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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 2 | 1 |
GAS LAWS
|
Boyle's Law - Introduction and Experimental Investigation
|
By the end of the
lesson, the learner
should be able to:
State Boyle's law Explain Boyle's law using kinetic theory of matter Investigate the relationship between pressure and volume of a fixed mass of gas Plot graphs to illustrate Boyle's law |
Teacher demonstration: Use bicycle pump to show volume-pressure relationship. Students observe force needed to compress gas. Q/A: Review kinetic theory. Class experiment: Investigate pressure-volume relationship using syringes. Record observations in table format. Discuss observations using kinetic theory.
|
Bicycle pump, Syringes, Gas jars, Chart showing volume-pressure relationship
|
KLB Secondary Chemistry Form 3, Pages 1-3
|
|
| 2 | 2 |
GAS LAWS
|
Boyle's Law - Mathematical Expression and Graphical Representation
Boyle's Law - Numerical Problems and Applications |
By the end of the
lesson, the learner
should be able to:
Express Boyle's law mathematically Apply the equation PV = constant Plot and interpret pressure vs volume graphs Plot pressure vs 1/volume graphs |
Q/A: Recall previous lesson observations. Teacher exposition: Derive P₁V₁ = P₂V₂ equation from experimental data. Students plot graphs of pressure vs volume and pressure vs 1/volume. Analyze graph shapes and interpret mathematical relationship.
|
Graph papers, Scientific calculators, Chart showing mathematical expressions
Scientific calculators, Worked example charts, Unit conversion tables |
KLB Secondary Chemistry Form 3, Pages 3-4
|
|
| 2 | 3 |
GAS LAWS
|
Charles's Law - Introduction and Temperature Scales
|
By the end of the
lesson, the learner
should be able to:
State Charles's law Convert temperatures between Celsius and Kelvin scales Define absolute zero temperature Explain the concept of absolute temperature |
Teacher demonstration: Flask with colored water column experiment. Q/A: Observe volume changes with temperature. Exposition: Introduce Kelvin scale and absolute zero concept. Practice: Temperature conversions between °C and K. Discuss absolute zero and ideal gas concept.
|
Round-bottomed flask, Narrow glass tube, Colored water, Rubber bung, Hot and cold water baths
|
KLB Secondary Chemistry Form 3, Pages 6-8
|
|
| 2 | 4 |
GAS LAWS
|
Charles's Law - Experimental Investigation and Mathematical Expression
|
By the end of the
lesson, the learner
should be able to:
Investigate relationship between volume and temperature Express Charles's law mathematically Plot volume vs temperature graphs Extrapolate graphs to find absolute zero |
Class experiment: Volume-temperature relationship using flask and capillary tube. Record data at different temperatures. Plot graphs: volume vs temperature (°C) and volume vs absolute temperature (K). Extrapolate graph to find absolute zero. Derive V₁/T₁ = V₂/T₂ equation.
|
Glass apparatus, Thermometers, Graph papers, Water baths at different temperatures
|
KLB Secondary Chemistry Form 3, Pages 8-10
|
|
| 2 | 5 |
GAS LAWS
|
Charles's Law - Numerical Problems and Applications
|
By the end of the
lesson, the learner
should be able to:
Solve numerical problems using Charles's law Apply V₁/T₁ = V₂/T₂ in calculations Predict gas behavior with temperature changes Relate Charles's law to everyday phenomena |
Worked examples: Step-by-step problem solving with temperature conversions. Supervised practice: Calculate volumes at different temperatures. Discuss applications: hot air balloons, tire pressure changes, weather balloons. Assignment: Practice problems with real-life contexts.
|
Scientific calculators, Temperature conversion charts, Application examples
|
KLB Secondary Chemistry Form 3, Pages 10-12
|
|
| 3 | 1 |
GAS LAWS
|
Combined Gas Law and Standard Conditions
Introduction to Diffusion - Experimental Investigation |
By the end of the
lesson, the learner
should be able to:
Derive the combined gas law equation Apply PV/T = constant in problem solving Define standard temperature and pressure (s.t.p) Define room temperature and pressure (r.t.p) |
Q/A: Combine Boyle's and Charles's laws. Teacher exposition: Derive P₁V₁/T₁ = P₂V₂/T₂. Define s.t.p (273K, 760mmHg) and r.t.p (298K, 760mmHg). Worked examples: Problems involving changes in all three variables. Supervised practice: Complex gas law calculations.
