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O Level Chemistry Acids Bases Salts Quiz
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Questions
O-Level Chemistry Quiz - Acids Bases Salts
Name: _________________ Class: _________ Date: _________
Score: _____ / 35 Duration: 45 minutes
Instructions:
- Answer all questions in the spaces provided
- Show all working for calculations
- Use appropriate chemical formulae and equations
- This quiz covers acids, bases and salts topics
Section A: Short Answer Questions [15 marks]
1. Define the term "weak acid". [2 marks]
2. State the pH range that would be shown by a strong alkali using Universal Indicator. [1 mark]
3. Complete the word equation for neutralisation: [1 mark]
acid + base → _____________ + _____________
4. Name the salt formed when magnesium carbonate reacts with nitric acid. [1 mark]
5. State two observations when zinc is added to dilute hydrochloric acid. [2 marks]
(i) _________________________________________________
(ii) _________________________________________________
6. Explain why copper does not react with dilute sulfuric acid. [2 marks]
7. Name a suitable drying agent for ammonia gas. [1 mark]
8. State the test for carbon dioxide gas. [2 marks]
Test: _________________________________________________
Positive result: _________________________________________________
9. Complete the ionic equation for neutralisation: [2 marks]
_______ + _______ → H₂O
10. Name the type of oxide formed by non-metals. [1 mark]
Section B: Structured Questions [20 marks]
11. A student wants to prepare pure, dry crystals of copper(II) sulfate from copper(II) oxide and dilute sulfuric acid. [6 marks]
(a) Write a balanced chemical equation for this reaction. [2 marks]
(b) Describe the method the student should use to prepare the pure, dry crystals. [4 marks]
Step 1: _________________________________________________
Step 2: _________________________________________________
Step 3: _________________________________________________
Step 4: _________________________________________________
12. The table shows the pH values of four solutions. [8 marks]
| Solution | pH |
|---|---|
| P | 2 |
| Q | 7 |
| R | 9 |
| S | 13 |
(a) Which solution is neutral? [1 mark]
(b) Which solution is the strongest acid? [1 mark]
(c) Which solution would turn red litmus paper blue? [1 mark]
(d) Solutions P and S are mixed in equal volumes. Predict the pH of the resulting mixture and explain your answer. [3 marks]
pH: _________________________________________________
Explanation: _________________________________________________
(e) Name a suitable indicator to distinguish between solutions R and S. [1 mark]
(f) State what happens to the pH when solution P is diluted with distilled water. [1 mark]
13. Ethanoic acid is a weak acid found in vinegar. [6 marks]
(a) Write the chemical formula of ethanoic acid. [1 mark]
(b) Write a balanced chemical equation for the reaction between ethanoic acid and sodium hydroxide. [2 marks]
(c) Explain why ethanoic acid has a higher pH than hydrochloric acid of the same concentration. [3 marks]
END OF QUIZ
Answers
O-Level Chemistry Quiz - Acids Bases Salts - ANSWERS
Section A: Short Answer Questions [15 marks]
1. Define the term "weak acid". [2 marks]
Answer: A weak acid is one that only partially ionizes/dissociates in aqueous solution [1]. Only a small fraction of the acid molecules release H⁺ ions [1].
Marking notes: Accept "partially ionizes" or "partially dissociates". Must mention incomplete ionization for full marks.
2. State the pH range that would be shown by a strong alkali using Universal Indicator. [1 mark]
Answer: pH 12-14 [1]
Marking notes: Accept any range within 12-14. Do not accept pH >7 as too vague.
3. Complete the word equation for neutralisation: [1 mark]
Answer: acid + base → salt + water [1]
Marking notes: Both words needed for the mark.
4. Name the salt formed when magnesium carbonate reacts with nitric acid. [1 mark]
Answer: Magnesium nitrate [1]
Marking notes: Accept Mg(NO₃)₂ as alternative.
5. State two observations when zinc is added to dilute hydrochloric acid. [2 marks]
Answer: (i) Effervescence/bubbles/fizzing [1] (ii) Zinc dissolves/disappears [1]
Marking notes: Accept "gas evolved" for (i). Accept "zinc gets smaller" for (ii).
