the standard reduction potenital of a silver chloride electrode is 0.2 V and that of a silver electrode is 0.79 V. The maximum amount of AgCl that can dissolve in `10^(6)`L of a 0.1 M `AgNO_(3)` solution is:

Options

A. 0.5 mmol
B. 1.0 mmol
C. 2.0 mmol
D. 2.5 mmol

Answer

B

Explanation

`AgCl+e^(-)toAgtoCl^(-)" "E^(@)=0.2V`
`underline(AgtoAg^(+)+e^(-)" "E^(@)=-0.79V`
`AgCloverset(e^(-))toAg^(+)+Cl^(-)" "E^(@)=-0.59V`
`E^(@)=(0.059)/(n)logKimplies-0.59=(0.059)/(1)logK_(SP)impliesK_(SP)=10^(-10)`
Now solubility of `AgCl` in 0.1 M `AgNO_(3)`
`S(S+0.1)=10^(-10)impliesS=10^(-9)mol//L`
Hence 1 mole dissolves in `10^(9)L` L solution.
Hence in `10^(6)L` L amount that dissoves in 1 m mol.