1.1.1 define acids and bases and state their properties.
Acids as proton donors Bases as proton acceptors.
Physical and chemical properties of acids and bases.
Brainstorm to bring out the definitions of acids and bases.
Discuss the properties and uses of acids and bases.
perform the following chemical tests to show the properties of acids and bases:
(a) Reaction of acid and base (neutralization reaction).
(b) Dilute acid + metal (production of H2 gas)
(c) Acid + trioxocarbonate (IV) compounds (production of CO2 gas).
(d) Reaction of a base and an ammonium salt (production of NH3 gas)
(a) Reaction of acid and base (neutralization reaction).
(b) Dilute acid + metal (production of H2 gas)
(c) Acid + trioxocarbonate (IV) compounds (production of CO2 gas).
(d) Reaction of a base and an ammonium salt (production of NH3 gas)
Test for hydrogen, carbon dioxide and ammonia gases.
Write word equation for reactions between a named:
i. Acid and metal.
ii. Base and ammonium salt.
i. Acid and metal.
ii. Base and ammonium salt.
Describe the laboratory preparation of NH3 gas. How would you test for Ammonia.
1.1.2 identify common chemical substances as acids or bases and classify them according to their sources and uses.
Acids and bases, e.g. Organic acids – vinegar,
Organic bases - ammonia,
Inorganic acids – dilute HCl
Inorganic base – milk of magnesia
Organic bases - ammonia,
Inorganic acids – dilute HCl
Inorganic base – milk of magnesia
Perform chemical tests to classify each chemical substance listed under the content as an acid or a base.
Discuss the uses of acids and bases in everyday life and in industry, e.g. sodium hydroxide and tetraoxosulphate(VI) acid.
Give two uses each of sodium Hydroxide (NaOH) and tetraoxosulphate (VI) acid (H2SO4) aq.
1.1.3 prepare salts.
Methods of preparation of salts.
prepare salts using any of the following methods:
neutralization, precipitation, acid decomposition of trioxocarbonate (IV) salt.
neutralization, precipitation, acid decomposition of trioxocarbonate (IV) salt.
Visit a salt/chemical industry and write a group report on the activities observed. Present your report to the class.
1.1.4 describe the effect of acid – base indicators.
describe the colours developed by phenolphthalein, litmus and methyl orange in aqueous solutions of dilute acids, dilute bases, dilute sodium chloride, distilled water and common fruit juice, e.g. citrus.
1.1.5 use universal indicators and the pHmeter to determine the pH of given solutions.
Determination of pH of given solutions.
Determination of soil pH.
discuss the use of the universal indicator and the pH-meter in the determination of the pH of common household chemicals, e.g. vinegar, palm oil, shampoo and local soap.
use colours developed by the universal indicator to deduce the pH of acidic, neutral and basic solutions.
NOTE:
Point out the limitations of the use of the pH scale for highly dilute/concentrated solutions: Their pH are outside pH = 0 to pH = 14.
Point out the limitations of the use of the pH scale for highly dilute/concentrated solutions: Their pH are outside pH = 0 to pH = 14.
1. Explain how to determine the pH of a given solution.
2. Which is more acidic: a solution of pH = 1 or a solution of pH = 9
3. Explain why the use of universal indicator in determining the pH of solution does not work well with coloured solutions?
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2. Which is more acidic: a solution of pH = 1 or a solution of pH = 9
3. Explain why the use of universal indicator in determining the pH of solution does not work well with coloured solutions?
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