The `EMF` of concentration cell consisting of two zinc electrodes, one dipping into `M//4` solution of `ZnSO_(4)` and the other into `M//16` solution of the same salt at `25^(@)C` is

The EMF of a concentration cell consisting of two zinc electrodes, one dipping into M/4 sol. Of zinc sulphate and the other into M/6 sol. Of the same salt at 25^(@) C. is:

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknonw concentration. It other half cell consists of a zinc electrode dipping in 1.0M solution of Zn(NO_3)_2 . A voltage of 1.48V is measure for this cell. Use this information to calculate the concentration of silver nitrate solution used (E_(Zn^(2+)//Zn)^0=-0.76V,E_(Ag^+//Ag)^0=+0.80V)

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknown concentration . Its other half-cell consists of a zinc electrode dipping in 1.0 M solution of Zn(NO_(3))_(2) . A voltage of 1.48 V is measured for this cell . Use this information to calculate the concentration of silver nitrate solution used. (E_(Zn^(2+)|Zn)^(@) = -0.76V , E_(Ag^(+)|Ag)^(@) = + 0.80V ).

A galvanic cell consists of two hydrogen electrodes. One is in a 1.0 M H^(+) solution and other in a solution of unknown pH. The cell potential is 0.025V. The unknown pH is

What is the potential of a half-cell consisting of zinc electrode in "0.01 M ZnSO_(4) solution 25^(@)C. E^(@) = 0.763 V.

What is the potential of a half-cell consisting of zinc electrode in "0.01 M ZnSO_(4) solution 25^(@)C. E^(@) = 0.763 V.

What is the potential of a half-cell consisting of zinc electrode in "0.01 M ZnSO_(4) solution 25^(@)C. E^(@) = 0.763 V.

The emf of a cell consisting of a copper and a lead electrode immersed in 1M solution of salts of these metals is 0.47V. Will the emf change if 0.001 solutions are taken?