Linked from

The 50 pages that link to Nernst equation, each with the reason it gives.

• Chemical potentialRelated: It translates chemical-potential differences into measurable electrical voltage.

• Fuel cellRelated: It predicts how fuel and oxidant conditions change a cell’s reversible voltage.

• Membrane potentialRelated: It predicts the voltage at which one ion’s chemical and electrical forces balance.

• Galvanic cellRelated: It predicts how concentration changes shift a galvanic cell’s voltage.

• Redox potentialRelated: It shows how concentrations and conditions shift a redox couple’s potential.

• Standard electrode potentialRelated: It calculates how a half-cell potential changes away from standard conditions.

• ElectrochemistryRelated: It predicts how solution composition shifts an electrochemical cell’s voltage.

• Electrode potentialRelated: It predicts how the potential shifts when concentrations or temperature change.

• Activity coefficientRelated: Using activities gives accurate electrode potentials in nonideal solutions.

• Electrochemical potentialRelated: It gives the voltage that cancels an ion’s chemical driving force.

• Electrochemical seriesRelated: It shows why the standard ranking may differ from potentials under nonstandard conditions.

• Faraday constantRelated: The constant appears in the equation's conversion between chemical potential and electrical potential.

• Half-reactionRelated: It adjusts half-reaction potentials when solution conditions depart from standard states.

• ElectrophysiologyRelated: It predicts the voltage at which that ion has no net movement.

• Resting membrane potentialRelated: It predicts the voltage at which one ion’s electrical and chemical forces balance.

• Debye–Hückel theoryRelated: The theory can provide activity estimates for dilute-solution applications of this equation.

• Dynamic equilibriumRelated: It connects a redox equilibrium to the voltage measured across an electrochemical cell.

• Reference electrodeRelated: It explains how changes in solution composition can shift an electrode’s potential.

• Chemical activityRelated: Electrochemical potentials depend on activities even when measurements report concentrations.

• Hodgkin–Huxley modelRelated: It provides the reversal potentials that set each modeled ion current’s driving force.

• Solid oxide fuel cellRelated: Fuel and oxygen partial pressures set the cell’s reversible voltage.

• Standard stateRelated: The standard cell potential is defined by the standard states of the electrochemical reaction.

• Reaction quotientRelated: The reaction quotient gives the composition-dependent term in the equation.

• OverpotentialRelated: It determines the equilibrium potential from composition and temperature.

• Walther NernstBroader topic: Nernst derived this relation to describe how electrode potential changes with solution composition.

• PotentiometryRelated: It predicts how potentiometric voltage changes with the activity of the target ion.

• Pourbaix diagramRelated: Potential-dependent equilibrium lines follow the Nernst equation, often varying with pH.

• Redox titrationRelated: It predicts how electrode potential changes as titrant is added.

• Reducing agentRelated: It shows how reaction conditions alter the electron-donating tendency of a redox couple.

• Standard hydrogen electrodeRelated: It predicts how the hydrogen electrode's potential changes when its conditions depart from standard values.

• Gas constantRelated: Its thermal voltage term contains R divided by Faraday’s constant.

• Permanganate titrationRelated: It describes how changing reaction conditions affect the redox potential near the endpoint.

• Thermodynamic activityRelated: Activity terms determine how cell voltage shifts away from standard conditions.

• Electrochemical sensorRelated: It describes the concentration-dependent voltage used by potentiometric sensors.

• Potassium dichromateRelated: It predicts how dichromate’s reduction potential varies with acidity and concentration.

• Concentration cellRelated: It quantifies how unequal activities of the same species generate the cell’s potential.

• Cyclic voltammetryRelated: It predicts equilibrium potentials that help interpret redox peak positions.

• Nernst heat theoremRelated: Nernst's broader thermodynamic work also connected chemical equilibria with measurable electrical potentials.

• Redox indicatorRelated: It describes how the indicator’s oxidized-to-reduced ratio shifts with potential.

• VoltammetryRelated: It connects redox composition to the potential range where voltammetric reactions occur.

• Depolarization (neuroscience)Related: It helps explain how ion gradients set the direction and strength of depolarizing currents.

• Nernst–Planck equationCompared with: It describes equilibrium potential, whereas Nernst–Planck describes transport flux.

• Passive transportRelated: It predicts the voltage at which passive electrical and chemical forces on one ion cancel.

• Zirconium dioxideRelated: Oxygen concentration differences across zirconia electrolytes produce voltages described by this relation.

• Reduction potentialRelated: It shows how a reduction potential shifts away from standard conditions.

• Ammonium iron(II) sulfateRelated: It describes how iron(II)/iron(III) concentrations affect the solution’s redox potential.

• Electroanalytical methodsRelated: It connects measured equilibrium potentials with analyte activity.

• Gibbs–Donnan effectRelated: It quantifies the electrical potential generated by unequal ion concentrations.

• Membrane potentialRelated: It predicts the equilibrium voltage produced by a concentration gradient for one permeant ion.

• Thermodynamic equationsRelated: It applies thermodynamic chemical potentials to electrochemical measurements.