O level Acids and Bases MCQ
Acids and Bases
1. Which one of the following can be added to lemon juice to increase its pH?
A lime juice
B baking powder
C concentrated hydrochloric acid
D ethanoic acid
2. Which one of the following can react with both acids and alkalis?
A sulphur dioxide
B carbon monoxide
C zinc oxide
D sodium oxide
3. Which one of the following has the highest pH? Aqueous ammonia is a weak alkali while sodium hydroxide is a strong alkali.
A 1.00 mol/dm3 aqueous ammonia
B 2.00 mol/dm3 aqueous ammonia
C 1.50 mol/dm3 sodium hydroxide
D 5.00 mol/dm3 ethanoic acid
4. Which one of the following acids require the largest volume of 1.00 mol/dm3 potassium hydroxide to neutralize?
A 1.50 dm3 0.20 mol/dm3 HCl
B 1.00 dm3 0.50 mol/dm3 H3PO4
C 1.00 dm3 1.00 mol/dm3 HCl
D 1.00 dm3 1.30 mol/dm3 CH3COOH
5. What volume of 1.00 mol/dm3 rubidium hydroxide, RbOH, is required to neutralize 25.0 cm3 of 0.500 mol/dm3 hydrochloric acid?
A 12.5 cm3
B 25.0 cm3
C 50.0 cm3
D 100 cm3
6. An element burns in air to form a compound which reacts with both acids and alkalis. Which element could it be?
A iron
B magnesium
C sulphur
D aluminium
7. Which magnesium compound does not increase the pH of dilute ethanoic acid?
A magnesium carbonate
B magnesium hydroxide
C magnesium
D magnesium chloride
8. How can you best prepare a solution of potassium sulfate safely?
A React potassium metal and sulfuric acid.
B Add potassium oxide to highly concentrated sulfuric acid.
C Titrate potassium hydroxide with sulfuric acid.
D Add potassium nitrate to dilute sulfuric acid.
9. What are the reagents you use to prepare barium sulfate safely?
A Add barium oxide to sulfuric acid.
B Add barium nitrate to sulfuric acid.
C Add barium to concentrated sulfuric acid.
D Add barium carbonate to dilute sulfuric acid.
10. Which one of the following is a neutral oxide?
A Sulphur dioxide
B Carbon monoxide
C Carbon dioxide
D Zinc oxide
11. 25 cm3 of 1 mol/dm3 dilute sulfuric acid was titrated with aqueous sodium hydroxide. A thermometer was placed in the conical flask containing initially the acid and the temperature reading was monitored.
Based on the data given, what was the volume of sodium hydroxide when the end point was reached?
Volume of sodium hydroxide added / cm3
Temperature / oC
Volume of sodium hydroxide added / cm3
Temperature / oC
5.0 33.0
10.2 35.7
6.0 33.4
10.3 35.8
7.0 34.0
10.4 35.7
8.0 34.3
10.5 35.6
9.0 35.0
11.0 35.0
10.0 35.5
12.0 34.5
10.1 35.6
13.0 33.9
A 10.1 cm3
B 10.2 cm3
C 10.3 cm3
D 11.0 cm3
12. A piece of magnesium does not react when put into a solution of hydrogen chloride in chloroform. Which one of the following changes will cause a reaction to occur?
A Adding a catalyst
B Increasing the temperature
C Increasing the concentration of hydrogen chloride in chloroform
D Adding water and stirring
13. Which salt can be prepared by precipitation?
A sodium nitrate
B ammonium sulfate
C silver chloride
D barium nitrate
14. Which statement describes a property of a weak acid in solution?
A The weak acid completely dissociates in water.
B The solution contains OH- ions.
C The solution turns Universal Indicator solution violet.
D The solution is likely to have a pH of 2.5 – 6.5
15. A solid, Y, when heated, gives off two gases, one of which turns red litmus blue.
The other gas is known to dissolve in water to give an acidic solution.
What could be solid Y?
A sodium carbonate
B zinc carbonate
C ammonium chloride
D magnesium hydroxide
16. The pH of an aqueous solution of ammonia is 9.
What is likely to be the pH after a little hydrogen chloride gas is bubbled into the solution?
A 1
B 7
C 12
D 13
17. Which of the following, when added to water, makes a solution that is a good conductor of electricity?
A gold
B barium sulfate
C silver chloride
D hydrogen chloride
18. Which molecule / ion is present in the highest concentration in a 1 mol/dm3 aqueous phosphoric acid, H3PO4?
A H+ ions
B OH- ions
C H3PO4 molecules
D H2O molecules
19. A piece of impure sodium hydroxide pellet, weighing 1.20 g, is dissolved in 100 cm3 of water. 25.0 cm3 of this solution is pipetted out and placed into a conical flask. This solution is titrated with 0.500 mol/dm3 hydrochloric acid and it is found that 10.0 cm3 of acid is required for complete neutralization.
(a) Calculate the concentration of the sodium hydroxide solution.
(b) Calculate the number of moles of sodium hydroxide dissolved in the original 100 cm3 of water.
(c) Calculate the percentage purity of sodium hydroxide.
(d) Define the terms of an acid, a base and a salt. Give an example of each of these terms.
