Experiment: Inorganic Chemistry: Structure and Bonding
Preparation of Tetraamminedichlorocobalt(III) Chloride
Materials:
- Cobalt(II) chloride hexahydrate (CoCl2·6H2O)
- Ammonium hydroxide (NH4OH)
- Hydrogen peroxide (H2O2) - 30% solution
- Ethanol (C2H5OH)
- Distilled water
- Concentrated Hydrochloric Acid (HCl)
Procedure:
- Dissolve 2.0 g of CoCl2·6H2O in 10 mL of distilled water.
- Add 10 mL of concentrated NH4OH to the solution. A blue precipitate will form.
- Add 5 mL of 30% H2O2 solution slowly with stirring. The solution will turn brown.
- Slowly add concentrated HCl until the solution turns purple/pink and a precipitate forms.
- Heat the mixture gently, with stirring, until the precipitate dissolves and the solution becomes a deep purple/pink color.
- Cool the solution in an ice bath.
- Filter the solution using a Buchner funnel and filter paper. Wash the precipitate with cold ethanol.
- Allow the precipitate to air dry.
Key Procedures and Observations:
- Dissolving cobalt(II) chloride hexahydrate provides cobalt(II) ions.
- Adding ammonium hydroxide forms a cobalt(II) hydroxide precipitate. This is then oxidized by H2O2.
- Addition of HCl provides chloride ions, lowers the pH, and helps form the tetraamminedichlorocobalt(III) complex ion ([Co(NH3)4Cl2]+).
- Heating the mixture ensures complete reaction and dissolution of the complex.
- Cooling and filtration isolate the product.
- Washing with ethanol removes impurities.
- Air drying removes excess solvent.
Significance:
This experiment demonstrates the synthesis of a coordination complex, tetraamminedichlorocobalt(III) chloride. It illustrates concepts of oxidation-reduction reactions, complex ion formation, and the influence of pH on reaction outcomes. The synthesis and the resulting product allow students to explore coordination chemistry principles, bonding theories (such as crystal field theory or valence bond theory), and isomerism (potentially). It also provides practical experience in experimental techniques like filtration and precipitation.