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Question
Give one chemical test to distinguish between the following pair of compounds:
Iron (II) chloride solution and iron (III) chloride solution
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Solution
| Iron (II) chloride | Iron (III) chloride |
|
Add sodium hydroxide to the above solution; a dirty green ppt. is formed. \[\ce{FeCl2 + 2NaOH -> 2NaCl + Fe(OH)2\downarrow}\] |
Add sodium hydroxide to the above solution; a reddish-brown ppt. is observed. \[\ce{FeCl3 + 3NaCl -> 3NaCl + Fe(OH)3\downarrow}\] |
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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 precipiatate (soluble or insoluble) in (vi) to (x)
| Aqueous salt Solution | Colour of Participitate when NaOH is added in a samll quantity | Nature of precipitate(soluble or insoluble) when NaOH added in excess |
| Copper (II) Solution | ||
| Zinc nitrate | ||
| Lead nitrate | ||
| Calcium chloride | ||
| Iron(III) sulphate |
The questions (i) to (v) refer 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
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(iv) Which solution becomes a deep/inky blue colour when excess of ammonium hydroxide is added to it?
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Give the balanced equations for the reaction with two different amphoteric oxides with a caustic alkali.
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