CHEMISTRY 13th EDITION LABORATORY MANUAL

CHEMISTRY 2
SK025

Chemistry Lab Manual – SK025

EXPERIMENT 1: RATE OF REACTION

Objectives

At the end of this lesson, students should be able to study the effect of
concentration, temperature, and catalyst on the reaction rate.

Introduction

The reaction rate is the change in concentration of the reactants or products
per unit time. The factors that influence the rate of reaction are
temperature, pressure, catalyst, size of particles and concentration of
reactants.

The rate of a reaction can be studied by observing the change in the
chemical or physical properties of species involved in the reaction. The
reaction rate is inversely proportional to the time of the reaction, i.e., the
faster the reaction occurs, the shorter is the time for the reaction to
complete.

Apparatus Chemical Reagents

Glass rod 0.1 M HCl
Water bath 10% MnSO4
Stopwatch 2.0 M H2SO4
Boiling tube 0.02 M KMnO4
Thermometer 0.2 M Na2S2O3
10 mL pipette 0.25 M H2C2O4
50 mL burette
10 mL measuring cylinder
100 mL conical flask
Laminated white paper with ‘X’ mark

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Procedure

(A) The effect of concentration on the reaction rate

1. Place 50 mL of 0.2 M sodium thiosulphate, Na2S2O3using a

burette into a 100 mL conical flask. Put the conical flask on the
white paper with ‘X’ mark.

2. Pipette 10 mL of 0.1 M HCl into the conical flask and
immediately start the stopwatch. Stir continuously with a glass
rod until the mark is no longer visible and record the time.

Note: The ‘X’ mark should be observed from the top of the
conical flask.

3. Repeat steps 1 till 2 with the addition of distilled water to the
sodium thiosulphate as instructed in Table 1.1.

Table 1.1
Concentration of reactant

Volume of Volume of Concentration Volume of Time 1
0.2 M Na2S2O3 distilled of Na2S2O3 0.1 M HCI (s)
solution (mL) (M) (s-1)
water solution
50.00 (mL) (mL)

0.00 10.00

40.00 10.00 10.00

30.00 20.00 10.00

20.00 30.00 10.00

10.00 40.00 10.00

4. Calculate the concentration of the sodium thiosulphate solution
after the dilution and the value of 1 .

5. Plot a graph of 1 against the concentration of sodium


thiosulphate solution.

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7. Based on the graph, state the relationship between the
concentration of the sodium thiosulphate solution with time
and the rate of reaction.

(B) The effect of temperature and catalyst on the reaction rate

1. Label 4 boiling tubes as A1, A2, B1 and B2.

2. Place 10 mL of 0.25 M oxalic acid, H2C2O4 solution into boiling
tubes A1 and A2.

3. Fill boiling tubes B1 and B2 with 5 mL of 0.02 M KMnO4
solution. Then add 10 mL of 2.0 M H2SO4 solution to both tubes.

4. Add 5 drops of 10% MnSO4 solution to B2. Stir the mixture.

5. Place tubes A1 and B1 in a water bath at temperature of 30°C for
about 3 minutes.

6. While tube A1 is still in the water bath, pour the solutions from
tube B1 into tube A1. Start the stopwatch immediately.

7. Record the time taken for the mixture to turn colourless.

8. Repeat Steps 5 till 7 for tubes A2 and B2.

9. Follow Steps 2 till 7 for the temperatures of 35°C, 40°C and
50°C. Record yourresults in Table 1.2.

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Table 1.2
Effect of temperature and catalyst on reaction rate

Temperature Without catalyst MnSO4 With catalyst MnSO4
(°C) (A1 + B1) (A2 + B2)

30 t (s) 1 (s-1) t (s) 1 (s-1)
35
40
50

10. Plot 1 against the temperature for the mixture of (A1 + B1) and


(A2 + B2) solutions on the same graph.

11. Based on the graph, deduce the relationship between:

i. temperature and rate of reaction;
ii. catalyst and rate of reaction.

POINT TO DISCUSS

1. What is the function of the catalyst in the above reactions?

2. What does 1 represent?


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Chemistry Lab Manual – SK025
EXPERIMENT 2: DETERMINING THE HEAT OF REACTION

Objectives

At the end of this lesson, students should be able to:
i. determine the heat capacity of a calorimeter; and
ii. determine the heat of neutralisation of HCl and NaOH.

Introduction

Heat released or absorbed during chemical reactions can be measured by
using a calorimeter. A calorimeter is a container that is thermally isolated
from the environment. Heat released by the chemical reaction, −q is absorbed
by the solution and the calorimeter.

