Rossita Radzak : SASER

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SALTS Preparation of soluble salt 1. Acid + reactive metal(Zn / Mg) salt + H2 / 2H+ + Mg Mg2+ + H2 2. Acid + base ( metal oxide) salt + water 3. Acid + alkali salt + water / H+ + OH- H2O ( NaOH, KOH, NH4OH) 4. Acid + carbonate metal salt + CO2 + H2O / 2H+ + CO3

2+ CO2 + H2O Procedure:

1. pour ( 25 – 100cm3) acid ( 0.5 – 2.0 mol dm-3) into a beaker 2. warm /heat slowly 3. add solid (metal / base/ carbonate ) a little until excess / no more dissolve 4. stir 5. filter the mixture into evaporating dish 6. heat (slowly) the filtrate until 1/3 from original volume / saturated solution formed 7. cool down the saturated solution (until crystallized ) 8. filter (to separate the crystals) 9. dry / transfer onto filter paper / dry between sheets of filter paper

Observation Chemical equation Preparation of insoluble salt – precipitation reaction / double decomposition reaction

Pb2+ + SO42- PbSO4

Procedure : 1. pour ( 25 – 50cm3) of soluble salt (Pb(NO3)2 into a beaker 2. add ( 25 – 50cm3) of soluble salt (Na2SO4) 3. stir 4. filter the mixture 5. rinse residue / solid / precipitate 6. dry between sheets of filter paper

Observation Chemical equation Ionic equation Action of heat on salt Carbonate oxide metal (base) + CO2 except Na, K and NH4

+

Example: CuCO3 CuO + CO2 Nitrate oxide metal + nitrogen oxide + oxygen except Na, K, Examples: (2NaNO3 2NaNO2 + O2 ) 2Mg(NO3)2 2MgO + 4NO2 + O2 (Brown gas) Ammonium chloride ammonia gas + hydrogen chloride gas, (NH4Cl NH3 + HCl )

Rossita Radzak : SASER

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Confirmatory test 1. State the material / chemical / reagent 2. procedure 3. observation 4. conclusion

Example: You are given a bottle of ammonium chloride solution. Describe chemical test to verify the cation and anion.

(a) test for cation (NH4+)

1. pour 2 cm3 the solutions into a test tube 2. add 1 cm3 copper (II) sulphate solution / Nessler reagent into the test tube 3. blue precipitate soluble in excess to form dark blue solution / brown precipitate 4. Ammonium ions (NH4

+) present (b) test for anion (Cl-)

1. pour 2 cm3 the solution into a test tube 2. add 1 cm3 of dilute nitric acid and silver nitrate solution 3. white precipitate formed 4. confirm the presence of chloride ions

Example: You are given lead (II) nitrate and aluminium nitrate solution. Describe chemical test to verify the cation and anion.

(c) test for cation 1. pour 2 cm3 the solutions into different test tubes 2. add 1 cm3 potassium iodide solution into the test tubes 3. yellow precipitate formed 4. lead (II) ion present.

(d) test for anion 1. pour 2 cm3 of lead (II) nitrate solution into a test tube 2. add 1 cm3 of dilute sulphuric acid 3. add 1 cm3 of iron (II) sulphate solution 4. shake the mixure 5. tilt the test tube, add concentrated sulphuric acid carefully // drop by drop down

the side of the test tube 6. the brown ring formed 7. nitrate ion, NO3

- present.

Rossita Radzak : SASER

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Paper 3 Aim : To construct the ionic equation for the formation of lead (II) chromate(VI) Problem Statement: How does an ionic equation for the formation of lead (II) chromate (VI) can be constructed? Hypothesis : As the volume potassium chromate (VI) used is increases, the height of the yellow precipitate increases until it achieves a maximum height. Variables: Manipulated : Volumes of 0.5 mol dm-3 potassium chromate (VI) solution. Responding : Height of yellow precipitate. Fixed : Size of test tubes, volume and concentration of lead (II) nitrate solution, concentration of potassium chromate (VI) solution. Apparatus : Test tubes of the same size, test tube rack, burette, retort stand with clamp, ruler, glass rod, dropper. Material : 0.5 mol dm-3 potassium chromate (VI) solution, 0.5 mol dm-3 lead (II) nitrate solution. Procedure :

1. Seven test tubes of the same size were labelled from number 1 to 7. They were placed in a test tube rack.

2. A burette was filled 0.5 mol dm-3 lead (II) nitrate solution, 5.00 cm3 of the lead (II) nitrate solution was run into each the seven tubes.

3. Another burette was filled with 0.5 mol dm-3 potassium chromate (VI) solution. 4. Potassium chromate (VI) solution from the burette was added into each of the seven test

tubes according to the volumes specified in the table. 5. The mixture in each test tube was stirred with a clean glass rod. 6. The test tubes were left aside for about an hour. 7. The height of the precipitate in each test tube was measured. The colour of the solution

above the precipitate in each test tube was observed and recorded. Results:

Test tube 1 2 3 4 5 6 7 Volume of 0.5 mol dm-3

Pb(NO3)2 /cm3

5.00 5.00 5.00 5.00 5.00 5.00 5.00

Volume of 0.5 mol dm-3

K2Cr O4 /cm3

1.00 2.00 3.00 4.00 5.00 6.00 7.00

Height of precipitate (cm)

0.60 1.20 1.80 2.40 3.00 3.00 3.00

Colour of solution above the precipitate

colourless colourless colourless colourless colourless yellow yellow

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Paper 2 Discussion The volume of 0.5 mol dm-3 potassium chromate (VI), solution required to exactly react with 5.00 cm3 of 0.5 mol dm-3 lead (II) nitrate solution is 5.00 cm3. Calculation: Number of moles lead (II) ions = MV = 0.5 x 5.00/1000 = 0.0025 mol. Number of moles chromate (VI) ions = MV = 0.5 x 5.00/1000 = 0.0025 mol. Simplest mole ratio of lead (II) ions : chromate (VI) ions

0.0025 : 0.0025 1 : 1

Discussions: 1. A yellow precipitate of lead (II) chromate (VI) is formed in each of the seven test tubes. 2. The height of the precipitate increases gradually from test tubes 1 to 5 because more and more lead (II) chromate (VI) is formed due to the increasing amount of potassium chromate (VI) added to the test tubes. 3. The colour of solution above the precipitate in test tubes 1 to 4 are colourless due to the excess lead (II) nitrate. 4. The colour of solution above the precipitate in test tubes 6 to 7 is yellow due to the excess potassium chromate (VI). 5. Ionic equation : Pb2+ + Cr2O7

2- Pb Cr2O7 Conclusion: As / when the volume of potassium chromate (VI) solution used increases, the height of the precipitate increases until it achieves a maximum height.