Consider the cell Ag|AgBr(s)|Cr^(-)||Cl^(-)|AgCl(s)|Ag at 25^(@)C the solubility product constants of AgBr & AgCl are respectively 5xx10^(-13)&1xx10^(-10). For what ratio of the concentrations of Br^(-) & Cl^(-) ions would the e.m.f. of the cell be zero?

Consider the cell Ag|AgBr(s)|Cr^(-)||Cl^(-)|AgCl(s)|Ag at 25^(@)C the

1.	Consider the cell Ag\|AgBr(s)\|Cr^(-)\|\|Cl^(-)\|AgCl(s)\|Ag at 25^(@)C the solubility product constants of AgBr & AgCl are respectively 5xx10^(-13)&1xx10^(-10). For what ratio of the concentrations of Br^(-) & Cl^(-) ions would the e.m.f. of the cell be zero?
Answer» Solution :If CELL is taken to be conc, cell `E_(cell)^(@)=0` Anode: `AgtoAg_(a)^(+)+e^(-)` cathode: `underline(Ag_(c)^(+)+e^(-)TOAG)` `AghArrAg_(a)^(+)` From nearest EQ, `E_(cell)=E_(cell)^(@)-(0.059)/(1)log(([Ag^(+)]_(a))/([Ag^(+)]_(c)))implies0=0-(0.059)/(1)log(([Ag^(+)]_(a))/([Ag^(+)]_(c)))` `therefore[Ag^(+)]_(a)=[Ag^(+)]_(c)implies(K_(sp)" of " AGBR)/([Br^(-)])=(K_(sp)" of " AgCl)/([Cl^(-)])` or, `(5xx10^(-13))/(10^(-10))=([Br^(-)])/([Cl^(-)])=([Br^(-)])/([Cl^(-)])=(1)/(200)`