| Method |
Precise Learning Objective |
Linked |
Question / Activity
(Designed for maximum working out) |
Stepping Stones |
Pitstop Check
(Thinking Map) |
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(WS) Students should be able to describe the use of universal indicator or a wide range indicator to measure the approximate pH of a solution |
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In what way can universal indicator be used to measure the approximate pH of a solution? |
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(WS) Students should be able to use the pH scale to identify acidic or alkaline solutions. |
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If a substance has the following pH is it classified as acid, alkali or neutral:
1) pH 3
2) pH 11
3) pH 7 |
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Aqueous solutions of alkalis contain hydroxide ions (OH-). |
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What ions are produced in alkalis in aqueous solutions? |
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A strong acid is completely ionised in aqueous solution. Examples of strong acids are hydrochloric, nitric and sulfuric acids. |
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What happens to strong acids in an aqueous solution in terms of ionisation? |
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A weak acid is only partially ionised in aqueous solution. Examples of weak acids are ethanoic, citric and carbonic acids. |
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What happens to weak acids in an aqueous solution in terms of ionisation? |
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Acids produce hydrogen ions (H ) in aqueous solutions. |
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What ions are produced in acids in aqueous solutions? |
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For a given concentration of aqueous solutions, the stronger an acid, the lower the pH. |
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When an acid is stronger, what effect does this have on the pH? |
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As the pH decreases by one unit, the hydrogen ion concentration of the solution increases by a factor of 10. |
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What happens to the hydrogen ion concentration of a solution when pH decreases by one unit? |
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Students should be able to use and explain the terms dilute and concentrated (in terms of amount of substance), and weak and strong (in terms of the degree of ionisation) in relation to acids |
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What is meant by 'dilute' and 'concentrated' (in terms of amount of substance) and 'weak acid' and 'strong acid' (in terms of the degree of ionisation)? |
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Students should be able to describe neutrality and relative acidity in terms of the effect on hydrogen ion concentration and the numerical value of pH (whole numbers only). |
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