−qrxn = qs + qc ….. (1)

where qs = heat absorbed by solution
qc = heat absorbed by calorimeter

The heat absorbed by a calorimeter is proportional to the change in
temperature. The proportionality constant, C, is known as the heat capacity
of a calorimeter. Heat capacity is defined as the amount of heat required to
increase the temperature of the calorimeter by 1°C.

qc = C∆T ….. (2)

For a solution, the heat absorbed is proportional to the mass of the
solution and the change in temperature. The constant, c, is known as the
specific heat capacity of solution per unit mass. The specific heat capacity
of a very dilute solution is equivalent to the specific heat capacity of
pure water, 4.18 J g−1 °C−1. The mass of the solution can be calculated by
assuming the density of the solution is the same as the density of water.

qs = mscs∆T ….. (3)

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Heat released can be determined by measuring the temperature before and
after the reaction:

−qrxn = CT + mscsT ….. (4)

where ∆T = final temperature of system – initial

temperature of system mass of solution
heat capacity of calorimeter
ms = specific heat capacity of solution

Cc =

cs =

Apparatus Chemical Reagents

25 mL pipette 1.0 M HCl
100 mL beaker 1.0 M NaOH
Thermometer
Calorimeter or styrofoam cup

Procedure
(A) Determination of the heat capacity of a calorimeter

1. Set up a simple calorimeter as shown in Figure 2.1.

Figure 2.1
A simple calorimeter (Chang, 2005)

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2. Measure the temperature, T1, of an empty calorimeter.

3. Pipette 50 mL of distilled water into a 100 mL beaker.

4. Heat the beaker to a temperature between 50 − 60°C.

5. Pour the hot water into the calorimeter. Close the lid
immediately and measure the initial temperature of the hot
water, T2.

6. Observe the decrease in temperature every 10 seconds for 2
minutes. Record the temperature that remains constant, T3.

7. Determine the heat capacity of the calorimeter.

(B) Determination of the heat of neutralisation of 1.0 M HCl and 1.0 M
NaOH

1. Pipette 25 mL of 1.0 M NaOH solution into the calorimeter
and 25 mL of 1.0 M HCl solution into a beaker. Record the
initial temperature of each solution.

2. Without removing the thermometer, lift the lid slightly and
quickly pour the HClsolution into the calorimeter.

3. Quickly replace the lid of the calorimeter.

4. Stir the solution and record the maximum temperature reached.

5. Calculate the heat of neutralisation.

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DATA SHEET

EXPERIMENT 2: DETERMINING THE HEAT OF REACTION

RESULTS

(A) Determination of the heat capacity of a calorimeter

i. Temperature of calorimeter, T1 = ________ °C

ii. Initial temperature of the hot water used, T2 = ________ °C

Time
Interval (s) 10 20 30 40 50 60 70 80 90 100 110 120

Temperature
(°C)

iii. Constant temperature of water, T3 = ________ °C
iv. Mass of water (assume ρwater = 1.0 g/mL) = ________ g

(B) Determination of the heat of neutralisation of 1.0 M HCl and 1.0 M
NaOH

Initial temperature of HCl (°C) =
Initial temperature of NaOH (°C) =
Average initial temperature (°C) =
Maximum temperature (°C) =
T =

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Chemistry Lab Manual – SK025
EXPERIMENT 3: ELECTROCHEMICAL CELLS

Objectives

At the end of this lesson, students should be able to:
i. arrange Al, Zn, Mg, Fe and Cu in an electrochemical series; and
ii. determine the Faraday’s constant by electrolysis of CuSO4 solution.

Introduction

Electrochemistry is a study of the relationship between electricity and
chemistry. Generally, there are two types of electrochemical cells, namely
galvanic and electrolytic cells. A galvanic cell is an electrochemical cell in
which redox reaction occurs spontaneously to generate electricity. For a
galvanic cell, oxidation occurs at the anode and electrons flow to the
cathode where reduction occurs.

A standard reduction potential is defined as a reduction potential obtained
at a standard condition where the concentration of solution is 1.0 M, the
gas partial pressure is 1 atm and temperature is 25°C. The standard
reduction potential values are arranged in a certain order and the list is
known as the Standard Reduction Potential Table or the emf Series.

The potential difference between the two half cells in an electrochemical
cell is called cell potential. The cell potential or the cell voltage at the
standard condition can be written as:

E°cell = E°cathode − E°anode

The cell potential at non-standard condition can be calculated by using the
Nernst equation.

