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Question
Sodium hydroxide solution is added to the solutions containing the ions mentioned in List X. List Y gives the details of the precipitate. Match the ions with their coloured precipitates.
| List X | List Y |
| (i) Pb2+ | (A) Reddish Brown |
| (ii) Fe2+ | (B) White insoluble inexcess |
| (iii) Zn2+ | (C) Dirty green |
| (iv) Fe3+ | (D) White soluble in excess |
| (v) Cu2+ | (E) White soluble in excess |
| (vi) Ca2+ | (F) Blue |
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Solution
| List X | List Y |
| (i) Pb2+ | (D) White soluble in excess |
| (ii) Fe2+ | (C) Dirty green |
| (iii) Zn2+ | (E) White soluble in excess |
| (iv) Fe3+ | (A) Reddish Brown |
| (v) Cu2+ | (F) Blue |
| (vi) Ca2+ | (B) White insoluble inexcess |
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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 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 | (i) | (vi) |
| Zinc nitrate | (ii) | (vii) |
| Lead nitrate | (iii) | (viii) |
| Calcium chloride | (iv) | (ix) |
| Iron (III) Sulphate | (v) | (x) |
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Sodium hydroxide solution when added to Solution C gives a white precipitate which is insoluble in excess of sodium hydroxide solution.
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To the copper nitrate solution, initially, few drops of sodium hydroxide solution is added and then added in excess.
