AgI (s) → Ag^{+} (aq) + I^{-} (aq)

$\overline{){{\mathbf{K}}}_{{\mathbf{sp}}}{\mathbf{}}{\mathbf{=}}\mathbf{\left[}{\mathbf{Ag}}^{\mathbf{+}}\mathbf{\right]}\mathbf{\left[}{\mathbf{I}}^{\mathbf{-}}\mathbf{\right]}}\phantom{\rule{0ex}{0ex}}\mathbf{\left[}{\mathbf{I}}^{\mathbf{-}}\mathbf{\right]}\mathbf{}\mathbf{=}\frac{{\mathbf{K}}_{\mathbf{sp}}}{\left[{\mathrm{Ag}}^{+}\right]}\phantom{\rule{0ex}{0ex}}\mathbf{\left[}{\mathbf{I}}^{\mathbf{-}}\mathbf{\right]}\mathbf{}\mathbf{=}\frac{\mathbf{8}\mathbf{.}\mathbf{51}\mathbf{}\mathbf{\times}\mathbf{}{\mathbf{10}}^{\mathbf{-}\mathbf{}\mathbf{17}}}{\mathbf{2}\mathbf{.}\mathbf{1}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{4}}}$

**[I ^{-}] = 4.0524x10^{-13} M**

A solution contains 2.1×10^{−4} *M* Ag^{+} and 1.6×10^{−3} *M* Pb^{2 + }.

Specify the concentration of I^{-} needed to begin precipitation.

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