The document outlines methods for preparing specified salts through various chemical reactions. It discusses using precipitation reactions when salts are insoluble and acid-base reactions when salts contain sodium, ammonium, or potassium ions. The document provides examples of reacting acids with metal oxides, metals, and metal carbonates to produce salts. It also gives guidance on purification techniques like filtration, washing, drying, heating, cooling/crystallization after reactions. Finally, it includes 5 examples of stoichiometric calculations to determine moles, masses or volumes of reactants and products in salt forming reactions.

1. NURUL ASHIKIN BT. ABD RAHMAN PART 3

2. LEARNING OUTCOMES
 Design an activity to prepare a specified
salt.
 Construct ionic equations through the
continuous variation method.
 Solve problems involving calculation of
quantities of reactants or products in
stoichiometric reactions.

3. Salt
Is the salt NO Use precipitation method
soluble?
YES
It it NAK?
Na,NH4+, K
YES Acid + Alkali  salt + water
NO
React with:
• Acid + metal oxide  salt + water
• Acid + metal  salt + hydrogen gas
• Acid + metal carbonate  salt + water + carbon dioxide

4. Use Precipitation Method
• Choose soluble salt solution
containing anion and cation
insoluble salt.
• Mix the two solution.
• Filter.
• Wash.
• Dry the precipitate.

5. Acid + Alkali  salt + water
Titration method
Evaporation/Heating
Cooling/crystallization
Filtration
Dry

6. React with:
• Acid + metal oxide  salt + water
• Acid + metal  salt + hydrogen gas
• Acid + metal carbonate  salt + water + carbon dioxide
Add metallic
oxide/metal/carbonate oxide
Heating
Filtration
Recrystallisation

7. A balanced chemical equation
provide information about the
number of moles of each
reactant and the product in the
reaction.

8. EXAMPLE 1:
Calculate the number of moles of aluminium
sulphate produced by the reaction of 0.5 mol
of sulphuric acid with excess aluminium
oxide?
Ans: 0.167 mol

9. EXAMPLE 2:
5.0 g of copper (II) carbonate powder is added
to 50cm3 of 21.9 g dm-3 hydrochloric acid.
Calculate the mass of unreacted copper (II)
carbonate.
[RAM: H, 1 ; C, 12; Cl, 35.5 ; Cu,64]
Ans: 3.14 g CuCO3

10. EXAMPLE 3:
4.05 g of aluminium oxide powder is mixed
with excess dilute nitric acid and the mixture
is heated. Calculate the mass of aluminium
nitrate produced.
[RAM: N,14; O,16; Al, 27]
Ans: 17.04 g

11. EXAMPLE 4:
150 cm3 of 1.0 mol dm-3 ammonia solution is
completely neutralised with phosphoric acid
using a titration methode. Calculate the mass
of ammonium phosphate formed.
[RAM: H,1 ; N,14; O,16; P,31]
Ans: 7.45 g

12. EXAMPLE 5:
What is the volume of 2.0 mol dm-3
hydrochloric acid required to dissolved 10 g of
marble ( calcium carbonate)?
[RAM: H,1 ; O,16; C,12; Ca,40]
Ans: 100 cm3