Chapter 1 – Rate of Reactions
List of PEKA experiments:
1. Average rate of of reaction reaction and instantan instantaneous eous rate rate of of reaction reaction 2. Effe Effect ct of surface surface area area on the rate rate of reacti reaction on 3. Effe Effect ct of concen concentrati tration on on the the rate of of reaction reaction 4. Effe Effect ct of tempe temperatu rature re on the the rate of of reaction reaction 5. Effe Effect ct of catal catalyst yst on the rate rate of reac reaction tion 6. Effe Effect ct of the amoun amountt of catalyst catalyst on the the rate of reacti reaction on Number Laboratory Work 1.2 Pg. 3 Titl Title e Avera verag ge ra rate of re reactio ction n an and in insta stantan taneous ra rate of re reactio ction n Aim Aim To dete determ rmin ine e the the aver averag age e rat rate e of of rea react ctio ion n and and the the ins insta tant ntan aneo eous us rate rate of reac reacti tion on 3 Apparatus 50 cm beaker Test tube Spatula Material Marble chip 2.0 mol dm-3 hydrochloric hydrochloric acid (HCl) -3 0.1 mol dm sodium thiosulphate, Na 2S2O3solution 1.0 mol dm -3 lead(II) nitrate solution
. Number Pg. Title Aim Problem Statement Hypothes Hypothesis is
Apparatus
Experiment 1.1 6 Effect of of su surface area on the rate of re reaction To in investig stiga ate the the eff effe ect of to total tal su surfa rface are area a of of th the re reacta ctant on on th the ra rate of reaction How does the total exposed surface area of a solid reactant affect the rate of reaction? When When the total total surfac surface e area of of marble marble chips chips increas increases, es, the the rate of of reaction reaction increases. / The smaller the size of the reactant particles, that is, the larger the total surface area of the reactant particles, the higher the rate of reaction. 50 cm3 measuring cylinder 150 cm3 conical flask Stopper with delivery tube Basin Burette Spatula Electronic balance Stopwatch
Material
0.5 mol dm -3 hydrochloric acid (HCl) 2 g large marble chips 2 g small marble chips Water Manipulated variable: Total surface area of marble chips Responding variable: Rate of reaction Controlled / Fixed variable: Mass of marble chips, volume and concentration of hydrochloric acid (HCl), temperature 1. Smaller marble chips have a larger total surface area than larger marble chips of the same mass. 2. For the graph of the volume of gas released against time, the curve with higher initial gradient indicates a higher initial rate of reaction.
Variables
Operational Definition
. Number Pg. Title Aim Problem Statement Hypothesis
Apparatus
Experiment 1.2 10 Effect of concentration on the rate of reaction To investigate the effect of concentration on the rate of reaction How does the concentration of a reactant affect the rate of reaction? / Does high concentration of sodium thiosulphate Na 2S2O3 solution decrease the time taken for the mark ‘X’ to disappear from sight? When the concentration of sodium thiosulphate, Na 2S2O3 solution increases, the rate of reaction increases. / The higher the concentration of sodium thiosulphate Na 2S2O3 solution, the shorter the time taken for the mark ‘X’ to disappear from sight. 150 cm3 conical flask 50 cm3 measuring cylinder 10 cm3 measuring cylinder Stopwatch 0.2 mol dm -3 sodium thiosulphate solution 1.0 mol dm -3 sulphuric acid Distilled water White paper marked ‘X’ at the centre Manipulated variable: Concentration of sodium thiosulphate, Na2S2O3 solution Responding variable: Rate of reaction Controlled / Fixed variable: Concentration, volume and initial temperature of sulphuric acid, H 2SO4. Total volume of reactants Rate of reaction is inversely proportional to the time taken for the the mark ‘X’ to disappear from sight
Material
Variables
Operational Definition . Number Pg.
