The potential range is not usually 0 to +1 V!

Although determined by the experiment, we can assume that the potential limits will be dictated by the decomposition of the solvent. If you use water, the limits will be 0 (hydrogen evolution reaction) and somewhere above 1.23 V (this will depend on how well your working electrode catalyses the oxygen-evolution reaction) vs. the reversible hydrogen electrode. But if you use other reference electrode, the limits will be different. The limits will also change if you use a pH-independent reference electrode (like the SGE, SCE or Ag/AgClsat. electrodes) and you change the pH. Other factor that can limit the (positive) limit or your experiments is the beginning of the oxidation of your working electrode, particularly if oxidation leads to dissolution.

The potential range depends on what electrode you use and what you are trying to detect. From your question I have the impression that you are using a solid electrode and with these you can go to about +1 V, but you can go as far negative as perhaps -1 V too. If you use a mercury electrode then you sweep between -1.4 and around 0 V, depending on water pH for instance. If you detect something organic you may have to scan positive, if you are detecting a metal, then may have to scan between -1.4 and 0.2 V. So, it depends on a few parameters and it is not restricted to between 0 and +1 V.

Hi Donya,

This depends of material under study, although is a commun range in Pt. Below 0 V vs RHE it produce the HER, above 1 V vs RHE, some materials dissolves,oxidize irreversebly, or whatever. For my materials I use such range to compare with platinum for ORR

Regards

This is not really true. The setting potential range usually depends on the sample that you invenstigate and the reference electrode that you use.

The hackground limits are the potentials where the cathodic and anodic currents start to ftow at a working eJectrode when it is immersed in a solution containing only an elecIrolyle added to decrease the solution resistance (a supporting electrolyte). Moving the potential to more extreme values the background limits (i.e., more negative than the limit for H2 evolution or more positive than that for electrode material or electrolite oxidation) simply causes the current to increase sharply with no additional electrode reactions, because the reactants are present at high concentrations (Bard and Faulkner “Electrochemical Methods”).

The potential range is usually between 0 to +1 V because at potential lower than 0 interferes dissolved oxygen the reduction of potential and greater than 1 V, the electrolyte is oxidized in aqueous medium.

For nonaqueous solvents, the range is critically dependent on purity and especially on elimination of traces of water (see figure E2 Bard).

I'm not sure. He does not say anything about electrodeposition in his question

Hi Ignacio. Donya only says linear sweep voltammetry, no stripping voltammetry

I do agree with Angel Cuesta. The mentioned potential is not mandatory but it is dependent on working and reference electrode.

The hackground limits are the potentials where the cathodic and anodic currents start to flow at a working eJectrode when it is immersed in a solution containing only an elecIrolyle added to decrease the solution resistance (a supporting electrolyte). Moving the potential to more extreme values the background limits (i.e., more negative than the limit for H2 evolution or more positive than that for electrode material or electrolite oxidation) simply causes the current to increase sharply with no additional electrode reactions, because the reactants are present at high concentrations (Bard and Faulkner “Electrochemical Methods”).

The potential range is usually between 0 to +1 V because at potential lower than 0 interferes dissolved oxygen the reduction of potential and greater than 1 V, the electrolyte is oxidized in aqueous medium.

For nonaqueous solvents, the range is critically dependent on purity and especially on elimination of traces of water (see figure E2 Bard and Faulkner “Electrochemical Methods”).