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Reaction of Acids with Metal Carbonates and Bicarbonates

Some methods ...

Question

Some methods used for the laboratory preparation of salts are:
(a) Metal + acid
(b) Carbonate + acid
(c) Precipitation (double decomposition)
(d) Direct combination
(e) Titration
Copy and complete the following table:

Salt Method of Preparation

Ammonium sulphate
Calcium carbonate
Iron (III) chloride
Lead nitrate
Zinc sulphate
E

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Solution

Salt Method of Preparation

Ammonium sulphate (e) Titration

Calcium carbonate (c) Precipitation (double decomposition)

Iron (III) chloride (d) Direct combination

Lead nitrate (b) Carbonate + acid and (a) Metal + acid

Zinc sulphate (a) Metal + acid

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Q. Name the method used for preparation of the following salts from the list given below:
(i) Sodium nitrate
(ii) Iron (III) chloride
(iii) Lead chloride
(iv) Zinc sulphate
(v) Sodium hydrogen sulphate.
List:
(a) Simple displacement
(b) Neutralization
(c) Decomposition by acid
(d) Double decomposition
(e) Direct synthesis

Q. Write equations for the laboratory preparation of the following salts, using sulphuric acid:
(i) iron (II) sulphate from the iron.
(ii) copper sulphate from copper.
(iii) lead sulphate from lead nitrate.
(iv) sodium sulphate from sodium carbonate.

Q. Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solutions of copper (II) sulphate, zinc nitrate, lead nitrate, calcium chloride and iron (III) sulphate. Copy the following table and write the colour of the precipitate in (i) to (v) and the nature of the precipitate (soluble or insoluble) in (vi) to (x).

Aqueous salt solution	Colour of precipitate when NaOH is added in a small quantity.	Nature of precipitate (soluble or insoluble) when NaOH is added in excess.
Copper(II) sulphate Zinc nitrate Lead nitrate Calcium chloride Iron(III) sulphate	(i) (ii) (iii) (iv) (v)	(vi) (vii) (viii) (ix) (x)

Q. Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solutions of copper (II) sulphate, zinc nitrate, lead nitrate, calcium chloride and iron (III) sulphate. Copy the following table and write the colour of the precipitate in (i) to (v) and the nature of the precipitate (soluble or insoluble) in (vi) to (x).

Aqueous salt Solution	Colour of precipitate when NaOH is added in a small quantity	Nature of precipitate (soluble or insoluble) when NaOH is added in excess
Copper (II) sulphate Zinc nitrate Lead nitrate Calcium chloride Iron (III) sulphate	(i) (ii) (iii) (iv) (v)	(vi) (vii) (viii) (ix) (x)

Q. Match the following:

Column A	Column B
1. Acid salt	A. Sodium sulphate decahydrate
2. Epsom salt	B. Basic lead chloride
3. Basic salt	C. Sodium carbonate
4. Glauber's salt	D. Magnesium sulphate heptahydrate
5. Normal salt	E. Sodium hydrogen carbonate

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Reaction of Acids with Metal Carbonates and Bicarbonates

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