Experiment 1.3 13
Title Aim Problem Statement Hypothesis Apparatus
Effect of temperature on the rate of reaction To investigate the effect of temperature on the rate of reaction How does temperature affect the rate of reaction? An increase in temperature will increase the rate of reaction. 150 cm3 conical flask 50 cm3 measuring cylinder 10 cm3 measuring cylinder Stopwatch Thermometer Bunsen burner Tripod stand Wire gauze 0.2 mol dm -3 sodium thiosulphate solution 1.0 mol dm -3 sulphuric acid White paper marked ‘X’ at the centre Manipulated variable: Temperature of sodium thiosulphate, Na2S2O3 solution Responding variable: The time taken for the cross ‘X’ to disappear Controlled / Fixed variable: volume and concentration of sodium thiosulphate Na 2S2O3solution, volume and concentration of sulphuric acid, size of conical flask Rate of reaction is inversely proportional to the time taken for the mark ‘X’ to disappear from sight
Material
Variables
Operational Definition . Number Pg. Title Aim Problem Statement Hypothesis Apparatus
Experiment 1.4 15 Effect of catalyst on the rate of reaction To investigate the effect of a catalyst on the rate of reaction How does a catalyst affect the rate of reaction? / How do catalysts affect the rate of decomposition of hydrogen peroxide? The presence of a catalyst increases the rate of reaction. / Manganese(IV) oxide increases the rate of decomposition of hydrogen peroxide. Test tube Test tube rack Spatula Wooden splinter Retort stand and clamp 10 cm3 measuring cylinder Electronic balance Weighing bottle 20-volume hydrogen peroxide, H 2O2 solution 1.0 g Manganese(IV) oxide powder Manipulated variable: Presence or absence of a catalyst Responding variable: The release of oxygen gas / Rate of reaction
Material
Variables
Controlled / Fixed variable: Volume and concentration of hydrogen peroxide (H2O2) solution, temperature The decomposition of hydrogen peroxide is fast if the glowing wooden splinter rekindles brightly and rapidly. The decomposition of hydrogen peroxide is slow if the glowing wooden splinter glows dimly and slowly.
Operational Definition
. Number Pg. Title Aim Problem Statement Hypothesis Apparatus
Experiment 1.5 17 Effect of the amount of catalyst on the rate of reaction To investigate the effect of the amount of catalyst on the rate of reaction. How does the amount of a catalyst affect the rate of reaction? / Does higher amount of catalysts increases the rate of reaction? When the amount of a catalyst used increases, the rate of reaction increases. / The higher the amount of the catalysts, the higher the rate of reaction. 50 cm3 measuring cylinder 150 cm3 conical flask Stopper with delivery tube Burette Retort stand and clamp Basin Stopwatch Electronic balance Spatula Weighing bottle Beakers 2-volume hydrogen peroxide solution 1.0 g manganese(IV) oxide powder Manipulated variable: amount / mass of catalyst Responding variable: Rate of reaction Controlled / Fixed variable: Temperature, volume and concentration of hydrogen peroxide solution The curves for the graph of volume of gas liberated against time a higher gradient indicated a higher rate of reaction.
Material
Variables
Operational Definition
Chapter 3 – Oxidation and Reduction
List of PEKA experiments:
1. Redox reaction as loss or gain of oxygen 2. Change of iron(II) to iron(III) ions and vice versa 3. Displacement of metals
4. Displacement of halogens 5. Transfer of electrons at a distance 6. Effect of other metals on rusting 7. Reactivity of metals with oxygen 8. (A) The position of carbon in the reactivity series of metals with oxygen (B) Heating carbon dioxide with metals 9. The position of hydrogen in the reactivity series of metals (Demonstration by teacher) 10. Oxidation and reduction in electrolytic cells 11. Oxidation and reduction in chemical cells 12. Oxidation and reduction in voltaic cell with a salt bridge 13. Number Pg. Title Aim
Laboratory Work 3.1 67 Redox reaction as loss or gain of oxygen To investigate oxidation and reduction A. Combustion of metal in oxygen To investigate redox reaction in the combustion of metal in oxygen gas, O2 B. Heating of metal oxide with carbon To investigate redox reaction in the heating of metal oxide with carbon A. Combustion of metal in oxygen In the reaction between metals in oxygen, which reagent undergoes oxidation and which reagent undergoes reduction? B. Heating of metal oxide with carbon
Problem Statement
In the reaction between metal oxide and carbon, which reagent undergoes oxidation and which reagent undergoes reduction? A. Combustion of metal in oxygen (I) Magnesium undergoes oxidation to form magnesium ion, Mg 2+ (II) Oxygen gas undergoes reduction to form oxide ion, O 2B. Heating of metal oxide with carbon
