KASEMPA DAY SECONDARY
Grade/Level: SSS1 Number of Pupils in Class: 60 Date: 16/07/2026 Duration: 40 minutes
Name of Teacher: Mr Masumba
Subject: Chemistry Theme: The Chemical World
Topic: Acids, Bases and Salts
Learning Outcome:
- Recognize natural sources of acids, bases and salts and their importance in everyday life
Focal Competence:
- Identifying acids, bases and salts in substances
Performance Objective(s):
By the end of the lesson, learners should be able to:
- Identify and prepare salts such as normal, acidic and basic salts.
Key Competencies and Values:
- Critical thinking: students interpret information and draw conclusions while testing for acids and bases, preparing indicators and testing solubility of substances.
- Communication: students communicate clearly through reports of investigations, equations of reactions and other activities.
Prerequisite Knowledge:
- Acids and bases definitions and examples.
- Neutralization reaction: acid + base → salt + water.
References:
- Osei Yaw Ababio, New School Chemistry for Senior Secondary Schools, Africana First Publishers.
- NERDC Senior Secondary Chemistry Curriculum, SSS1-3.
- Chemistry Made Easy for Senior Secondary Schools by S.O. Onyeidu.
Teaching and Learning Resources:
- Ripe and unripe fruits
- Sour milk
- Flowers and leaves of plants
- Chemicals such as NaOH, KOH, HCl and H2SO4
- Distilled water
- Acetone
- Ethanol
- Filter paper
- Mortar and pestle
- Litmus paper
- Universal indicator
- Phenolphthalein
- Methyl orange
- Beakers
- Test tubes
- pH meter
- Bunsen burner
- Smart phones
- Functional computers with Internet facility
- Power source
METHODOLOGIES, STRATEGIES AND APPROACHES:
Approach: Concept Development Approach
Method:
- Discussion Method - Introduction
- Demonstration Method - Development Step 1, Step 2
- Group Work - Step 3
Strategy:
- Visual Aids Strategy - Development Step 1, Step 2
- Cooperative Learning Strategy - Step 3
Lesson Implementation:
| Stage | Teaching Methods | Teacher Activities | Learner Activities | Learning Points |
|---|---|---|---|---|
| Introduction - 5 min | Discussion Method | Teacher asks learners to recall what happens when an acid reacts with a base, and writes their responses on the board. Teacher then states the focus for the lesson: types of salts and how to prepare them. | Learners recall that an acid and a base react to form salt and water only. They express readiness to learn about salt types and preparation. | Neutralization is the reaction between an acid and a base to produce salt and water only. The salt formed can be normal, acidic, or basic depending on the completeness of the reaction. |
| Development Step 1 - 10 min | Demonstration Method | Teacher displays a drawn chart showing definitions and examples of normal, acidic, and basic salts. Teacher explains each type, pointing to the chart: a normal salt has all replaceable H⁺ of the acid replaced by a metal or ammonium ion (e.g., NaCl, KNO₃, CuSO₄); an acidic salt contains replaceable H⁺ ions and is formed by partial neutralization of a polybasic acid (e.g., NaHSO₄, NaHCO₃); a basic salt contains replaceable OH⁻ ions, formed by incomplete neutralization of a polyacidic base (e.g., Pb(OH)Cl, Mg(OH)NO₃). Teacher asks learners to classify given salt formulas on the chart. | Learners observe the chart, copy the definitions and examples, and classify the salts: NaCl as normal, NaHSO₄ as acidic, Pb(OH)Cl as basic. They answer the teacher's classification questions correctly. | Types of Salts: 1. Normal Salt – formed by complete replacement of all replaceable hydrogen ions of an acid by a metal or ammonium ion. Examples: NaCl, KNO₃, CuSO₄. 2. Acidic Salt – contains replaceable hydrogen ions; formed when a polybasic acid is partially neutralised. Examples: NaHSO₄ (sodium hydrogen sulphate), NaHCO₃ (sodium hydrogen carbonate). 3. Basic Salt – contains replaceable hydroxide ions; formed when a polyacidic base is incompletely neutralised. Examples: Pb(OH)Cl (lead(II) hydroxide chloride), Mg(OH)NO₃ (magnesium hydroxide nitrate). |
