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प्रश्न
The questions (i) to (v) refer to the following salt solutions listed A to F:
- Copper nitrate
- Iron (II) sulphate
- Iron (III) chloride
- Lead nitrate
- Magnesium sulphate
- Zinc chloride
- Which two solutions will give a white precipitate when treated with dilute hydrochloric acid followed by barium chloride solution?
- Which two solutions will give a white precipitate when treated with dilute nitric acid followed by silver nitrate solution ?
- Which solution will give a white precipitate, when either dilute hydrochloric acid or dilute sulphuric acid is added to it?
- Which solution becomes a deep/inky blue colour when excess of ammonium hydroxide is added to it ?
- Which solution gives a white precipitate with excess ammonium hydroxide solution?
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उत्तर
- Magnesium sulphate, Lead nitrate
- Magnesium sulphate, Iron (III) chloride
- Lead nitrate
- Copper nitrate
- Lead nitrate
संबंधित प्रश्न
Name a colourless cation not a representative element.
Write the probable colour of the following salt:
Potassium nitrate
Write the probable colour of the following salts:
Calcium carbonate
Name the probable cation present in each of the following solution:
Pink coloured solution
Fill in the blanks.
Salts of ______ [normal / transition] elements are generally coloured. From the ions K1+, Cr3+, Fe2+, Ca2+, \[\ce{SO^2-_3}\], \[\ce{Mn^1-_4}\],\[\ce{NO^1_3}\] the ions generally coloured are ______.
One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Calcium nitrate solution and zinc nitrate solution.
Write balanced equation for the following reaction:
Chlorine and cold dilute sodium hydroxide solution.
Write balanced equation for the following reaction:
Zinc and sodium hydroxide solution
Name the probable cation present based on the following observation:
White precipitate insoluble in NH4OH but soluble in NaOH.