6. Explain why copper does not react with dilute sulfuric acid. [2 marks]
Answer: Copper is below hydrogen in the reactivity series [1], so it cannot displace hydrogen from acids [1].
Marking notes: Must mention reactivity series and position relative to hydrogen for full marks.
7. Name a suitable drying agent for ammonia gas. [1 mark]
Answer: Calcium oxide / CaO [1]
Marking notes: Accept "quicklime". Do not accept concentrated sulfuric acid (reacts with ammonia).
8. State the test for carbon dioxide gas. [2 marks]
Answer: Test: Bubble through limewater/calcium hydroxide solution [1] Positive result: Limewater turns milky/cloudy [1]
Marking notes: Both parts needed. Accept Ca(OH)₂ for limewater.
9. Complete the ionic equation for neutralisation: [2 marks]
Answer: H⁺ + OH⁻ → H₂O [2]
Marking notes: Both ions needed with correct charges for full marks.
10. Name the type of oxide formed by non-metals. [1 mark]
Answer: Acidic oxide [1]
Marking notes: Do not accept just "oxide".
Section B: Structured Questions [20 marks]
11. A student wants to prepare pure, dry crystals of copper(II) sulfate from copper(II) oxide and dilute sulfuric acid. [6 marks]
(a) Write a balanced chemical equation for this reaction. [2 marks]
Answer: CuO + H₂SO₄ → CuSO₄ + H₂O [2]
Marking notes: Correct formulae [1], balanced equation [1]. Accept state symbols as bonus.
(b) Describe the method the student should use to prepare the pure, dry crystals. [4 marks]
Answer:
Step 1: Add excess copper(II) oxide to dilute sulfuric acid until no more dissolves [1]
Step 2: Filter to remove unreacted copper(II) oxide [1]
Step 3: Heat the filtrate gently to evaporate water until crystals start to form/concentrate the solution [1]
Step 4: Allow to cool and crystallize, then filter and dry the crystals [1]
Marking notes: Key points: excess reactant, filtration, evaporation/concentration, crystallization. Accept washing crystals with distilled water.
12. The table shows the pH values of four solutions. [8 marks]
(a) Which solution is neutral? [1 mark]
Answer: Q [1]
(b) Which solution is the strongest acid? [1 mark]
Answer: P [1]
(c) Which solution would turn red litmus paper blue? [1 mark]
Answer: R and S [1]
Marking notes: Accept either R or S or both.
(d) Solutions P and S are mixed in equal volumes. Predict the pH of the resulting mixture and explain your answer. [3 marks]
Answer: pH: Around 7/neutral [1] Explanation: P is a strong acid (pH 2) and S is a strong alkali (pH 13) [1]. When mixed in equal volumes, they neutralize each other to form salt and water [1].
Marking notes: pH must be around 7. Explanation must mention neutralization.
(e) Name a suitable indicator to distinguish between solutions R and S. [1 mark]
Answer: Phenolphthalein [1]
Marking notes: Accept any indicator that changes color between pH 9-13. Universal indicator also acceptable.
(f) State what happens to the pH when solution P is diluted with distilled water. [1 mark]
Answer: pH increases/becomes less acidic [1]
Marking notes: Accept "moves towards 7" or "becomes higher".
13. Ethanoic acid is a weak acid found in vinegar. [6 marks]
(a) Write the chemical formula of ethanoic acid. [1 mark]
Answer: CH₃COOH [1]
Marking notes: Accept C₂H₄O₂. Do not accept CH₃COO⁻.
(b) Write a balanced chemical equation for the reaction between ethanoic acid and sodium hydroxide. [2 marks]
Answer: CH₃COOH + NaOH → CH₃COONa + H₂O [2]
Marking notes: Correct formulae [1], balanced equation [1].
(c) Explain why ethanoic acid has a higher pH than hydrochloric acid of the same concentration. [3 marks]
Answer: Ethanoic acid is a weak acid that only partially ionizes in water [1], producing fewer H⁺ ions than hydrochloric acid [1]. Hydrochloric acid is a strong acid that completely ionizes, so it has a higher concentration of H⁺ ions and therefore lower pH [1].
Marking notes: Must mention partial vs complete ionization and relate to H⁺ ion concentration for full marks.
Total: 35 marks