6.14: Standard Potential
- Page ID
- 371724
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Standard Potential
John Moore, Jia Zhou, and Etienne Garand
Standard Electrode Potentials in Acidic Aqueous Solution (a table for basic solution is below)
at 25 °C.
| 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.
| 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.