Answer: Equilibrium concentration of ![[Cl^-]](https://tex.z-dn.net/?f=%5BCl%5E-%5D) at
 at  is 4.538 M
 is 4.538 M
Explanation:
Initial concentration of  = 0.056 M
 = 0.056 M
Initial concentration of  = 4.60 M
 = 4.60 M
The given balanced equilibrium reaction is,
                ![COCl_2+2Cl^-\rightleftharpoons [CoCl_4]^{2-}+6H_2O](https://tex.z-dn.net/?f=COCl_2%2B2Cl%5E-%5Crightleftharpoons%20%5BCoCl_4%5D%5E%7B2-%7D%2B6H_2O)
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) M
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{[CoCl_4]^{2-}\times [H_2O]^6}{[CoCl_2]^2\times [Cl^-]^2}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BCoCl_4%5D%5E%7B2-%7D%5Ctimes%20%5BH_2O%5D%5E6%7D%7B%5BCoCl_2%5D%5E2%5Ctimes%20%5BCl%5E-%5D%5E2%7D)
Given : equilibrium concentration of ![[CoCl_4]^{2-}](https://tex.z-dn.net/?f=%5BCoCl_4%5D%5E%7B2-%7D) =x =  0.031 M
 =x =  0.031 M
Concentration of  = (4.60-2x) M  =
 = (4.60-2x) M  =  =4.538 M
 =4.538 M   
Thus equilibrium concentration of ![[Cl^-]](https://tex.z-dn.net/?f=%5BCl%5E-%5D) at
 at  is 4.538 M
 is 4.538 M
 
        
             
        
        
        
Explanation:
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