**BaSO**_{4}**(s) ****⇌ Ba ^{2+}(aq)**

The **K _{sp} expression** for BaSO

${\mathbf{K}}_{\mathbf{sp}}\mathbf{=}\mathbf{\left[}{\mathbf{Ba}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}\mathbf{\left[}{{\mathbf{SO}}_{\mathbf{4}}}^{\mathbf{2}\mathbf{-}}\mathbf{\right]}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{1}\mathbf{.}\mathbf{1}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{10}}}{\mathbf{0}\mathbf{.}\mathbf{0758}}\mathbf{=}\frac{\mathbf{\left(}\overline{)\mathbf{0}\mathbf{.}\mathbf{0758}}\mathbf{\right)}\mathbf{\left(}\mathbf{x}\mathbf{\right)}}{\overline{)\mathbf{0}\mathbf{.}\mathbf{0758}}}$

Calculate the concentration of sulfate ion when BaSO_{4} just begins to precipitate from a solution that is 0.0758 M in Ba^{2+}.

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