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Quiz Chapter 6: Acid, Base and Salt

10 questions · Form 4 Chemistry Bab 4: Acid, Base and Salt

10 questions · plays in fullscreen

Full Question List & Answer Key

Prefer reading to quizzing? All 10 questions are listed below with the answer and explanation under each one.

1. In a titration experiment, 25.0 cm3 of 0.1 mol dm-3 NaOH solution requires 20.0 cm3 of H2SO4 for complete neutralisation. What is the molarity of H2SO4?

  1. 0.03125 mol dm-3
  2. 0.0625 mol dm-3
  3. 0.125 mol dm-3
  4. 0.250 mol dm-3
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Answer: B

Balanced eq: H2SO4 + 2NaOH -> Na2SO4 + 2H2O (a=1, b=2). Using MaVa/MbVb = ab => Ma * 200.1 * 25 = 12 => Ma = 0.1 * 2540 = 0.0625 mol dm-3.

2. Which of the following is classified as a diprotic acid?

  1. Hydrochloric acid (HCl)
  2. Nitric acid (HNO3)
  3. Sulfuric acid (H2SO4)
  4. Ethanoic acid (CH3COOH)
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Answer: C

Sulfuric acid (H2SO4) ionises in water to produce 2 hydrogen ions per acid molecule, making it diprotic.

3. When sodium hydroxide (NaOH) solution is added until excess to an unknown cation solution, a white precipitate forms which DISSOLVES in excess NaOH. Adding aqueous ammonia (NH3) until excess also produces a white precipitate which DISSOLVES in excess NH3. Which cation is present?

  1. Al3+
  2. Pb2+
  3. Zn2+
  4. Mg2+
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Answer: C

Zinc ion (Zn2+) is the only cation whose white hydroxide precipitate dissolves in EXCESS of both NaOH and NH3 solutions.

4. What is the ionic equation for the neutralisation reaction between nitric acid and potassium hydroxide?

  1. K+(aq) + NO3-(aq) -> KNO3(s)
  2. H+(aq) + OH-(aq) -> H2O(l)
  3. HNO3(aq) + KOH(aq) -> KNO3(aq) + H2O(l)
  4. H+(aq) + KOH(aq) -> K+(aq) + H2O(l)
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Answer: B

The ionic equation for any strong acid-strong base neutralisation is H+(aq) + OH-(aq) -> H2O(l).

5. Which reagent is used to confirm the presence of chloride ions (Cl-) in an aqueous solution?

  1. Barium chloride solution acidified with hydrochloric acid
  2. Silver nitrate solution acidified with dilute nitric acid
  3. Iron(II) sulfate solution and concentrated sulfuric acid
  4. Potassium iodide solution
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Answer: B

Acidifying with dilute HNO3 and adding AgNO3 yields a white precipitate of AgCl if Cl- ions are present.

6. What is the pH value of a 0.01 mol dm-3 hydrochloric acid (HCl) solution?

  1. 1.0
  2. 2.0
  3. 12.0
  4. 13.0
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Answer: B

pH = -log[H+]. For 0.01 mol dm-3 HCl (10-2 mol dm-3), pH = -log(0.01) = 2.0.

7. Which salt is INSOLUBLE in water at room temperature?

  1. Barium chloride (BaCl2)
  2. Lead(II) sulfate (PbSO4)
  3. Potassium nitrate (KNO3)
  4. Sodium carbonate (Na2CO3)
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Answer: B

Lead(II) sulfate (PbSO4) is one of the insoluble sulfates (PBC: PbSO4, BaSO4, CaSO4).

8. What observation confirms the formation of a brown ring in the confirmatory test for nitrate ions (NO3-)?

  1. A brown precipitate settling at the bottom of the test tube
  2. A brown gas escaping from the mouth of the test tube
  3. A brown ring forming at the boundary between two liquid layers
  4. The entire solution turning dark brown immediately
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Answer: C

The nitrate brown ring test forms a distinct brown ring of [Fe(H2O)5(NO)]2+ at the junction of the concentrated sulfuric acid and aqueous layer.

9. Why does glacial ethanoic acid dissolved in dry propanone fail to turn dry blue litmus paper red?

  1. Ethanoic acid is too concentrated to react
  2. Absence of water prevents the acid from ionising to release free-moving hydrogen ions (H+)
  3. Propanone neutralises the ethanoic acid molecules
  4. Glacial ethanoic acid is a strong alkali when dissolved in organic solvents
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Answer: B

Acids require water to ionise and produce hydrogen ions (H+), which are responsible for displaying acidic properties.

10. What gas is evolved when ammonium chloride is heated with sodium hydroxide solution?

  1. Ammonia gas
  2. Chlorine gas
  3. Nitrogen dioxide gas
  4. Hydrogen gas
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Answer: A

Alkalis react with ammonium salts upon heating to produce salt, water, and ammonia gas (NH3).

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