Ecell = E°cell − 0.0592 log Q


In this experiment, the cell potential is obtained from the voltmeter
reading. By inserting the value and the concentration of the electrolyte in
the Nernst equation, the standard cell potential, E°cell can be determined.

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An electrolytic cell uses electricity to produce chemical changes in an
electrolyte. The cell is made up of two electrodes connected to a battery
which functions as a source of direct current. During electrolysis, cations
are reduced at the cathode while anions are oxidised at the anode. The
amount of substance formed at each electrode can be predicted based on
Faraday’s first law.

Apparatus Chemical Reagents

Tons 0.1 M CuSO4
Ammeter 0.1 M ZnSO4
Hair dryer 0.1 M FeSO4
Voltmeter 0.1 M MgSO4
Stopwatch 0.1 M Al(NO3)3
Transformer Zinc strip
Sandpaper or abrasive cloth Copper strip
Crocodile clips Magnesium strip
50 mL beaker Aluminium strip
Analytical balance Carbon rod
Salt bridge Saturated KNO3 or KCl
50 mL measuring cylinder

Note:
1. Clean the electrodes with sandpaper or abrasive cloth before use.

2. Ensure that the filter paper to be used as salt bridge is completely soaked
insaturated KNO3 or KCl solution. Avoid handling the salt bridge with
bare hands.

Procedure

(A) Galvanic cell

1. Clean the metal strips with sandpaper or abrasive cloth.

2. Fill a 50 mL beaker with 35 mL of 0.1 M CuSO4 and the other
beaker with 35 mLof 0.1 M ZnSO4.

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3. Set up the apparatus as shown in Figure 3.1.

Zn Salt bridge Cu
ZnSO4 CuSO4

Figure 3.1
Galvanic cell

4. Record the cell potential.

5. Repeat Steps 1 till 4 by replacing Zn2+/Zn half cell with a

(a) magnesium strip in 0.1 M MgSO4
(b) aluminium strip in 0.1 M Al(NO3)3
(c) iron strip in 0.1 M FeSO4
6. Arrange the metals in ascending order of strength as reducing
agents.

7. Verify the above order by calculating the standard reduction
potential, E°reduction of each electrode.

(B) Determination of Faraday’s constant

1. Clean a copper electrode with a piece of sandpaper or abrasive
cloth.

2. Weigh the copper electrode accurately.

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3. Set up apparatus as show in Figure 3.2. Fill a 50 mL beaker
with 35 mL 0.1 MCuSO4.

+ DC

−

Carbon Copper
(anode) (cathode
)

0.1 M CuSO4

Figure 3.2
An electrolytic cell

4. Complete the circuit by connecting the wires from each
electrode to the ammeter and transformer. Set the transformer to
supply the direct current with a voltage of 3 V.

5. Run the electrolysis for 15 minutes.

6. Record the ammeter reading and your observation of each
electrode.

7. Disconnect the circuit and record the exact time of electrolysis.

8. Dry the copper strip using a hair dryer.

9. Weigh again the copper strip.

10. Calculate the mass of copper deposited. Determine the
Faraday’s constant.

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Chemistry Lab Manual – SK025
DATA SHEET

EXPERIMENT 3: ELECTROCHEMICAL CELLS

RESULTS Cell Potential, Ecell (V)
(A) Galvanic cell

Galvanic Cell

(B) Determination of Faraday’s number

Electrode Observation
Cathode
Anode

Final mass of Cu electrode (g) =
Initial mass of Cu electrode (g) =
Mass of Cu deposited (g) =
Moles of Cu (mol) =
Ammeter reading (A) =
Time (s) =
Quantity of charge, Q (C) =

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EXPERIMENT 4: REACTIONS OF ALIPHATIC AND AROMATIC
HYDROCARBONS

Objectives

At the end of this lesson, students should be able to:
i. study the chemical properties of an alkane, alkene and arene; and
ii. differentiate an alkane from an alkene and arene.

Introduction

Hydrocarbons are organic compounds that contain only carbon and
hydrogen. Alkanes which are also known as paraffins are saturated
hydrocarbons. They do not contain double or triple bonds. Hence, alkanes
are relatively inert to chemical reactions.

Example of alkanes:

H HH Cyclohexane

HCH HC CH

H HH

Methane Ethane

Alkanes undergo free radical substitution reaction.

+CH4 Br2 CH2Cl2 +CH3Br HBr
uv

Alkenes are unsaturated hydrocarbons with at least one double bond

between two carbonatoms.

