When cobalt chloride is added to pure water, the co2 ions hydrate?

The question is incomplete, the complete question is:

When cobalt chloride is added to pure water, the Co2+ ions hydrate. The hydrated form then reacts with the Cl- ions to set up the equilibrium shown here:

[Co(H2O)6]^2+ + 4Cl^- > [CoCl4]^2- + 6H2O

(pink) (blue)

Which statement accurately describes the change that the system will undergo if water is added?

A. The color will become more blue.

B. The equilibrium will shift to the right.

C. More water will be produced.

D. More chloride ions will be produced.

E. There will be less of the hydrated cobalt ion at the new equilibrium position.

More chloride ions will be produced.

Explanation:

When more water is added to the system,

[Co(H2O)6]^2+ + 4Cl^- > [CoCl4]^2- + 6H2O, the equilibrium position will shift to the left. When the equilibrium position shifts to the left, more chloride ions are produced. and the hexaaquacobalt II complex is formed and the solution turns pink as shown hence the answer given.

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