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In a acid-base reaction, a salt is formed when a metallic ion or an ammonium ion replaces one or more hydrogen ions in an acid.
E.g. Zinc hydroxide + sulfuric acid zinc sulfate + water
Zn(OH)2 (s) + H2SO4 (aq) ZnSO4 (aq) + H20 (l)
ZnSO4Zn2+ comes from
the base, Zn(OH)2
SO42- comes from
sulfuric acid, H2SO4
Soluble Salts Insoluble Salts
All Sodium
All Potassium
All Ammonium
All Nitrates
All Chlorides Lead(II)Silver
All Sulfates BariumCalciumLead
PotassiumSodiumAmmonium
All Carbonates
PotassiumSodiumAmmonium
Hydroxides and Oxides
except
except
except
except
Methods of preparing saltsMethods of preparing salts
Yes No
Yes No
Is the starting material for making the salt soluble in water?
Titration method• Acid + alkali solution• Acid + carbonate solution
Reaction with acids• Acid + excess metal *• Acid + excess insoluble base• Acid + insoluble carbonate
Salt solution Salt crystals (dry with filter paper)
1. Concentrating2. Crystallizing3. Filtering
Aqueous solutions of two suitable soluble salts are mixed.Eg. Prepare lead(II) sulfate
The insoluble salt appears as a precipitate and can be obtained by filtration.
PbSO4Pb2+ comes from
soluble lead(II) salt
SO42- comes from
sulfuric acid, H2SO4 or any soluble sulfate
Methods of preparing saltsMethods of preparing salts
Yes No
Yes No
Is the starting material for making the salt soluble in water?
Titration method• Acid + alkali solution• Acid + carbonate solution
Reaction with acids with insoluble substances• Acid + excess metal *• Acid + excess insoluble base• Acid + insoluble carbonate
Salt solution Salt crystals (dry with filter paper)
1. Concentrating2. Crystallizing3. Filtering
2. The substance (MCB) must also be insoluble in water.
1. We react the acid with an excess of the substance (MCB).
Reason:This ensures that all the acid is used up. The reaction is complete.
Reason:This allows the excess (unreacted) substance to be filtered from the salt solution produced.
E.g. Prepare zinc sulfate
1. Think of the relevant starting materials.
Zinc + Sulfuric acid Zinc Sulfate + Hydrogen
Zn(s) + H2SO4(aq) ZnSO4(aq) + H2(g)
ZnSO4Zn2+ comes from
the metal, ZnSO4
2- comes from sulfuric acid, H2SO4
To ensure that the sulfuric acid is completely used up (Why?)
To ensure that the unreacted zinc does not
contaminate the salt formedBy heating to dryness, ZnSO4 will lose
its water of crystallisation
Salts
combine with
water
molecules to
form crystals
This method is suitable for moderately reactive metals such as magnesium, aluminium, zinc, iron and lead.
It is not suitable for reactive metals such as potassium, sodium and calcium. They react violently with acids.
It is not suitable for unreactive metals such as copper and silver. These metals do not react with dilute acids.
PotassiumSodiumCalcium
Magnesium*Aluminium*Zinc*IronLead
CopperSilver
Methods of preparing saltsMethods of preparing salts
Yes No
Yes No
Is the starting material for making the salt soluble in water?
Titration method• Acid + alkali solution• Acid + carbonate solution
Reaction with acids with insoluble substances• Acid + excess metal *• Acid + excess insoluble base• Acid + insoluble carbonate
Salt solution Salt crystals (dry with filter paper)
1. Concentrating2. Crystallizing3. Filtering
E.g. Prepare copper sulfate
1. Think of the relevant starting materials.
Copper(II) oxide + Sulfuric acid Copper (II) Sulfate + Water
CuO(s) + H2SO4(aq) CuSO4(aq) + H2O(l)
CuSO4Cu2+ comes from
the insoluble baseSO4
2- comes from sulfuric acid, H2SO4
To ensure that the sulfuric acid is
completely used up (Why?)
To ensure that the unreacted CuO does not contaminate the
salt formedBy heating to dryness, CuSO4 will lose its
water of crystallisation.
In the making of copper(II) sulfate, why is copper not used to react with sulfuric acid?
This method is used to prepare metal salts whose metal is not too reactive.
Methods of preparing saltsMethods of preparing salts
Yes No
Yes No
Is the starting material for making the salt soluble in water?
Titration method• Acid + alkali solution• Acid + carbonate solution
Reaction with acids with insoluble substances• Acid + excess metal *• Acid + excess insoluble base• Acid + insoluble carbonate
Salt solution Salt crystals (dry with filter paper)
1. Concentrating2. Crystallizing3. Filtering
In the preparation of soluble salt, what happens if the solid reactant is
soluble in water?
How can we tell if the acid has completely neutralised?
We use the method TITRATION! Use of indicator help identify that the acid
has been completely used up.
Suitable for preparing sodium, potassium, ammonium salts. (Why?)
Find your end point with the help of a suitable indicator then repeat experiment without indicator to get a pure salt sample.