Answers:
1. B
2. C
3. C
4. B
5. A
6. D
7. D
8. C
9. B
10. B
11. C
12. D
13. C
14. D
15. C
16. B
17. D
18. D (Water is present in excess in phosphoric acid; water is the solvent in large quantity)
1. Which one of the following can be added to lemon juice to increase its pH?
A lime juice
B baking powder
C concentrated hydrochloric acid
D ethanoic acid
2. Which one of the following can react with both acids and alkalis?
A sulphur dioxide
B carbon monoxide
C zinc oxide
D sodium oxide
3. Which one of the following has the highest pH? Aqueous ammonia is a weak alkali while sodium hydroxide is a strong alkali.
A 1.00 mol/dm3 aqueous ammonia
B 2.00 mol/dm3 aqueous ammonia
C 1.50 mol/dm3 sodium hydroxide
D 5.00 mol/dm3 ethanoic acid
4. Which one of the following acids require the largest volume of 1.00 mol/dm3 potassium hydroxide to neutralize?
A 1.50 dm3 0.20 mol/dm3 HCl
B 1.00 dm3 0.50 mol/dm3 H3PO4
C 1.00 dm3 1.00 mol/dm3 HCl
D 1.00 dm3 1.30 mol/dm3 CH3COOH
5. What volume of 1.00 mol/dm3 rubidium hydroxide, RbOH, is required to neutralize 25.0 cm3 of 0.500 mol/dm3 hydrochloric acid?
A 12.5 cm3
B 25.0 cm3
C 50.0 cm3
D 100 cm3
6. An element burns in air to form a compound which reacts with both acids and alkalis. Which element could it be?
A iron
B magnesium
C sulphur
D aluminium
7. Which magnesium compound does not increase the pH of dilute ethanoic acid?
A magnesium carbonate
B magnesium hydroxide
C magnesium
D magnesium chloride
8. How can you best prepare a solution of potassium sulfate safely?
A React potassium metal and sulfuric acid.
B Add potassium oxide to highly concentrated sulfuric acid.
C Titrate potassium hydroxide with sulfuric acid.
D Add potassium nitrate to dilute sulfuric acid.
9. What are the reagents you use to prepare barium sulfate safely?
A Add barium oxide to sulfuric acid.
B Add barium nitrate to sulfuric acid.
C Add barium to concentrated sulfuric acid.
D Add barium carbonate to dilute sulfuric acid.
10. Which one of the following is a neutral oxide?
A Sulphur dioxide
B Carbon monoxide
C Carbon dioxide
D Zinc oxide
11. 25 cm3 of 1 mol/dm3 dilute sulfuric acid was titrated with aqueous sodium hydroxide. A thermometer was placed in the conical flask containing initially the acid and the temperature reading was monitored.
Based on the data given, what was the volume of sodium hydroxide when the end point was reached?
Volume of sodium hydroxide added / cm3
Temperature / oC
Volume of sodium hydroxide added / cm3
Temperature / oC
5.0 33.0
10.2 35.7
6.0 33.4
10.3 35.8
7.0 34.0
10.4 35.7
8.0 34.3
10.5 35.6
9.0 35.0
11.0 35.0
10.0 35.5
12.0 34.5
10.1 35.6
13.0 33.9
A 10.1 cm3
B 10.2 cm3
C 10.3 cm3
D 11.0 cm3
12. A piece of magnesium does not react when put into a solution of hydrogen chloride in chloroform. Which one of the following changes will cause a reaction to occur?
A Adding a catalyst
B Increasing the temperature
C Increasing the concentration of hydrogen chloride in chloroform
D Adding water and stirring
13. Which salt can be prepared by precipitation?
A sodium nitrate
B ammonium sulfate
C silver chloride
D barium nitrate
14. Which statement describes a property of a weak acid in solution?
A The weak acid completely dissociates in water.
B The solution contains OH- ions.
C The solution turns Universal Indicator solution violet.
D The solution is likely to have a pH of 2.5 – 6.5
15. A solid, Y, when heated, gives off two gases, one of which turns red litmus blue.
The other gas is known to dissolve in water to give an acidic solution.
What could be solid Y?
A sodium carbonate
B zinc carbonate
C ammonium chloride
D magnesium hydroxide
16. The pH of an aqueous solution of ammonia is 9.
What is likely to be the pH after a little hydrogen chloride gas is bubbled into the solution?
A 1
B 7
C 12
D 13
17. Which of the following, when added to water, makes a solution that is a good conductor of electricity?
A gold
B barium sulfate
C silver chloride
D hydrogen chloride
18. Which molecule / ion is present in the highest concentration in a 1 mol/dm3 aqueous phosphoric acid, H3PO4?
A H+ ions
B OH- ions
C H3PO4 molecules
D H2O molecules
19. A piece of impure sodium hydroxide pellet, weighing 1.20 g, is dissolved in 100 cm3 of water. 25.0 cm3 of this solution is pipetted out and placed into a conical flask. This solution is titrated with 0.500 mol/dm3 hydrochloric acid and it is found that 10.0 cm3 of acid is required for complete neutralization.
(a) Calculate the concentration of the sodium hydroxide solution.
(b) Calculate the number of moles of sodium hydroxide dissolved in the original 100 cm3 of water.
(c) Calculate the percentage purity of sodium hydroxide.
(d) Define the terms of an acid, a base and a salt. Give an example of each of these terms.
Answers:
1. B
2. C
3. C
4. B
5. A
6. D
7. D
8. C
9. B
10. B
11. C
12. D
13. C
14. D
15. C
16. B
17. D
18. D (Water is present in excess in phosphoric acid; water is the solvent in large quantity)
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