1. State how you would prepare a soluble salt from a solid base, carbonate or metal

2. Example:
CuCO3(s) + H2SO4(aq)  CuSO4(aq) CO2(g) + H2O
Add the excess solid to the acid until no more reacts. Heating may be required
Filter off the excess solid into an evaporating dish
Evaporate the water by heating gently until the solution is ready to crystallise
A glass rod is dipped into the solution and removed. If crystals form on the glass rod , the solution is ready to crystallise
Leave the solution to cool and form crystals

3. State how you would prepare a soluble salt from an alkali

4. Use a pipette to accurately measure the volume of alkali – usually 25
Use a pipette to accurately measure the volume of alkali – usually 25.0 cm3
Put the alkali in a conical flask and add a few drops of indicator
Fill a burette with acid and note the initial volume.
Allow the acid to run into the conical flask until the indicator just changes colour. This is the neutralisation point. Note the final volume to find out how much acid has been used
Repeat steps 1-3 without adding indicator and use the burette to deliver the exact volume of acid used in step 4
Evaporate the solution to the crystallisation point
Allow to crystallise
Then filter and allow to dry

5. State how you would prepare an insoluble salt

6. Choose a metal ion (cation) of the salt you are preparing and negative ion (anion) of the salt you are preparing
Dissolve them in water to make an aqueous solution
Mix the two solutions and a precipitate forms. This is the insoluble salt
Filter
Wash the residue with deionized water
Dry on filter paper