For two redox couple `A^(2+)//A and B^(2)//B` the reduction potential values are -1.28V and +0.34V. Which is a strong reduction agent? Can both of them displace `H_(2)` from dilute hydro chloric acid? Why?

Consider the following four electrode : A = Cu^(2+) (0.0001 M)// Cu(S) B= Cu^(2+) (0.1M)//Cu(s) C = Cu^(2+) (0.01 M )//Cu(s) D) = Cu^(2+) (0.001 M )// Cu(s) If the standard reduction potential of Cu^(+2)// Cu is + 0.34 V , the reduction potential ( in volts ) of the above electrodes follow the order

For the cell reaction, Mg_((s))+Cu_((aq))^(2+) rarr Cu_((s)) +g^(2+)(aq.) the standard reduction potentials of Mg and Cu are -2.37 V and 0.34 V respectively. The e.m.f. of the cell is

The standard reduction potential for Cu^(2+)//Cu is +0.34V. If ksp of Cu(OH)_2 is 1.0 xx 10^(-19) , the reduction potential at pH =14 for the above couple is

The cell reaction of a cell is Mg(s) + Cu^(2+)(aq) to Cu(s) + Mg^(2+)(aq) If the standard reduction potentials of magensium and copper are -0.33 and +2.38 V respectively, the emf of the cell is

Standard reduction electrode potential of three metals A, B and C are respectively +0.05 V, -3.0 and -1.2 V. The reducing powers of

Aluminium displaces hydrogen from dilute HCl whereas silver does not. The e.m.f. of a cell prepared by combining Al//Al^(3+) and Ag//Ag^(+) is 2.46 V. The reduction potential of silver electrode is + 0.80 V. The reduction potential of aluminium electrode is

What is the reduction electrode potential (in volts) of copper electrode, when [Cu^(2+)] = 0.01 M is in a solution at 25^@ C? ( E^@ of Cu^(2+)//Cu electrode is + 0.34 V.)