Electrode Potential, Standard
Standard Electrode Potentials in Acidic Aqueous Solution (a table for basic solution is below)
at 25 °C.
You can change the number of rows shown per page (navigate using "previous" and "next" at the bottom of the page), or search the table.
| Acidic Solution | Standard Electrode Potential, E° (volts) |
|---|---|
|
F2(g) + 2e− ⟶ 2 F−(aq)
|
2.87
|
|
Co3+(aq) + e− ⟶ Co2+(aq)
|
1.92
|
|
Au+(aq) + e− ⟶ Au(s)
|
1.83
|
|
H2O2(aq) + 2 H+(aq) + 2 e− ⟶ 2 H2O(ℓ)
|
1.763
|
|
Ce4+(aq) + e− ⟶ Ce3+(aq)
|
1.72
|
|
Pb4+ (aq) + 2 e− ⟶ Pb2+(aq)
|
1.69
|
|
PbO2(s) + SO42− (aq) + 4 H+(aq) + 2 e− ⟶ PbSO4(s) + 2 H2O(ℓ)
|
1.690
|
|
NiO2(s) + 4 H+(aq) + 2 e− ⟶ Ni2+(aq) + 2 H2O(ℓ)
|
1.68
|
|
2 HClO(aq) + 2 H+(aq) + 2 e− ⟶ Cl2(g) + 2 H2O(ℓ)
|
1.63
|
|
Au3+(aq) + 3 e− ⟶ Au(s)
|
1.52
|
|
MnO4− (aq) + 8 H+(aq) + 5 e− ⟶ Mn2+(aq) + 4 H2O(ℓ)
|
1.51
|
|
BrO3−(aq) + 6 H+(aq) + 5 e− ⟶ 1⁄2 Br2(aq) + 3 H2O(ℓ)
|
1.478
|
|
2 ClO3−(aq) + 12 H+(aq) + 10 e− ⟶ Cl2(g) + 6 H2O(ℓ)
|
1.47
|
|
Cr2O72−(aq) + 14 H+(aq) + 6 e− ⟶ 2 Cr3+(aq) + 7 H2O(ℓ)
|
1.36
|
|
Cl2(g) + 2 e− ⟶ 2 Cl−(aq)
|
1.358
|
|
N2H5+(aq) + 3 H+(aq) + 2 e− ⟶ 2 NH4+(aq)
|
1.275
|
|
MnO2(s) + 4 H+(aq) + 2 e− ⟶ Mn2+(aq) + 2 H2O(ℓ)
|
1.23
|
|
O2(g) + 4 H+(aq) + 4 e− ⟶ 2 H2O(ℓ)
|
1.229
|
|
ClO4−(aq) + 2 H+(aq) + 2 e− ⟶ ClO3−(aq) + H2O(ℓ)
|
1.201
|
|
IO3−(aq) + 6 H+(aq) + 5 e− ⟶ 1⁄2 I2(aq) + 3 H2O(ℓ)
|
1.195
|
|
Pt2+(aq) + 2 e− ⟶ Pt(s)
|
1.188
|
|
Br2(ℓ) + 2 e− ⟶ 2 Br−(aq)
|
1.066
|
|
[AuCl4]−(aq) + 3 e− ⟶ Au(s) + 4 Cl−(aq)
|
1.00
|
|
NO3−(aq) + 4 H+(aq) + 3 e− ⟶ NO(g) + 2 H2O(ℓ)
|
0.96
|
|
NO3−(aq) + 3 H+(aq) + 2 e− ⟶ HNO2(aq) + H2O(ℓ)
|
0.94
|
|
Pd2+(aq) + 2 e− ⟶ Pd(s)
|
0.915
|
|
2 Hg2+(aq) + 2 e− ⟶ Hg22+(aq)
|
0.9110
|
|
Hg2+(aq) + 2 e− ⟶ Hg(ℓ)
|
0.8535
|
|
SbCl6−(aq) + 2 e− ⟶ SbCl4−(aq) + 2 Cl−(aq)
|
0.84†
|
|
Ag+(aq) + e− ⟶ Ag(s)
|
0.7991
|
|
Hg22+(aq) + 2 e− ⟶ 2 Hg(ℓ)
|
0.7960
|
|
Fe3+(aq) + e− ⟶ Fe2+(aq)
|
0.771
|
|
[PtCl4]2−(aq) + 2 e− ⟶ Pt(s) + 4 Cl−(aq)
|
0.758
|
|
[PtCl6]2−(aq) + 2 e− ⟶ [PtCl4]2−(aq) + 2 Cl−(aq)
|
0.726
|
|
O2(g) + 2 H+(aq) + 2 e− ⟶ H2O2(aq)
|
0.695
|
|
TeO2(s) + 4 H+(aq) + 4 e− ⟶ Te(s) + 2 H2O(ℓ)
|
0.604
|
|
H3AsO4(aq) + 2 H+(aq) + 2 e− ⟶ HAsO2(aq) + 2 H2O(ℓ)
|
0.560
|
|
I2(s) + 2 e− ⟶ 2 I−(aq)
|
0.535
|
|