Hypothesis
(I) Carbon undergoes oxidation to form carbon dioxide gas (II) Copper(II) oxide, iron(III) oxide and lead(II) oxide undergo reduction to form copper, iron and lead respectively A. Combustion of metal in oxygen A pair of tongs Bunsen burner
Apparatus
B. Heating of metal oxide with carbon Crucible Pipe-clay triangle Tripod stand Bunsen burner Spatula A. Combustion of metal in oxygen 5cm magnesium ribbon Sandpaper Gas jar containing oxygen B. Heating of metal oxide with carbon
Material
Carbon powder Copper(II) oxide powder / Iron(III) oxide powder / Lead(II) oxide powder A. Combustion of metal in oxygen Manipulated variable: Type of metal Responding variable: Reaction product Controlled / Fixed variable: Oxygen gas and the conditions of reaction B. Heating of metal oxide with carbon
Variables
Manipulated variable: Type of metal oxide Responding variable: Reaction product Controlled / Fixed variable: Carbon and the conditions of reaction
. Number Pg. Title Aim
Apparatus
Laboratory Work 3.2 71 Change of iron(II) to iron(III) ions and vice versa To investigate oxidation and reduction in the change of iron(II) ions, Fe 2+ to iron(III) ions, Fe 3+ and vice versa (change of iron(III) ions, Fe 3+ to iron(II) ions, Fe2+) Dropper Spatula Test tube Test tube holder Test tube rack Bunsen burner Filter funnel Measuring cylinder 0.5 mol dm -3 freshly prepared iron(II) sulphate, FeSO 4 solution 0.5 mol dm -3 iron(III) sulphate, Fe 2(SO4)3solution Bromine water Zinc powder Filter paper (1 piece) 2.0 mol dm -3 sodium hydroxide, NaOH solution
Material
0.5 mol dm -3 potassium hexacynoferrate(III), K 3Fe(CN) 6 solution
. Number Pg. Title Aim Problem Statement Hypothesis
Laboratory Work 3.3 73 Displacement of metals To investigate oxidation and reduction in the displacement of metals from their salt solutions How does redox reaction occur in a displacement reaction in which a metal is displaced from its salt solution? (I) The metal that acts as a reducing agent will form metal ion (II) The metal ion that acts as an oxidising agent will be precipated as metal Test tubes Test tube rack Zinc strip Copper strip Magnesium ribbon 0.5 mol dm -3 silver nitrate 0.5 mol dm -3 copper(II) sulphate 0.5 mol dm -3 magnesium sulphate Manipulated variable: A pair of metals and salt solutions Responding variable: Precipitation of metal and colour changes in the solutions Controlled / Fixed variable: Volumes and concentrations of solutions containing the metal ions
Apparatus
Material
Variables
. Number Pg. Title Aim Problem Statement Hypothesis Apparatus
Laboratory Work 3.4 74 Displacement of halogens To investigate oxidation and reduction in the displacement of halogen from its halide solution How do redox reactions occur in displacement reactions between halogens and aqueous solutions of halide ions? A more reactive halogen displace a less reactive halogen from an aqueous solutions of its halide ions Test tubes Test tube rack Chlorine water Bromine water Iodine water 0.5 mol dm -3 potassium chlorine, KCl solution 0.5 mol dm -3 potassium bromine, KBr solution
Material
0.5 mol dm -3 potassium iodine, KI solution 1,1,1-tricholoethane, CH 3CCl3 Manipulated variable: A pair of halogens and their halide ions Responding variable: Changes in colour in 1,1,1-trichloroethane, CH3CCl3 Controlled / Fixed variable: Volume of reaction mixture
Variables
. Number Pg. Title Aim Problem statement Hypothesis Apparatus
Laboratory Work 3.5 77 Transfer of electrons at a distance To investigate oxidation and reduction in the transfer of electrons at a distance How do redox reactions occur in displacement reactions between halogens and aqueous solutions of halide ions? A more reactive halogen displace a less reactive halogen from an aqueous solution of its halide ions U-tube Galvanometer Connecting wire with crocodile clips Graphite electrode Retort stand and clamp Test tube Dropper / glass tube Stopper with 1 hole 2.0 mol dm -3 sulphuric acid, H 2SO4 0.5 mol dm -3 freshly prepared iron(II) sulphate, FeSO 4 solution 0.2 mol dm -3 acidified potassium manganate(VII), KMnO 4 solution 0.5 mol dm -3 potassium iodide, KI solution 0.2 mol dm -3 acidified potassium dichromate(VI), K 2Cr 2O7 solution Bromine water 0.2 mol dm -3 potassium thiocyanate, KSCN solution 1% starch solution Manipulated variable: A pair of halogen and their halide ions Responding variable: Changes in colour in 1,1,1-trichloroethana, CH3CCl3 Controlled / Fixed variable: Volume of reaction mixture
Material
Variables
. Number Pg. Title Aim Problem Statement
Experiment 3.1 81 Effect of other metals on rusting To investigate the effect of other metals on rusting How do different types of metals in contact with iron affect rusting?
