A solution with a pH=6.00 is 4.0E-3M in each of the metal cations Mn2+, Fe2+, Co2+, Ni2+, and Zn2+ and 0.10M in H2S. Under these conditions, which of the metal cations will be precipitated as a sulfide? Hint: Calculate IP.
General Equilibrium MS(s) + 2H3O+(aq) = M2+(aq) + 2H2O(l) + H2S(aq); Kspa
Metal Sulfide Kspa
MnS 3E10
FeS 6E2
CoS 3
NiS 8E-1
ZnS 3E-2
a.) Mn2+ and Fe2+
b.) Zn2+ only
c.) Zn2+ and Ni2+
d.) none of the above
I know the answer is d, from the back of my book, I just don't know how to solve it. Thanks a lot
0 answers