Cu+(aq) + e− ⟶ Cu(s)
|
0.521
|
|
[RhCl6]3−(aq) + 3 e− ⟶ Rh(s) + 6 Cl−(aq)
|
0.5
|
|
Cu2+(aq) + 2e− ⟶ Cu(s)
|
0.340
|
|
Hg2Cl2(s) + 2e− ⟶ 2 Hg(ℓ) + 2 Cl−(aq)
|
0.27
|
|
AgCl(s) + e− ⟶ Ag(s) + Cl−(aq)
|
0.222
|
|
Cu2+(aq) + e− ⟶ Cu+(aq)
|
0.159
|
|
SO42−(aq) + 4 H+(aq) + 2 e− ⟶ H2SO3(aq) + H2O(ℓ)
|
0.158
|
|
Sn4+(aq) + 2e− ⟶ Sn2+(aq)
|
0.15
|
|
S(s) + 2 H+(aq) + 2 e− ⟶ H2S(aq)
|
0.144
|
|
AgBr(s) + e− ⟶ Ag(s) + Br−(aq)
|
0.0713
|
|
2 H+(aq) + 2 e− ⟶ H2(g) (reference electrode)
|
0
|
|
N2O(g) + 6 H+(aq) + H2O(ℓ) + 4 e− ⟶ 2 NH3OH+(aq)
|
−0.05
|
|
HgS(s, black) + 2 H+(aq) + 2 e− ⟶ Hg(ℓ) + H2S(g)
|
−0.085
|
|
Se(s) + 2 H+(aq) + 2 e− ⟶ H2Se(aq)
|
−0.115
|
|
Pb2+(aq) + 2 e− ⟶ Pb(s)
|
−0.125
|
|
Sn2+(aq) + 2 e− ⟶ Sn(s)
|
−0.1375
|
|
AgI(s) + e− ⟶ Ag(s) + I−(aq)
|
−0.1522
|
|
[SnF6]2−(aq) + 4 e− ⟶ Sn(s) + 6 F−(aq)
|
−0.200
|
|
Ni2+(aq) + 2 e− ⟶ Ni(s)
|
−0.25
|
|
Co2+(aq) + 2 e− ⟶ Co(s)
|
−0.277
|
|
Tl+(aq) + e− ⟶ Tl(s)
|
−0.3363
|
|
PbSO4(s) + 2 e− ⟶ Pb(s) + SO42−(aq)
|
−0.3505
|
|
Cd2+(aq) + 2 e− ⟶ Cd(s)
|
−0.403
|
|
Cr3+(aq) + e− ⟶ Cr2+(aq)
|
−0.424
|
|
Fe2+(aq) + 2 e− ⟶ Fe(s)
|
−0.44
|
|
2 CO2(g) + 2 H+(aq) + 2 e− ⟶ (COOH)2(aq)
|
−0.481
|
|
TiO2(s)+ 4 H+(aq) + 2 e− ⟶ Ti2+(aq) + 2 H2O(ℓ)
|
−0.502
|
|
Ga3+(aq) + 3 e− ⟶ Ga(s)
|
−0.53
|
|
Cr3+(aq) + 3 e− ⟶ Cr(s)
|
−0.74
|
|
Zn2+(aq) + 2 e− ⟶ Zn(s)
|
−0.763
|
|
Cr2+(aq) + 2 e− ⟶ Cr(s)
|
−0.90
|
|
V2+(aq) + 2 e− ⟶ V(s)
|
−1.13
|
|
Mn2+(aq) + 2 e− ⟶ Mn(s)
|
−1.18
|
|
Zr4+(aq) + 4 e− ⟶ Zr(s)
|
−1.55
|
|
Al3+(aq) + 3 e− ⟶ Al(s)
|
−1.676
|
|
H2(g) + 2 e− ⟶ 2 H−(aq)
|
−2.25
|
|
Mg2+(aq) + 2 e− ⟶ Mg(s)
|
−2.356
|
|
Na+(aq) + e− ⟶ Na(s)
|
−2.714
|
|
Ca2+(aq) + 2 e− ⟶ Ca(s)
|
−2.84
|
|
Sr2+(aq) + 2 e− ⟶ Sr(s)
|
−2.89
|
|
Ba2+(aq) + 2 e− ⟶ Ba(s)
|
−2.92
|
|
Rb+(aq) + e− ⟶ Rb(s)
|
−2.925
|
|
K+(aq) + e− ⟶ K(s)
|
−2.925
|
|
Li+(aq) + e− ⟶ Li(s)
|
−3.045
|
| From Bard, A. J., Parsons, R., and Jordan, J., Standard Potentials in Aqueous Solution, New York: Marcel Dekker, 1985. International Union of Pure and Applied Chemistry, Commission on Electrochemistry and Electroanalytical Chemistry. †From Brown, R. A., and Swift, E. H., Journal of the American Chemical Society, Vol. 71, 1949, pp. 2719-2723. |
|
Standard Electrode Potentials in Basic Aqueous Solution
at 25 °C.