|
Scientific calculators, Combined law derivation charts, Standard conditions reference table
KMnO₄ crystals, Bromine liquid, Gas jars, Combustion tube, Litmus papers, Stopwatch |
KLB Secondary Chemistry Form 3, Pages 12-14
|
|
| 3 | 2 |
GAS LAWS
|
Rates of Diffusion - Comparative Study
|
By the end of the
lesson, the learner
should be able to:
Compare diffusion rates of different gases Investigate factors affecting diffusion rates Measure relative distances covered by diffusing gases Calculate rates of diffusion using distance and time data |
Class experiment: Ammonia and HCl diffusion in glass tube. Insert cotton wool soaked in concentrated NH₃ and HCl at opposite ends. Time the formation of white NH₄Cl ring. Measure distances covered by each gas. Calculate rates: distance/time. Compare molecular masses of NH₃ and HCl.
|
Glass tube (25cm), Cotton wool, Concentrated NH₃ and HCl, Stopwatch, Ruler, Safety equipment
|
KLB Secondary Chemistry Form 3, Pages 16-18
|
|
| 3 | 3 |
GAS LAWS
|
Graham's Law of Diffusion - Theory and Mathematical Expression
|
By the end of the
lesson, the learner
should be able to:
State Graham's law of diffusion Express Graham's law mathematically Relate diffusion rate to molecular mass and density Explain the inverse relationship between rate and √molecular mass |
Teacher exposition: Graham's law statement and mathematical derivation. Discussion: Rate ∝ 1/√density and Rate ∝ 1/√molecular mass. Derive comparative expressions for two gases. Explain relationship between density and molecular mass. Practice: Identify faster diffusing gas from molecular masses.
|
Graham's law charts, Molecular mass tables, Mathematical derivation displays
|
KLB Secondary Chemistry Form 3, Pages 18-20
|
|
| 3 | 4 |
GAS LAWS
|
Graham's Law of Diffusion - Theory and Mathematical Expression
|
By the end of the
lesson, the learner
should be able to:
State Graham's law of diffusion Express Graham's law mathematically Relate diffusion rate to molecular mass and density Explain the inverse relationship between rate and √molecular mass |
Teacher exposition: Graham's law statement and mathematical derivation. Discussion: Rate ∝ 1/√density and Rate ∝ 1/√molecular mass. Derive comparative expressions for two gases. Explain relationship between density and molecular mass. Practice: Identify faster diffusing gas from molecular masses.
|
Graham's law charts, Molecular mass tables, Mathematical derivation displays
|
KLB Secondary Chemistry Form 3, Pages 18-20
|
|
| 3 | 5 |
GAS LAWS
|
Graham's Law - Numerical Applications and Problem Solving
|
By the end of the
lesson, the learner
should be able to:
Solve numerical problems using Graham's law Calculate relative rates of diffusion Determine molecular masses from diffusion data Compare diffusion times for equal volumes of gases |
Worked examples: Calculate relative diffusion rates using √(M₂/M₁). Problems involving time comparisons for equal volumes. Calculate unknown molecular masses from rate data. Supervised practice: Various Graham's law calculations. Real-life applications: gas separation, gas masks.
|
Scientific calculators, Worked example charts, Molecular mass reference tables
|
KLB Secondary Chemistry Form 3, Pages 20-22
|
|
| 4 | 1 |
THE MOLE
|
Relative Mass - Introduction and Experimental Investigation
|
By the end of the
lesson, the learner
should be able to:
Define relative mass using practical examples Compare masses of different objects using a reference standard Explain the concept of relative atomic mass Identify carbon-12 as the reference standard |
Experiment: Weighing different sized nails using beam balance. Use smallest nail as reference standard. Q/A: Discuss everyday examples of relative measurements. Teacher exposition: Introduction of carbon-12 scale and IUPAC recommendations. Calculate relative masses from experimental data.
|
Different sized nails ( 5-15cm), Beam balance, Fruits of different masses, Reference charts
|
KLB Secondary Chemistry Form 3, Pages 25-27
|
|
| 4 | 2 |
THE MOLE
|
Relative Mass - Introduction and Experimental Investigation
|
By the end of the
lesson, the learner
should be able to:
Define relative mass using practical examples Compare masses of different objects using a reference standard Explain the concept of relative atomic mass Identify carbon-12 as the reference standard |
Experiment: Weighing different sized nails using beam balance. Use smallest nail as reference standard. Q/A: Discuss everyday examples of relative measurements. Teacher exposition: Introduction of carbon-12 scale and IUPAC recommendations. Calculate relative masses from experimental data.
