Preparing Soluble Salts (Cambridge (CIE) IGCSE Chemistry)

Preparing soluble salts

What is a salt?

• A salt is a compound that is formed when the hydrogen atom in an acid is replaced by a metal

• For example if we replace the H in HCl with a potassium atom, then the salt potassium chloride is formed, KCl

• Salts are an important branch of chemistry due to the varied and important uses of this class of compounds

• These uses include fertilisers, batteries, cleaning products, healthcare products and fungicides

• The method used depends on the solubility of the salt being prepared

How to name a salt

• The name of salt has two parts

• The first part comes from the metal, metal oxide or metal carbonate used in the reaction

• The second part comes from the acid

• The name of the salt can be determined by looking at the reactants

• For example hydrochloric acid always produces salts that end in chloride and contain the chloride ion, Cl^-

• Other examples:

  • Sodium hydroxide reacts with hydrochloric acid to produce sodium chloride

  • Zinc oxide reacts with sulfuric acid to produce zinc sulfate

Preparing soluble salts

• There are two methods of preparing a solution salt:

  • Method A

    • Adding acid to a solid metal, insoluble base or insoluble carbonate

  • Method B

    • Reacting a dilute acid and alkali (soluble base)

Method A

Method A: Adding acid to a solid metal, insoluble base or insoluble carbonate

Diagram showing the preparation of soluble salts 

Method

• Add dilute acid into a beaker and heat using a Bunsen burner flame

• Add the insoluble metal, base or carbonate, a little at a time, to the warm dilute acid and stir until the base is in excess (i.e. until the base stops disappearing and a suspension of the base forms in the acid)

• Filter the mixture into an evaporating basin to remove the excess base

• Heat the solution to evaporate water and to make the solution saturated. Check the solution is saturated by dipping a cold, glass rod into the solution and seeing if crystals form on the end

• Leave the filtrate in a warm place to dry and crystallize

• Decant excess solution and allow crystals to dry or blot to dry with filter paper

Example: preparation of pure, hydrated copper(II) sulfate crystals using method A

• Add dilute sulfuric acid into a beaker and heat using a Bunsen burner flame

• Add copper(II) oxide (insoluble base), a little at a time to the warm dilute sulfuric acid and stir until the copper (II) oxide is in excess (stops disappearing)

• Filter the mixture into an evaporating basin to remove the excess copper(II) oxide

• Leave the filtrate in a warm place to dry and crystallize

• Decant excess solution

• Blot crystals dry with filter paper

copper(II) oxide + sulfuric acid → copper(II) sulphate + water

CuO (s) + H₂SO₄ (aq) → CuSO₄ (aq) + H₂O (l)

Method B

 Method B: Reacting a dilute acid and alkali (soluble base)

Diagram showing the apparatus needed to prepare a salt by titration

Method

• Use a pipette to measure the alkali into a conical flask and add a few drops of indicator (thymolphthalein or methyl orange)

• Add the acid into the burette

• Record the starting volume of acid in the burette

• Add the acid very slowly from the burette to the conical flask until the indicator changes to the appropriate colour

• Record the final volume of acid in the burette

• Calculate the volume of acid added

  • Final volume of acid - initial volume of acid

• Add this same volume of acid to the same volume of alkali without the indicator

• Heat the resulting solution in an evaporating basin to partially evaporate, leaving a saturated solution (crystals just forming on the sides of the basin or on a glass rod dipped in and then removed)

• Leave to crystallise, decant excess solution and allow crystals to dry