CorroZone Podcast · 16 Jun 2026
Potential Measurements, Reference Electrodes, and the Nernst Equation
- Free
- Lecture
- Beginner
- ~35 min
Why an electrode potential is always measured against a reference: the construction and conventions of the SHE, SCE, Ag/AgCl and Cu/CuSO4 electrodes, converting potentials between their scales, and using the Nernst equation and the electrochemical series to predict equilibrium potentials and corrosion tendency.
Show notes
What you'll learn
- Explain why absolute electrode potentials cannot be measured directly and why a reference electrode is needed
- Describe the construction and conventions of the standard hydrogen electrode (SHE), SCE, Ag/AgCl, and Cu/CuSO4 reference electrodes
- Convert measured potentials between SHE, SCE, Ag/AgCl, and CSE reference scales
- Derive and apply the Nernst equation to calculate equilibrium potentials at non-standard concentrations
- Apply the Nernst equation to reactions involving H+ ions and predict pH dependence of equilibrium potentials
- Use the electrochemical series to make first-order thermodynamic predictions of corrosion tendency
Who this is for
Anyone beginning their study of corrosion — students, engineers, and technical staff who want a solid foundation in why metals corrode and what can be done about it. No prior background assumed.
What you'll learn
- Explain why absolute electrode potentials cannot be measured directly and why a reference electrode is needed
- Describe the construction and conventions of the standard hydrogen electrode (SHE), SCE, Ag/AgCl, and Cu/CuSO4 reference electrodes
- Convert measured potentials between SHE, SCE, Ag/AgCl, and CSE reference scales
- Derive and apply the Nernst equation to calculate equilibrium potentials at non-standard concentrations
- Apply the Nernst equation to reactions involving H+ ions and predict pH dependence of equilibrium potentials
- Use the electrochemical series to make first-order thermodynamic predictions of corrosion tendency