Distinguish by adding :
(a) sodium hydroxide solution and
(b) ammonium hydroxide solution to
(i) calcium salt solution and lead salt solution
(ii) lead salt solution and zinc salt solution
(iii) copper salt solution an and ferrous salt sol.
(iv) Fe(II) salt sol. and Fe(III) salt sol.
(v) ferrous nitrate and lead nitrate

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Solution

From the given table you can distinguish the salt solutions given
(i) Sodium Hydroxide

Small amount In excess

Calcium salt White precipitate Sparingly soluble

Zinc salt White precipitate Soluble

Lead salt White precipitate Soluble

Copper salt Pale Blue precipitate Insoluble

Ferrous salt Gelatinous Green precipitate Insoluble

Ferric salt Brown precipitate Insoluble

(ii) Ammonium Hydroxide

Small amount In excess

Calcium salt No visible reaction No change

Zinc salt White precipitate Soluble

Lead salt White precipitate Insoluble

Copper salt Pale Blue precipitate Deep blue solution

Ferrous salt Gelatinous Green precipitate Insoluble

Ferric salt Brown precipitate Insoluble

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Similar questions

Distinguish by adding : Sodium hydroxide solution and ammonium hydroxide solution to
(a) Calcium salt solution and lead salt solution.
(b) Lead salt solution and zinc salt solution.
(c) Copper salt solution and ferrous salt solution.
(d) Fe(II) salt solution and Fe(III) salt solution.
(e) Ferrous nitrate and lead nitrate

(b) From the list of substances given below, choose the pair required to prepare the salts (i) to (iii) in the laboratory and write down the relevant equations. The substances are
chlorine, iron, lead, lead nitrate solution, sodium nitrate solution, iron (III) carbonate, lead carbonate, iron (III) hydroxide, sodium hydroxide solution and dilute hydrochloric acid. The salts are
(i) sodium chloride.
(ii) lead chloride.
(iii) anhydrous iron (III) chloride.

Q. State the effect of adding a small amount of a] sodium hydroxide b] ammonium hydroxide followed by an excess in each case to samples of each of the salt solutions: zinc nitrate, calcium nitrate and lead nitrate.

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)

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)

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	Small amount	In excess
Calcium salt	White precipitate	Sparingly soluble
Zinc salt	White precipitate	Soluble
Lead salt	White precipitate	Soluble
Copper salt	Pale Blue precipitate	Insoluble
Ferrous salt	Gelatinous Green precipitate	Insoluble
Ferric salt	Brown precipitate	Insoluble