Hypothesis
Apparatus
When a more electropositive metal is in contact with iron, the metal inhibits rusting. When a less electropositive metal is in contact with iron, the metal speeds up rusting Test tube Test tube rack Iron nail Magnesium ribbon Copper strip Zinc strip Tin strip Hot jelly solution with a little potassium hexacyanoferrate(III), K3Fe(CN) 6 solution and phenolphthalein Sandpaper Manipulated variable: Types of metals that are in contact with iron / Different types of metals Responding variable: Presence of colouration / Intensity of dark blue colouration / Rusting of iron Controlled / Fixed variable: Clean iron nails, medium in which the iron nails are kept / hot jelly solution, temperature Blue colouration indicates rusting of iron
Material
Variables
Operational Definition . Number Pg. Title Aim
Laboratory Work 3.6 85 Reactivity of metals with oxygen (I) To investigate the reactivity of metals with oxygen (II) To arrange metals in terms of their reactivity with oxygen How do different types of metals react with oxygen?
Problem Statement Hypothesis Apparatus
The more reactive metal react more vigorously with oxygen Boiling tube Retort stand and clamp Bunsen burner Spatula Forceps Magnesium powder Copper powder Iron filings Lead powder Zinc powder Solid potassium manganate(VII), KMnO 4 Asbestos paper Glass wool Manipulated variable: Different types of metals Responding variable: the brightness of the flame
Material
Variables
Controlled / Fixed variable: The amount of the metal and potassium manganate(VII) powder
. Number Pg. Title
Laboratory Work 3.7 87 A. The position of carbon in the reactivity series of metals with oxygen B. Heating carbon dioxide with metals A. To determine the position of carbon in the reactivity series of metals B. To determine the ability of a metal to remove oxygen from carbon dioxide. How is the position of carbon in the reactivity series of metals determined?
Aim
Problem Statement Hypothesis
(I) A reaction occur if carbon is more reactive than the metal (II) A reaction not occur if carbon is less reactive than the metal (III) Carbon is placed between aluminium and zinc in the reactivity series of metals A. The position of carbon in the reactivity series of metals with oxygen Crucible / Porcelain dish / Asbestos paper Spatula Bunsen burner Pipe-clay triangle Tripod stand B. Heating carbon dioxide with metals
Apparatus
Gas jar Gas jar cover A pair of tongs A. The position of carbon in the reactivity series of metals with oxygen Carbon powder Solid copper(II) oxide, CuO Solid magnesium oxide, MgO Solid aluminium oxide, Al 2O3 Solid zinc oxide, ZnO B. Heating carbon dioxide with metals
Material
Variables
Magnesium ribbon Gas jar filled with carbon dioxide gas, CO 2 Sandpaper
A.
Manipulated variable: Type of metal oxide Responding variable: Intensity of flame Controlled / Fixed variable: Carbon powder
Manipulated variable: Type of metal
B.