Example of alkenes:

H2C CH2 Cyclohexene

Ethene

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Alkenes undergo electrophilic addition reactions at the C=C bond. For
example, alkenes undergo hydrogenation and halogenation to form alkanes
and dihalides, respectively.

+CH3CH CH2 Br2 CH2Cl2 +CH3CHCH3 HBr

Br

Alkenes also react with potassium permanganate solution in two different
conditions:

a) In basic medium to form a diol.

H2C CH2 KMnO4, OH- HH
cold, dilute HC C H

OH OH

b) In hot acidic medium to form a carboxylic acid.

H3C CH3 KMnO4, H+ O
C C Δ
2 CH3 C OH
H H

Arenes are aromatic hydrocarbons with stable molecular structures.
Example of aromatic hydrocarbons:

CH3

Toluene Naphthalene Anthracene

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Although arenes have a very high degree of unsaturation, they are
relatively inert towards alladdition reactions except at a very high pressure
and temperature.

+ H2 Ni
high pressure, 200°C

Arenes undergo electrophilic aromatic substitution reactions in the
presence of a Lewis acid catalyst.

+ Br2 FeBr3 Br

+ HBr

Apparatus Chemical Reagents

Dropper Toluene
Test tube Cyclohexane
Rubber band Cyclohexene
Labeling paper Dichloromethane
Test tube rack 0.01 M KMnO4
Black sugar paper (6 cm × 12 cm) 4% bromine in dichloromethane

Procedure

(A) Reaction with bromine in dichloromethane

1. Label 6 dry, clean test tubes, A to F.

2. Place 1 mL of cyclohexane in test tubes A and B, 1 mL of
cyclohexene in test tubes C and D, and 1 mL of toluene in test
tubes E and F.

3. Wrap test tubes A, C and E with black sugar papers.

4. Add 4 to 5 drops of 4% bromine in dichloromethane into each
test tube.

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5. Keep test tubes A, C and E in a dark place, and test tubes
B, D and F in the sunlight. Leave them for 15 minutes.

6. Record the observations.

(B) Oxidation with cold alkaline solution of KMnO4 (Baeyer’s Test)
1. Label dry, clean test tubes, G, H and I.
2. Place 1 mL each of cyclohexane, cyclohexene and toluene in
test tubes G, H and I, respectively.
3. Add a few drops of alkaline KMnO4 solution into each test tube
and shake.
4. Record the observations.

POINT TO DISCUSS
1. Write the mechanism for the reaction of cyclohexane with bromine.
2. State the function of sunlight in Part (B).

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DATA SHEET

EXPERIMENT 4: REACTIONS OF ALIPHATIC AND AROMATIC
HYDROCARBONS

RESULTS Bromine in dichloromethane Oxidation with
Test Under sunlight In the dark
alkaline KMnO4
Hydrocarbons (Baeyer’s test)

Cyclohexane

Cyclohexene

Toluene

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Chemistry Lab Manual – SK025
EXPERIMENT 5: REACTIONS OF HYDROXY COMPOUNDS

Objectives

At the end of this lesson, students should be able to:
i. identify classes of alcohols; and
ii. study the chemical properties of alcohols and phenol.

Introduction

Alcohols are organic compounds containing hydroxyl group, −OH, as the
functional group.Alcohols can be classified into:

H H R

R C OH R C OH R C OH

H R R

Primary Secondary Tertiary
alcohol (1o) alcohol (2o ) alcohol (3o)

Lucas reagent, a mixture of concentrated hydrochloric acid and anhydrous
zinc chloride, can be used to differentiate the three classes of alcohols.
Tertiary alcohols turn cloudy or appear in two layers almost immediately.
Secondary alcohols turn cloudy within 5 to 10 minutes whereas primary
alcohols do not show any changes.

Alcohol can be oxidised to aldehyde, ketone or carboxylic acid. The product
formed depends on the class of alcohol used. Various oxidizing agent such
as KMnO4, Na2Cr2O7 and H2CrO4 can be used.

Phenol, an example of aromatic alcohol can be distinguished from aliphatic
alcohol through reactions with FeCl3 solution or bromine water.

