Chemistry 9th Chap 10 : Topic 3 - Maryam Publications

Chemistry Chapter 10 : Topic 3

Strong and Weak Acids

1 / 20

A student prepares four aqueous solutions of acids. Which observation best indicates a strong acid?

A) It produces few ions in water and shows weak electrical conductivity.

B) It forms a precipitate when dissolved in water.

C) It completely ionizes in water producing a large number of hydrogen ions.

D) It partially reacts with water to form ions and un-ionized molecules.

2 / 20

Which statement correctly defines a weak acid?

A) It does not dissolve in water at all.

B) It produces only hydroxide ions in solution.

C) It completely ionizes in aqueous solution.

D) It partially ionizes in water, establishing equilibrium.

3 / 20

Which equation correctly represents the dissociation of hydrochloric acid in water?

A) HCl → H⁺+Cl⁻ (complete)

B) HCl ⇌ H⁺+Cl⁻

C) HCl+H₂O → H₃O⁺+Cl⁻ (reversible)

D) HCl ⇌ H₂+Cl₂

4 / 20

Which acid is correctly classified as a weak acid?

A) HNO₃

B) HCl

C) CH₃COOH

D) H₂SO₄

5 / 20

A solution conducts electricity very strongly and shows complete ion formation. The solution most likely contains:

A) NH₄OH

B) H₂CO₃

C) HCl

D) CH₃COOH

6 / 20

Which statement best describes a strong base?

A) It does not produce ions in solution.

B) It completely dissociates in water producing OH⁻ ions.

C) It partially dissociates in water producing OH⁻ ions.

D) It reacts only with acids in solid form.

7 / 20

Which equation correctly represents nitric acid dissociation?

A) HNO₃ → H⁺+NO₃⁻

B) HNO₃+H₂O ⇌ NH₄⁺+NO₃⁻

C) HNO₃ ⇌ H⁺+NO₃⁻

D) HNO₃ ⇌ NO₂+H₂O

8 / 20

Why does ethanoic acid show weak conductivity compared to hydrochloric acid?

A) It partially ionizes producing fewer ions.

B) It contains no hydrogen atoms.

C) It completely ionizes in water.

D) It is insoluble in water.

9 / 20

Which of the following is TRUE about strong acids?

A) They do not produce hydrogen ions.

B) They completely dissociate into ions in water.

C) They ionize partially in aqueous solution.

D) They exist mostly as molecules in water.

10 / 20

A student writes: HA ⇌ H⁺+A⁻
This equation most likely represents:

A) Strong base dissociation

B) Neutral salt formation

C) Strong acid dissociation

D) Weak acid dissociation

11 / 20

Which acid is diprotic and strong?

A) HNO₃

B) CH₃COOH

C) H₂SO₄

D) HCl

12 / 20

What happens when a strong acid is dissolved in water?

A) Only molecules are present.

B) Few ions are formed.

C) No ions are formed.

D) Complete ionization occurs.

13 / 20

Which of the following represents a weak base?

A) Ca(OH)₂

B) NH₄OH

C) KOH

D) NaOH

14 / 20

Which statement best compares strong and weak acids?

A) Strong acids are concentrated, weak acids are dilute.

B) Strong acids fully ionize, weak acids partially ionize.

C) Weak acids produce more ions than strong acids.

D) Strong acids do not react with water.

15 / 20

Which pair correctly shows a strong acid and a weak acid?

A) CH₃COOH and HNO₃

B) H₂SO₄ and HCl

C) HCl and HNO₃

D) HCl and CH₃COOH

16 / 20

Why is sulphuric acid considered strong in its first ionization step?

A) It partially ionizes in all steps.

B) It forms no ions in water.

C) It is insoluble in water.

D) It completely dissociates in first step.

17 / 20

Which observation indicates a weak acid solution?

A) High electrical conductivity

B) Rapid and complete ion formation

C) Low ion concentration and partial dissociation

D) Strong heating effect in water

18 / 20

Which equation shows correct dissociation of ethanoic acid?

A) CH₃COOH ⇌ CH₃COO⁻+H⁺

B) CH₃COOH ⇌ CH₄+CO₂

C) CH₃COOH → CH₃COO⁻+H⁺

D) CH₃COOH → CO₂+H₂O

19 / 20

What is the key difference between strong and weak acids in terms of ion formation?

A) Both produce equal ions.

B) Strong acids produce more ions due to complete dissociation.

C) Strong acids form no ions.

D) Weak acids form more ions than strong acids.

20 / 20

Which of the following best explains why acids conduct electricity?

A) They contain ions that move in solution.

B) They contain free electrons.

C) They are metallic in nature.

D) They have covalent bonds only.

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