|
Different sized nails ( 5-15cm), Beam balance, Fruits of different masses, Reference charts
|
KLB Secondary Chemistry Form 3, Pages 25-27
|
|
| 4 | 3 |
THE MOLE
|
Avogadro's Constant and the Mole Concept
|
By the end of the
lesson, the learner
should be able to:
Define Avogadro's constant and its value Explain the concept of a mole as a counting unit Relate molar mass to relative atomic mass Calculate number of atoms in given masses of elements |
Experiment: Determine number of nails with mass equal to relative mass in grams. Teacher exposition: Introduce Avogadro's constant (6.023 × 10²³). Discussion: Mole as counting unit like dozen. Worked examples: Calculate moles from mass and vice versa.
|
Beam balance, Various sized nails, Scientific calculators, Avogadro's constant charts
|
KLB Secondary Chemistry Form 3, Pages 27-30
|
|
| 4 | 4 |
THE MOLE
|
Avogadro's Constant and the Mole Concept
|
By the end of the
lesson, the learner
should be able to:
Define Avogadro's constant and its value Explain the concept of a mole as a counting unit Relate molar mass to relative atomic mass Calculate number of atoms in given masses of elements |
Experiment: Determine number of nails with mass equal to relative mass in grams. Teacher exposition: Introduce Avogadro's constant (6.023 × 10²³). Discussion: Mole as counting unit like dozen. Worked examples: Calculate moles from mass and vice versa.
|
Beam balance, Various sized nails, Scientific calculators, Avogadro's constant charts
|
KLB Secondary Chemistry Form 3, Pages 27-30
|
|
| 4 | 5 |
THE MOLE
|
Interconversion of Mass and Moles for Elements
|
By the end of the
lesson, the learner
should be able to:
Apply the formula: moles = mass/molar mass Calculate mass from given moles of elements Convert between moles and number of atoms Solve numerical problems involving moles and mass |
Worked examples: Mass-mole conversions using triangle method. Supervised practice: Calculate moles in given masses of common elements. Problem solving: Convert moles to atoms using Avogadro's number. Assignment: Practice problems on interconversion.
|
Scientific calculators, Periodic table, Worked example charts, Formula triangles
|
KLB Secondary Chemistry Form 3, Pages 30-32
|
|
| 5 | 1 |
THE MOLE
|
Molecules and Moles - Diatomic Elements
|
By the end of the
lesson, the learner
should be able to:
Distinguish between atoms and molecules Define relative molecular mass Calculate moles of molecules from given mass Determine number of atoms in molecular compounds |
Discussion: Elements existing as molecules (O₂, H₂, N₂, Cl₂). Teacher exposition: Difference between atomic and molecular mass. Worked examples: Calculate moles of molecular elements. Problem solving: Number of atoms in molecular compounds.
|
Molecular models, Charts showing diatomic elements, Scientific calculators
|
KLB Secondary Chemistry Form 3, Pages 29-30
|
|
| 5 | 2 |
THE MOLE
|
Molecules and Moles - Diatomic Elements
|
By the end of the
lesson, the learner
should be able to:
Distinguish between atoms and molecules Define relative molecular mass Calculate moles of molecules from given mass Determine number of atoms in molecular compounds |
Discussion: Elements existing as molecules (O₂, H₂, N₂, Cl₂). Teacher exposition: Difference between atomic and molecular mass. Worked examples: Calculate moles of molecular elements. Problem solving: Number of atoms in molecular compounds.
|
Molecular models, Charts showing diatomic elements, Scientific calculators
|
KLB Secondary Chemistry Form 3, Pages 29-30
|
|
| 5 | 3 |
THE MOLE
|
Empirical Formula - Experimental Determination
|
By the end of the
lesson, the learner
should be able to:
Define empirical formula Determine empirical formula from experimental data Calculate mole ratios from mass data Express results as simplest whole number ratios |
Experiment: Burning magnesium in air to form magnesium oxide. Measure masses before and after reaction. Calculate moles of Mg and O from mass data. Determine mole ratio and empirical formula. Safety precautions during heating.
|
Crucible and lid, Magnesium ribbon, Bunsen burner, Beam balance, Tongs, Safety equipment
|
KLB Secondary Chemistry Form 3, Pages 32-35
|
|
| 5 | 4 |
THE MOLE
|
Empirical Formula - Reduction Method
|
By the end of the
lesson, the learner
should be able to:
Determine empirical formula using reduction reactions Calculate empirical formula from reduction data Apply reduction method to copper oxides Analyze experimental errors and sources |
Experiment: Reduction of copper(II) oxide using laboratory gas. Measure masses before and after reduction. Calculate moles of copper and oxygen. Determine empirical formula from mole ratios. Discuss experimental precautions.
