Before reading this post, please read the first post here : Physical Chemistry - Electrochemistry - 1
STANDARD HYDROGEN ELECTRODE
A standard hydrogen electrode is prepared by dipping a Platinum strip in around which gas at atm pressure is bubbled in an inverted test tube. At , its standard reduction potential is defined to be zero.
STANDARD ELECTRODE POTENTIALS
As discussed in the previous post, the potential of any electrode is the potential difference between it and the electrolyte surrounding the electrode.
However, this potential depends upon the nature of the metal, concentration of the metallic ions in solution and the temperature of the solution.
Hence, again, we have to define a standard.
When the ions are at unit activity and the temperature is (), the potential difference is called a Standard Electrode Potential ().
the potential of a single electrode cannot be determined, but the potential difference between two electrodes can be accurately measured.
By convention, the electrode potential of S.H.E has been assigned a value of zero Volts.
POSITIVE(+) AND NEGATIVE(-) POTENTIALS
If, on combining an electrode with the S.H.E, a reduction process (gain of electrons) occurs at the electrode, the potential of the electrode is called as reduction potential.
It is given a "+" sign as reduction potential or a "-" sign as oxidation potential.
On the other hand, if, on combining an electrode with the S.H.E, an oxidation process (loss of electrons) occurs at , the electrode potential (half-cell potential) is called as the oxidation potential.
It is given a "+" sign as oxidation potential or a "-" sign as reduction potential.
Thus, in short,
at Standard conditions,
Oxidation Potential for any half cell (Reduction Potential)
Reduction Potential for any half cell (Oxidation Potential)
In the next post, we shall discuss, the experimentally determined Electrochemical Series, and how it is used to determine the EMF of any cell.
Read the next post here : Physical Chemistry - Electrochemistry - 3