Tests for cations in solution

1. Tests for cations in solution

2. Cations are positive ions. The cations you need to be able to identify are: • copper • iron(III) • silver • iron(II) • magnesium • zinc • aluminium • lead • barium • sodium

3. Copper Solutions containing Cu2+(aq) will be blue/green in colour. Pour a little of the test solution into a clean test tube.

4. Add a few drops of dilute sodium hydroxide solution. A pale blue precipitate indicates the presence of copper ions. Cu2+(aq) + 2OH–(aq) → Cu(OH)2(s)

5. To confirm the presence of Cu2+(aq), add about 5 mL of ammonia solution. The pale blue precipitate redissolves to form a clear, royal blue solution. Cu(OH)2(s) + 4NH3(aq) → [Cu(NH3)4]2+(aq) + 2OH–(aq)

6. Iron(III) Solutions containing Fe3+(aq) will be orange in colour (or yellow if very dilute). Pour a little of the test solution into a clean test tube.

7. Add a few drops of dilute sodium hydroxide solution. An orange or dark brown precipitate forms. Fe3+(aq) + 3OH–(aq) → Fe(OH)3(s)

8. Silver Silver ions also react with sodium hydroxide solution to form a brown precipitate Iron(III) solutions are usually coloured and the precipitate is dark brown or orange. Silver solutions are colourless and the precipitate is mud-brown or the colour of milky coffee. 2Ag+(aq) + 2OH–(aq) → Ag2O(s) + H2O(l)

9. To confirm Fe3+ Potassium thiocyanate, KSCN, can be used to detect the presence of Fe3+. This test can be used on very dilute solutions or in the presence of other metal ions (especially Fe2+).

10. To a fresh sample of the test solution, add a few drops of potassium thiocyanate solution. If Fe3+ is present the solution will turn blood-red. Fe3+(aq) + SCN–(aq) → [FeSCN]2+(aq)

11. Iron(II) Solutions of Fe2+ are colourless or pale green. Pour a little of the test solution into a clean test tube.

12. Add a few drops of sodium hydroxide solution. If Fe2+ is present you will see an olive-green precipitate or gel form. Fe2+(aq) + 2OH–(aq) → Fe(OH)2(s)

13. Magnesium, zinc, aluminium and lead These four cations all form white precipitates with sodium hydroxide solution. Three form soluble complexes with excess hydroxide, one also forms a soluble complex with ammonia solution. It is very important when adding sodium hydroxide to colourless solutions that you start with one or two drops only – otherwise you might miss the formation of the precipitate when it redissolves in excess hydroxide.

14. Magnesium Pour a little of the test solution into a clean test tube. Add one or two drops only of sodium hydroxide solution. If Mg2+ is present a white precipitate forms. Mg2+(aq) + 2OH–(aq) → Mg(OH)2(s)

15. When excess sodium hydroxide is added, more precipitate is formed: the precipitate does NOT redissolve.

16. Zinc Pour a little of the test solution into a clean test tube. Add one or two drops only of sodium hydroxide solution. If Zn2+ is present a white precipitate forms. Zn2+(aq) + 2OH–(aq) → Zn(OH)2(s)

17. Add excess sodium hydroxide solution (about 5 mL). The white precipitate slowly redissolves to form a clear, colourless solution. Zn(OH)2(s) + 2OH–(aq) → [Zn(OH)4]2–(aq) Al3+ and Pb2+ also form complexes with OH–, but only Zn2+ also forms a complex with ammonia.

18. To a fresh sample of the test solution add a few drops of sodium hydroxide to form a white precipitate as before.

19. Add excess ammonia solution (about 5 mL). If Zn2+ is present the white precipitate will slowly redissolve to form a clear, colourless solution. Zn(OH)2(s) + 4NH3(aq) → [Zn(NH3)4]2+(aq) + 2OH–(aq)

20. Aluminium Pour a little of the test solution into a clean test tube. Add one or two drops only of sodium hydroxide solution. If Al3+ is present a white precipitate forms. Al3+(aq) + 3OH–(aq) → Al(OH)3(s)

21. Add excess hydroxide (about 5 mL). The precipitate redissolves to form a clear, colourless solution. Al(OH)3(s) + OH–(aq) → [Al(OH)4]–(aq)

22. To a fresh sample of the test solution, add a few drops of sodium hydroxide solution to form a white precipitate as before.

23. Add excess (5 mL) ammonia solution. The white precipitate does NOT redissolve.

24. Both Al3+ and Pb2+ form white precipitates with OH– which redissolve in excess OH– but not in excess NH3. However, aluminium sulfate is soluble in water, while lead sulfate is not. To a fresh sample of the test solution add a few drops of sulfuric acid. If Al3+ is present there will be NO precipitate.

25. Lead Pour a little of the test solution into a clean test tube. Add one or two drops only of sodium hydroxide solution. A white precipitate forms. Pb2+(aq) + 2OH–(aq) → Pb(OH)2(s)

26. Add excess (5 mL) sodium hydroxide solution. If Pb2+ is present the white precipitate redissolves to form a clear, colourless solution. Pb(OH)2(s) + 2OH–(aq) → [Pb(OH)4]–(aq)

27. To a fresh sample of the test solution add a few drops of sodium hydroxide solution as before.

28. Add excess (5 mL) ammonia solution. If Pb2+ is present the white precipitate does NOT redissolve.

29. To a fresh sample of the test solution add a few drops of dilute sulfuric acid. If Pb2+ is present a white precipitate will form. Pb2+(aq) + SO42–(aq) → PbSO4(s)

30. Barium and sodium Solutions containing Ba2+ or Na+ will be colourless. Barium hydroxide is moderately soluble, while sodium hydroxide is very soluble.

31. Add a few drops of sodium hydroxide. No precipitate suggests barium or sodium. Add more hydroxide (5 mL). If barium is present there may be a slight cloudiness after excess hydroxide is added. If sodium is present the solution will remain clear and colourless. Ba2+(aq) + 2OH–(aq) → Ba(OH)2(s)

32. Barium salts form a white precipitate with sulfuric acid. Sodium salts do not form a precipitate with sulfuric acid. Ba2+(aq) + SO42–(aq) → BaSO4(s)