|
Combustion tube, Porcelain boat, Copper(II) oxide, Laboratory gas, Beam balance, Bunsen burner
|
KLB Secondary Chemistry Form 3, Pages 35-37
|
|
| 5 | 5 |
THE MOLE
|
Empirical Formula - Reduction Method
|
By the end of the
lesson, the learner
should be able to:
Determine empirical formula using reduction reactions Calculate empirical formula from reduction data Apply reduction method to copper oxides Analyze experimental errors and sources |
Experiment: Reduction of copper(II) oxide using laboratory gas. Measure masses before and after reduction. Calculate moles of copper and oxygen. Determine empirical formula from mole ratios. Discuss experimental precautions.
|
Combustion tube, Porcelain boat, Copper(II) oxide, Laboratory gas, Beam balance, Bunsen burner
|
KLB Secondary Chemistry Form 3, Pages 35-37
|
|
| 6 | 1 |
THE MOLE
|
Empirical Formula - Percentage Composition Method
|
By the end of the
lesson, the learner
should be able to:
Calculate empirical formula from percentage composition Convert percentages to moles Determine simplest whole number ratios Apply method to various compounds |
Worked examples: Calculate empirical formula from percentage data. Method: percentage → mass → moles → ratio. Practice problems: Various compounds with different compositions. Discussion: When to multiply ratios to get whole numbers.
|
Scientific calculators, Percentage composition charts, Worked example displays
|
KLB Secondary Chemistry Form 3, Pages 37-38
|
|
| 6 | 2 |
THE MOLE
|
Empirical Formula - Percentage Composition Method
|
By the end of the
lesson, the learner
should be able to:
Calculate empirical formula from percentage composition Convert percentages to moles Determine simplest whole number ratios Apply method to various compounds |
Worked examples: Calculate empirical formula from percentage data. Method: percentage → mass → moles → ratio. Practice problems: Various compounds with different compositions. Discussion: When to multiply ratios to get whole numbers.
|
Scientific calculators, Percentage composition charts, Worked example displays
|
KLB Secondary Chemistry Form 3, Pages 37-38
|
|
| 6 | 3 |
THE MOLE
|
Molecular Formula - Determination from Empirical Formula
|
By the end of the
lesson, the learner
should be able to:
Define molecular formula Relate molecular formula to empirical formula Calculate molecular formula using molecular mass Apply the relationship (empirical formula)ₙ = molecular formula |
Teacher exposition: Difference between empirical and molecular formulas. Worked examples: Calculate molecular formula from empirical formula and molecular mass. Formula: n = molecular mass/empirical formula mass. Practice problems with various organic compounds.
|
Scientific calculators, Molecular mass charts, Worked example displays
|
KLB Secondary Chemistry Form 3, Pages 38-40
|
|
| 6 | 4 |
THE MOLE
|
Molecular Formula - Combustion Analysis
|
By the end of the
lesson, the learner
should be able to:
Determine molecular formula from combustion data Calculate moles of products in combustion Relate product moles to reactant composition Apply combustion analysis to hydrocarbons |
Worked examples: Hydrocarbon combustion producing CO₂ and H₂O. Calculate moles of C and H from product masses. Determine empirical formula, then molecular formula. Practice: Various combustion analysis problems.
|
Scientific calculators, Combustion analysis charts, Molecular models of hydrocarbons
|
KLB Secondary Chemistry Form 3, Pages 40-41
|
|
| 6 | 5 |
THE MOLE
|
Molecular Formula - Combustion Analysis
|
By the end of the
lesson, the learner
should be able to:
Determine molecular formula from combustion data Calculate moles of products in combustion Relate product moles to reactant composition Apply combustion analysis to hydrocarbons |
Worked examples: Hydrocarbon combustion producing CO₂ and H₂O. Calculate moles of C and H from product masses. Determine empirical formula, then molecular formula. Practice: Various combustion analysis problems.
|
Scientific calculators, Combustion analysis charts, Molecular models of hydrocarbons
|
KLB Secondary Chemistry Form 3, Pages 40-41
|
|
| 7 | 1 |
THE MOLE
|
Concentration and Molarity of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define concentration and molarity of solutions Calculate molarity from mass and volume data Convert between different concentration units Apply molarity calculations to various solutions |
Teacher exposition: Definition of molarity (moles/dm³). Worked examples: Calculate molarity from mass of solute and volume. Convert between g/dm³ and mol/dm³. Practice problems: Various salt solutions and their molarities.
