Electrode Potential, Standard

Standard Electrode Potentials in Acidic Aqueous Solution (a table for basic solution is below)

at 25 °C.

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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()

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()

1.690

NiO2(s) + 4 H+(aq) + 2 e ⟶ Ni2+(aq) + 2 H2O()

1.68

2 HClO(aq) + 2 H+(aq) + 2 e ⟶ Cl2(g) + 2 H2O()

1.63

Au3+(aq) + 3 e ⟶ Au(s)

1.52

MnO4 (aq) + 8 H+(aq) + 5 e ⟶ Mn2+(aq) + 4 H2O()

1.51

BrO3(aq) + 6 H+(aq) + 5 e12 Br2(aq) + 3 H2O()

1.478

2 ClO3(aq) + 12 H+(aq) + 10 e ⟶ Cl2(g) + 6 H2O()

1.47

Cr2O72(aq) + 14 H+(aq) + 6 e ⟶ 2 Cr3+(aq) + 7 H2O()

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()

1.23

O2(g) + 4 H+(aq) + 4 e ⟶ 2 H2O()

1.229

ClO4(aq) + 2 H+(aq) + 2 e ⟶ ClO3(aq) + H2O()

1.201

IO3(aq) + 6 H+(aq) + 5 e12 I2(aq) + 3 H2O()

1.195

Pt2+(aq) + 2 e ⟶ Pt(s)

1.188

Br2() + 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()

0.96

NO3(aq) + 3 H+(aq) + 2 e ⟶ HNO2(aq) + H2O()

0.94

Pd2+(aq) + 2 e ⟶ Pd(s)

0.915

2 Hg2+(aq) + 2 e ⟶ Hg22+(aq)

0.9110

Hg2+(aq) + 2 e ⟶ Hg()

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()

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()

0.604

H3AsO4(aq) + 2 H+(aq) + 2 e ⟶ HAsO2(aq) + 2 H2O()

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() + 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()

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() + 4 e ⟶ 2 NH3OH+(aq)

0.05

HgS(s, black) + 2 H+(aq) + 2 e ⟶ Hg() + 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()

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.

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Basic Solution Standard Electrode Potential, E° (volts)

ClO(aq) + H2O() + 2 e ⟶ Cl(aq) + 2 OH(aq)

0.89

OOH(aq) + H2O() + 2 e ⟶ 3 OH(aq)

0.867

2 NH2OH(aq) + 2 e ⟶ N2H4(aq) + 2 OH(aq)

0.73

ClO3(aq) + 3 H2O() + 6 e ⟶ Cl(aq) + 6 OH(aq)

0.622

MnO4(aq) + 2 H2O() + 3 e ⟶ MnO2(s) + 4 OH(aq)

0.60

MnO4(aq) + e ⟶ MnO42(aq)

0.56

NiO2(s) + 2 H2O() + 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() + 4 e ⟶ 4 OH(aq)

0.401

ClO4(aq) + H2O() + 2 e ⟶ ClO3(aq) + 2 OH(aq)

0.374

Ag2O(s) + H2O() + 2 e ⟶ 2 Ag(s) + 2 OH(aq)

0.342

2 NO2(aq) + 3 H2O() + 4 e ⟶ N2O(g) + 6 OH(aq)

0.15

N2H4(aq) + 2 H2O() + 2 e ⟶ 2 NH3(aq) + 2 OH(aq)

0.10

HgO(s) + H2O() + 2 e ⟶ Hg() + 2 OH(aq)

0.0977

O2(g) + H2O() + 2 e ⟶ OOH(aq) + OH(aq)

0.0649

[Co(NH3)6]3+(aq) + e ⟶ [Co(NH3)6]2+(aq)

0.058

NO3(aq) + H2O() + 2 e ⟶ NO2(aq) + 2 OH(aq)

0.01

MnO2(s) + 2 H2O() + 2 e ⟶ Mn(OH)2(s) + 2 OH(aq)

0.05

CrO42(aq) + 4 H2O() + 3 e ⟶ Cr(OH)3(s) + 5 OH(aq)

0.11

Cu2O(s) + H2O() + 2 e ⟶ 2 Cu(s) + 2 OH(aq)

0.365

FeO2(aq) + H2O() + e ⟶ HFeO2(aq) + OH(aq)

0.69

HFeO2(aq) + H2O() + 2 e ⟶ Fe(s) + 3 OH(aq)

0.8

2 H2O() + 2 e ⟶ H2(g) + 2 OH(aq)

0.8277

2 NO3(aq) + 2 H2O() + 2 e ⟶ N2O4(g) + 4 OH(aq)

0.86

SO42(aq) + H2O() + 2 e ⟶ SO32(aq) + 2 OH(aq)

0.936

N2(g) + 4 H2O() + 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() + 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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Chemistry 109 Fall 2021 by John Moore, Jia Zhou, and Etienne Garand is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.