In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains `Ag^(+) " and " Pb^(+)` at a concentration of 0.10M. Aqueous HCl is added to this solution until be `Cl^(-)` concentration is 0.10M. What will be concentration of `Ag^(+) " and " Pb^(2+)` be at equilibrium ?
(`K_(sp) " for AgCl " = 1.8xx10^(-10)`
`K_(sp) " for " PbCl_(2) = 1.7xx10^(-5)`)

Options

A. `[Ag^+]=1.8xx10^(-9)M [Pb^(2+)]=1.7 xx10^(-3) M`
B. `[Ag^+]=1.8xx10^(-11)M [Pb^(2+)]=1.7 xx10^(-4) M`
C. `[Ag^+]=1.8xx10^(-6)M [Pb^(2+)]=1.7 xx10^(-11) M`
D. `[Ag^+]=1.8xx10^(-11)M [Pb^(2+)]=8.5 xx10^(-5) M`

Answer

A