The pink and blue species below form a violet colored mixture at equilibrium: [co(h2o)6]2+ (aq) + 4 cl- (aq) -> [cocl4]2- (aq) + 6 h2o (l) (pink) (blue) if the concentration of [co(h2o)6]2+ is increased, what happens to the solution? a) the concentration of [cocl4]2- increases. b) the concentration of [cocl4]2- decreases. c) the solution becomes colorless. d) no color change is observed.

Option (A) is the correct answer.

Explanation:

According to Le Chatelier's principle, any disturbance caused in an equilibrium reaction will tend to shift the equilibrium in a direction away from the disturbance.

As the complex [Co(H_{2}O)_{6}]^{2+}[/tex] is present on the reactant side. So, when its concentration is increased then the equilibrium will shift in a direction that will oppose the change, that is, in the forward direction.

Therefore, it means that the product side will be favored. Hence, concentration of will be favored.

Thus, we can conclude that if the concentration of is increased then the concentration of increases.

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