chemistry form 4 - salt
TRANSCRIPT
Prepared byMOHD KHAIRUL ABADI BIN PUTEH
SMK RAJA JUMAAT
A+ sasaranku……………..
Jadi……….berikan tumpuan sepenuhnya
IMPORTANCE FORMULAEElectrochemical Series (Cations)
Electrochemical Series (Anions)Reactivity SeriesGas and characteristics
ELECTROCHEMICAL SERIES - CATIONS
‘Kalau Nak Cari Mangkuk Aladdin, Zon Felda
Sediakan Pelumba Haram, Cuba Hubungi Abang Aku’
‘ Farah Suruh Noni Clorox Berus Itu..Ohhhhh’
ELECTROCHEMICAL SERIES - ANIONS
‘Kalau Nak Cari Mangkuk
Aladdin
Cina
Zon
Haram
Felda
Sediakan Pelumba, Cuba Hubungi Abang
Aku’
REACTIVITY SERIES
GAS AND CHARACTERISTICSGAS CHARACTERISTICS
Oxygen Colourless, relights glowing splinter
Chlorine Acidic, yellowish green gas
Bromine Acidic, reddish brown
Iodine Yellowish brown
Hydrogen Colourless, give a ‘pop’ sound to burning splinter
Carbon dioxide Colourless, turns limewater chalky
Sulphur dioxide Colourless, acidic turns KMnO4 (Purple to colorless)
SOLUBILITY OF SALTSSALT SOLUBILITY OF SALTS
ANaK All are ………………………………………………
….
Nitrate salt (NO3-)
All are ………………………………………………
….
Chloride salts (Cl-)
All chloride salts are soluble EXCEPT
PbAgHg
Sulphate (SO42-)
All chloride salts are soluble EXCEPT
PbBaCa
Carbonate (CO32-)
All carbonate salts are INSOLUBLE EXCEPT
TEST YOURSELF!
PREPARATION OF SALTSSoluble saltsInsoluble salts
NUMERICAL PROBLEMS Step 1 : Write the balanced chemical
equation
CuO + 2HCl → CuCl2 + H2O
Step 2 : Write the information given
CuO + 2HCl → CuCl2 + H2O 200 cm3
2.0 mol dm-3
Step 3 : Calculate the number of moleMol of HCl = MV/1000
= (200)(2.0)/1000= 0.4 mol
Step 4 : Relate the number of mol with the ratio to expected answer
2 mol HCl = 1 mol CuOMol of CuO = 0.2 molof CuO
Step 5 : Mass of copper (II) oxide, CuOMol of CuO X RMM of Cuo0.2 mol x (64 + 16) = 16 g
TEST YOURSELF!
QUALITATIVE ANALYSIS OF SALTSAluminium ion Carbonate ionZinc ion Sulphate ionLead ion Chloride ionMagnesium ion Nitrate ionCalsium ionCopper (II) ionsIron (II)ionsAmmonium ions
SUBSTANCESubstance
Colour in hot
Colour in cold
Lead (II) oxide,PbO
Zinc oxide, ZnO
Copper (II) oxide
CONFIRMATORY TESTS ON GASES
TEST ON CATIONS
Brown precipitate formed when added sodium
hydroxide solution or ammonia solution
Dirty green precipitate formed when added with sodium
hydroxide or ammonia solution.
Dissolve in excess of ammonia solution to form dark blue
solution.
Comparison between Cu2+ in ammonia solution (light blue precipitate) and Cu2+ in
excess of ammonia solution (dark blue solution).
Added with potassium thiocyanate (KSCN), blood red colour is observed
When added with potassium iodide (KI),
yellow precipitate is observed
When added with Nessler's Reagent, brown precipitate is observed.
When solution is added with dilute sulphuric acid and iron(II) sulphate,
then followed by a few drops of concentrated sulphuric acid, a
brown ring will formed.
Test for Cation : With NaOH solution
Cation
NaOH(aq) solution
Some NaOH(aq)
No precipitate
White Precipitate Coloured Precipitate
Soluble and Colourless Precipitate
Insoluble Precipitate
Heat
NH4+
With precipitate
Concentrated HCL Drops
Precipitate
Green Brown Blue
Fe2+ Fe3+ Cu2+
Insoluble Precipitate
Mg2+ Ca2+ Pb2+ Al2+ Zn2+
Mg2+ Ca2+ Pb2+ Al2+ Zn2+
Test for Cation: With Ammonia Solution
Cation
NH3(aq) Solution
Some NH3(aq)
No Precipitate
White Precipitate Coloured Precipitate
Soluble and Colourless Precipitate
Insoluble Precipitate
NH4+,
Ca2+
Precipitate
Precipitate
Green Brown Blue
Fe2+ Fe3+ Cu2+
Soluble Precipitat
e
Mg2+ Pb2+ Al2+ Zn2+
Mg2+ Pb2+ Al2+ Zn2+ Insoluble Precipitat
e
Test for Anion
Anion X
1. Add in diluteNitric acid.
2. Add in Argentumnitrrate.
White precipitatesoluble in excessAmmonia.
Cl- ion present
Test for Anion
1. Add in dilute HCL until excess.
2. Add in BaCl2
1. Add in FeSO4 2. A few drops of
concentrated H2SO4
1. Add in dilute HCl
2. Produced gas is being transferred to lime water.
White precipitateIs formed.
Brown ring Lime
Water turnsMilky/cloudy/chalky.
SO42- ion
presentNO3
- ion present.
CO32- ion
present.
