Flash Education

Question

Choosing the substances from the list given:
dil. Sulphuric acid, Copper, Iron, Sodium, Copper (II) carbonate, Sodium carbonate, Sodium chloride, Zinc nitrate
Write balanced equations for the reactions which would be used in the laboratory to obtain the following salts:
(a) Sodium sulphate
(b) Zinc carbonate
(c) Copper (II) sulphate
(d) Iron (II) sulphate.

Acids Bases and Salts

Chemistry, Class 10, ICSE, J Dalal

July 30, 2024

Answer

(a) Sodium sulphate

Na₂CO₃ + H₂SO₄ (dil.) ⟶ Na₂SO₄ + H₂O + CO₂

(b) Zinc carbonate

Zn(NO₃)₂ + Na₂CO₃⟶ 2NaNO₃ + ZnCO₃

(c) Copper (II) sulphate

CuCO₃ + H₂SO₄ (dil.) ⟶ CuSO₄ + H₂O + CO₂

(d) Iron (II) sulphate

Fe + H₂SO₄ (dil.) ⟶ FeSO₄ + H₂

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💡 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.

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

Acids Bases and Salts

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

Acids Bases and Salts

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.

Acids Bases and Salts

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.

Acids Bases and Salts

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

Acids Bases and Salts

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.

Acids Bases and Salts

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

Acids Bases and Salts

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

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