| Step 2 - 10 min | Demonstration Method | Teacher uses a drawn chart illustrating the preparation of normal salts: reaction between dilute HCl and NaOH to produce NaCl, and reaction between CuO and dilute H₂SO₄ to produce CuSO₄. Teacher writes the word and symbolic equations on the board and asks learners to identify the type of salt formed. Teacher then challenges learners to write the equation for preparing an acidic salt using NaOH and H₂SO₄ in a 1:1 mole ratio, and a basic salt using Pb(OH)₂ and HCl. | Learners observe the illustrated reactions, copy the equations, and state that NaCl and CuSO₄ are normal salts. They write the equation for the acidic salt: NaOH + H₂SO₄ → NaHSO₄ + H₂O, and for the basic salt: Pb(OH)₂ + HCl → Pb(OH)Cl + H₂O, and classify these products accordingly. | Preparation of Salts by Neutralisation: - Normal salt (NaCl): HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) (complete neutralisation). - Normal salt (CuSO₄): CuO(s) + H₂SO₄(aq) → CuSO₄(aq) + H₂O(l). - Acidic salt (NaHSO₄): H₂SO₄(aq) + NaOH(aq) → NaHSO₄(aq) + H₂O(l) (1:1 ratio, partial neutralisation). - Basic salt (Pb(OH)Cl): Pb(OH)₂(s) + HCl(aq) → Pb(OH)Cl(s) + H₂O(l) (incomplete neutralisation). |
| Step 3 - 10 min | Group Work | Teacher distributes drawn cards containing formulas of various salts (e.g., KNO₃, NaHCO₃, Ca(OH)Cl, KHSO₄, Mg(OH)NO₃) to small groups. Teacher instructs groups to classify each salt as normal, acidic, or basic and to write a chemical equation for the preparation of one salt of each type. Teacher moves around to guide. | In groups, learners examine the cards, classify KNO₃ as normal, NaHCO₃ and KHSO₄ as acidic, Ca(OH)Cl and Mg(OH)NO₃ as basic. They prepare a summary: e.g., normal salt: KOH + HNO₃ → KNO₃ + H₂O; acidic salt: H₂CO₃ + NaOH → NaHCO₃ + H₂O; basic salt: Ca(OH)₂ + HCl → Ca(OH)Cl + H₂O. A group representative presents findings. | Application of classification and preparation: - KNO₃ is a normal salt because all H⁺ of HNO₃ are replaced. - NaHCO₃ and KHSO₄ are acidic salts because they still contain replaceable H⁺. - Ca(OH)Cl and Mg(OH)NO₃ are basic salts because they contain replaceable OH⁻. - Preparation equations confirm these types (examples shown above). |
| Evaluation questions - 5 min | Discussion Method | Teacher asks the following questions orally and instructs learners to write answers in their notebooks: 1. Write a word and balanced chemical equation for the preparation of copper(II) sulphate from copper(II) oxide and sulphuric acid. State the type of salt formed. 2. Identify whether the following are normal, acidic, or basic salts: (a) KNO₃ (b) NaHCO₃ (c) Ca(OH)Cl. 3. Describe how you would prepare an acidic salt using sodium hydroxide and sulphuric acid, giving the chemical equation. | Learners write: 1. Copper(II) oxide + sulphuric acid → copper(II) sulphate + water; CuO + H₂SO₄ → CuSO₄ + H₂O; it is a normal salt. 2. (a) KNO₃ – normal, (b) NaHCO₃ – acidic, (c) Ca(OH)Cl – basic. 3. Add dilute sulphuric acid to sodium hydroxide solution in a 1:1 mole ratio, evaporate to obtain sodium hydrogen sulphate crystals; H₂SO₄ + NaOH → NaHSO₄ + H₂O. | Assessment of performance objective: Learners successfully identify salt types and write preparation equations. Salts can be classified based on the presence of replaceable H⁺ or OH⁻ ions. Preparation typically involves neutralisation reactions. |
Lesson Evaluation:
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