In an aqueous chloride solution cobalt$($II$)$ exists in equilibrium with the complex ion $CoC{l}_4^{2-}*C{o}^{2+}(aq)$ is pink and $CoC{l}_4^{2-}(aq)$ is blue.

At low temperature the pink At high temperature the color predominates. blue color is strong.

If we represent the equilibrium as:

$C{o}^{2+}(aq)+4C{l}^{-}(aq)CoC{l}_4^{2-}(aq)$

We can conclude that:

This reaction is

exothermic.

endothermic.

neutral.

More information is needed to answer this question.

When the temperature is increased the equilibrium constant, $K$ :

increases.

decreases.

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