The ion precipitating first when a solution containing 0.01 M each of Pb2+,Zn2+,Mn2+ and Co2+ is saturated with H2S is (which provides 1.0×10−14M of S2−n the solution) is (Given: Ksp(PbS)=2.3×10−27M2,Ksp(ZnS)=1.0×10−21M2,Ksp(MnS)=7.9×10−13M2)

The ion precipitating first when a solution containing $0.01 M$ each of ${Pb}^{2 +}, {Zn}^{2 +}, {Mn}^{2 +}$ and ${Co}^{2 +}$ is saturated with $H_{2} S$ is (which provides $1.0 \times 10^{- 14} M$ of $S^{2 -}$ n the solution) is
(Given: $K_{sp} (PbS) = 2.3 \times 10^{- 27} M^{2}, K_{sp} (ZnS) = 1.0 \times 10^{- 21} M^{2}, K_{sp} (MnS) = 7.9 \times 10^{- 13} M^{2}$ )

A
${Pb}^{2 +}$
B
${Zn}^{2 +}$
C
${Mn}^{2 +}$
D
${Co}^{2 +}$

Solution:

Lesser the value of $K_{sp}$ , earlier the salt precipitates. Hence, ${Pb}^{2 +}$ is precipitated first.

When cations and anions in an aqueous solution interact, a precipitate, an insoluble ionic solid, is created. The common ionic solids' solubility principles can be used to determine whether or not such a reaction takes place.

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Solution:

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