A silver wire dipped in `0.1M HCI` solution saturated with `AgCI` develops a potential of `-0.25V`. If `E_(Ag//Ag^(+))^(@) =- 0.799V`, the `K_(sp)` of `AgCI` in pure water will be

What would be the electrode potential of a silver electrode dipped in a saturated solution of AgCl in contact with 0.1 M KCl solution at 25^(@)C ? E^(c-)._(Ag^(o+)|Ag)=0.799 V K_(sp) of AgCl=1xx10^(-10)

What would be the electrode potential of a silver electrode dipped in a saturated solution of AgCl in contact with 0.1 M KCl solution at 25^(@)C ? E^(c-)._(Ag^(o+)|Ag)=0.799 V K_(sp) of AgCl=1xx10^(-10)

What would be the electrode potential of a silver electrode dipped in a saturated solution of AgCl in contact with 0.1 M KCl solution at 25^(@)C ? E^(c-)._(Ag^(o+)|Ag)=0.799 V K_(sp) of AgCl=1xx10^(-10)

A copper wire is dipped in silver nitrate solution in beaker A and a silver wire is dipped in a solution of copper sulphate kept in a beaker B . If the standard electrode potential for Cu^(2+) + 2e^(-) to Cu is +0.34 for Ag^(+) + e^(-) to Ag is 0.80 V Predict in which beaker the ions present will get reduced ?

For Zn^(2+) //Zn, E^(@) =- 0.76 , for Ag^(+)//Ag, E^(@) = -0.799V . The correct statement is

For Zn^(2+) //Zn, E^(@) =- 0.76 , for Ag^(+)//Ag, E^(@) = -0.799V . The correct statement is

For Zn^(2+) //Zn, E^(@) =- 0.76 , for Ag^(+)//Ag, E^(@) = -0.799V . The correct statement is