CHEMISTRY 2 SK025
Chemistry Lab Manual – SK025 Updated: 18/05/2022 36 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 Water bath Stopwatch Boiling tube Thermometer 10 mL pipette 50 mL burette 10 mL measuring cylinder 100 mL conical flask Laminated white paper with ‘X’ mark 0.1 M HCl 10% MnSO4 2.0 M H2SO4 0.02 M KMnO4 0.2 M Na2S2O3 0.25 M H2C2O4
Chemistry Lab Manual – SK025 Updated: 18/05/2022 37 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 0.2 M Na2S2O3 solution (mL) Volume of distilled water (mL) Concentration of Na2S2O3 (M) Volume of 0.1 M HCI solution (mL) Time (s) 1 (s-1 ) 50.00 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 38 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 39 Table 1.2 Effect of temperature and catalyst on reaction rate Temperature (°C) Without catalyst MnSO4 (A1 + B1) With catalyst MnSO4 (A2 + B2) t (s) 1 (s-1 ) t (s) 1 (s-1 ) 30 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?
Chemistry Lab Manual – SK025 Updated: 18/05/2022 40 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)
Chemistry Lab Manual – SK025 Updated: 18/05/2022 41 Heat released can be determined by measuring the temperature before and after the reaction: −qrxn = CT + mscsT ….. (4) where ∆T = final temperature of system – initial temperature of system ms = mass of solution Cc = heat capacity of calorimeter cs = specific heat capacity of solution Apparatus Chemical Reagents 25 mL pipette 100 mL beaker Thermometer Calorimeter or styrofoam cup 1.0 M HCl 1.0 M NaOH 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)
Chemistry Lab Manual – SK025 Updated: 18/05/2022 42 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 HClsolution 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 43 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 =
Chemistry Lab Manual – SK025 Updated: 18/05/2022 44 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 45 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 Ammeter Hair dryer Voltmeter Stopwatch Transformer Sandpaper or abrasive cloth Crocodile clips 50 mL beaker Analytical balance Salt bridge 50 mL measuring cylinder 0.1 M CuSO4 0.1 M ZnSO4 0.1 M FeSO4 0.1 M MgSO4 0.1 M Al(NO3)3 Zinc strip Copper strip Magnesium strip Aluminium strip Carbon rod Saturated KNO3 or KCl 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 in saturated KNO3 or KClsolution. Avoid handling the salt bridge with bare hands. Procedure (A) Galvanic cell 1. Clean the metalstrips 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 46 3. Set up the apparatus as shown in Figure 3.1. Zn Cu Salt bridge ZnSO CuSO4 4 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 47 3. Set up apparatus as show in Figure 3.2. Fill a 50 mL beaker with 35 mL 0.1 MCuSO4. 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. + DC − Carbon (anode) Copper (cathode ) 0.1 M CuSO4
Chemistry Lab Manual – SK025 Updated: 18/05/2022 48 DATA SHEET EXPERIMENT 3: ELECTROCHEMICAL CELLS RESULTS (A) Galvanic cell Galvanic Cell Cell Potential, Ecell (V) (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) =
Chemistry Lab Manual – SK025 Updated: 18/05/2022 49 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: C H H H H C C H H H H H H Methane Ethane Cyclohexane Alkanes undergo free radicalsubstitution reaction. CH4 + Br CH3Br + HBr 2 CH2Cl2 uv Alkenes are unsaturated hydrocarbons with at least one double bond between two carbonatoms. Example of alkenes: H2C CH2 Ethene Cyclohexene
Chemistry Lab Manual – SK025 Updated: 18/05/2022 50 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 + Br + HBr 2 CH2Cl2 CH3CHCH3 Br Alkenes also react with potassium permanganate solution in two different conditions: a) In basic medium to form a diol. H2C CH2 C C OH H H OH H H KMnO4 , OH - cold, dilute b) In hot acidic medium to form a carboxylic acid. C C H3C H H CH3 KMnO4 , H + Δ 2 CH3 C OH O Arenes are aromatic hydrocarbons with stable molecular structures. Example of aromatic hydrocarbons: CH3 Toluene Naphthalene Anthracene
Chemistry Lab Manual – SK025 Updated: 18/05/2022 51 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 Test tube Rubber band Labeling paper Test tube rack Black sugar paper (6 cm × 12 cm) Toluene Cyclohexane Cyclohexene Dichloromethane 0.01 M KMnO4 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 52 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).
Chemistry Lab Manual – SK025 Updated: 18/05/2022 53 DATA SHEET EXPERIMENT 4: REACTIONS OF ALIPHATIC AND AROMATIC HYDROCARBONS RESULTS Test Hydrocarbons Bromine in dichloromethane Oxidation with alkaline KMnO4 (Baeyer’s test) Under sunlight In the dark Cyclohexane Cyclohexene Toluene
Chemistry Lab Manual – SK025 Updated: 18/05/2022 54 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: C OH H R H C OH H R R C OH R R R Primary alcohol (1o ) Secondary alcohol (2o ) Tertiary 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 dependson 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 55 Apparatus Chemical Reagents Stopper Dropper Test tube Stopwatch Water bath 10 mL measuring cylinder Ethanol 1-Butanol 2-Butanol 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 56 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 57 DATA SHEET EXPERIMENT 5: REACTIONS OF HYDROXY COMPOUNDS RESULTS Hydroxy compound Observation (A) Lucas Test (B) Oxidation with sodium dichromate 1-butanol 2-butanol 2-methyl-2-propanol Unknown (Alcohol X) (C) Confirmatory test for phenol Compound Observation Phenol
Chemistry Lab Manual – SK025 Updated: 18/05/2022 58 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: C OH O R 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, Apparatus Chemical Reagents Stopper Dropper Test tube Boiling tube Water bath themometer 5 mL measuring cylinder Ethanal Benzaldehyde Propanone Unknown Y 5% NH3 10% NaOH 0.3 M AgNO3 2,4-dinitrophenylhydrazine Fehling’s solution I2 in KI solution Note: Use distilled or ANALAR grade for propanone R C O CH3
Chemistry Lab Manual – SK025 Updated: 18/05/2022 59 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 60 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.
Chemistry Lab Manual – SK025 Updated: 18/05/2022 61 DATA SHEET EXPERIMENT 6: ALDEHYDES AND KETONES RESULTS Test Ethanal Benzaldehyde Propanone Unknown Y Brady’s test Fehling’s test Tollens’ test Iodoform test
Updated: 18/05/2022 62 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, 2 nd 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, 4 th 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.
Updated: 18/05/2022 63 ACKNOWLEDGEMENTS The Matriculation Division, Ministry of Education Malaysia wish to thank everyone who has contributed in shaping and writing this CHEMISTRY LABORATORY MANUAL (13 th 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 13 th 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
SK015 & SK025