol sodium thiosulphate, 322 OSNa solution
Procedure:
1. Measure 20 3cm of sodium thiosulphate solution into a beaker and add 60 3cm of distilled
water. Record the temperature of the solution mixture.
2. Place the beaker over the filter paper marked X.
3. Add 20 3cm of 2.0 3dmmol HCl and at once start the stop-watch.
4. Swirl the beaker a few times and put the beaker back on the filter paper over the mark X.
5. Observe the mark X through the solution mixture.
6. Stop the stop-watch when the mark X just disappears from sight. Record the time taken in the
table provided.
7. Repeat the experiment at different temperatures by heating the mixtures of 20 3cm of sodium
thiosulphate and 60 3cm of distilled water to 40C, 50C, 60C and 70C.
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Results:
Temperature Reaction time in seconds Rate ( t1 )
Room temperature
40C
50C
60C
70C
Draw the graph of rate against temperature.
Conclusion:As the temperature increases ..
...
...
...
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Activity 16.3
SPEED OF REACTIONS
Aim: To show the effect of particle size using calcium carbonate (lump and powder) with
hydrochloric acid.
Apparatus:Conical flask connected to gas syringeStop-clockElectronic balance
Measuring cylinder 50 3cm
Materials:
Hydrochloric acid 0.25 3dmmol
Calcium carbonate (powder and lump forms)
Procedure:1. Use an electronic balance to weigh exactly 0.5 g of marble chips and put them in a conical
flask connected to a gas syringe.
2. Use a measuring cylinder to measure exactly 30.0 3cm of 0.25 3dmmol hydrochloric acid and
pour into the conical flask containing the marble chips.
3. Immediately cork the conical flask to the gas syringe and at the same time start the stop-clock.
4. Read the volume of the carbon dioxide collected in the gas syringe for every 10 seconds until
the reaction stops.
5. Create your own table to tabulate the readings.
6. Repeat the above experiment by using marble chips of (a) smaller size and (b) powdered
calcium carbonate.
7. Draw on the same graph paper the volume of carbon dioxide gas against time for the three
experiments.
Result:
Conclusion:As the particle size increases ..
...
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Activity 16.4
SPEED OF REACTIONS
Aim: To show the decomposition of hydrogen peroxide using manganese(IV) oxide.
Apparatus:
50 3cm measuring cylinderClockSpatulaConical flaskGas syringe
Delivery tubeRubber bungRubber tubing connectorRetort stand and clamp
Materials:
0.2 3dmmol or 2 volume hydrogen peroxide (20 volume diluted 10 x)
Powdered manganese(IV) oxide
Procedure:1. Set up the apparatus shown in the diagram.
2. Measure 50 3cm of hydrogen peroxide solution in the conical flask.
3. Add a little amount of manganese (IV) oxide into the hydrogen peroxide solution.
4. Immediately cork rubber bung to the conical flask and start timing.
5. Gently swirl the flask while recording the volume of gas collected in the gas syringe every
minute. Do this for 10 minutes or until the gas syringe is full. Take care not to undo the rubber
tube connector.
6. Record your results in table provided.
hydrogen peroxidesolution
manganese(IV) oxide
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Results:
Time/min 0 1 2 3 4 5 6 7 8 9 10
Volumeof gas/cm3
Plot a graph of volume of gas evolved (vertical axis) against time.
Conclusion:
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Activity 17.1
REVERSIBLE REACTIONS
Aim: To show reversible reactions.
Apparatus:Test tubes with rack
Materials:Potassium chromate(VI) solution
Aqueous sodium hydroxideAqueous copper (II) sulphateConcentrated hydrochloric acidConcentrated ammonium hydroxideDilute sulphuric acid
Procedure:1. (a) Pour potassium chromate(VI) solution in a test-tube until it is about one-fifth full and
slowly adds dilute sulphuric acid until a change is seen.
