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SALTS (type (Chloride, Cl (PB, Ag, other), Sulphate, SO4 (Pb,Ca,Ba, other)…

- - - - insoluble
  - - - soluble
- - - - Carbonate salt
        
        MCO3 → MO + CO2
      - Nitrate salt
        
        2M(NO3)2 → MO + 4 MO2 +O2
  - - - Sulphate
        
        add BaCl2
        
        Ba 2+ + SO4 2- → BaSO4
        
        white precipitate formed
      - Chloride
        
        add AgNO3
        
        Ag+ + Cl- → AgCl
      - Carbonate
        
        add acid
        
        CO3 2- + 2H + → CO2 + H2O
      - Nitrate
        
        add H2SO4
        
        brown ring formed
    - - add Sodium Hydroxide, NaOH
        
        White precpitate
        
        PZAlMC
        
        add more
        
        not dissolves
        
        Ca 2+
        
        Mg 2+
        
        dissolves
        
        Zn 2+
        
        2 more items...
        
        No changes
        
        NH4 +
      - add Ammonia, NH3
        
        white precipitate
        
        ZnMAP
        
        add more
        
        not dissolves
        
        AP
        
        Mg 2+
        
        dissolves - Zn 2+
        
        No changes
        
        NH4+
        
        Ca 2+
        
        coloured precipitate
        
        Fe2+ - light green
        
        Fe3+ - brown
        
        Cu2+ - blue
  - - - Fe2+ - light green
      - Fe3+ - brown
      - other cation - white
      - Cu2+ - blue
    - - ZnO - yellow if hot, white if cold
      - CuO - balck
      - PbO - brown if hot, ye;;ow if cold
      - CuCO3 -green
- - - - filter using filter funnel
      - 4.rinse the residue with distilled water
      - 2.stir with glass rod
      - dry the residue by pressing it between filter paper
      - 1.mix two solution that contain of cation and anion of insoluble salt
  - - - titration method
        
        Acid + Alkali→ Salt + Water
        
        1.conducted to determined the volume of acid needed to neutralise a fixed volume of alkali with aid of an indicator.
        
        same volume of acid is added to the same volume of alkali without any indicator to obtain pure and natural salt solution.
    - - Neutralisation reaction
        
        Acid + Metal Oxide→ Salt + water
      - Acid + Metal Carbonate→ Salt + water +carbon dioxide
        
        1.add M powder until excess into a fixed volume of the heated acid
        
        Filter the mixture to remove the excess M.
        
        crystallization process
        
        dip in glass rod, if crystals are formed, the solution is saturated
        
        cooled at room temperature
        
        evaporate the filtrate until it becomes a saturated solution
        
        Filter and dry the salt crystals by pressing them between two filter paper
      - Displacement method
        
        Acid + Metal→ Salt + Hydrogen