The Co(H2O)6 + 4 Cl- <- -> [CoCl4]2- + 6H20 Considering that the [CoCl4]2- complex is...

The Co(H2O)6 + 4 Cl- <- -> [CoCl4]2- + 6H20

Considering that the [CoCl4]2- complex is deep blue and the [Co(H2O)6]2+ is pink explain the color of the contents of the test tube which was held at room temperature.

Expert Solution

The two different coloured Co(II) complex ions, [Co(H₂O)₆]²⁺ and [CoCl₄]^2-, exist together in equilibrium in solution in the presence of chloride ions:

[Co(H₂O)₆]²⁺(aq)(pink) + 4Cl^-(aq) ⇌ [CoCl₄]^2-(aq)(blue) + 6H₂O(l)

This equilibrium can be disturbed by changing the chloride ion concentration or by changing the temperature. The colour changes accompanying the changes in equilibrium position are as predicted by Le Chatelier’s principle.

The distinctive colours of the two cobalt(II) species in solution produce an attractive visual demonstration of a reversible reaction and the effect of concentration and temperature on the position of equilibrium.

queen_honey_blossom answered 2 years ago

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