Equilibrium of cobalt complexes. When cobalt(II) chloride (CoCl2) is dissolved in water, two different coloured cobalt(II) complexes exist in equilibrium: pink hexaaquacobalt(II) ((Co(H2O)6)2+) and blue tetrachlorocobalt ((CoCl4)2-). The reaction (Co(H2O)6)2+ + Cl - <-> (CoCl4)2 - + H2O is endothermic. In accordance with Le Chatelier's principle, when the temperature is raised, the position of the equilibrium will move to the right, forming more of the blue complex ion at the expense of the pink complex. The effect is demonstrated here by keeping one test tube with 0.5M CoCl2 solution at room temperature (right) and placing a second test tube with the same solution in a hot water bath (left). | |
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