|
Scientific calculators, Molarity charts, Various salt samples for demonstration
|
KLB Secondary Chemistry Form 3, Pages 41-43
|
|
| 7 | 2 |
THE MOLE
|
Preparation of Molar Solutions
|
By the end of the
lesson, the learner
should be able to:
Describe procedure for preparing molar solutions Use volumetric flasks correctly Calculate masses needed for specific molarities Prepare standard solutions accurately |
Experiment: Prepare 1M, 0.5M, and 0.25M NaOH solutions in different volumes. Use volumetric flasks of 1000cm³, 500cm³, and 250cm³. Calculate required masses. Demonstrate proper dissolution and dilution techniques.
|
Volumetric flasks (250, 500, 1000cm³), Sodium hydroxide pellets, Beam balance, Wash bottles, Beakers
|
KLB Secondary Chemistry Form 3, Pages 43-46
|
|
| 7 |
Midterm Break |
|||||||
| 8 | 1 |
THE MOLE
|
Dilution of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define dilution process Apply dilution formula M₁V₁ = M₂V₂ Calculate concentrations after dilution Prepare dilute solutions from concentrated ones |
Experiment: Dilute 25cm³ of 2M HCl to different final volumes (250cm³ and 500cm³). Calculate resulting concentrations. Worked examples using dilution formula. Safety precautions when diluting acids.
|
Volumetric flasks, Hydrochloric acid (2M), Measuring cylinders, Pipettes, Safety equipment
|
KLB Secondary Chemistry Form 3, Pages 46-50
|
|
| 8 | 2 |
THE MOLE
|
Dilution of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define dilution process Apply dilution formula M₁V₁ = M₂V₂ Calculate concentrations after dilution Prepare dilute solutions from concentrated ones |
Experiment: Dilute 25cm³ of 2M HCl to different final volumes (250cm³ and 500cm³). Calculate resulting concentrations. Worked examples using dilution formula. Safety precautions when diluting acids.
|
Volumetric flasks, Hydrochloric acid (2M), Measuring cylinders, Pipettes, Safety equipment
|
KLB Secondary Chemistry Form 3, Pages 46-50
|
|
| 8 | 3 |
THE MOLE
|
Dilution of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define dilution process Apply dilution formula M₁V₁ = M₂V₂ Calculate concentrations after dilution Prepare dilute solutions from concentrated ones |
Experiment: Dilute 25cm³ of 2M HCl to different final volumes (250cm³ and 500cm³). Calculate resulting concentrations. Worked examples using dilution formula. Safety precautions when diluting acids.
|
Volumetric flasks, Hydrochloric acid (2M), Measuring cylinders, Pipettes, Safety equipment
|
KLB Secondary Chemistry Form 3, Pages 46-50
|
|
| 8 | 4 |
THE MOLE
|
Stoichiometry - Experimental Determination of Equations
|
By the end of the
lesson, the learner
should be able to:
Determine chemical equations from experimental data Calculate mole ratios from mass measurements Write balanced chemical equations Apply stoichiometry to displacement reactions |
Experiment: Iron displacement of copper from CuSO₄ solution. Measure masses of iron used and copper displaced. Calculate mole ratios. Derive balanced chemical equation. Discuss spectator ions.
|
Iron filings, Copper(II) sulphate solution, Beam balance, Beakers, Filter equipment
|
KLB Secondary Chemistry Form 3, Pages 50-53
|
|
| 8 | 5 |
THE MOLE
|
Stoichiometry - Precipitation Reactions
|
By the end of the
lesson, the learner
should be able to:
Investigate stoichiometry of precipitation reactions Determine mole ratios from volume measurements Write ionic equations for precipitation Analyze limiting and excess reagents |
Experiment: Pb(NO₃)₂ + KI precipitation reaction. Use different volumes to determine stoichiometry. Measure precipitate heights. Plot graphs to find reaction ratios. Identify limiting reagents.
|
Test tubes, Lead(II) nitrate solution, Potassium iodide solution, Burettes, Ethanol, Rulers
|
KLB Secondary Chemistry Form 3, Pages 53-56
|
|
| 9 | 1 |
THE MOLE
|
Stoichiometry - Gas Evolution Reactions
|
By the end of the
lesson, the learner
should be able to:
Determine stoichiometry of gas-producing reactions Collect and measure gas volumes Calculate mole ratios involving gases Write equations for acid-carbonate reactions |
Experiment: HCl + Na₂CO₃ reaction. Collect CO₂ gas in plastic bag. Measure gas mass and calculate moles. Determine mole ratios of reactants and products. Write balanced equation.
