Question

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.

Answer 1

Answer: 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 $[CoCl_{4}]^{2-}$ will be favored.

Thus, we can conclude that if the concentration of $[Co(H2O)_6]^{2+}$ is increased then the concentration of $[CoCl_{4}]^{2-}$ increases.