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?

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Аноним Аноним · Answer 1 · 2020-03-26T05:08:36+01:00

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

Explanation:

We are given:

Initial molarity of [tex][CoCl_2.6H_2O][/tex] = 0.054 M

Initial molarity of HCl = 4.60 M

Equilibrium molarity of [tex][CoCl_4]^{2-}[/tex] = 0.034 M

The chemical equation for the reaction of [tex][CoCl_2.6H_2O][/tex] and HCl follows:

[tex][CoCl_2.6H_2O]+2HCl\rightarrow H_2[CoCl_4]+6H_2O[/tex]

Or,

[tex][CoCl_2.6H_2O]+2Cl^-\rightarrow [CoCl_4]^{2-}+6H_2O[/tex]

Initial: 0.054 4.60

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

Evaluating the value of 'x':

[tex]x=0.034[/tex]

So, equilibrium concentration of [tex]Cl^-[/tex] = (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