Identification of Cations (Cambridge (CIE) IGCSE Chemistry)

Identification of cations

Test for ammonium ions

• Ammonium ions, NH₄⁺, can be identified by gently warming a solution containing the ions with sodium hydroxide solution

  • The sodium hydroxide solution is a source of hydroxide ions, OH^–, for the test

• This releases ammonia gas which turns damp red litmus paper blue

Testing for ammonium ions

 Heating ammonium ions with sodium hydroxide solution releases ammonia gas which turns damp red litmus blue 

• Metal cations in aqueous solution can be identified by the colour of the precipitate they form on addition of sodium hydroxide and ammonia

  • Most transition metals produce hydroxides with distinctive colours

Test for metal ions with sodium hydroxide solution

• If a small amount of sodium hydroxide solution is used, the resulting metal hydroxide normally precipitates out of solution

• If excess sodium hydroxide solutionis used, some of the precipitates may re-dissolve

  • For this reason, just a few drops of sodium hydroxide solutionare added at first and very slowly

• The sodium hydroxide test for the metal ion is:

  • Add a few drops of sodium hydroxide solution

  • Record any colour changes or precipitates formed 

  • Add excess sodium hydroxide solution

  • Record any colour changes or changes to precipitates

Test for metal ions with ammonia solution 

• If a small amount of ammonia solution is used, the resulting metal hydroxide normally precipitates out of solution

• If excess ammonia solution is used, some of the precipitates may re-dissolve

  • For this reason, just a few drops of ammonia solution are added at first and very slowly

• The ammonia test for the metal ion is:

  • Add a few drops of ammonia solution

  • Record any colour changes or precipitates formed 

  • Add excess ammonia solution

  • Record any colour changes or changes to precipitates

Metal ion tests summary

• Initially, sodium hydroxide solution and ammonia solution give the same results for 2 - 3 drops

  • This is because they both contain the hydroxide ion, OH^–

Analysing results

• The tables above contain the results for all metal cations included in the syllabus

• If a precipitate is formed from either sodium hydroxide or ammonia solution, then the hydroxide is insoluble in water

• For example, zinc chloride:

ZnCl₂ (aq) + 2NaOH (aq) →  Zn(OH)₂ (s) + 2NaCl (aq)

• There are 3 metal ions that all form white precipitates:

  • Aluminium ions, Al³⁺ 

  • Calcium ions, Ca²⁺ 

  • Zinc ions, Zn²⁺ 

• Calcium ions, Ca²⁺, can be easily distinguished from Zn²⁺ and Al³⁺

  • The white precipitate of calcium hydroxide does not dissolve in excess sodium hydroxide solution

  • The white precipitates of zinc hydroxide and aluminium hydroxide dissolve in excess sodium hydroxide solution

• Zinc ions, Zn²⁺, can then be distinguished from Al³⁺ ions as

  • The white precipitate of zinc hydroxide dissolves in excess ammonia solution

  • The white precipitate of aluminium hydroxide does not dissolve in excess ammonia solution

Flame tests for metal ions

• The flame test is used to identify the metal cations by the colour of the flame they produce

  • Ions from different metals produce different colours

• Dip the loop of an unreactive metal wire such as nichrome or platinum in concentrated acid and then hold it in the blue flame of a Bunsen burner until there is no colour change

  • This is an important step as the test will only work if there is just one type of ion present

    • Two or more ions means the colours will mix, making identification erroneous

    • This cleans the wire loop and avoids contamination

• A small sample of the compound is placed on an unreactive metal wire loop such as nichrome or platinum

• Dip the loop into the solid sample / solution and place it in the edge of the blue Bunsen flame

  • Avoid letting the wire get so hot that it glows red otherwise this can be confused with a flame colour

Diagram showing the technique for carrying out a flame test

• The colour of the flame is observed and used to identify the metal ion present:

Metal ions form distinctive coloured flames