Question

Give balanced equations for the preparation of the following salts:
1. Calcium oxide ⟶ Calcium chloride ⟶ Calcium carbonate
2. Zinc sulphide ⟵ Zn ⟶ Zinc sulphate
3. Iron [II] chloride ⟵ Fe ⟶ Iron [III] chloride
4. Lead [II] oxide ⟶ Lead nitrate ⟶ Lead sulphate
5. Copper [II] oxide ⟶ Copper [II] sulphate ⟵ Copper [II] hydroxide

July 30, 2024

Answer

Calcium oxide ⟶ Calcium chloride ⟶ Calcium carbonate

CaO + 2HCl ⟶ CaCl₂ + H₂O
CaCl₂ + Na₂CO₃ ⟶ 2NaCl + CaCO₃

Zinc sulphide ⟵ Zn ⟶ Zinc sulphate

Zn + S ⟶ ZnS
Zn + H₂SO₄ ⟶ ZnSO₄ + H₂

Iron [II] chloride ⟵ Fe ⟶ Iron [III] chloride

Fe + 2HCl ⟶ FeCl₂ + H₂
2Fe + 3Cl₂ ⟶ 2FeCl₃

Lead [II] oxide ⟶ Lead nitrate ⟶ Lead sulphate

PbO + 2HNO₃ ⟶ Pb(NO₃)₂ + H₂O
Pb(NO₃)₂ + Na₂SO₄ ⟶ 2NaNO₃ + PbSO₄

Copper [II] oxide ⟶ Copper [II] sulphate ⟵ Copper [II] hydroxide

CuO + H₂SO₄ ⟶ CuSO₄ + H₂O
Cu(OH)₂ + H₂SO₄ ⟶ CuSO₄ + 2H₂O

💡 Some Related Questions

The questions below refers to the following salt solutions listed A to F:
A: Copper nitrate
B: Iron [II] sulphate
C: Iron [III] chloride
D: Lead nitrate
E: Magnesium sulphate
F: Zinc chloride
(i) Which soln. becomes a deep/inky blue colour when excess of ammonium hydroxide is added to it.
(ii) Which solution gives a white precipitate with excess ammonium hydroxide solution.

Write balanced equations for — (a) Aluminium (b) Zinc — is warmed with NaOH [caustic soda] soln.

Give reasons for the following:
Sulphurous acid forms two types of salts on reaction with an alkali.

Give reasons for the following:
Acetic acid does not form an acid salt but forms a normal salt.

Give reasons for the following:
In the preparation of an insoluble salt from another insoluble salt by precipitation [double decomposition], dilute nitric acid and not dilute sulphuric acid is generally used.

Give reasons for the following:
An aqueous solution of the salt ammonium chloride is acidic in nature while an aqueous solution of sodium chloride is neutral.

Give reasons for the following:
Concentrated sulphuric acid is a weaker acid compared to dilute sulphuric acid.

The diagram represents the preparation of sodium sulphate salt from dil. H2SO4 acid and sodium hydroxide.

1. Name the apparatus ‘A’.
2. Name the substance ‘X’ placed in ‘A’ and the substance ‘Y’ placed in B.
3. State the reason for conducting the titration using the apparatus ‘A’ and ‘B’.
4. State which solution is transferred to the evaporating dish and evaporated to point of crystallization for obtaining the salt.
5. State why titration is not conducted for the preparation of copper [II] sulphate crystals by neutralization.

State which of the following methods is generally used for preparing the salts 1 to 5 given below:
A: Neutralisation — insoluble base and dil. acid
B: Neutralisation — alkali and dil. acid
C: Simple displacement — active metal and dil. acid
D: Direct combination
E: Precipitation [double decomposition]
1. PbCO3
2. Zn(NO3)2
3. NaCl
4. Cu(NO3)2
5. FeS

Identify which of the following terms matches with the appropriate descriptions 1 to 5.
A: Hydracid
B: Monobasic acid
C: Less volatile acid
D: Weak acid
E: Tribasic acid
F: Dibasic acid
G: More volatile acid
1. An acid having basicity 1 and having only one replaceable hydrogen ion per molecule of the acid.
2. An acid which dissociates to give a low concentration of H+ ions.
3. An acid containing hydrogen and a non-metallic element other than oxygen.
4. The type of acid which generally displaces another acid when the acid is heated with a salt.
5. The type of acid which reacts with a base to give an acid salt and a normal salt.