electrode potential

Standard electrode potentials are available in a table of values.

You can do this experiment several times increasing electrode potentials from low to high.

An extract from the table of standard electrode potentials is shown below.

As noted above, changing the electrolyte concentration changes the electrode potential.

Then one looks up the standard electrode potential, E, in volts, for each of the two half reactions.

Yet it is also a strongly electropositive metal, with a high negative electrode potential.

This method of calibration avoids the need to know the standard electrode potential.

A related concept in electrochemistry is the electrode potential at the point of zero charge.

Potentiometer: An instrument that measures the electrode potential of the solution.

The standard electrode potential is the tendency of a bulk material to draw free electrons to itself.

This is because the dissimilar metals have different electrode potentials.

We have thus related the standard electrode potential and the equilibrium constant of a redox reaction.

The difference in voltage between electrode potentials gives a prediction for the potential measured.

The standard electrode potential for the SHE is zero, by definition.

The electrode potential may not be obtained empirically.

Therefore, standard electrode potential is commonly written as standard reduction potential.

The sulfate radical formed in situ has a standard electrode potential of 2.7 V.

Titanium has many different standard electrode potentials depending on the oxidation state it is in.

The calomel electrode is used to work out the electrode potential of half cells.

(written this way by convention) the electrode potential for the half reactions are written as and respectively.

Notation for half-reaction standard electrode potentials is as follows.

The standard electrode potential for this compound is +1.44 V with a half reaction generating the hydrogen sulfate.

Sulfate-reducers require reducing environment; an electrode potential lower than -100 mV is required for them to thrive.

If the electrode is polarizable, then its surface charge depends on the electrode potential.

In the same way given two half-reactions it is possible, with knowledge of appropriate electrode potentials, to arrive at the full (original) reaction.