Advertisements
Advertisements
प्रश्न
Give one chemical test to distinguish between the following pair of compounds:
Zinc sulphate solution and Zinc chloride solution
Advertisements
उत्तर
| Zinc sulphate | Zinc chloride |
|
Add BaCl2 solution to the above solution for white precipitates of BaSO4 + ZnCl2. \[\ce{ZnSO + BaCl -> BaSO4\downarrow + \underset{(White ppt)}{ZnCl2}}\] |
Add BaCl2 solution to the above solution; no effect is visualised. \[\ce{ZnCl2 + BaCl2 -> No visual effect}\] |
APPEARS IN
संबंधित प्रश्न
Match the salts given in Column I with their method of preparation given in Column II.
| Column I | Column II | ||
| 1 | Pb(NO3)2 from PbO | A | Simple displacement |
| 2 | MgCl2 from Mg | B | Titration |
| 3 | FeCl3 from Fe | C | Neutralization |
| 4 | NaNO3 from NaOH | D | Precipitation |
| 5 | ZnCO3 from ZnSO4 | E | Combination |
Sodium hydroxide solution can be used to distinguish between i. iron (II) sulphate solution and (ii) iron (III) sulphate solution; because these solutions give different coloured precipitates with sodium hydroxide solution. Give the colour of the precipitate formed with each of the solution.
What will you observe when barium chloride solution is added to iron(II) sulphate solution.
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 |
Write a balanced equation for the following conversion:
\[\ce{CuSO4 ->[A]Cu(OH)2 ->[B] [Cu(NH3)4]SO4}\]
A given white crystalline salt was tested as follows:
The addition of barium chloride solution into this solution gave a white precipitate. What conclusions can be drawn for the observation?
When an ammonium hydroxide solution is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide giving an inky blue solution. What is the cation present in solution B?
The hydroxide soluble in excess of ammonium hydroxide is ______.
Write a balanced equation of a coloured metallic oxide which dissolves in alkalis to yield colourless solutions.
Write a balanced equation for a coloured metallic oxide which dissolves in alkalis to yield colourless solutions.
