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Question

An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What is the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS?
Use KSP(ZnS)=1.25×1022 and overall dissociation constant of H2S.
KNET=K1K2=1×1021

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Solution

For ZnSZn2++S2

Ksp(ZnS)=[Zn+2][S2]
To stop precipitation of ZnS,
[Zn+2][S2]Ksp(ZnS)
[S2]1.25×10220.05
For H2S2H++S2

[S2]=KNET×[H2S][H+]2

KNET×[H2S][H+]21.25×1022102×5
[H+]21021×101×41020
[H+]2×101=0.2
Alternate:
[Zn+2][S2]K
[S2)1.25×10220.05=14×1020
H2S2H++S2
[H+]2=K1K2×[H2S][S2]=1021×0.1[S2]
[S2]=1022[H+]214×1020
[H+]0.2


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