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Secondary 4 Pure Chemistry Acids Bases Salts Quiz

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Questions

Secondary 4 Pure Chemistry Quiz - Acids Bases Salts

Name: __________________________
Class: __________________________
Date: __________________________
Score: ________ / 40

Duration: 45 minutes
Total Marks: 40

Instructions:

Answer all questions.
Write your answers in the spaces provided.
The number of marks is indicated in brackets [ ] at the end of each question or part question.
You may use a calculator.

Section A: Multiple Choice & Short Concepts (10 Marks)

1. Which of the following statements correctly describes a strong acid?
A. It has a high concentration of hydrogen ions.
B. It is completely ionised in water.
C. It reacts vigorously with all metals.
D. It has a pH value close to 7.
[1]

2. A student tests a solution with universal indicator. The solution turns red. Which of the following could be the pH of the solution?
A. 1
B. 7
C. 9
D. 13
[1]

3. Which oxide is amphoteric?
A. Calcium oxide
B. Carbon dioxide
C. Aluminium oxide
D. Sodium oxide
[1]

4. What is the colour of precipitate formed when aqueous sodium hydroxide is added to aqueous iron(III) chloride?
A. Green
B. White
C. Blue
D. Reddish-brown
[1]

5. Which gas is produced when ammonium sulfate is heated with sodium hydroxide solution?
A. Chlorine
B. Ammonia
C. Hydrogen
D. Sulfur dioxide
[1]

6. State the formula of the ion responsible for the alkaline properties of aqueous potassium hydroxide.
[1]

7. Explain, in terms of ions, what happens during the neutralisation reaction between hydrochloric acid and sodium hydroxide.
[1]

8. A solution has a pH of 2. If water is added to dilute the solution by a factor of 100, what will be the new pH?
[1]

9. Why is barium sulfate suitable for use as a "barium meal" in X-rays, whereas barium carbonate is not?
[1]

10. Complete the equation for the reaction between zinc oxide and sulfuric acid:
$ZnO + H_2SO_4 \rightarrow$ _______________ + _______________
[1]

Section B: Structured Questions (20 Marks)

11. Sulfuric acid is an important industrial chemical.
(a) Describe the contact process for the manufacture of sulfuric acid. Include the name of the catalyst and the approximate temperature and pressure used.
[3]

(b) Sulfur dioxide is a pollutant that causes acid rain.
(i) Write a balanced chemical equation for the formation of sulfur dioxide from the combustion of sulfur.
[1]
(ii) Explain how sulfur dioxide contributes to the formation of acid rain.
[2]

12. A student is asked to prepare pure, dry crystals of copper(II) sulfate from copper(II) oxide and dilute sulfuric acid.
(a) Why is copper(II) oxide added in excess?
[1]
(b) Describe the steps the student should take to obtain pure, dry crystals after the reaction is complete.
[3]
(c) Write the ionic equation for this reaction.
[1]

13. Three white solids are labelled A, B, and C. They are known to be sodium chloride, sodium carbonate, and sodium sulfate.
Describe simple chemical tests to identify each solid. Include the reagents used and the expected observations.
[4]

14. The pH curve below shows the change in pH when aqueous sodium hydroxide is added to 25 cm³ of aqueous ethanoic acid.

Image pending generation for this question.

(a) What is the initial pH of the ethanoic acid?
[1]
(b) Explain why the initial pH is higher than that of hydrochloric acid of the same concentration.
[2]
(c) What volume of sodium hydroxide is required to neutralise the acid?
[1]
(d) Name a suitable indicator for this titration.
[1]

15. Ammonia is manufactured by the Haber Process.
$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \quad \Delta H = -92 \text{ kJ/mol}$

(a) State the conditions used in the Haber Process.
[2]
(b) Explain why a high pressure is used, referring to Le Chatelier’s principle.
[2]

Section C: Free Response & Application (10 Marks)

16. Magnesium reacts with two different acids, X and Y, of the same concentration.

With acid X, the reaction is very vigorous and completes in 30 seconds.
With acid Y, the reaction is slow and completes in 5 minutes.
Both reactions produce hydrogen gas.

(a) Suggest the identity of acid X and acid Y.
[1]
(b) Explain the difference in the rate of reaction in terms of particle collision and ionisation.
[3]
(c) If excess magnesium is used, will the total volume of hydrogen gas produced be different for the two acids? Explain your answer.
[2]

17. A farmer finds that the soil in his field is too acidic for crops to grow well.
(a) Name a cheap chemical commonly added to soil to neutralise acidity.
[1]
(b) Write a chemical equation for the reaction between this chemical and nitric acid present in the soil.
[2]
(c) Why is sodium hydroxide not used for this purpose?
[1]

18. Lead(II) iodide is an insoluble salt.
(a) Describe how you would prepare a pure, dry sample of lead(II) iodide starting from solid lead(II) nitrate and solid potassium iodide.
[3]
(b) Write the ionic equation for the precipitation reaction.
[1]

19. Calcium oxide is a basic oxide.
(a) Write a balanced chemical equation for the reaction between calcium oxide and water.
[1]
(b) The resulting solution is tested with red litmus paper. State the observation.
[1]
(c) Explain why calcium oxide is classified as a basic oxide.
[1]

20. A student investigates the reaction between dilute hydrochloric acid and excess calcium carbonate.
$CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + H_2O(l) + CO_2(g)$
(a) Describe a test to confirm the identity of the gas produced.
[1]
(b) Explain why the mass of the reaction flask decreases during the reaction.
[1]
(c) Suggest one method to increase the rate of this reaction, other than changing the concentration of the acid.
[1]

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Answers

Secondary 4 Pure Chemistry Quiz - Acids Bases Salts (Answer Key)

1. B
[1] Strong acids are defined by complete ionisation in water, not just concentration.

2. A
[1] Red indicates strong acidity (pH 1-2).

3. C
[1] Aluminium oxide reacts with both acids and bases.

4. D
[1] Iron(III) hydroxide is reddish-brown.

5. B
[1] Ammonium salts + alkali $\rightarrow$ Ammonia gas.

6. $OH^-$
[1]

7. $H^+(aq) + OH^-(aq) \rightarrow H_2O(l)$
[1] Hydrogen ions from acid combine with hydroxide ions from alkali to form water.

