A solution containing $$M{n^{2 + }},F{e^{2 + }},Z{n^{2 + }}$$ and $$H{g^{2 + }}$$ with a molar concentration of $${10^{ - 3}}M$$ each is treated with $${10^{ - 16}}M$$ sulphide ion solution. Which ions will precipitate first if $${K_{sp}}$$ of $$MnS,FeS,ZnS$$ and $$HgS$$ are $${10^{ - 15}},{10^{ - 23}},{10^{ - 20}}$$ and $${10^{ - 54}}$$ respectively?
A.
$$FeS$$
B.
$$MnS$$
C.
$$HgS$$
D.
$$ZnS$$
Answer :
$$HgS$$
Solution :
$${M^{2 + }} + {s^{2 - }} \to MS$$
Lower the value of $${K_{sp}},$$ lower will be solubility. Hence, $$HgS$$ will precipitate first.
Releted MCQ Question on Physical Chemistry >> Ionic Equilibrium
Releted Question 1
Molten sodium chloride conducts electricitry due to the presence of