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The 139 pages that link to Chemical equilibrium, each with the reason it gives.

• SolubilityNarrower topic: Dissolution and crystallization reach a dynamic balance at saturation.

• Nernst equationNarrower topic: The Nernst relation gives the electrode potential at which the redox reaction is in equilibrium.

• Brønsted–Lowry acid–base theoryNarrower topic: Many proton-transfer reactions are reversible and described by equilibrium.

• Solubility productNarrower topic: Ksp describes the equilibrium state of solid dissolution.

• Carbonic acidNarrower topic: Carbonic acid formation and dissociation are reversible reactions governed by equilibrium.

• Equilibrium constantNarrower topic: The equilibrium constant characterizes the composition at this state.

• Le Chatelier's principleNarrower topic: Le Chatelier's principle describes how these balanced systems respond when disturbed.

• Precipitation reactionNarrower topic: Solubility equilibria determine whether dissolved ions remain in solution or enter a solid.

• Acid–base equilibriumNarrower topic: Proton-transfer forms coexist because their interconversion reaches this balance.

• Henderson–Hasselbalch equationNarrower topic: The equation is derived from the equilibrium expression for proton dissociation.

• Haber processNarrower topic: Ammonia formation is reversible, so operating conditions shift the equilibrium toward the product.

• AcidNarrower topic: Acid dissociation is an equilibrium whose position varies among acids.

• Partition coefficientNarrower topic: Partition coefficients describe phase distributions after transfer reaches equilibrium.

• pKaNarrower topic: An acid’s Ka describes the equilibrium reached during dissociation.

• Dissociation (chemistry)Narrower topic: Reversible dissociation often settles into an equilibrium mixture rather than going to completion.

• Liquid–liquid extractionNarrower topic: Solute distribution between phases is evaluated at equilibrium.

• GeothermobarometryNarrower topic: Most calibrations assume minerals recorded equilibrium rather than partial reaction.

• Ion exchangeNarrower topic: Reversible ion exchange reaches a condition governed by equilibrium between bound and dissolved ions.

• Hypochlorous acidNarrower topic: The acid, hypochlorite ion, and related species redistribute as solution conditions change.

• Strong acidNarrower topic: Acid dissociation is an equilibrium, even when it lies overwhelmingly toward products.

• Strong baseNarrower topic: Near-complete ionization corresponds to an equilibrium strongly favoring products.

• Weak acidNarrower topic: Partial dissociation is an equilibrium between molecular acid and ions.

• Solubility equilibriumNarrower topic: Solubility equilibrium is a phase-specific instance of this general balance.

• Acid–base chemistryNarrower topic: Acid dissociation and proton transfer are governed by equilibrium constants.

• Common-ion effectNarrower topic: The common-ion effect is a concentration-driven change in an equilibrium system.

• Qualitative inorganic analysisNarrower topic: Equilibria explain why test outcomes depend on reagent amounts and solution conditions.

• Van ’t Hoff equationNarrower topic: The equation describes how this state shifts when temperature changes.

• Water chemistryNarrower topic: Equilibrium predicts how dissolved species divide among chemical forms.

• Acid strengthNarrower topic: Acid dissociation is an equilibrium, so strength depends on the relative amounts of products and reactants.

• Langmuir adsorption modelNarrower topic: The isotherm describes site populations after adsorption and desorption reach equilibrium.

• Jacobus Henricus van ’t HoffNarrower topic: His temperature relation describes how equilibrium constants change as conditions change.

• Phosphorus pentachlorideNarrower topic: In the gas phase, PCl₅ can reversibly dissociate into PCl₃ and Cl₂.

• Water–gas shift reactionNarrower topic: The reaction’s reversible conversion reaches an equilibrium set by temperature and gas composition.

• Weak baseNarrower topic: A weak base’s partial reaction with water is an equilibrium, not a one-way conversion.

• Microscopic reversibilityNarrower topic: Microscopic reversibility specifies how that macroscopic balance holds at the elementary-step level.

• Dinitrogen tetroxideNarrower topic: The balance between N₂O₄ and NO₂ shifts with temperature and pressure.

• Acidity functionNarrower topic: Indicator ratios encode the equilibrium constants used to calculate acidity functions.

• Calcium bicarbonateNarrower topic: Dissolution and precipitation depend on the balance among carbon dioxide, bicarbonate, and carbonate.

• Chromate and dichromateNarrower topic: The observed colors reflect the equilibrium mixture rather than a one-way conversion.

• Gibbs–Donnan effectNarrower topic: Donnan ion ratios arise when membrane-permeant species reach equilibrium.

• Law of dilutionNarrower topic: Weak-electrolyte ionization is an equilibrium rather than a one-way conversion.