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A solution containing Mn^(2+),Fe^(2+),Zn...

A solution containing `Mn^(2+),Fe^(2+),Zn^(2+)andHg^(2+)` with a molar concentration of `10^(-3)` M each is treated with `10^(-16)M` sulphide ion solution. Which ion will precipitate first if `K_(sp)` of MnS, FeS, ZnS and HgS are `10^(-15),1-^(-23),10^(-20)and10^(-54)` respectively ?

A

FeS

B

MgS

C

HgS

D

ZnS

Text Solution

Verified by Experts

The correct Answer is:
C
Minimum `S^(2-)` concentration would be required for precipitation of least soluble HgS
For HgS , `S^(2-)`required for precipitation is `[S^(2-)] = K_(sp)/[Hg^(2+)] = 10^(-54)/10^(-3)M`
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