To find the standard potential of `M^(3+)//M` electrode, the following cell is constituted :
`Pt|M|M^(3+) (0.0018 mol^(-1) L)||Ag^(+) (0.01 mol^(-1) L(|Ag`
The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the half reaction `M^(3+)+3e^(-) rarr M`. `E_(Ag^(+)//Ag)^(@)=0.80` volt.

To find the standard potential of M^(3+)//M electrode , the following cell is constituted : Pt|M|M^(3+((.001moLL^(-1)|| Ag ^(+) ((0.01moLL^(-1))| Ag. The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction M^(3+)+ 3e^(-) to M at 298 K will be : (Given E_(Ag^(+)//Ag^(@) at 298 K = 0.80 Volt)

To find the standard potential of M^(3+)//M electrode , the following cell is constituted : Pt|M|M^(3+((.001moLL^(-1)|| Ag ^(+) ((0.01moLL^(-1))| Ag. The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction M^(3+)+ 3e^(-) to M at 298 K will be : (Given E_(Ag^(+)//Ag^(@) at 298 K = 0.80 Volt)

Converting measured potentials to standard potentials: In investigating the properties of rare and expensive metal such as rhenium (Z = 75) , it is both impractical and uneconomical to prepare cells with standard concentrations. The find the standard potential of the Re^(3+)(aq.)//Re(s) electrode, the following cell is constructed: Pt(s) | Re(s)| Re^(3+)(aq., 0.018 M)|| Ag^(+)(aq., 0.010 M) | Ag(s) The potential of this cell is found to be 0.42 V with the Re electrode as the node. Calculate the standard potential of the half reaction Re^(3+)(aq.)+3e^(-)hArrRe(s) Strategy: Table 3.1 lists the E_(@) for the Ag^(+)(aq.) | Ag(s) electrode as 0.80 . We can find the E^(@) of the other electrode by finding the E^(@) of the cell through the application of the Nernst equation.

Calculate the reduction potentials for the following half cells: Ag|Ag^+ (10^-5 M),E_(Ag^+,Ag)^@=0.80V

Calculate the standard reduction potential of (Ag^+)/ (Ag) electrode when the cell potential for the cell Cu | Cu^2+ (1M) | | Ag^+(1M) | Ag is 0.46 V .

E_(Ag^(+),Ag)^(0) = 0.8 V . Calculate the single electrode potential in 0.01 M Ag^(+)

Calculate the emf of the following cell at 25^(@)C Ag(s)|AgNO_(3) (0.01 M)||AgNO_(3) (0.05 M)|Ag (s)

The standard emf of the following cell is 0.552 V. Cd|cd^(2+) (1M)|Ag^+(1M)|Ag If the standard potential of Cd electrode is 0.431V. what is the standard potential of Ag electrode?