ICSE Class 10

General instructions: Answer all questions. Marks are shown in brackets [ ].

Objective

1. 1.
   Colour of ferric salts:

   1. A. Brown
   2. B. Reddish-Brown
   3. C. Red
   4. D. Orange
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2. 2.
   What do you observe when freshly precipitated aluminium hydroxide reacts with caustic soda solution?

   1. A. A white precipitate forms and remains insoluble.
   2. B. The aluminium hydroxide dissolves, forming sodium meta aluminate.
   3. C. A gas evolves with effervescence, leaving a residue.
   4. D. The mixture turns blue due to complex formation.
   [1]
3. 3.
   Zinc hydroxide forms gelatinous ………… ppts.

   1. A. red soluble
   2. B. yellow insoluble
   3. C. white soluble
   4. D. white insoluble
   [1]
4. 4.
   A solution of ferric chloride is treated with sodium hydroxide drop by drop. Which of the following observations and reactions correctly describes what happens?

   1. A. A white precipitate of ferric hydroxide forms, soluble in excess sodium hydroxide.
   2. B. A reddish-brown precipitate of ferric hydroxide forms, insoluble in excess sodium hydroxide.
   3. C. A yellow precipitate of ferric chloride forms, soluble in excess sodium hydroxide.
   4. D. No precipitate forms; the solution turns colorless with excess sodium hydroxide.
   [1]
5. 5.
   Colour of potassium permanganate is:

   1. A. Pink
   2. B. Green
   3. C. Brown
   4. D. Purple
   [1]
6. 6.
   Amphoteric Nature of Metals, their Oxides and their Hydroxides: Which of the following correctly represents the reaction of Zinc Hydroxide with dilute sulphuric acid?

   1. A. Zn(OH)₂ + H₂SO₄ (dil.) → ZnSO₄ + H₂↑
   2. B. Zn(OH)₂ + H₂SO₄ (dil.) → ZnSO₄ + 2H₂O
   3. C. Zn(OH)₂ + H₂SO₄ (dil.) → ZnSO₃ + 2H₂O
   4. D. Zn(OH)₂ + H₂SO₄ (dil.) → ZnS + 2H₂O + O₂↑
   [1]
7. 7.
   Action of sodium hydroxide on freshly precipitated aluminium hydroxide:

   1. A. $\mathrm{Al(OH)_3 + NaOH \longrightarrow NaAlO_2 + 2H_2}$
   2. B. $\mathrm{Al(OH)_3 + NaOH \longrightarrow NaAlO + 2H_2O}$
   3. C. $\mathrm{Al(OH)_3 + NaOH \longrightarrow NaAlO_2 + 2H_2O}$
   4. D. $\mathrm{Al(OH)_3 + NaOH \longrightarrow NaAlO_2 + 2OH}$
   [1]
8. 8.
   Lead hydroxide is soluble in but insoluble in

   1. A. HCl, $\mathrm{H_2SO_4}$
   2. B. $\mathrm{H_2SO_4}$, NaOH
   3. C. $\mathrm{NH_4OH}$, HCl
   4. D. NaOH, $\mathrm{NH_4OH}$
   [1]
9. 9.
   Which equation correctly represents the reaction when ammonium hydroxide is added to ferrous sulphate solution?

   1. A. FeSO₄ + NH₄OH → (NH₄)₂SO₄ + Fe(OH)₂
   2. B. FeSO₄ + 2NH₄OH → (NH₄)₂SO₄ + Fe(OH)₂↓
   3. C. FeSO₄ + NH₄OH → NH₄SO₄ + Fe(OH)₂
   4. D. 2FeSO₄ + NH₄OH → (NH₄)₂SO₄ + 2Fe(OH)₂
   [1]
10. 10.
    A small amount of sodium hydroxide is added and then excess of sodium hydroxide is added. Which of the following occurs?

    1. A. Lead iodide is formed at the end of the product side.
    2. B. Sodium Hydroxide and Oxygen gas is released at the product side.
    3. C. A yellow coloured precipitate of lead hydroxide is formed.
    4. D. Sodium Plumbate is formed at the product side.
    [1]
11. 11.
    Which solution gives a white precipitate with excess ammonium hydroxide solution?

    1. A. Lead nitrate
    2. B. Iron [II] sulphate
    3. C. Iron [III] chloride
    4. D. Copper nitrate
    [1]
12. 12.
    The substance/s which react/s with hot concentrated NaOH solution and undergoes a neutralization reaction:

    1. A. Al
    2. B. Al₂O₃
    3. C. Al(OH)₃
    4. D. None of these
    [1]
13. 13.
    Detection of Sulphite: On adding dilute Sulphuric acid to a metallic Sulphite, a colourless gas having burning sulphur smell evolves which turns acidified Potassium dichromate solution from orange to green and Potassium permanganate solution from purple to colourless. Which of the following sets of balanced chemical equations correctly represents the reactions involved?