|
Conical flask, Thistle funnel, Plastic bags, Rubber bands, Sodium carbonate, HCl solution
|
KLB Secondary Chemistry Form 3, Pages 56-58
|
|
| 9 | 2 |
THE MOLE
|
Stoichiometry - Gas Evolution Reactions
|
By the end of the
lesson, the learner
should be able to:
Determine stoichiometry of gas-producing reactions Collect and measure gas volumes Calculate mole ratios involving gases Write equations for acid-carbonate reactions |
Experiment: HCl + Na₂CO₃ reaction. Collect CO₂ gas in plastic bag. Measure gas mass and calculate moles. Determine mole ratios of reactants and products. Write balanced equation.
|
Conical flask, Thistle funnel, Plastic bags, Rubber bands, Sodium carbonate, HCl solution
|
KLB Secondary Chemistry Form 3, Pages 56-58
|
|
| 9 | 3 |
THE MOLE
|
Volumetric Analysis - Introduction and Apparatus
|
By the end of the
lesson, the learner
should be able to:
Define volumetric analysis and titration Identify and use titration apparatus correctly Explain functions of pipettes and burettes Demonstrate proper reading techniques |
Practical session: Familiarization with pipettes and burettes. Practice filling and reading burettes accurately. Learn proper meniscus reading. Use pipette fillers safely. Rinse apparatus with appropriate solutions.
|
Pipettes (10, 20, 25cm³), Burettes (50cm³), Pipette fillers, Conical flasks, Various solutions
|
KLB Secondary Chemistry Form 3, Pages 58-59
|
|
| 9 | 4 |
THE MOLE
|
Volumetric Analysis - Introduction and Apparatus
|
By the end of the
lesson, the learner
should be able to:
Define volumetric analysis and titration Identify and use titration apparatus correctly Explain functions of pipettes and burettes Demonstrate proper reading techniques |
Practical session: Familiarization with pipettes and burettes. Practice filling and reading burettes accurately. Learn proper meniscus reading. Use pipette fillers safely. Rinse apparatus with appropriate solutions.
|
Pipettes (10, 20, 25cm³), Burettes (50cm³), Pipette fillers, Conical flasks, Various solutions
|
KLB Secondary Chemistry Form 3, Pages 58-59
|
|
| 9 | 5 |
THE MOLE
|
Titration - Acid-Base Neutralization
|
By the end of the
lesson, the learner
should be able to:
Perform acid-base titrations accurately Use indicators to determine end points Record titration data properly Calculate average titres from multiple readings |
Experiment: Titrate 25cm³ of 0.1M NaOH with 0.1M HCl using phenolphthalein. Repeat three times for consistency. Record data in tabular form. Calculate average titre. Discuss accuracy and precision.
|
Burettes, Pipettes, 0.1M NaOH, 0.1M HCl, Phenolphthalein indicator, Conical flasks
|
KLB Secondary Chemistry Form 3, Pages 59-62
|
|
| 10 | 1 |
THE MOLE
|
Titration - Diprotic Acids
|
By the end of the
lesson, the learner
should be able to:
Investigate titrations involving diprotic acids Determine basicity of acids from titration data Compare volumes needed for mono- and diprotic acids Write equations for diprotic acid reactions |
Experiment: Titrate 25cm³ of 0.1M NaOH with 0.1M H₂SO₄. Compare volume used with previous HCl titration. Calculate mole ratios. Explain concept of basicity. Introduce dibasic and tribasic acids.
|
Burettes, Pipettes, 0.1M H₂SO₄, 0.1M NaOH, Phenolphthalein, Basicity reference chart
|
KLB Secondary Chemistry Form 3, Pages 62-65
|
|
| 10 | 2 |
THE MOLE
|
Titration - Diprotic Acids
|
By the end of the
lesson, the learner
should be able to:
Investigate titrations involving diprotic acids Determine basicity of acids from titration data Compare volumes needed for mono- and diprotic acids Write equations for diprotic acid reactions |
Experiment: Titrate 25cm³ of 0.1M NaOH with 0.1M H₂SO₄. Compare volume used with previous HCl titration. Calculate mole ratios. Explain concept of basicity. Introduce dibasic and tribasic acids.
