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SALT

SALT. MODULE 2. TESTING FOR GASES. red litmus paper. limewater. milky. blue litmus paper. bleached. lighted. ‘pop’ sound. glowing. ignited. white fumes. Acidified potassium manganate(VII). Purple. Orange solution change to green solution. Acidified potassium dichromate(VI).

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SALT

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  1. SALT MODULE 2

  2. TESTING FOR GASES red litmus paper limewater milky

  3. blue litmus paper bleached lighted ‘pop’ sound

  4. glowing ignited white fumes

  5. Acidified potassium manganate(VII) Purple Orange solution change to green solution Acidified potassium dichromate(VI)

  6. Glowing wooden splinter Burning wooden splinter to blue Limewater

  7. red con.ammonia colourless red potassium manganate(VII)

  8. Action of heat on carbonate salts • 1. All carbonates decompose on heating except …………………………………… • Most carbonate decompose on heating to produce ………………….and ……… Ammonium, sodium and potassium carbonate Metal oxide Carbon dioxide

  9. Write a chemical equation for reaction of zinc carbonate when heated • How can you identify the gas that is produced when a carbonate metal is heated? • ……………………………………………………………… Bubble the gas through limewater, it will turns cloudy

  10. Yellow when Hot,white when cold white brown when hot,yellow when cold white green black

  11. white white white white white white

  12. ACTION OF HEAT ON NITRATE SALTS

  13. 1) All nitrate decompose on heating to produce metal oxide , nitrogen dioxide and oxygen gas Eg. Mg(NO3)2 MgO + NO2 + O2 Mg(NO3)2 MgO + 2NO2 + ½ O2 2Mg(NO3)2 2MgO + 4NO2 + O2

  14. 1) All nitrate decompose on heating to produce metal oxide , nitrogen dioxide and oxygen gas 2Cu(NO3)2 2CuO + 4NO2 + O2 2Zn(NO3)2 2ZnO + 4NO2 + O2 2Pb(NO3)2 2PbO + 4NO2 + O2

  15. How to identify the gas produced when nitrate salt is heated? • OXYGEN GAS , O2: INSERT / PUT GLOWING WOODEN SPLINTER at the mouth of TEST TUBE containing OXYGEN GAS. AND it will IGNITE/ BURN Method, substance apparatus result

  16. How to identify the gas produced when nitrate salt is heated? b) NITROGEN DIOXIDE GAS, NO2: PUT / PLACE DAMP BLUE LITMUS PAPER on the mouth of TEST TUBE containing NITROGEN DIOXIDE GAS. AND it will TURN RED Method, substance apparatus result

  17. Colour changes BLUE SALT CRYSTAL BLACK SOLID WHITE SALT CRYSTAL YELLOW WHEN HOT WHITE WHEN COLD

  18. SOLVE THESE PROBLEMS HEAT SOLID Y SALT X GAS W THAT TURNS LIMEWATER MILKY ADD DILUTE HNO3 ADD NH3 SOLUTION SALT X DISSOLVES FORMING COLOURLESS SOLUTION P WHITE PRECIPITATE THAT DISSOLVES IN EXCESS AMMONIA SOLUTION

  19. CARBON DIOXIDE YELLOW WHEN HOT WHITE WHEN COLD ZnCO3 / zinc carbonate ZnCO3 ZnO + CO2

  20. If 12.5 g of salt X was heated to produce solid Y and gas W, calculate :[ RAM X is 125 and Y is 81. Molar volume is 24dm3mol-1 ] • THE MASS OF SOLID Y FORMED Mol ZnCO3 = mass/ molar mass = 12.5/ 125 = 0.1 mole From equation, 1 mol ZnCO3 produced 1 Mol of ZnO. Therefore , 0.1 mol ZnCO3 produced 0.1 mol ZnO Mass ZnO = 0.1 mol x 81 = 8.1 g

  21. ii) THE volume of gas W FORMED MOL ZnCO3 = mass/ molar mass = 12.5/ 125 = 0.1 mole From equation, 1 mol ZnCO3 produced 1 Mol of CO2. So , 0.1 mol ZnCO3 produced 0.1 mol CO2 Mass ZnO = 0.1 mol x 24 = 2.4 dm3

  22. Salt R1consist of one cation and one anion.The chemical test is done to identified the cation and anion present in R1. Based on procedure and observation given, state the inference in the space provided R1 is insoluble salt

  23. Salt R1consist of one cation and one anion.The chemical test is done to identified the cation and anion present in R1. Based on procedure and observation given, state the inference in the space provided CO2 is released. Carbonate ion is present in R1

  24. Pb2+ or Zn2+ or Al3+ might present

  25. Pb2+ or Al3+ might present

  26. Present Pb2+

  27. SALT R1 CONTAIN : CATION : Pb2+ ANION : CO32-

  28. volume various

  29. Draw a graph volume of potassium iodide against height of precipitate formed from the above table

  30. yellow b) What is the colour of the precipitate formed? ……………………………………………………………………………………………. c) Name the precipitate formed …………………………………………………………………………….. Lead (II) iodide

  31. Calculate the number of moles of lead (II) nitrate solution in 5 cm 3 No of mole = MV/1000 = 0.5 x 5 / 1000 = 0.0025 mol

  32. What is the volume of potassium iodide that exactly react with 5.00 cm 3 of lead (II) nitrate solution? (volume that exactly react is the volume when the height of precipitate start constant) Volume = 5.00 cm3

  33. Calculate the number of moles of potassium iodide that reacts with 5 cm3 lead (II) nitrate solution No of mole = MV/1000 = 1.0 x 5 / 1000 = 0.005 mol

  34. Deduce empirical formula of the precipitate formed mole Pb2+ : mole I- 0.0025 : 0.0050 1:2 PbI2

  35. Hence, construct ionic equation for the reaction above Pb2+ + 2I- PbI2

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