salt module 2. gastestresult of test ammonia place a damp in the gas red litmus paper turns blue...
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SALTMODULE 2
Gas Test Result 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
limewater milky
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
Oxygen Put a wooden splint near the gas
Glowing splinter is
Hydrogen chloride
Dip a glass rod into concentrated ammonia, NH3 solution, bring a drop of ammonia to the mouth of the test tube.
Dense
are observed
glowingignited
white fumes
Sulphur dioxide
Bubble the gas through a
solution OrBubble the gas through a
solution
colour decolorized
Acidified potassium manganate(VII)
Acidified potassium dichromate(VI)
Purple
Orange solutionchange to green solution
Glowingwooden splinter Burning
wooden splinter
Limewater
to blue
red
colourless
potassium manganate(VII)
con.ammonia
red
Action of heat on carbonate salts1. All carbonates decompose on heating except ……………………………………
1.Most carbonate decompose on heating to produce ………………….and ………
Ammonium, sodium and potassium carbonate
Metal oxide Carbon dioxide
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? ………………………………………………………………
23 COZnOZnCO
Bubble the gas through limewater, it will turns cloudy
Colour of carbonate salt
Colour of oxide formed
A. zinc carbonate
B . lead(II) carbonate
C . copper(II) carbonate
whiteYellow whenHot,white whencold
white
green
brown whenhot,yellow whencold
black
Colour of carbonate salt
Colour of oxide formed
D .calcium carbonate
E . magnesium carbonate
F . Aluminium carbonate
white
white
white
white
white
white
ACTION OF HEAT ON NITRATE SALTS
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
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
How to identify the gas produced when nitrate salt is heated?
a) 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
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
How to identify the gas produced when nitrate salt is heated?
Method, substance apparatus
result
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 HOTWHITE WHEN COLD
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 HNO3
ADD NH3 SOLUTION
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
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 ]
i) THE MASS OF SOLID Y FORMED
Mol ZnCO3 = mass/ molar mass = 12.5/ 125 = 0.1 moleFrom equation, 1 mol ZnCO3 produced 1 Mol of ZnO.
Therefore , 0.1 mol ZnCO3 produced 0.1 mol ZnOMass ZnO = 0.1 mol x 81 = 8.1 g
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
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
TEST PROCEDURE OBSERV INFERENCEWATER, H2O
Pour distilled water into test tube . Add R1 salt and shake well
R1 do not dissolve in water
R1 is insoluble salt
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
TEST PROCEDURE OBSERV INFERENCENitric acid, HNO3
Pour nitric acid into test tube.Add R1Pass the gas through lime water
Bubbles of gas release
Limewater turn chalky
CO2 is released.Carbonate ion is present in R1
Test Procedure Observation Inference
NaOH Add a few drop of NaOH to R1, shake.Add NaOH until excess and shake well
White precipitate formed
Dissolves in excess
Pb2+ or Zn2+ or Al3+
might present
Test Procedure Observation Inference
NH3 Add a few drop of NH3 solution to R1, shake.Add NH3 solution until excess and shake well
White precipitate formedWhite precipitate do not dissolves in excess NH3
solution
Pb2+ or Al3+
might present
Test Procedure Observation Inference
KI Add KI to R1 and shake well
Yellow precipitate is formed
Present Pb2+
SALT R1 CONTAIN :
CATION : Pb2+
ANION : CO32-
volume
various
Draw a graph volume of potassium iodide against height of precipitate formed from the above table
b) What is the colour of the precipitate formed? …………………………………………………………………………………………….
c) Name the precipitate formed ……………………………………………………………………………..
yellow
Lead (II) iodide
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
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
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
Deduce empirical formula of the precipitate formed
mole Pb2+ : mole I-
0.0025 : 0.0050
1:2
PbI2
Hence, construct ionic equation for the reaction above
Pb2+ + 2I- PbI2