You can change the number of rows shown per page (navigate using "previous" and "next" at the bottom of the page), or search the table.
| Basic Solution | Standard Electrode Potential, E° (volts) |
|---|---|
|
ClO−(aq) + H2O(ℓ) + 2 e− ⟶ Cl−(aq) + 2 OH−(aq)
|
0.89
|
|
OOH−(aq) + H2O(ℓ) + 2 e− ⟶ 3 OH−(aq)
|
0.867
|
|
2 NH2OH(aq) + 2 e− ⟶ N2H4(aq) + 2 OH−(aq)
|
0.73
|
|
ClO3−(aq) + 3 H2O(ℓ) + 6 e− ⟶ Cl−(aq) + 6 OH−(aq)
|
0.622
|
|
MnO4−(aq) + 2 H2O(ℓ) + 3 e− ⟶ MnO2(s) + 4 OH−(aq)
|
0.60
|
|
MnO4−(aq) + e− ⟶ MnO42−(aq)
|
0.56
|
|
NiO2(s) + 2 H2O(ℓ) + 2 e− ⟶ Ni(OH)2(s) + 2 OH−(aq)
|
0.49
|
|
Ag2CrO4(s) + 2 e− ⟶ 2 Ag(s) + CrO42−(aq)
|
0.4491
|
|
O2(g) + 2 H2O(ℓ) + 4 e− ⟶ 4 OH−(aq)
|
0.401
|
|
ClO4−(aq) + H2O(ℓ) + 2 e− ⟶ ClO3−(aq) + 2 OH−(aq)
|
0.374
|
|
Ag2O(s) + H2O(ℓ) + 2 e− ⟶ 2 Ag(s) + 2 OH−(aq)
|
0.342
|
|
2 NO2−(aq) + 3 H2O(ℓ) + 4 e− ⟶ N2O(g) + 6 OH−(aq)
|
0.15
|
|
N2H4(aq) + 2 H2O(ℓ) + 2 e− ⟶ 2 NH3(aq) + 2 OH−(aq)
|
0.10
|
|
HgO(s) + H2O(ℓ) + 2 e− ⟶ Hg(ℓ) + 2 OH−(aq)
|
0.0977
|
|
O2(g) + H2O(ℓ) + 2 e− ⟶ OOH−(aq) + OH−(aq)
|
0.0649
|
|
[Co(NH3)6]3+(aq) + e− ⟶ [Co(NH3)6]2+(aq)
|
0.058
|
|
NO3−(aq) + H2O(ℓ) + 2 e− ⟶ NO2−(aq) + 2 OH−(aq)
|
0.01
|
|
MnO2(s) + 2 H2O(ℓ) + 2 e− ⟶ Mn(OH)2(s) + 2 OH−(aq)
|
−0.05
|
|
CrO42−(aq) + 4 H2O(ℓ) + 3 e− ⟶ Cr(OH)3(s) + 5 OH−(aq)
|
−0.11
|
|
Cu2O(s) + H2O(ℓ) + 2 e− ⟶ 2 Cu(s) + 2 OH−(aq)
|
−0.365
|
|
FeO2−(aq) + H2O(ℓ) + e− ⟶ HFeO2−(aq) + OH−(aq)
|
−0.69
|
|
HFeO2−(aq) + H2O(ℓ) + 2 e− ⟶ Fe(s) + 3 OH−(aq)
|
−0.8
|
|
2 H2O(ℓ) + 2 e− ⟶ H2(g) + 2 OH−(aq)
|
−0.8277
|
|
2 NO3−(aq) + 2 H2O(ℓ) + 2 e− ⟶ N2O4(g) + 4 OH−(aq)
|
−0.86
|
|
SO42−(aq) + H2O(ℓ) + 2 e− ⟶ SO32−(aq) + 2 OH−(aq)
|
−0.936
|
|
N2(g) + 4 H2O(ℓ) + 4 e− ⟶ N2H4(aq) + 4 OH−(aq)
|
−1.16
|
|
Zn(OH)2(s) + 2 e− ⟶ Zn(s) + 2 OH−(aq)
|
−1.246
|
|
[Zn(OH)4]2−(aq) + 2 e− ⟶ Zn(s) + 4 OH−(aq)
|
−1.285
|
|
Cr(OH)3(s) + 3 e− ⟶ Cr(s) + 3 OH−(aq)
|
−1.33
|
|
[Zn(CN)4]2−(aq) + 2 e− ⟶ Zn(s) + 4 CN−(aq)
|
−1.34
|
|
SiO32−(aq) + 3 H2O(ℓ) + 4 e− ⟶ Si(s) + 6 OH−(aq)
|
−1.69
|
| From Bard, A. J., Parsons, R., and Jordan, J., Standard Potentials in Aqueous Solution, New York: Marcel Dekker, 1985. International Union of Pure and Applied Chemistry, Commission on Electrochemistry and Electroanalytical Chemistry. | |
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