    1. A. Na₂SO₃ + H₂SO₄ → Na₂SO₄ + H₂O + SO₂; K₂Cr₂O₇ + 3SO₂ + H₂SO₄ → K₂SO₄ + Cr₂(SO₄)₃ + H₂O; 2KMnO₄ + 2H₂O + 5SO₂ → K₂SO₄ + 2MnSO₄ + 2H₂SO₄
    2. B. Na₂SO₃ + H₂SO₄ → Na₂SO₄ + H₂O + SO₃; K₂Cr₂O₇ + SO₃ + H₂SO₄ → K₂SO₄ + Cr₂(SO₄)₃ + H₂O; 2KMnO₄ + H₂O + 5SO₃ → K₂SO₄ + 2MnSO₄ + 2H₂SO₄
    3. C. Na₂SO₃ + H₂SO₄ → Na₂SO₄ + H₂O + S; K₂Cr₂O₇ + 3S + H₂SO₄ → K₂SO₄ + Cr₂(SO₄)₃ + H₂O; 2KMnO₄ + 2H₂O + 5S → K₂SO₄ + 2MnSO₄ + 2H₂SO₄
    4. D. Na₂SO₃ + H₂SO₄ → Na₂SO₄ + H₂ + SO₂; K₂Cr₂O₇ + 3SO₂ + H₂ → K₂SO₄ + Cr₂(SO₄)₃ + H₂O; 2KMnO₄ + 5SO₂ → K₂SO₄ + 2MnSO₄ + 2H₂SO₄
    [1]
14. 14.
    Aqueous lead (II) nitrate can be distinguished from aqueous zinc nitrate by adding any of the following solution in excess, except:

    1. a. aqueous potassium chloride
    2. b. aqueous sodium sulphate
    3. c. dilute sulphuric acid
    4. d. sodium hydroxide solution
    [1]
15. 15.
    A white compound which is insoluble in nitric acid but soluble in ammonium hydroxide.

    1. A. Calcium Chloride (CaCl₂)
    2. B. Manganese oxide (MnO₂)
    3. C. Magnesium Chloride (MgCl₂)
    4. D. Silver Chloride AgCl
    [1]
16. 16.
    How can you distinguish between lead carbonate and zinc carbonate in solution?

    1. A. Add dilute nitric acid: lead carbonate dissolves completely, while zinc carbonate forms a white precipitate.
    2. B. Add dilute nitric acid: lead carbonate forms a white precipitate of lead nitrate, while zinc carbonate dissolves completely.
    3. C. Add sodium hydroxide: both lead carbonate and zinc carbonate dissolve completely in excess NaOH.
    4. D. Heat both carbonates: lead carbonate releases CO₂ gas, while zinc carbonate remains unchanged.
    [1]
17. 17.
    Which pair of balanced chemical equations correctly represents the reaction when sodium hydroxide solution is added to zinc sulphate first a little, then in excess?

    1. A. ZnSO₄ + NaOH → Zn(OH)₂ + Na₂SO₄; Zn(OH)₂ + NaOH → NaZnO₂ + H₂O
    2. B. ZnSO₄ + 2NaOH → Zn(OH)₂ + Na₂SO₄; Zn(OH)₂ + 2NaOH → Na₂ZnO₂ + 2H₂O
    3. C. ZnSO₄ + NaOH → ZnO + Na₂SO₄ + H₂O; ZnO + NaOH → Na₂ZnO₂ + H₂O
    4. D. ZnSO₄ + 2NaOH → Zn(OH)₂ + Na₂SO₄; Zn(OH)₂ + NaOH → NaZnO₂ + H₂O
    [1]
18. 18.
    The salt whose solution gives a pale green precipitate with NaOH solution and a white ppt. with BaCl₂ soln. is:

    1. A. Iron (III) sulphate
    2. B. Iron (II) chloride
    3. C. Iron (II) sulphate
    4. D. Iron (III) chloride
    [1]
19. 19.
    You are given three white powders: Calcium carbonate, Lead carbonate, and Zinc carbonate. Which of the following procedures correctly identifies the metal in each compound by testing their solutions, including how the solutions are prepared?

    1. A. Dissolve each powder in dilute nitric acid, then add ammonium hydroxide: Calcium forms no precipitate, Lead forms a white precipitate insoluble in excess, and Zinc forms a white precipitate soluble in excess.
    2. B. Dissolve each powder in water, then add sodium hydroxide: Calcium forms a white precipitate, Lead forms no precipitate, and Zinc forms a precipitate soluble in excess.
    3. C. Dissolve each powder in dilute hydrochloric acid, then add potassium iodide: Calcium forms a yellow precipitate, Lead forms no precipitate, and Zinc forms a white precipitate.
    4. D. Dissolve each powder in dilute sulfuric acid, then add ammonium hydroxide: Calcium forms a precipitate soluble in excess, Lead forms no precipitate, and Zinc forms a precipitate insoluble in excess.
    [1]
20. 20.
    You are given three white powders: calcium carbonate, lead carbonate, and zinc carbonate. To identify the metal in each compound, you dissolve each powder in dilute nitric acid and then add ammonium hydroxide to the resulting solutions. Which of the following observations correctly matches the behavior of zinc carbonate?

    1. A. No visible reaction occurs.
    2. B. A white precipitate forms and is insoluble in excess ammonium hydroxide.
    3. C. A white precipitate forms and dissolves in excess ammonium hydroxide.
    4. D. A colored precipitate forms immediately.
    [1]