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प्रश्न
A student was asked to perform an experiment in the laboratory based on the instructions given:
Observe the picture given below and state one observation for the experiment you would notice on mixing the given solution.
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उत्तर
Blue precipitate dissolves to form an inky blue/deep blue solution.
Explanation:
The light blue precipitate of copper(II) hydroxide (Cu(OH)2) dissolves in excess of ammonium hydroxide due to the formation of a deep blue complex, tetraamminecopper(II) ([Cu(NH3)4]2+), making it soluble.
संबंधित प्रश्न
Name the kind of particles present in sodium hydroxide solution.
What do you observe when caustic soda solution is added to the following solution, first a little and then in excess:
ZnSO4
Write a balanced equation for this reaction.
Using sodium hydroxide solution, how will you distinguish: Zinc nitrate solution from calcium nitrate solution
Write equation for the reaction that will take place when copper sulphate solution is added to sodium hydroxide solution.
Using Sodium hydroxide solution, how would you distinguish: Iron(II) chloride from Iron (III) chloride
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 |
Distinguish by adding:
Sodium hydroxide solution and ammonium hydroxide solution to Fe(II) salt solution and Fe(III) salt solution.
Distinguish by adding:
Sodium hydroxide solution and ammonium hydroxide solution to ferrous nitrate and lead nitrate.
What is observed when hot, concentrated caustic soda solution is added to aluminium? Write a balanced equation.
State one relevant observation for the following:
To the copper nitrate solution, initially, few drops of sodium hydroxide solution is added and then added in excess.
