The standard reduction potential for `Cu^(2+)|Cu` is +0.34V. Calculate the reduction potential at pH=14 for above couple. `K_(sp)` of `Cu(OH)_2` is `1.0xx10^-19`.

The standard electrode potential for Daniell cell is 1. IV. Calculate the standard Gibbs energy for the reaction: Zn(s) + Cu^(2+) (aq) rarr Zn^(2+)(aq) + Cu(s)

The standard reduction potential of normal calomel electrode and reduction potential of saturated calomel electrodes are 0.27 and 0.33 volt respectively. What is the concentration of Cl^- in saturated solution of KCL?

The standard reduction potential for the half cell: NO_3^- (aq)+2H^+ (aq)+barerarrNO_2+H_2O is 0.78v. What will be the reduction of the half cell in a neutral solution? Assume all the other species to be at unit concentration.

What is the pH of a saturated solution of Cu(OH)_(2) ? (K_(sp)=2.6xx10^(-19)

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Ag^+ (aq) and Cu(s)

The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is

The equilibrium constant of the following redox reaction is 298K is 1xx10^8 2Fe^(3+)(aq)+2I^-(aq)Leftrightarrow2Fe^(2+)(aq)+I_2(s) If the standard reduction potential of iodine becoming iodide is +0.54V, what is the standard reduction potential of Fe^(3+)/Fe^(2+) ?

The standard reduction potentials of Co^(2+) and Co^(3+) are -0.28 V and 1.8 V respectively. Which should be a better oxidising agent in water : Co^(2+) or Co^(3+) ?

Calculate the reduction potential of the following electrode at 298K Pt,Cl_2(2.5atm)|HCl(0.01M), E^@ Cl_2|2Cl^-=1.36V .

When the silver electrode having reduction potential 0.80V is attached to NHE, will it act as anode or cathode?