Responding variable: Intensity of flame Controlled / Fixed variable: Carbon dioxide gas and the conditions of reaction
. Number Pg. Title Aim Problem Statement Hypothesis Apparatus
Laboratory Work 3,8 89 The position of hydrogen in the reactivity series of metals (Demonstration by teacher) To determine the position of hydrogen in the reactivity series of metals How is the position of hydrogen in the reactivity series of metals determined? Hydrogen is placed between zinc and iron in the reactivity series of metals Combustion tube Porcelain dish Flat-bottomed flask U-tube Thistle funnel Delivery tube Bunsen burner Retort stand and clamps Stopper with 1 hole Stopper with 2 holes 2.0 mol dm -3 sulphuric acid, H 2SO4 1.0 mol dm -3 copper(II) sulphate, CuSO 4 solution Zinc granules Solid copper(II) oxide Solid zinc oxide Solid lead(II) oxide Solid iron(III) oxide Anhydrous calcium chloride Manipulated variable: Different types of metal oxides Responding variable: Intensity of flameControlled / Fixed variable: Hydrogen gas and the conditions of reaction
Material
Variables
. Number Pg. Title Aim Apparatus
Laboratory Work 3.9 95 Oxidation and reduction in electrolytic cells To investigate oxidation and reduction in electrolytic cellsA. Electrolytic cell involving molten electrolyteB. Electrolytic cell involving aqueous electrolyte A. Electrolytic cell involving molten electrolyte Crucible Cardboard Battery
Connecting wire with crocodile clips Tripod stand Bunsen burner Pipe-clay triangle Carbon electrode Switch Ammeter Light bulb A pair of tongs Spatula B. Electrolytic cell involving aqueous electrolyte
Battery Connecting wire with crocodile clips Electrolytic cell Carbon electrode Switch Ammeter Light bulb Small test tube Beaker A pair of tongs A. Electrolytic cell involving molten electrolyte Solid lead(II) bromide, PbBr 2 B. Electrolytic cell involving aqueous electrolyte
Material
0.5 mol dm -3 potassium iodide, KI solution Starch solution Sandpaper Wooden splinter
. Number Pg. Title Aim Apparatus
Laboratory Work 3.10 97 Oxidation and reduction in chemical cells To investigate the oxidation and reduction in chemical cells Porous pot Voltmeter Connecting wires with crocodile clips Beaker Measuring cylinder 1.0 mol dm -3 copper(II) sulphate, CuSO 4 solution 1.0 mol dm -3 zinc sulphate ZnSO 4 solution Copper strip Zinc strip Sandpaper
Material
. Number Pg. Title Aim Apparatus
Laboratory Work 3.10 (Similar experiment) 97 Oxidation and reduction in voltaic cell with a salt bridge To investigate the oxidation and reduction in chemical cells Voltmeter Connecting wires with crocodile clips 100 cm3 beakers Measuring cylinder 1.0 mol dm -3 copper(II) sulphate, CuSO 4 solution 1.0 mol dm -3 zinc sulphate ZnSO 4 solution 1.0 mol dm -3 lead(II) nitrate Pb(NO 3)2 solution 1.0 mol dm -3 iron(II) sulphate FeSO 4 solution Copper plate Zinc plate Lead plate Iron nail Sandpaper Saturated potassium chloride, KCl solution Filter paper strip
Material
Chapter 4 – Thermochemistry
List of PEKA experiments:
1. Exothermic and endothermic reactions 2. Heat of precipitation 3. Heat of displacement 4. Heat of neutralisation 5. Heat of neutralisation of acids and alkalis of different strength 6. Heat of neutralisation 7. Heats of combustion for alcohols Number Laboratory Work 4.1 Pg. 101 Title Exothermic and endothermic reactions Aim To identify an exothermic or endothermic reaction Problem How to identify exothermic or endothermic reactions? Statement Hypothesis Exothermic reaction occurs when the temperature of the reaction mixture
Apparatus
increases.Endothermic reaction occurs when the temperature of the reaction mixture decreases. Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Spatula Glass rod 50 cm3 measuring cylinder Solid sodium hydrogen carbonate, NaHCO 3 Solid sodium hydroxide, NaOH Solid ammonium chloride, NH 4Cl Solid ammonium nitrate, NH 4NO3 Solid ammonium sulphate, (NH 4)2SO4 2.0 mol dm -3 hydrochloric acid, HCl Distilled water Manipulated variable: Pairs of reactants Responding variable: The temperature change in the reaction mixture Controlled / Fixed variable: Types of container, volume of solution or water
Material
Variables
=============================================== Number Pg. Title Aim Apparatus
Laboratory Work 4.2 104 Heat of precipitation To determine the heat of precipitation of silver chloride, AgCl Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Glass rod 50 cm3 measuring cylinder 0.5 mol dm -3 silver nitrate solution 0.5 mol dm -3 sodium chloride solution
