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You're provided with a bottle labled [CoCl2.6H2O] = 0.051 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-] = 0.031 M at 50 ∘C at equilibrium, what must be the equilibrium concentration of [Cl-] at 50 ∘C?

Respuesta :

Answer : The concentration of [tex]Cl^-[/tex] at equilibrium is 4.54 M

Explanation :

The equilibrium reaction will be:

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

Initial           0.051 M         4.60 M          0

At eqm.     (0.051-x) M     (4.60-2x) M    x

As we are given:

Concentration of [tex][CoCl_4]^{2-}[/tex] at equilibrium = 0.031 M

That means,

x = 0.031 M

Concentration of [tex]Cl^-[/tex] at equilibrium = (4.60-2x) M = [4.60-2(0.031)] M = 4.54 M

Hence, the concentration of [tex]Cl^-[/tex] at equilibrium is 4.54 M

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