Zinc sulphate solution and Zinc chloride solution.

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asked Feb 1 in Class X Science by priya12 (-12,182 points)
  1. Zinc sulphate solution and Zinc chloride solution.
  2. Iron (II) chloride solution and Iron (III) chloride solution.
  3. Calcium nitrate solution and Calcium chloride solution.
  4. Sodium carbonate and sodium sulphite.
  5. Ferrous nitrate and Lead nitrate
  6. Manganese dioxide and Copper (II) oxide.
  7. Sodium chloride and sodium nitrate.
  8. Calcium nitrate and lead nitrate.
  9. Lead nitrate and zinc nitrate.
  10. Sodium sulphite anti sodium sulphate
  11. Ammonium chloride and ammonium nitrae.
  12. Zinc carbonate and lead carbQnate.
  13. Potassium chloride and sodium chloride.
  14. Powdered coke and manganese dioxide.
  15. Copper oxide and manganese dioxide.
  16. Washing soda and baking soda..
  17. Potassium nitrate and potassium nitrite.
  18. Mercuric oxide and red lead.
  19. Ferrous ions and ferric ions.

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1 Answer

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answered Feb 1 by muskan15 (-3,172 points)
  1. When BaCl2 solution is added to the given solution, ZnSO4 gives a white ppt while no ppt. is obtained with ZnCl2 solution.
  2. When NaOH solution is added to the given solution, Iron (II) chloride gives dirty green ppt. while reddish brown ppt. is obtained with Iron (III) chloride.
  3. When AgNO3 solution is added to the given solution, CaCl2 solution will give a white ppt. while no change is observed with calcium nitrate solution.
  4. Sodium carbonate when treated with dil H2SO4 will liberate colourless odourless gas with brisk effervescence. The gas will turn lime water milky and will have no effect on acidified potassium permanganate solution.
    Sodium sulphite when treated with dil H2SO4 will liberate a colourless gas having suffocating – smell of burning sulphur. The gas will turn acidified potassium permanganate solution from pink to colourless.
  5. Aqueous ferrous nitrate when treated with NaOH solution gives a dirty green ppt. Aqueous lead nitrate when treated with NaOH solution gives a white ppt. which dissolves in excess of NaOH.
  6. When manganese dioxide is heated with cone. HCl a pungent smelling greenish yellow chlorine gas is evolved. When copper oxide is heated with cone. HCl no such gas is evolved.
  7. On heating with cone. H2SO4 sodium chloride gives pungent colourless gas which turns silver nitrate solution curdy white, whereas sodium nitrate gives a brown gas which shows no effect on silver nitrate solution.
  8. Aqueous solution of calcium nitrate gives a white precipitate with sodium hydroxide which is insoluble in excess of sodium hydroxide solution. The aqueous solution of lead nitrate gives a white precipitate with caustic soda solution which dissolves in excess of canstic soda solution.
  9. Aqueous solution of lead nitrate gives white precipitate with ammounium hydroxide which is insoluble in excess ammonium hydroxide white the sodium of zinc nitrate gives a white precipitate which is soluble in excess ammonium hydroxide.
  10. Solution of both gives white precipitate with barium chloride solution. The precipitate of barium Sulphite is soluble in dil hydrochloric acid, white the precipitate of barium sulphite is insoluble in dil. hydrochloric acid.
  11. Heat each of salt strongly in a hard glass test tube. In case of ammonium chloride, sublimation takes place and white powdery deposits settles near the mouth of test tube. In case of ammonium nitrate, an explosion takes place and nitrous oxide and stream are given off. No residue is left in the test tube.
  12. Heat each of the carbonates strongly in a hard glass test tube. In case of zinc carbonate, residue is yellow when hot and white then cold. In case of lead carbonate, residue is reddish-brown when hot and yellow when cold.
  13. Make a thick paste of each salt in HCl. Take a small amount of the paste on clean platinum wire and introduce it in non-luminous bunsen flame. In case of potassium chloride, a non-persistent lilac flame is formed. In case of sodium chloride, a persistent golden yellow Marne is formed.
  14. Heat each of the susbtances with cone, hydrochloric add. In case of coke, no visible
    reaction takes place. In case of manganese dioxide, greenish-yellow gas chlorine is evolved.
  15. Warm each of the oxides with dilute hydrochloric acid. In case of copper oxide, a greenish-blue solution of copper chloride is formed. In case of manganese dioxide, no reaction takes place.
  16. Heat each of the salt strongly in a hard glass test tube and pass the gas evolved through lime-water. In case of washing soda, lime-water does not turn milky. In case of baking soda, lime-water turns milky.
  17. Treat each of the salts with dilute sulphuric acid and gently warm. In case of potassium nitrate, no visible reaction takes place. In case of potassium nitrite, reddish-brown gas, nitrogen dioxide is given off.
  18. Heat each of the oxides strongly in a hard glass test tube. In case of mercuric oxide, tiny droplets of mercury are seen near the mouth of the test tube and residue is black. In case of red lead, no tiny droplets are seen. The residue is reddish-brown when.hot and yellow when cold.
  19. Treat the solution of each ion with sodium hydroxdide solution. In case of ferrous ions, a dirty green ppt. of ferrous hydroxide is formed. In case of ferric ions, a reddish-brown ppt. of ferric hydroxide is formed.

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