Question

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

Answer 1

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.

Answer:

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.

Answer 2

Answer : The question is incomplete and the complete question is attached in the answer;

Answer 1) When HCl was added to the system of cobalt chloride it will eventually produce more Cl ions in the solutions which will shift the equilibrium to the right and make the solution look more blue than before. To accommodate extra Cl ions in the system the equilibrium gets shifted. 

Answer 2) When in the reaction system water is added the Cobalt chloride compound forms a hydrated mixture; this means the equilibrium reaction shifts to the left and produces more hydrated ions along with more chlorine ions in the solution.

Which then turns the resultant solution tinto pink in colour.