You're provided with a bottle labled [CoCl2.6H2O] = 0.056 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?

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Question:

You're provided with a bottle labled [CoCl2.6H2O] = 0.056 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?

Answers

The equilibrium concentration of Cl⁻ at 50°C is 4.54 M, after the solution of 0.056 M CoCl₂·6H₂O with 4.60 M HCl is heated in a water bath to 50°C. It was calculated knowing that the equilibrium concentration of CoCl₄²⁻ at 50°C is 0.031 M.   The reaction between CoCl₂·6H₂O and HCl is the following:CoCl₂·6H₂O + 2HCl → H₂CoCl₄ + 6H₂O The initial concentrations are:[CoCl₂·6H₂O] = 0.056 M[HCl] = 4.60 MAt equilibrium, we have:CoCl₂·6H₂O + 2HCl → H₂CoCl₄ + 6H₂O0.056-x        4.60-2x         x            6xWe know that the CoCl₄²⁻ concentration at equilibrium is 0.031 M, so:             [tex] [CoCl4^{-2}] = x = 0.031 M [/tex]With this, we can find the equilibrium concentration of Cl⁻ and CoCl₂·6H₂O:[tex] [Cl^{-}] = (4.60 - 2*0.031) M = 4.54 M [/tex]              [tex] [CoCl_{2}\cdot 6H_{2}O] = (0.056 - 0.031) M = 0.025 M [/tex]Therefore, the equilibrium concentration of Cl⁻ is 4.54 M.Find more here:https://brainly.com/question/7145687?referrer=searchResultshttps://brainly.com/question/9173805?referrer=searchResultsI hope it helps you!                      

Answer: Equilibrium concentration of [tex][Cl^-][/tex] at [tex]50^0C[/tex] is 4.538 MExplanation:Initial concentration of [tex]CoCl_2[/tex] = 0.056 MInitial concentration of [tex]Cl^-[/tex] = 4.60 MThe given balanced equilibrium reaction is,                [tex]COCl_2+2Cl^-\rightleftharpoons [CoCl_4]^{2-}+6H_2O[/tex]Initial conc.          0.056 M      4.60 M        0 M       0 M At eqm. conc.     (0.056-x) M   (4.60-2x) M   (x) M    (6x) MThe expression for equilibrium constant for this reaction will be,[tex]K_c=\frac{[CoCl_4]^{2-}\times [H_2O]^6}{[CoCl_2]^2\times [Cl^-]^2}[/tex]Given : equilibrium concentration of [tex][CoCl_4]^{2-}[/tex] =x =  0.031 MConcentration of [tex]Cl^-[/tex] = (4.60-2x) M  = [tex](4.60-2\times 0.031)[/tex] =4.538 M   Thus equilibrium concentration of [tex][Cl^-][/tex] at [tex]50^0C[/tex] is 4.538 M

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