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.
Answers: 1
ion is used to represent a ![[Hg(H_2O)_4]^{2+}](/tpl/images/1394/5126/65dfb.png)
.
![[Hgl_4]^{2-}](/tpl/images/1394/5126/970b6.png)
. ![[Hg(H_2O)_4]^{2+} +4I^{-} \to [HgI_4]^{2-}+4H_20](/tpl/images/1394/5126/c93e6.png)
![k_f=\frac{[HgI_4]^{2-}}{[Hg(H_2O)_4]^{2+} [I^{-}]^4}](/tpl/images/1394/5126/9ffc5.png)
![[Hg(H_2O)_4]^{2+} +I^{-} \to [HgI(H_2O)_3]^{+}+H_20](/tpl/images/1394/5126/c074d.png)
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In aqueous solution the Hg2+ ion forms a complex with four iodide anions. Write the formation consta...
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