# Problem: Calculate the concentration of sulfate ion when BaSO4 just begins to precipitate from a solution that is 0.0758 M in Ba2+.

###### FREE Expert Solution

BaSO4(s)  Ba2+(aq) + SO42–(aq) The Ksp expression for BaSO4 is:

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

99% (483 ratings) ###### Problem Details

Calculate the concentration of sulfate ion when BaSO4 just begins to precipitate from a solution that is 0.0758 M in Ba2+.

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