|
Burettes, Pipettes, 0.1M H₂SO₄, 0.1M NaOH, Phenolphthalein, Basicity reference chart
|
KLB Secondary Chemistry Form 3, Pages 62-65
|
|
| 10 | 3 |
THE MOLE
|
Standardization of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define standardization process Standardize HCl using Na₂CO₃ as primary standard Calculate accurate concentrations from titration data Understand importance of primary standards |
Experiment: Prepare approximately 0.1M HCl and standardize using accurately weighed Na₂CO₃. Use methyl orange indicator. Calculate exact molarity from titration results. Discuss primary standard requirements.
|
Anhydrous Na₂CO₃, Approximately 0.1M HCl, Methyl orange, Volumetric flasks, Analytical balance
|
KLB Secondary Chemistry Form 3, Pages 65-67
|
|
| 10 | 4 |
THE MOLE
|
Standardization of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define standardization process Standardize HCl using Na₂CO₃ as primary standard Calculate accurate concentrations from titration data Understand importance of primary standards |
Experiment: Prepare approximately 0.1M HCl and standardize using accurately weighed Na₂CO₃. Use methyl orange indicator. Calculate exact molarity from titration results. Discuss primary standard requirements.
|
Anhydrous Na₂CO₃, Approximately 0.1M HCl, Methyl orange, Volumetric flasks, Analytical balance
|
KLB Secondary Chemistry Form 3, Pages 65-67
|
|
| 10 | 5 |
THE MOLE
|
Back Titration Method
|
By the end of the
lesson, the learner
should be able to:
Understand principle of back titration Apply back titration to determine composition Calculate concentrations using back titration data Determine atomic masses from back titration |
Experiment: Determine atomic mass of divalent metal in MCO₃. Add excess HCl to carbonate, then titrate excess with NaOH. Calculate moles of acid that reacted with carbonate. Determine metal's atomic mass.
|
Metal carbonate sample, 0.5M HCl, 0M NaOH, Phenolphthalein, Conical flasks
|
KLB Secondary Chemistry Form 3, Pages 67-70
|
|
| 11 | 1 |
THE MOLE
|
Redox Titrations - Principles
|
By the end of the
lesson, the learner
should be able to:
Explain principles of redox titrations Identify color changes in redox reactions Understand self-indicating nature of some redox reactions Write ionic equations for redox processes |
Teacher exposition: Redox titration principles. Demonstrate color changes: MnO₄⁻ (purple) → Mn²⁺ (colorless), Cr₂O₇²⁻ (orange) → Cr³⁺ (green). Discussion: Self-indicating reactions. Write half-equations and overall ionic equations.
|
Potassium manganate(VII), Potassium dichromate(VI), Iron(II) solutions, Color change charts
|
KLB Secondary Chemistry Form 3, Pages 68-70
|
|
| 11 | 2 |
THE MOLE
|
Redox Titrations - Principles
|
By the end of the
lesson, the learner
should be able to:
Explain principles of redox titrations Identify color changes in redox reactions Understand self-indicating nature of some redox reactions Write ionic equations for redox processes |
Teacher exposition: Redox titration principles. Demonstrate color changes: MnO₄⁻ (purple) → Mn²⁺ (colorless), Cr₂O₇²⁻ (orange) → Cr³⁺ (green). Discussion: Self-indicating reactions. Write half-equations and overall ionic equations.
|
Potassium manganate(VII), Potassium dichromate(VI), Iron(II) solutions, Color change charts
|
KLB Secondary Chemistry Form 3, Pages 68-70
|
|
| 11 | 3 |
THE MOLE
|
Redox Titrations - KMnO₄ Standardization
|
By the end of the
lesson, the learner
should be able to:
Standardize KMnO₄ solution using iron(II) salt Calculate molarity from redox titration data Apply 1:5 mole ratio in calculations Prepare solutions for redox titrations |
Experiment: Standardize KMnO₄ using FeSO₄(NH₄)₂SO₄·6H₂O. Dissolve iron salt in boiled, cooled water. Titrate with KMnO₄ until persistent pink color. Calculate molarity using 5:1 mole ratio.
|
Iron(II) ammonium sulfate, KMnO₄ solution, Dilute H₂SO₄, Pipettes, Burettes
|
KLB Secondary Chemistry Form 3, Pages 70-72
|
|
| 11 | 4 |
THE MOLE
|
Redox Titrations - KMnO₄ Standardization
|
By the end of the
lesson, the learner
should be able to:
Standardize KMnO₄ solution using iron(II) salt Calculate molarity from redox titration data Apply 1:5 mole ratio in calculations Prepare solutions for redox titrations |
Experiment: Standardize KMnO₄ using FeSO₄(NH₄)₂SO₄·6H₂O. Dissolve iron salt in boiled, cooled water. Titrate with KMnO₄ until persistent pink color. Calculate molarity using 5:1 mole ratio.
