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Sodium hydroxide solution is added first in a small amount, then in excess to the aqueous salt solutions of:
1. copper [II] sulphate
2. zinc nitrate
3. lead nitrate
4. iron [III] sulphate
State in each case :
(i) the colour of the precipitate when NaOH is added in a small quantity;
(ii) the nature of the precipitate [i.e. soluble or insoluble] when NaOH is added in excess.

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Answer

(i) The colour of the precipitate when NaOH is added in a small quantity are as follows —

  1. Pale blue — copper [II] sulphate
  2. White — zinc nitrate
  3. Chalky white — lead nitrate
  4. Reddish brown — iron [III] sulphate

(ii) the nature of the precipitate [i.e. soluble or insoluble] when NaOH is added in excess are as follows —

  1. Insoluble — copper [II] sulphate
  2. Soluble — zinc nitrate
  3. Soluble — lead nitrate
  4. Insoluble — iron [III] sulphate

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Action of Ammonium Hydroxide – on solutions of salts

Magnesium chloride MgCl2 + NH4OH ⟶ ____ + ____ ↓
Iron [II] sulphate FeSO4 + NH4OH ⟶ ____ + ____ ↓
Iron [III] chloride FeCl3 + NH4OH ⟶ ____ + ____ ↓
Copper [II] sulphate CuSO4 + NH4OH ⟶ ____ + ____ ↓ [Cu(OH)2 + (NH4)2SO4 + NH4OH [in excess] ⟶ ____ + ____]
Zinc sulphate ZnSO4 + NH4OH ⟶ ____ + ____ ↓ [Zn(OH)2 +(NH4)2SO4 + NH4OH [in excess] ⟶ ____ + ____]
Lead nitrate Pb(NO3)2 + NH4OH ⟶ ____ + ____↓

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