Question

In aqueous solution the Hg2+ ion forms a complex with four iodide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex.

Answer 1

Answer:

Following are the solution to the given question:

Explanation:

In the aqueous solution of $Hg^{2+}$ ion is used to represent a $[Hg(H_2O)_4]^{2+}$.

It is used to form a complex with iodide ions as $[Hgl_4]^{2-}$.  

Conversion reaction:

$[Hg(H_2O)_4]^{2+} +4I^{-} \to [HgI_4]^{2-}+4H_20$

Following are the formation constants:

$k_f=\frac{[HgI_4]^{2-}}{[Hg(H_2O)_4]^{2+} [I^{-}]^4}$

Following are the first step to the conversion:  

$[Hg(H_2O)_4]^{2+} +I^{-} \to [HgI(H_2O)_3]^{+}+H_20$