Question

Give balanced equations for the decomposition of
(a) calcium bicarbonate by dil. HCl
(b) calcium carbonate by dil. HNO3
(c) sodium sulphite by dil. H2SO4
(d) zinc sulphide by dil. H2SO4.

July 30, 2024

Answer

Decomposition of calcium bicarbonate by dil. HCl

Ca(HCO₃)₂ + 2HCl ⟶ CaCl₂ + 2H₂O+ 2CO₂

Decomposition of calcium carbonate by dil. HNO₃

CaCO₃ + 2HNO₃ ⟶ Ca(NO₃)₂ + H₂O+ CO₂

Decomposition of sodium sulphite by dil. H₂SO₄

Na₂SO₃ + H₂SO₄ (dil.) ⟶ Na₂SO₄ + H₂O + SO₂

Decomposition of zinc sulphide by dil. H₂SO₄

ZnS + H₂SO₄ ⟶ ZnSO₄ + H₂S

Was this answer helpful?

Didn't liked the above answer ?

Text Generation Tool

💡 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.

Acids Bases and Salts

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

error: Content is protected !! 💀