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SALT MODULE 2. GasTestResult of test Ammonia Place a damp in the gas Red litmus paper turns blue Carbon dioxide Bubble the gas through Lime water turns.

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Presentation on theme: "SALT MODULE 2. GasTestResult of test Ammonia Place a damp in the gas Red litmus paper turns blue Carbon dioxide Bubble the gas through Lime water turns."— Presentation transcript:

1 SALT MODULE 2

2 GasTestResult of test Ammonia Place a damp in the gas Red litmus paper turns blue Carbon dioxide Bubble the gas through Lime water turns TESTING FOR GASES red litmus paper limewatermilky

3 Chlorine Place a piece of damp in the gas Blue litmus paper turns red, then is Hydrogen Put a wooden splint near the gas Gas burns with blue litmus paper bleached lighted ‘pop’ sound

4 Oxygen Put a wooden splint near the gas Glowing splinter is Hydrogen chloride Dip a glass rod into concentrated ammonia, NH 3 solution, bring a drop of ammonia to the mouth of the test tube. Dense are observed glowing ignited white fumes

5 Sulphur dioxide Bubble the gas through a solution Or Bubble the gas through a solution colour decolorized Acidified potassium manganate(VII) Acidified potassium dichromate(VI) Purple Orange solution change to green solution

6 Glowing wooden splinter Burning wooden splinter Limewater to blue

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

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

9 1.Write a chemical equation for reaction of zinc carbonate when heated 1.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 Colour of carbonate salt Colour of oxide formed A. zinc carbonate B. lead(II) carbonate C. copper(II) carbonate white Yellow when Hot,white when cold white green brown when hot,yellow when cold black

11 Colour of carbonate salt Colour of oxide formed D.calcium carbonate E. magnesium carbonate F. Aluminium carbonate white

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13 ACTION OF HEAT ON NITRATE SALTS

14 1) All nitrate decompose on heating to produce metal oxide, nitrogen dioxide and oxygen gas Eg. Mg(NO 3 ) 2 MgO + NO 2 + O 2 Mg(NO 3 ) 2 MgO + 2NO 2 + ½ O 2 2Mg(NO 3 ) 2 2MgO + 4NO 2 + O 2

15 1) All nitrate decompose on heating to produce metal oxide, nitrogen dioxide and oxygen gas 2Cu(NO 3 ) 2 2CuO + 4NO 2 + O 2 2Zn(NO 3 ) 2 2ZnO + 4NO 2 + O 2 2Pb(NO 3 ) 2 2PbO + 4NO 2 + O 2

16 How to identify the gas produced when nitrate salt is heated? a)OXYGEN GAS, O 2 : INSERT / PUT GLOWING WOODEN SPLINTER at the mouth of TEST TUBE containing OXYGEN GAS. AND it will IGNITE/ BURN Method, substance apparatus result

17 b) NITROGEN DIOXIDE GAS, NO 2 : PUT / PLACE DAMP BLUE LITMUS PAPER on the mouth of TEST TUBE containing NITROGEN DIOXIDE GAS. AND it will TURN RED How to identify the gas produced when nitrate salt is heated? Method, substance apparatus result

18 Colour changes COLOUR OF NITRATE SALT COLOUR OF OXIDE FORMED A.Copper(II) nitrate B. Zinc nitrate BLUE SALT CRYSTAL BLACK SOLID WHITE SALT CRYSTAL YELLOW WHEN HOT WHITE WHEN COLD

19 SOLVE THESE PROBLEMS SALT X SOLID Y GAS W THAT TURNS LIMEWATER MILKY SALT X DISSOLVES FORMING COLOURLESS SOLUTION P WHITE PRECIPITATE THAT DISSOLVES IN EXCESS AMMONIA SOLUTION HEAT ADD DILUTE HNO 3 ADD NH 3 SOLUTION

20 1)NAME GAS W 2) STATE THE COLOUR OF SOLID Y 3) IDENTIFY SALT X 4) Write chemical equation of salt X when heated CARBON DIOXIDE YELLOW WHEN HOT WHITE WHEN COLD ZnCO3 / zinc carbonate ZnCO3 ZnO + CO2

21 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 24dm 3 mol -1 ] i)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

22 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 CO 2. So, 0.1 mol ZnCO3 produced 0.1 mol CO 2 Mass ZnO = 0.1 mol x 24 = 2.4 dm3

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 TESTPROCEDUREOBSERVINFERENCE WATER, H2O Pour distilled water into test tube. Add R1 salt and shake well R1 do not dissolve in water R1 is insoluble salt

24 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 TESTPROCEDUREOBSERVINFERENCE Nitric acid, HNO3 Pour nitric acid into test tube. Add R1 Pass the gas through lime water Bubbles of gas release Limewater turn chalky CO2 is released. Carbonate ion is present in R1

25 TestProcedureObservationInferenc e NaOHAdd a few drop of NaOH to R1, shake. Add NaOH until excess and shake well White precipitate formed Dissolves in excess Pb 2+ or Zn 2+ or Al 3+ might present

26 TestProcedureObservationInference NH3Add a few drop of NH 3 solution to R1, shake. Add NH 3 solution until excess and shake well White precipitate formed White precipitate do not dissolves in excess NH 3 solution Pb 2+ or Al 3+ might present

27 TestProcedureObservationInferenc e KIAdd KI to R1 and shake well Yellow precipitate is formed Present Pb 2+

28 SALT R1 CONTAIN : CATION : Pb 2+ ANION : CO 3 2-

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31 volume various

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

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

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

36 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

37 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 = mol

38 Deduce empirical formula of the precipitate formed mole Pb 2+ : mole I : :2 P b I 2

39 Hence, construct ionic equation for the reaction above Pb I -  PbI 2


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