The concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0 × 10–19 M. If 10 mL of this is added to 5 mL of 0.04M solution of the following: FeSO4, MnCl2, ZnCl2 and CdCl2 . in which of these solutions precipitation will take place?
If the ionic product exceeds the Ksp value, then only precipitation can take place.
Before mixing:[S2-]
=\( K_{sp} = 1.0\times 10^{-19}\)
[M2+] = 0.04M
Volume = 10mL
Volume = 5mL
After mixing:[S2-] = ?
and [M2+] = ?
Total volume = (10 + 5) = 15mL
Volume = 15mL
\( [S^{2-}] = \dfrac{1.0\times 10^{-19}\times 10}{15} \)
\( = 6.67\times 10^{-20}M[M^{2+}] \)
\( = \dfrac{0.04\times 5}{15} = 1.33\times 10^{-2}\)
Now, the ionic product
=\( [M^{2+}][S^{2-}]\)
\( = (1.33\times 10^{-2})(6.67\times 10^{-20})\)
\( = 8.87\times 10^{-22}\)
Here, the ionic product of CdS and ZnS exceeds its corresponding Ksp value. Thus, precipitation will occur in ZnCl2 and CdCl2 solutions.
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