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Apparatus Chemistry Lab Manual – SK025

Stopper Chemical Reagents
Dropper
Test tube Ethanol
Stopwatch 1-Butanol
Water bath 2-Butanol
10 mL measuring cylinder Alcohol X
Lucas reagent
2-Methyl-2-propanol
Concentrated H2SO4
0.04 M Na2Cr2O7
Glacial acetic acid
Phenol
Bromine water

Procedure

(A) Lucas test

1. Place approximately 1 mL of 1-butanol, 2-butanol, 2-methyl-2-
propanol, and alcohol X in 4 separate test tubes.

2. Add 2 mL of Lucas reagent into the test tube.

3. Stopper and shake the test tube.

Note: If no change occurs within 10 minutes, place the test tube
in a water bath at 70°C – 80°C

4. Record the observation and the time taken for the reaction to
occur.

5. Deduce the class of alcohol X.

(B) Oxidation

1. Place 5 mL of 0.04 M Na2Cr2O7 solution in 4 separate test tube.

2. Add 2 to 3 drops of concentrated H2SO4 to the Na2Cr2O7
solution in the fume cupboard.

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3. Add 3 drops of 1-butanol, 2-butanol, 2-methyl-2-propanol, and
alcohol X to each of the mixture accordingly and heat in a water
bath at 70°C – 80°C.

4. Record the colour change.

(C) Confirmatory test for phenol
1. Place approximately 1.0 ml of phenol solution in a test tube.
2. Add bromine water dropwise until precipitate is formed.
3. Record the observation.
Note: Carry out this test in a fume cupboard.

POINTS TO DISCUSS
1. Explain the formation of the two layers in the Lucas test.
2. Write the equations for all reactions.

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DATA SHEET

EXPERIMENT 5: REACTIONS OF HYDROXY COMPOUNDS
RESULTS

Observation

Hydroxy (A) (B)
compound Lucas Test Oxidation with sodium

1-butanol dichromate

2-butanol

2-methyl-2-propanol
Unknown
(Alcohol X)

(C) Confirmatory test for phenol

Compound Observation
Phenol

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Chemistry Lab Manual – SK025
EXPERIMENT 6: ALDEHYDES AND KETONES

Objectives

At the end of this lesson, students should be able to differentiate between
aldehydes andketones using qualitative analysis:

Introduction

Aldehydes and ketones are organic compounds containing carbonyl group:

O

C
R OH

A carbonyl compound forms an orange or a yellow precipitate with Brady’s
reagent, 2,4-dinitrophenylhydrazine.

Aldehydes can be differentiated from ketones by using Fehling’s, Schiff’s, or
Tollens’ reagents. An aldehyde gives a positive result with the above
reagents whereas a ketone does not. The Iodoform test is used to determine
whether a carbonyl compound contains any methyl carbonyl structure. The
formation of a yellow precipitate indicates the presence of the methyl
carbonyl group, R C CH3

O

Apparatus Chemical Reagents

Stopper Ethanal
Dropper Benzaldehyde
Test tube Propanone
Boiling tube Unknown Y
Water bath 5% NH3
themometer 10% NaOH
5 mL measuring cylinder 0.3 M AgNO3
2,4-dinitrophenylhydrazine
Fehling’s solution
I2 in KI solution

Note: Use distilled or ANALAR grade for propanone

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Procedure
(A) Brady’s test

1. Place approximately 1 mL of 2,4-dinitrophenylhydrazine into 4
separate test tubes.

2. Add 5 drops of ethanal, benzaldehyde, propanone, and unknown
Y into the 4 test tubes accordingly.

3. Shake the test tubes.

4. Observe the formation of a precipitate.

Note:
If there is no precipitate, add 2 mL of distilled water and heat it
in a water bath at 60 – 70°C.

(B) Fehling’s test
1. Place approximately 1 mL of ethanal, benzaldehyde,
propanone, and unknown Y in 4 separate test tubes.
2. Add 2 mL of Fehling’s solution in each test tube.
3. Shake the test tubes gently.
4. Heat the mixture in the hot water bath for 15 - 20 minutes.
5. Record the observations.

(C) Tollens’ test

1. Prepare Tollens’ reagent by adding one drop of 10% NaOH
to 2 mL of 0.3 MAgNO3 in a boiling tube.

2. Add 5% NH3 dropwise until the precipitate dissolves.

3. Place approximately 1 mL of ethanal, benzaldehyde,
propanone, and unknown Y in separate test tubes.

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4. Add 1 mL of Tollens’ reagent to each test tube and shake the
mixtures gently.

5. Allow the mixtures to stand for 3 minutes. If there is no
change, warm themixture in a water bath at 60 – 70°C for 5
minutes.

