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A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at...

A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at 0.010 M, was saturated with H2S(g) at room temperature. Assume that the pH of the solution remains constant and that the [H2S]sat = 0.10 M. The Ksp for MnS9S) is 2.5 x 10-13 , Ksp for CdS(s) is 8.0 x 10 -27 and Ksp for FeS(s) is 6.3 x10-18 . For H2S:Ka1=1.3 x 10-7. Ka2=8.5 x 10-14. Calculate the equilibrium concentrations of Mn2+(aq),Cd2+(aq), and Fe2+(aq).

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The ph of the solution is 0,5228 (ph = -log[H+]) , this mean, ph is to low to let Fe2+,Mn2+ and Cd+2 precipitate, and also the concentration of S-2 will be too low, [S-2] = 1.2277x10-20, we could say that the concentration of those ions stay basically constant.

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