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

Explanation

`{:(" "AgCl+e" "rarr" "Ag+Cl^(-)," "E^(@)=0.2V),( " "Ag" "rarr" "Ag^(+)+e," "E^(@)=-0.79V),(_),(" "AgCl" "rarr" "Ag^(+)+Cl^(-)," "E^(@)=-0.59,):}`
`therefore" "E^(@)=(0.059)/(n)logK" or, "-0.59=(0.059)/(1)logK_(sp)`
`"or, "logK_(sp)=-(0.59)/(0.059)" "therefore" "K_(sp)=10^(-10)`
Solubility of AgCl in 0.1 M `AgNO_(3)=S(S+0.1)`
`therefore" "S(S+0.1)=10^(-10)" or, "S=10^(-9)M`
`therefore" Amount of AgCl dissolved in "10^(9)L" solution = 1 mol."`
`therefore" Amount of AgCl that dissolves in "10^(6)L" of the solution"`
`=(1)/(10^(9))xx10^(6)=10^(-3)"mol"="1.0 mmol"`