6. Record the observations.

(D) Iodoform test

1. Place 10 drops of I2 in KI solution into 3 mL of distilled water
in a boiling tube.

2. Add 5 drops of ethanal into the boiling tube and shake gently.

3. Add 10% NaOH to the boiling tube drop by drop until the
colour of the I2 fades.

4. Allow it to stand for 2 to 3 minutes. If no precipitate forms,
warm the boiling tubein a water bath at 60 – 70oC.

5. If the colour of I2 disappears, add more I2 in KI solution
until the colour of I2 isretained. Repeat Step 4.

6. Record the observations.

7. Repeat the above steps with benzaldehyde, propanone, and
unknown Y.

POINT TO DISCUSS

1. Deduce the structure of an unknown based on the following
observations:
(a) A yellow precipitate with 2,4-dinitrophenylhydrazine.
(b) Silver mirror formed with Tollens’ reagents.
(c) A yellow precipitate with a solution of iodine in sodium
hydroxide.

2. State the tests that show the reducing property of an aldehyde and a
ketone.

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DATA SHEET

EXPERIMENT 6: ALDEHYDES AND KETONES

RESULTS

Test Ethanal Benzaldehyde Propanone Unknown
Y
Brady’s
test

Fehling’s
test

Tollens’
test

Iodoform
test

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REFERENCES

Ali, R. (1995) Panduan Amali Kimia Asas, Kursus Pengajian Tinggi Fajar
Bakti, Selangor.

Baum, S.J., Sandwick, R.K. (1994) Laboratory Exercises in Organic and
Biological Chemistry. Prentice Hall. New Jersey. United States of
America.

Beran, J.A. (1996) A Study of Chemical and Physical Changes, 2nd
Edition. John Wiley & Sons Inc. United States of America.

Brown, T. E., LeMay, H. E., Bursten, B. E., Murphy, C., Woodward, P. &
Stoltzfus, M. E. (2018). Chemistry: The Central Science (14th ed.).
Pearson Education

Chang, R & Overby, J. (2019). Chemistry (13th ed.). McGraw-Hill. United
States of America.

Chemistry Department of University Malaya. (2001) Laboratory Manual
Organic Chemistry (SCES1220). Universiti Malaya. Malaysia.

Ritchie, R. (2000) Revise AS Chemistry. Letts Educational Ltd. United
States of America.

Seager, S.L., Slabaugh, M.R. (2000) Introductory Chemistry for Today, 4th
Edition. Thomson Learning. California. United States of America.

Silberberg, M. & Amateis, P. (2021). Chemistry: The Molecular Nature of
Matter and Change (9th ed.). McGraw-Hill

Stanley, A.J. et.al (2000) Discovering Chemistry : A Year-12 Chemistry
Text Book. Openbook Publishers. South Australia, Australia.

Universiti Teknologi Malaysia (2001) Amali Kimia Am, Jawatankuasa
Penerbitan dan Penulisan Fakulti Sains UTM. Penerbit UTM.
Malaysia.

Ware, G., Deretic, G. (1995) Senior Chemistry : Practical Manual,
Heinemann. Victoria.

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ACKNOWLEDGEMENTS

The Matriculation Division, Ministry of Education Malaysia wish to thank
everyone who has contributed in shaping and writing this CHEMISTRY
LABORATORY MANUAL (13th Edition) for the Two Semester
Matriculation Programme. Special thanks go to those for their many
valuable suggestions and conscientiousness in completing this manual.

Dr. Hajah Rosnarizah binti Abdul Halim
Director of Matriculation Division

Haji Mohd Yusof bin Samad
Deputy Director of Matriculation Division (Academic)

Mohd Junaidi bin Abd Aziz
Senior Principal Assistant Director

Siti Warda binti Selamat
Assistant Director

Reviewers for the 13th Edition:

• Prof. Dr. Zanariah binti Abdullah, UM
• Prof. Dr. Rosiyah binti Yahya, UM
• Norasyikin binti Ismail @ Chik, KMK
• Wan Zai Azlin binti Wan Aziz, KMPh
• Byron MC Michael Kadum, KML
• Zuraidah binti Ahmad, KMJ
• Fara Nur Hani binti Musa, KMP
• Fauziah binti Ismail, KMPk
• Sariah binti Ali, KMM
• Noor Fatihah binti Zulkeply, KMNS
• Wan Syafinas binti Wan Salim, KMKK
• Nur Afiqah binti Rosali, KMKPh
• Ahmad Farid bin Yang Abd Talib, KMSw
• Azfa Ilhamuna binti Ahmad Badri, KMPP

Cover designed by Syed Nassir bin Syed Ahmad, KML

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SK015 & SK025