8. 4
[1] Diluting a strong acid by 100 times ( $10^2$ ) increases pH by 2 units. $2 + 2 = 4$ .

9. Barium sulfate is insoluble and non-toxic, whereas barium carbonate reacts with stomach acid to form soluble, toxic barium ions.
[1]

10. $ZnSO_4 + H_2O$
[1]

11.
(a)

Catalyst: Vanadium(V) oxide / $V_2O_5$ [1]
Temperature: 450°C [1]
Pressure: 1-2 atm (or atmospheric pressure) [1]

(b)
(i) $S(s) + O_2(g) \rightarrow SO_2(g)$ [1]
(ii) Sulfur dioxide reacts with water/oxygen in the atmosphere to form sulfuric acid ( $H_2SO_4$ ) or sulfurous acid, which falls as acid rain. [2] (1 for reaction with water/oxygen, 1 for forming acid)

12.
(a) To ensure all the sulfuric acid reacts. [1]
(b)

Filter the mixture to remove excess copper(II) oxide. [1]
Heat the filtrate to evaporate some water / until saturated. [1]
Allow to cool for crystallisation, then filter and dry crystals between filter papers. [1]
(c) $CuO(s) + 2H^+(aq) \rightarrow Cu^{2+}(aq) + H_2O(l)$ [1]

13.

Add dilute nitric acid followed by aqueous silver nitrate.
- Sodium chloride: White precipitate (AgCl). [1]
Add dilute nitric acid followed by aqueous barium nitrate.
- Sodium sulfate: White precipitate (BaSO₄). [1]
Add dilute hydrochloric acid.
- Sodium carbonate: Effervescence / bubbles of gas ( $CO_2$ ) produced. [1]
(Alternatively, test for carbonate first with acid, then distinguish Cl and SO₄ with respective reagents).
Correct identification of all three based on observations. [1]

14.
(a) 3 [1]
(b) Ethanoic acid is a weak acid and is only partially ionised, so the concentration of $H^+$ ions is lower than in hydrochloric acid (strong acid) of the same concentration. [2]
(c) 25 cm³ [1]
(d) Phenolphthalein (or Thymolphthalein). Methyl orange is less suitable due to the gradual change, but Phenolphthalein is standard for weak acid-strong base. [1]

15.
(a) Temperature: 450°C [1], Pressure: 200 atm [1] (Iron catalyst is also acceptable if asked, but question asked for conditions).
(b) There are 4 moles of gas on the left and 2 moles on the right. High pressure favours the side with fewer moles of gas to reduce pressure, thus increasing the yield of ammonia. [2]

16.
(a) X: Hydrochloric acid (or Sulfuric/Nitric); Y: Ethanoic acid (or any weak acid). [1]
(b) Acid X is a strong acid and fully ionised, providing a higher concentration of $H^+$ ions. This leads to a higher frequency of effective collisions between $H^+$ ions and Magnesium atoms compared to Acid Y (weak acid, partial ionisation, lower $[H^+]$ ). [3] (1 for ionisation difference, 1 for collision frequency, 1 for link to rate)
(c) No. The volume of hydrogen depends on the number of moles of $H^+$ ions available. Since both acids have the same concentration and volume (implied same amount of acid), and Mg is in excess, the total moles of $H_2$ produced will be the same. [2]

17.
(a) Calcium hydroxide (slaked lime) or Calcium carbonate (limestone). [1]
(b) $Ca(OH)_2 + 2HNO_3 \rightarrow Ca(NO_3)_2 + 2H_2O$ OR $CaCO_3 + 2HNO_3 \rightarrow Ca(NO_3)_2 + H_2O + CO_2$ [2] (1 for formulae, 1 for balancing)
(c) Sodium hydroxide is a strong alkali/corrosive and too expensive. It can also raise the pH too high, damaging crops. [1]

18.
(a)

Dissolve lead(II) nitrate and potassium iodide separately in distilled water. [1]
Mix the two solutions. A yellow precipitate forms. [1]
Filter, wash the residue with distilled water, and dry between filter papers/in an oven. [1]
(b) $Pb^{2+}(aq) + 2I^-(aq) \rightarrow PbI_2(s)$ [1]

19.
(a) $CaO(s) + H_2O(l) \rightarrow Ca(OH)_2(aq)$ [1]
(b) Red litmus paper turns blue. [1]
(c) It reacts with acids to form salt and water only (or it produces hydroxide ions in water). [1]

20.
(a) Bubble the gas through limewater; it turns milky/cloudy. [1]
(b) Carbon dioxide gas escapes from the flask into the atmosphere. [1]
(c) Increase temperature / Use smaller pieces of calcium carbonate (increase surface area) / Stir the mixture. [1]