Given : `Cu^(2+)+2e rarrCu, E^(@)=+0.34V and AG^(+)+e rarr Ag, E^(@)=+0.80V`. (i) Construct a galvanic cell with these two electrodes. (ii) If at `25^(@)C` the concentration of `Cu^(2+)` is 0.01 (M), what should be the value of concentration of `Ag^(+)` to make the cell potential equal to zero?

Cu^(2+)+2e^(-)hArrCu,E^(0)=+0.34V Ag^(+)+e^(-)hArr Ag, E^(0)=+0.80V For what concentration of Ag^(+) ions will the emf of the cell be zero at 25^(@)C. The concentration of Cu^(2+) is 0.1M. (log 3.919 =0.539).

The standard reduction potential of Cu^(2+)//Cu and Ag^(+)//Ag electrodes are 0.337 and 0.799 V respectively. Construct a galvanic cell using these electrodes so that its standard emf is positive. For what concentration of Ag^(+) will the emf of the cell, at 25^(@)C , be zero if the concentration of Cu^(2+) is 0.01 M?

The standard reduction potential of Cu^(2+)|Cu and Ag^+|Ag electrodes are 0.337 and 0.799 volt respectively. Construct a galvanic cell using these electrodes so that its standard emf is positive. For what concentration of Ag^(+) will the emf of the cell at 25^@ C be zero if the concentration of Cu^(2+) is 0.01M?

The standard reduction potentials of Cu^(2+)//Cu and Ag^(+)//Ag electrodes are 0.337 volt and 0.799 volt respectively. Construct a galvanic cell using these electrols so that its standard e.m.f. is positive. For what concentration of Ag^(+) , will the e.m.f. of the cell at 25^(@)C be zero if the concentration of Cu^(2+) is 0.01 M.

(A) : If E^(0) " of " Cu^(2+)//Cu=+0.34V and E^(0) " of "Ag^(+) // Ag = + 0.80 V then galvanic cell constructed from these is Ag//Ag^(+) // // Cu^(2+ ) // Cu (R) : In any galvanic cell the reaction that takes place is a redox reaction Electrode potentials & EMF

E_(Cu)^(0)=+0.34V and E_(Ag)^(0)=+0.8V" calculate "E_(cell")^(0) .