Material
=============================================== Number Pg. Title Aim Apparatus
Laboratory Work 4.3 106 Heat of displacement To determine the heat of displacement of copper Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Glass rod 50 cm3 measuring cylinder 0.5 mol dm -3 copper(II) sulphate solution Zinc power
Material
===============================================
Number Pg. Title Aim Apparatus
Laboratory Work 4.4 108 Heat of neutralisation To determine the heats of neutralisation between strong acids and strong alkalis Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Glass rod 50 cm3 measuring cylinder 2.0 mol dm -3 hydrochloric acid, HCl 2.0 mol dm -3 sodium hydroxide, NaOH solution 2.0 mol dm -3 nitric acid, HNO3 2.0 mol dm -3 potassium hydroxide, KOH solution
Material
=============================================== Number Pg. Title Aim Problem Statement Hypothesis
Apparatus
Laboratory Work 4.5 109 Heat of neutralisation of acids and alkalis of different strength To determine and compare the heats of neutralisation between acids and alkalis of different strength How do the heat of neutralisation for reactions between acids and alkalis of different strength? The values of heat of neutralisation for reactions between strong acids and strong alkalis are higher than that of reactions between strong acids and weak alkalis / weak acids and strong alkalis or weak acids and weak alkalis. Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Glass rod 50 cm3 measuring cylinder 2.0 mol dm -3 ethanoic acid, CH 3COOH 2.0 mol dm -3 hydrochloric acid, HCl 2.0 mol dm -3 sodium hydroxide, NaOH solution 2.0 mol dm -3 ammonia, NH3 solution Manipulated variable: Different strength of acids and alkalis Responding variable: The value of heat of neutralisation Controlled / Fixed variable: Volume and concentration of acids used, volume and concentration of alkalis used.
Material
Variables
=============================================== Number Pg. Title Aim
Laboratory Work 4.6 110 Heat of neutralisation To determine and compare the heats of neutralisation between: Hydrochloric acid (strong acid), HCl and sodium hydroxide (strong
base), NaOH solution Ethanoic acid (weak acid), CH 3COOH and sodium hydroxide (strong base), NaOH solution Hydrochloric acid (strong acid), HCl and ammonia (weak base), NH3 solution Ethanoic acid (weak acid), CH 3COOH and ammonia(weak base), NH3 solution How are the heats of neutralisation determined and compared?
Problem Statement Hypothesis
Apparatus
The heat of neutralisation between hydrochloric acid and sodium hydroxide is higher than the heat of neutralisation between ethanoic acid and ammonia solution. 50 cm3 burette 25.0 cm3 pipette Pipette filler Retort stand and clamps Plastic cup / Polystyrene cup 250 cm3 beaker Magnetic stirrer Magnetic stir bar Temperature sensor Computer Computer interface Stopwatch 1.0 mol dm -3 hydrochloric acid, HCl 1.0 mol dm -3 sodium hydroxide, NaOH solution 1.0 mol dm -3 ethanoic acid, CH 3COOH 1.0 mol dm -3 ammonia, NH3 solution Manipulated variable: Different types of acids and bases Responding variable: Heat of neutralisation Controlled / Fixed variable: Volume and concentration of acid and alkali used
Material
Variables
=============================================== Number Pg. Title Aim Problem Statement Hypothesis Apparatus
Experiment 4.1 112 Heats of combustion for alcohols To determine the heats of combustion for alcohols Does alcohol with a higher number of carbon atoms per molecule have a higher heat of combustion? The higher the number of carbon atoms in the alcohol molecules, the higher is the heat of combustion. Copper can Thermometer Glass rod / Stirrer Measuring cylinder
Tripod stand Spirit lamp Wooden block Weighing balance Wind shield / Asbestos screen Methanol Ethanol Propanol / Prop-1-ol Butanol / But-1-ol Water Manipulated variable: Different types of alcohols Responding variable: Heat of combustion of alcohol Controlled / Fixed variable: Volume of water and copper can / metal container (calorimeter)
Material
Variables
Chapter 5 – Chemicals for Consumers
List of PEKA experiments:
1. Soap preparation process Number Laboratory Work 5.1 Pg. 117 Title Soap preparation process Aim To prepare soap using the saponification process Apparatus 250 cm3 beakers 50 cm3 measuring cylinder Spatula Glass rod Filter funnel Wire gauze Tripod stand Bunsen burner Wash bottle Test tube Material Palm oil 5.0 mol dm -3 sodium hydroxide, NaOH solution Sodium chloride powder Filter paper (3 pieces) Distilled water
