Let the solubilities of `AgCl` in pure water be `0.01 M CaCl_(2)`, `0.01 M NaCl` and `0.05 M AgNO_(3)` be `s_(1)`, `s_(2)`, `s_(3)` and `s_(4)` respectively. What is the correct order of these quantities? Neglect any complexation.

Options

A. `S_(1)gtS_(2)gtS_(3)gtS_(4)`
B. `S_(1)gtS_(3)gtS_(2)gtS_(4)`
C. `S_(1)gtS_(2)=S_(3)gtS_(4)`
D. `S_(1)gtS_(3)gtS_(4)ltS_(2)`

Answer

B

Explanation

`AgClhArrAg^(+)+Cl^(-)`
In `CaCl_(2)`
`underset(0.01)(CaCl_(2))hArrunderset(0.01)(Ca^(+2))+underset(2xx0.01)(2Cl^(-))`
In `NaCl`
`underset(0.01)(NaCl)hArrunderset(0.01)(Na^(+))+underset(0.01)(Cl^(-))`
In `AgNO_(3)`
`underset(0.05)(AgNO_(3))hArrunderset(0.05)(Ag^(+))+underset(0.05)(Cl^(-))`
common ion effect is maximum in `AgNO_(3)`
So, `S_(1)gtS_(3)gtS_(2)gtS_(4)`