Year 12 Chemistry Acidic Environment Quiz 1
/ 100
Data
Avogadro constant, NA = 6.022x1023 mol-1
Volume of 1 mole of ideal gas:
at 100 kPa and
0°C (273.15 K) = 22.71 L
25°C (298.15 K) = 24.79 L
pH = -log10[H+]
1. Which of the following is an everyday use of indicators? Multiple Choice: 1 mark each
a) Neutralisation.
b) The testing of soil pH.
c) The thermal decomposition of calcium carbonate.
d) The cryogenic separation of air.
2. Identify one everyday substance that is acidic, one that is basic and one that is neutral.
3 marks
Acidic substance
Basic substance
Neutral substance
3. Identify 4 commonly used indicators other than universal indicator.
4. Describe a first-hand investigation you did to prepare and test a natural indicator.
4 marks
3 marks
5. Describe the conditions under which CO2, NO2 and SO3 act as acids and identify the acids formed by name
and chemical formula.
4 marks
Oxide of non-metal Name of acid formed Formula of acid formed Conditions under which they act as acids
CO2
NO2
SO2
SO3
6. Write balanced chemical equations for the production of acid rain for the two main pollutants.
2 marks
7. Which of the following elements form amphoteric oxides?
a) Sodium, scandium, chromium, gallium and arsenic
b) All metal oxides
c) All non-metal oxides
d) Beryllium, zinc, aluminium, tin and lead
8. Define Le Châtelier's principle.
9. Identify the factors which can affect the equilibrium in a reversible reaction.
2 marks
2 marks
10. Identify the four reversible reactions that affect the solubility of carbon dioxide in water.
•
•
•
•
11. Identify one natural and one industrial source of oxides of sulfur and nitrogen.
Oxides of sulfur
Oxides of Nitrogen
•
•
•
•
2 marks
4 marks
12. Which of the following represents a balanced chemical equation of the smelting of zinc sulfide?
a) 2ZnS + 3O2 → 2ZnO + 2SO2
b) ZnS + O2 → Zn + 2SO2
c) ZnSO4 → ZnO + SO3
d) ZnSO4 → Zn + SO2 + O2
13. What is the correct chemical formula for nitric oxide?
a) NO2
b) NO
c) N2O
d) NOx
14. The sulfur in coal forms sulfur dioxide when combusted in air according to the following equation:
S + O2 → SO2. What volume of sulfur dioxide, measured at 25oC and 100kPa, is produced when 1kg of coal
containing 1.5% w/w sulfur is completely combusted in air?
3 marks
15. Which of the following is NOT an effect of acid rain?
a) Dissolve wax coating on the leaves of plants.
b) Global warming.
c) Dissolve structures made of carbonate minerals such as cement and marble
d) Kill aquatic animals.
16. Define a Bronsted-Lowry acid and base.
2 marks
17. Draw the structural formulas and write the systematic names for acetic acid, citric acid and sulfuric acid.
6 marks
18. What is the pH of 0.1M H2SO4?
a) Between 0.1 and 0.2
b) Between 1 and 0.7
c) Less than 7
d) Greater than 7
19. Account for the difference in the pH of equal concentrations of citric, acetic and hydrochloric acid.
3 marks
20. Which solution is most concentrated – HCl with a pH of 3, H2SO4 with a pH of 5, NaOH with a pH of 13 and
KOH with a pH of 9?
a) NaOH
b) H2SO4
c) HCl
d) KOH
21. Nitric acid is a strong acid. What is the pH of 0.33M nitric acid?
22. Lithium hydroxide is a strong base. What is the pH of 0.34M lithium hydroxide?
2 marks
2 marks
23. What volume of 0.05M barium hydroxide solution is required to neutralise 100ml of HCl with a pH of 3.0?
3 marks
24. What is the final pH when 73ml of pure water is added to 96ml of 0.36M HNO3?
25. What is the final pH when 45ml of 0.07M Ca(OH)2 solution is added to 76ml of 0.08M HCl?
3 marks
3 marks
26. What volume of gas is released at a temperature of 25oC and 100kPa pressure when 0.05L of HClO3 with a
pH of 2.9 reacts with 1.1g of magnesium?
27. What is the final pH when 95ml of 0.3M HNO3 is added to 210ml of 0.09M HCl?
28. What is the final pH when 94ml of 0.34M NaOH is added to 65ml of 0.55M KOH?
3 marks
2 marks
2 marks
29. What is the concentration of acetic acid when 19.7ml of acetic acid is required to titrate 20ml of 0.1M KOH?
2 marks
30. Outline the historical development of ideas about the acids of Lavoisier, Davy and Arrhenius.
•
6 marks
•
•
31. Write a balanced chemical equation for the reaction between hydrogen cyanide (HCN) and water and
identify both conjugate acid/base pairs.
2 marks
32. Describe how to correctly prepare 250ml of a 0.1M sodium carbonate primary standard for use in titration.
7 marks







33. Zinc is an amphoteric metal. Write a balanced chemical equation for the reaction between zinc metal and
hydrochloric acid. Show all states.
2 marks
34. Zinc is an amphoteric metal. Write a balanced chemical equation for the reaction between zinc metal and
sodium hydroxide solution. Show all states.
3 marks
35. Write a balanced chemical equation to show what would happen if a small amount of hydrochloric acid was
added to a solution buffered with equal concentrations of acetic acid and sodium acetate.
2 marks
36. Write a balanced chemical equation to show what would happen if a small amount of sodium hydroxide was
added to a solution buffered with equal concentrations of acetic acid and sodium acetate.
2 marks
37. What are the reactants needed to produce ethyl butanoate?
a) Concentrated sulfuric acid.
b) Butyloic acid and ethanol.
c) Butyric (butanoic) acid and ethanol.
d) Butanol and methanoic acid.
38. Which ester is produced by reacting propanol and acetic (ethanoic) acid?
a) Propyl ethanoate.
b) Ethyl propanoate.
c) Ethylene propanoate.
d) Ester propanoate.
39. Why is refluxing commonly used in esterification reactions?
a) For safety and to avoid losing volatile compounds.
b) To speed up the reaction.
c) To lower the activation energy.
d) To lower the pressure in the reaction vessel.
40. Draw a fully labelled diagram of the apparatus you used to produce an ester.
4 marks