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First group of basic radicals (cation) i...

First group of basic radicals (cation) involve analysis of presence of `Pb^(2+), Ag^(+)` and `Hg_(2)^(+2)` ions in the salt. The chloride salts of these metal ions are sparingly soluble in water and their `K_(sp)` values are as follows.
`K_(sp) [PbCl_(2)] = 10^(-12), K_(sp)[AgCl] = 10^(-10), K_(sp)[Hg_(2)Cl_(2)] = 10^(-18)`
Then sequence of precipitation of these salts on adding dilute HCl to the equimolar mixture of these metal ions will be :

A

`PbCl_(2), AgCl` and then `Hg_(2)Cl_(2)`

B

`Hg_(2)Cl_(2), PbCl_(2)` and then AgCl

C

`AgCl, PbCl_(2)` and then `Hg_(2)Cl_(2)`

D

`Hg_(2)Cl_(2), AgCl` and then `PbCl_(2)`

Text Solution

Verified by Experts

The correct Answer is:
D
On using equimolar mixture of these metal ions the required `Cl^(-)` concentration is in order `Hg_(2)Cl_(2) lt AgCl lt PbCl_(2)`
Hence sequence of ppt. will follow this order.
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