ELECTRODE POTENTIAL

- Electrode potential refers to the potential difference or voltage between an electrode and its surrounding solution/electrolyte.
- It is a measure of the tendency of an electrode to gain or lose electrons, which determines its ability to undergo oxidation or reduction reactions.
- The electrode potential is influenced by various factors, including the nature of the electrode material, concentration of ions in the solution, temperature, and pressure.
- The standard electrode potential (E°) is the electrode potential measured under standard conditions, which include a concentration of 1 mole per liter, temperature of 298 Kelvin, and atmospheric pressure of 1 bar.
- Standard hydrogen electrode (SHE) is often used as a reference electrode for measuring electrode potentials. Its electrode potential is defined as zero.
- Electrons flow from the electrode with a lower potential to the electrode with a higher potential, following the direction of the electrochemical reaction.
- The difference in electrode potentials of two electrodes is related to the cell potential (Ecell) of an electrochemical cell, which can be used to determine the spontaneity and feasibility of a redox reaction.
- A positive electrode potential indicates a tendency for reduction, while a negative electrode potential indicates a tendency for oxidation.
- Electrode potential can be measured using various techniques, such as potentiometry, voltammetry, and electrochemical cells.

Please note that these are just summarized notes. If you require more in-depth information on any specific aspect, please let me know!