A metal-aqua ion consists of a central metal ion with six water ligands co-ordinately bonded to it. Aluminium hydroxide is amphoteric. Test tube reactions can be used to identify metal-aqua ions.
Equations
The general equations for the formation of metal precipitates are shown below.
When transition metal compounds are added to water, water ligands co-ordinately bond with the metal ions to form metal-aqua complex ions. A lone pair on the oxygen in water is donated to the metal ion to form the co-ordinate bond.
Usually six water ligands co-ordinate with the central metal ion. The general formula for metal-aqua ions is [M(H2O)6]n+.
Example
A [Fe(H2O)6]3+ ion.
Acidity
An acidity or a hydrolysis reaction takes place in a solution containing metal-aqua 2+ ions and water. An acidic solution forms because the metal-aqua 2+ ions release H+ ions. The solution formed is only weakly acidic as there is partial dissociation of the H+ions, only.
Metal-aqua 3+ ions dissociate more readily than metal-aqua 2+ ions, so their solutions are more acidic. This is because metal 3+ ions have a higher charge density than metal 2+ ions, therefore they are more polarising and are able to attract the lone pair on the oxygen atom in water more strongly. This leads to the weakening of the O−H bond and the H+ dissociates more readily.
Insoluble metal hydroxide precipitates form when OH− ions are added to a solution containing metal-aqua ions. The table below explains how the precipitate forms.
Procedure
1.
Metal-aqua 3+ ions dictate the position of equilibrium in water. Addition of OH− ions removes the H3O+ ions. This shifts the position of equilibrium to the right.
Metal-aqua 2+ ions undergo the same process. Although, only two water ligands are deprotonated to form the insoluble, uncharged metal hydroxide precipitate.
Metal hydroxide precipitates dissolve in acids. When metal hydroxides are added to an acid, they accept H+ ions and act as a Brønsted-Lowry base. The hydrolysis reaction is reversed and the metal-aqua ions reform.
Some metal hydroxides are amphoteric, which means that they can act as acids and bases. Amphoteric metal hydroxides will dissolve in an excess amount of an acid and base.
Example
Aluminium hydroxide is amphoteric. Aluminium hydroxide acts as a Brønsted-Lowry acid in the presence of a base and a soluble compound forms. Aluminium hydroxide donates H+ ions to the OH− of the base.
A solution of ammonia can be used to introduce hydroxide ions to a solution, instead of using a strong alkali. When ammonia dissolves in water ammonium ions and hydroxide ions form. Only a small amount of ammonia is required.
NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq)
Sometimes when an excess amount of ammonia is added to a metal hydroxide precipitate, it dissolves. This is because a ligand-exchange reaction occurs. The ammonia ligands displace the water and hydroxide ligands and a soluble, charged complex forms.
When metal 2+ ions and sodium carbonate react, an insoluble metal carbonate forms.
[M(H2O)6]2+(aq)+CO32−(aq)⇌MCO3(s)+6H2O(l)
When sodium carbonate is added to a solution containing metal3+3+ ions the carbonate ions do not displace the water ligands. In a solution containing metal3+ ions there is a higher concentration of H3O+ as metal 3+ ions are stronger acids.
The carbonate ions react with the H3O+ ions and removes them from the solution. This shifts the position of the hydrolysis reaction to the right and a M(OH)3(H2O)3 precipitate forms instead of M2(CO3)3.
Simple test tube reactions can be used to identify whether copper(II) ,iron(II), iron(III) and aluminium(III) metal-aqua ions are present in a solution.
1.
Dropping pipette used to add reagents.
2.
Test tubes containing unknown metal ion solution.
3.
Test tube containing sodium hydroxide solution.
4.
Test tube containing sodium carbonate solution.
5.
Test tube containing ammonia solution.
Procedure
1.
Add equal volumes of the unknown metal ion solution to three separate test tubes.
2.
Add sodium hydroxide solution to the first test tube. Record any observations.
3.
Add more sodium hydroxide drop-wise until it is in excess. Record any observations.
4.
Add sodium carbonate solution to the second test tube. Record any observations.
5.
Add more sodium carbonate drop-wise until it is in excess. Record any observations.
6.
Add ammonia solution to the third test tube. Record any observations.
7.
Add more ammonia drop-wise until it is in excess. Record any observations.
Reaction with sodium hydroxide
When sodium hydroxide is added to solutions of all four metal-aqua ions, a precipitate forms. However, upon addition of excess sodium hydroxide, only the aluminium hydroxide precipitate will dissolve, because aluminium hydroxide is amphoteric.
1.
Al3+ ions in solution
2.
Precipitate forms.
3.
Precipitate dissolves.
Reaction with sodium carbonate
When sodium carbonate is added to solutions of all four metal-aqua ions, a precipitate forms. Carbon dioxide will also form in the test tubes containing Fe3+ and Al3+ ions and bubbles will be seen. This test can be used to identify between Fe2+ and Fe3+ ions.
1.
Fe2+ ions in solution.
2.
Precipitate forms.
1.
Fe3+ ions in solution
2.
Precipitate forms.
Carbon dioxide bubbles given off.
Reaction with ammonia
When sodium carbonate is added to solutions of all four metal-aqua ions, a precipitate forms. However, upon addition of excess ammonia only the copper hydroxide precipitate dissolves as a ligand exchange reaction takes place.
1.
Cu2+ ions in solution.
2.
Precipitate forms.
3.
Precipitate disappears.
A deep blue solution forms.
Colours
The table below shows the formulae and colours of all the complex ion solutions and precipitates.
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FAQs - Frequently Asked Questions
How can you identify between Fe(III) and Fe(II) metal aqua ions using sodium carbonate solution?
When sodium carbonate solution is added to solutions containing Al(II) and Fe(III) metal aqua ions, carbon dioxide gas is given off. This reaction can be used to identify between solutions containing Fe(II) and Fe(III) metal aqua ions.
What happens when hydroxide ions are added to solutions containing metal aqua ions?
Insoluble metal hydroxides form when OH- ions are added to a solution of metal aqua ions.
What happens when transition metal compounds are added to water?
When transition metal compounds are added to water, water ligands co-ordinately bond with the metal ions to form metal-aqua complex ions. A lone pair on the oxygen in water is donated to the metal ion to form the co-ordinate bond.