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

14. volume various

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

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

18. 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

19. 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

20. 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

21. Deduce empirical formula of the precipitate formed mole Pb 2+ : mole I - 0.0025 : 0.0050 1:2 P b I 2

22. Hence, construct ionic equation for the reaction above Pb 2+ + 2I -  PbI 2