The standard reduction potentials are all based on the standard hydrogen electrode.
Standard oxidation potentials can be calculated by reversing the half-reactions and changing the sign of the standard reduction potential.
E0REDUCTION = - E0OXIDATION
Reference: Handbook of Chemistry and Physics, 89th Edition, CRC Press 2008
| Reduction Half-reaction | Reduction Potential - E0 in Volts |
| Ag+ + e- → Ag | 0.7996 |
| Ag2+ + e- → Ag+ | 1.980 |
| Ag3+ + e- → Ag2+ | 1.8 |
| AgBr + e- → Ag + Br- | 0.0713 |
| AgCl + e- → Ag + Cl- | 0.2223 |
| AgF + e- → Ag + F- | 0.779 |
| AgI + e- → Ag + I- | -0.1522 |
| AgNO2 + e- → Ag + 2 NO2- | 0.564 |
| Ag2S + 2 e- → 2 Ag + S2- | -0.691 |
| Ag2S + 2 H+ + 2 e- → 2 Ag + H2S | -0.0366 |
| Al3+ + 3 e- → Al | -1.662 |
| Br2(aq) +2 e- → 2 Br- | 1.0873 |
| Br2(ℓ) +2 e- → 2 Br- | 1.066 |
| Ca2+ + 2 e- → Ca | -2.868 |
| Cd2+ + 2 e- → Cd | -0.4030 |
| Cl2 + 2 e- → 2 Cl-(g) | 1.3583 |
| Cr2+ + 2 e- → Cr | -0.913 |
| Cr3+ + e- → Cr2+ | -0.407 |
| Cr3+ + 3 e- → Cr | -0.744 |
| Cr2O72- + 14 H+ + 6 e- → 2 Cr3+ + 7 H2O | 1.36 |
| Cu+ + e- → Cu | -3.026 |
| Cu2+ + e- → Cu+ | 0.153 |
| Cu2+ + 2 e- → Cu | 0.3419 |
| Cu3+ + e- → Cu2+ | 2.4 |
| F2 + 2 H+ + 2 e- → 2 HF | 3.053 |
| F2 + 2 e- → 2 F- | 2.866 |
| Fe2+ + 2 e- → Fe | -0.447 |
| Fe3+ + 3 e- → Fe | -0.037 |
| Fe3+ + e- → Fe2+ | 0.771 |
| 2 H+ + 2 e- → H2 | 0.0000 |
| H2O2 + 2 H+ + 2 e- → 2 H2O | 1.776 |
| I2 + 2 e- → 2 I- | 0.5355 |
| K+ + e- → K | -2.931 |
| Li+ + e- → Li | -3.0401 |
| Mg+ + e- → Mg | -2.70 |
| Mg2+ + 2 e- → Mg | -2.372 |
| Mn2+ + 2 e- → Mn | -1.185 |
| Mn3+ + e- → Mn2+ | 1.5415 |
| Na+ + e- → Na | -2.71 |
| Ni2+ + 2 e- → Ni | -0.257 |
| O2 + 2 H+ + 2 e- → 2 H2O2 | 0.695 |
| O2 + 4 H+ + 4 e- → H2O | 1.229 |
| Pb2+ + 2 e- → Pb | -0.1262 |
| PbSO4 + 2 e- → Pb + SO42- | -0.3588 |
| Pt2+ + 2 e- → Pt | 1.18 |
| S + 2 e- → S2- | -0.4284 |
| S + 2 H+ + 2 e- → H2S | 0.142 |
| SO42- + H2 + 2 e- → SO32- + 2 OH- | -0.93 |
| Zn2+ + 2 e- → Zn | -0.7618 |
