A 0.10 M Mn 2+ solution is saturated with H2S. At what pH will MnS begin to precipitate? [H2S] sat'd=0.10M
We start with the solubility product expression for MnS.
<br>Ksp = [Mn2+]* [S2-] = 3 * 10^-13
<br>We then substitute what we know about the Mn2+ ion concentration into this equation and calculate the S2- ion concentration at which MnS just starts to precipitate.
<br>[0.10]*[S2-] = 3 * ...
Answer with more than 20 step explanations.