# Problem: A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M in Ag+.How much Na2SO4 solution must be added to initiate the precipitation?

###### FREE Expert Solution

Recall:

$\overline{){{\mathbf{K}}}_{{\mathbf{sp}}}{\mathbf{=}}\frac{\mathbf{products}}{\overline{)\mathbf{reactants}}}}$

$\frac{{\mathbf{K}}_{\mathbf{sp}}}{\mathbf{\left[}{\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}}\mathbf{=}\frac{\overline{)\mathbf{\left[}{\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}}\mathbf{\left[}{\mathbf{SO}}_{\mathbf{4}}^{\mathbf{2}\mathbf{-}}\mathbf{\right]}}{\overline{)\mathbf{\left[}{\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\mathbf{\left[}{\mathbf{SO}}_{\mathbf{4}}^{\mathbf{2}\mathbf{-}}\mathbf{\right]}\mathbf{=}\frac{{\mathbf{K}}_{\mathbf{sp}}}{\mathbf{\left[}{\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}}$

3.55×10-4 M

87% (130 ratings)
###### Problem Details

A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M in Ag+.

How much Na2SO4 solution must be added to initiate the precipitation?