You're provided with a bottle labled [CoCl2.6H2O] = 0.054 M in 4.60 M HCl. You heat a small volume of the solution in a hot water bath to 50 ∘C. If you determine that [CoCl42-] = 0.034 M at 50 ∘C at equilibrium, what must be the equilibrium concentration of [Cl-] at 50 ∘C?

The equilibrium concentration of chloride ions in the solution is 4.532 M

Explanation:

We are given:

Initial molarity of = 0.054 M

Initial molarity of HCl = 4.60 M

Equilibrium molarity of = 0.034 M

The chemical equation for the reaction of and HCl follows:

Or,

Initial:              0.054          4.60    

At eqllm:        0.054-x     4.60-2x           x              6x

Evaluating the value of 'x':

So, equilibrium concentration of = (4.60 - 2x) = [4.60 - 2(0.034)] = 4.532 M

Hence, the equilibrium concentration of chloride ions in the solution is 4.532 M

the answers would be

the first one and the second one