Observation:
Write ionic equation for the reaction in (a).
(b) To the mixture from (a) slowly add dilute sodium hydroxide solution and observe the
change.
Observation:
..
..
Explain in terms of reversibility the observation in the experiment (b).
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2. (a) Pour copper (II) sulphate solution into a test-tube until it is about one-fifth full and slowly
add concentrated hydrochloric acid until a change is seen.
Observation:
..
..
Write the ionic equation for the reaction in (a).
..
(b) To the mixture from (a) add concentrated ammonia solution a little at a time until a change
is seen.
Observation:
3. State Le Chateliers principle.
......
......................................................................................................................................................
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Activity 17.2
REVERSIBLE REACTIONS
Aim: To prepare fertilizer using nitric acid (The manufacture of fertilizer from ammonia).
Apparatus:BurettePipettePipette filler2 conical flasksRetort stand
Evaporating dishBunsen burnerTripod stand and wire gauzeWhite tile
Materials:Dilute nitric acid
Aqueous ammonium hydroxide
Methyl orange indicator
Procedure:1. Place nitric acid in burette.
2. Pipette 25.0 cm3 of aqueous ammonium hydroxide into a conical flask. Add a few drops of the
indicator.
3. Titrate the acid with the alkali until neutralise.
4. Repeat titration, this time without the indicator.
5. Heat the mixture (ammonium nitrate solution) until it is saturated.
6. Transfer some mixture into an evaporating dish and leave to crystallise.
Conclusion:
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Activity 18.1
REDOX
Aim: To show the colour change in oxidizing agents - acidified potassium manganate(VII) and
acidified potassium dichromate(VI) solution.
Apparatus:Measuring cylinderBeakerConical flask
Test-tubeBurette
Material:Potassium manganate(VII) solutionPotassium dichromate(VI) solution
Dilute sulphuric acidSodium sulphite solution
Procedure:
1. Measure 20 3cm of potassium manganate(VII) solution into a conical flask and add about 5
3cm of dilute sulphuric acid.
2. From the burette, slowly add sodium sulphite solution (Na2SO3) into the conical flask until the
purple colour of potassium manganate(VII) disappears.
3. Repeat the experiment above using potassium dichromate(VI) solution.
Observations:
(a) Potassium manganate (VII) solution is (colour) due to the presence of
ions.
(b) As sodium sulphite solution is added, the colour changes to (colour) due to
the formation of ion.
(c) Potassium dichromate(VI) solution is (colour) due to the presence of
ions.
(d) As sodium sulphite solution is added the colour changes to (colour) due tothe formation of ion.
Conclusion:Potassium manganate(VII) and potassium dichromate(VI) are oxidizing agents. They are
by the reducing agent, sodium sulphite.
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Activity 18.2
REDOX
Aim: To show the colour change of iodide ion in redox reaction.
Apparatus:Boiling tubeTest tube
Materials:Hydrogen peroxide 20-volume,
1.0 3dmmol potassium iodide solution
Starch solution
Procedure:1. Pour about 5 3cm of potassium iodide solution into a boiling tube and slowly add equal volume
of 20-volume hydrogen peroxide, and observe.
2. Leave the mixture for a few minutes and observe for the formation of any solid substance.
3. Transfer some solution from the boiling tube into a test tube and add a few drops of starch
solution.
Results:(a) Potassium iodide solution changed from . (colour) to
. (colour) when added with hydrogen peroxide.
(b) When left to stand for a few minutes a . (colour) solid substance was
seen at the bottom of the boiling tube.
(c) When starch was added, the solution turned . (colour) showing that
. was formed.
Questions:1. Write an ionic equation to show oxidation of iodide ion.
2. Write an ionic equation for the reduction of hydrogen peroxide.
3. Write ionic equation to show redox reaction between potassium iodide and hydrogen peroxide.
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Activity 19.2
ATMOSPHERE AND ENVIRONMENT
Aim: To demonstrate water treatment using alum (Potassium aluminium sulphate).
