The standard reduction potential of a silver chloride electrode (metal -sparingly soluble salt electrode) is `0.209V` and for silver electrode is `0.80V`. If the moles of `AgCl` that can dissolve in `10L` of a `0.01M NaCl` solution is represented as `10^(-z)` then find the value of `z`.

Options

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

Answer

B

Explanation

`({:(AgCl +1e^(-)toAg+Cl^(-) " " E^@=0.2 V),(" " Ag to Ag^+ +1e^(-) " " E^@= -0.79 V):})/ {:"AgCl" overset(1e^(-))toAg^+ + Cl^(-) " " E^@=-0.59 V:}`
`E^@=0.0599/n"log" K implies -0.59=0.059/1"log" K_(SP)`
`implies K_(SP)=10^(-10)`
Now solubility of AgCl in 0.1 M `AgNO_3`
`S(S+0.1)=10^(-10) implies S=10^(-9)` mol/L
Hence 1 mole dissolves in `10^6` solution
hence in `10^6` L amount that dissolves in 1 m mol.