|
Iron(II) ammonium sulfate, KMnO₄ solution, Dilute H₂SO₄, Pipettes, Burettes
|
KLB Secondary Chemistry Form 3, Pages 70-72
|
|
| 11 | 5 |
THE MOLE
|
Water of Crystallization Determination
|
By the end of the
lesson, the learner
should be able to:
Determine water of crystallization in hydrated salts Use redox titration to find formula of hydrated salt Calculate value of 'n' in crystallization formulas Apply analytical data to determine complete formulas |
Experiment: Determine 'n' in FeSO₄(NH₄)₂SO₄·nH₂O. Dissolve known mass in acid, titrate with standardized KMnO₄. Calculate moles of iron(II), hence complete formula. Compare theoretical and experimental values.
|
Hydrated iron(II) salt, Standardized KMnO₄, Dilute H₂SO₄, Analytical balance
|
KLB Secondary Chemistry Form 3, Pages 72-73
|
|
| 12 | 1 |
THE MOLE
|
Atomicity and Molar Gas Volume
|
By the end of the
lesson, the learner
should be able to:
Define atomicity of gaseous elements Classify gases as monoatomic, diatomic, or triatomic Determine molar gas volume experimentally Calculate gas densities and molar masses |
Experiment: Measure volumes and masses of different gases (O₂, CO₂, Cl₂). Calculate densities and molar masses. Determine volume occupied by one mole. Compare values at different conditions.
|
Gas syringes (50cm³), Various gases, Analytical balance, Gas supply apparatus
|
KLB Secondary Chemistry Form 3, Pages 73-75
|
|
| 12 | 2 |
THE MOLE
|
Atomicity and Molar Gas Volume
|
By the end of the
lesson, the learner
should be able to:
Define atomicity of gaseous elements Classify gases as monoatomic, diatomic, or triatomic Determine molar gas volume experimentally Calculate gas densities and molar masses |
Experiment: Measure volumes and masses of different gases (O₂, CO₂, Cl₂). Calculate densities and molar masses. Determine volume occupied by one mole. Compare values at different conditions.
|
Gas syringes (50cm³), Various gases, Analytical balance, Gas supply apparatus
|
KLB Secondary Chemistry Form 3, Pages 73-75
|
|
| 12 | 3 |
THE MOLE
|
Combining Volumes of Gases - Experimental Investigation
|
By the end of the
lesson, the learner
should be able to:
Investigate Gay-Lussac's law experimentally Measure combining volumes of reacting gases Determine simple whole number ratios Write equations from volume relationships |
Experiment: React NH₃ and HCl gases in measured volumes. Observe formation of NH₄Cl solid. Measure residual gas volumes. Determine combining ratios. Apply to other gas reactions.
|
Gas syringes, Dry NH₃ generator, Dry HCl generator, Glass connecting tubes, Clips
|
KLB Secondary Chemistry Form 3, Pages 75-77
|
|
| 12 | 4 |
THE MOLE
|
Gas Laws and Chemical Equations
|
By the end of the
lesson, the learner
should be able to:
Apply Avogadro's law to chemical reactions Use volume ratios to determine chemical equations Calculate product volumes from reactant volumes Solve problems involving gas stoichiometry |
Worked examples: Use Gay-Lussac's law to determine equations. Calculate volumes of products from given reactant volumes. Apply Avogadro's law to find number of molecules. Practice: Complex gas stoichiometry problems.
|
Scientific calculators, Gas law charts, Volume ratio examples
|
KLB Secondary Chemistry Form 3, Pages 77-79
|
|
| 12 | 5 |
THE MOLE
|
Gas Laws and Chemical Equations
|
By the end of the
lesson, the learner
should be able to:
Apply Avogadro's law to chemical reactions Use volume ratios to determine chemical equations Calculate product volumes from reactant volumes Solve problems involving gas stoichiometry |
Worked examples: Use Gay-Lussac's law to determine equations. Calculate volumes of products from given reactant volumes. Apply Avogadro's law to find number of molecules. Practice: Complex gas stoichiometry problems.
|
Scientific calculators, Gas law charts, Volume ratio examples
|
KLB Secondary Chemistry Form 3, Pages 77-79
|
|
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