Apparatus:
500 3cm beakersSpatula
Materials:Sample of muddy water
Alum
Procedure:1. Fill two beakers with muddy water until three quarter full.
2. Add a spoonful of alum in one but not the other.
3. Leave the two beakers for about 10 minutes and compare the appearance of the water in the
two beakers.
Observations:
...
...
muddy water
alum
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Activity 20.1
ORGANIC CHEMISTRY
Aim: To show incomplete combustion of hydrocarbon.
Apparatus:Bunsen burnerWooden splint
Evaporating dish
Materials:BenzeneTolueneKerosene
Procedure:
1. Place a little of each hydrocarbon into an evaporating dish.
2. Burn the hydrocarbon with a lighted wooden splint and observe for the products. (Note:
Burning should be carried out outside the lab as its burning will produce dense smoke and
carbon monoxide).
3. Observe the colour of the flame and record it in the table below
Results:
Hydrocarbon Formula Mr % of carbon Colour of the flame
Benzene 66HC
Toluene 356 CHHC
Kerosene 3215HC
Lightedwooden splint
Evaporating dish
Benzene
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Questions:1. Do you think these hydrocarbons make good fuel? Explain.
2. Which of the three hydrocarbons produces the least smoke? Relate your observations in terms
of percentage of carbon in the compound.
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Activity 20.3
ORGANIC CHEMISTRY
Aim: To test for alkenes with bromine
Apparatus:Test tube
Materials:Liquid bromineHexene
Procedure:
1. Add about 2 cm 3 of liquid bromine in a test tube.
2. Then, add about 2 cm 3 of hexene to the liquid bromine.
3. Shake the mixture gently.
4. Observe the colour changes that take place in the test tube.
Results:
1. The brown colour of liquid bromine is ...
2. State the molecular formula of hexene: .
3. Write the equation for the addition of bromine to hexene.
4. Name the product of addition of bromine to hexene.
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Activity 20.4
ORGANIC CHEMISTRY
Aim: To compare the flammability and the colour of the flame produced by different alcohols and
to show the variation of physical properties of the first four alcohols.
Apparatus:Evaporating dishesWooden splint
Bunsen burner
Materials:MethanolEthanolPropanol
ButanolCobalt(II) chloride paper
Procedure:1. Pour a little of each of the following alcohols (methanol, ethanol, propanol and butanol) into
four different evaporating dishes.
2. Burn the alcohols with the lighted wooden splint.
3. Compare the colour of the flame and the ease of it burning.
4. Observe what is left on the evaporating dishes. Test it with blue cobalt(II) chloride paper.
Lightedwooden splint
Evaporating dish
Methanol
Lightedwooden splint
Evaporating dish
Ethanol
Lightedwooden splint
Evaporating dish
Propanol
Lightedwooden splint
Evaporating dish
Butanol
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Questions:
1. Note the differences of the colour of the flames from the burning of methanol to butanol.
Explain this variation.
2. Which alcohol is the most flammable?
3. Work out the molecular masses of the four alcohols.
Alcohol Molecular mass
Methanol
Ethanol
Propanol
Butanol
4. How is the flammability of the alcohols related to their molecular masses?
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Activity 20.5
ORGANIC CHEMISTRY
Aim: To compare fluidity of the alcohols.
Apparatus:Test tubes with rack
Materials:MethanolEthanol
PropanolButanol
Procedure:1. Half fill the four test tubes with four different alcohols and compare their fluidity.
2. Place the order of fluidity among the four alcohols.
Results:
most fluid least fluid1 2 3 4
Questions:
As the molecular mass increases the alcohols become . fluid.
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Activity 20.6
ORGANIC CHEMISTRY
Aim: To show oxidation of ethanol to ethanoic acid.
