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Preparation of Salts - Coggle Diagram
Preparation of Salts
Soluble salts
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All chlorides
Except lead(II) chloride and silver chloride, they are both insoluble
All sulphates
Except barium sulphate, calcium sulphate (sparingly soluble), lead(II) sulphate, they are are insoluble
Examples: NaCl, FeCl3, ZnCl2, K2SO4, NH4CL, Na2SO4, Fe(SO4)3, ZnSO4
Insoluble salts
All carbonates
Except sodium carbonate, potassium carbonate, and ammonium carbonate
Examples: CaSO4, BaSO4, PbSO4
Hydrated salts
They have water molecules chemically bonded within the crystal structure. The water molecules can also be called the water of crystallization.
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Reacting an acid with an insoluble metal, carbonate or base
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Titration (e.g. NaNO3)
- Fill up a burette with dilute nitric acid.
- Pipette 25.0cm^3 of dilute sodium hydroxide solution into a conical flask.
- Add 1 or 2 drops of methyl orange (indicator) to the sodium hydroxide solution. It turns yellow.
- Add dilute nitric acid from the burette slowly until the solution turns orange permanently. This is the end-point.
- Record the final burette reading.
- After titration, pipette 25.0cm^3 of sodium hydroxide solution into a beaker.
- Add the volume of acid required for complete neutralisation.
- Heat the solution to evaporate the water until it is saturated.
- Allow it to cool and crystallize.
- Filter to collect the crystals.
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