# At what conc. of the Ba2+ ions would BaSO4 start precipitating from a solution in which the concentration of the Ba2+ ions is 0.0010M(Ksp of BaSO4 is 10^-10)

We have to find the concentration of Ba

^{2+}ions at which BaSO

_{4 }would start precipitating.

So, assuming that the concentration mentioned by you is of SO

_{4}

^{2}

^{-}ions, and not Ba

^{2+}ions,

we can find use the solubility product to get the concentration of Ba

^{2+}ions.

${K}_{sp}=\left[B{a}^{2+}\right]\left[S{{O}_{4}}^{2-}\right]\phantom{\rule{0ex}{0ex}}{10}^{-10}=\left[B{a}^{2+}\right]\left[0.001\right]\phantom{\rule{0ex}{0ex}}\left[B{a}^{2+}\right]=\frac{{10}^{-10}}{{10}^{-3}}={10}^{-7}M$

Hope it helps.

Regards

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