Apparatus:Bunsen burnerBoiling tubeTest tube
Retort stand with clampBeakerDelivery tube
Materials:EthanolPotassium dichromate(VI) solutionDilute sulphuric acid
Cold waterBlue litmus paper
Procedure:
1. The boiling tube is filled with approximately 5 3cm of potassium dichromate(VI) solution.
2. About 5 3cm of dilute sulphuric acid is added to the potassium dichromate(VI) solution.
3. About 5 3cm of ethanol is added to the acidified potassium dichromate(VI) solution.
4. A rubber stopper fitted with a delivery tube is inserted into the boiling tube. The delivery tube is
inserted into a test tube placed in a beaker half-filled with cold water.
5. The mixture of ethanol and acidified potassium dichromate(VI) is boiled slowly. The distillate is
collected in the test tube.6. Observe the colour change of acidified potassium dichromate(VI) to show that oxidation of
ethanol to ethanoic acid has taken place.
7. The colour and the odour of the distillate are recorded.
8. The distillate is tested with a piece of blue litmus paper.
Test tube
Distillate
Cold water
Boiling tube
Mixture of ethanol andacidified potassiumdichromate(VI)
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Results:
Test on the distillate Observations
Colour
Smell
Action on blue litmus paper
Questions:
1. When ethanol is boiled with acidified potassium dichromate(VI) solution, it is oxidised to
ethanoic acid which has the smell of ..
2. The colour of acidified potassium dichromate changes from . to
..
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Activity 20.7
ORGANIC CHEMISTRY
Aim: To show acidic properties of carboxylic acid.
Apparatus:Evaporating dishTripod standBunsen burnerSpatula
Wooden splintsTest tubesGlass rodDelivery tube
Materials:Ethanoic acid
Aqueous sodium hydroxideSodium carbonate powder
Magnesium ribbonLimewaterRed litmus paper
Procedure:
(a) Reaction of ethanoic acid with sodium hydroxide
1. About 10 3cm of ethanoic acid is poured into an evaporating dish.
2. Drop a piece of red litmus paper into the evaporating dish to act as indicator.
3. Slowly add sodium hydroxide solution to the ethanoic acid until the red litmus paper just turns
blue.
4. Remove the litmus paper and heat the solution mixture until dryness.
Observations:
Describe the product left behind the evaporating dish after the solution mixture is evaporated to
dryness.
...
.............................................................................................................................................................
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(b) Reaction between ethanoic acid with magnesium ribbon
1. The test tube is filled with about 5 3cm of ethanoic acid.
2. A piece of magnesium ribbon (about 3 cm long) is added to ethanoic acid.
3. Test the gas given off with the lighted wooden splint.
Observations:
...
(c) Reaction between ethanoic acid with sodium carbonate
1. About 5 3cm of ethanoic acid is added to a test tube.
2. A spatula of sodium carbonate powder is added to the ethanoic acid.3. The gas released is passed into limewater.
Observations:
...
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1. T.Y. Toon, L.W. Leng & T.O Tin. Success Chemistry SPM. Selangor Darul Ehsan: Oxford
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4. C.N. Prescott. Chemistry A Course for O Level. Practical Workbook. Volume 2. Singapore:
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5. L.J. Rasanayagam. Practical Chemistry. A course for O Level. Volume 1. Singapore: Federal
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6. L.J. Rasanayagam. Practical Chemistry. A course for O Level. Volume 2. Singapore: Federal
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8. J.G.R. Briggs. Chemistry O Level Practical. Volume 2 (2nd Ed.). Singapore: Pearson
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9. T.Y. Toon & C.L. Kwong. Chemistry Matters for GCE O Level. Practical Workbook.
Singapore: Times Media Private Limited, 2002.
10. L.J. Rasanayagam & R.M. Kok. GCE O Level Chemistry Matters. Practical Book. Singapore:
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11. R.M. Heyworth & J.G.R. Briggs. Chemistry Insights O Level (2nd Ed.) Practical Workbook.
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