Linked from

The 31 pages that link to Acid–base equilibrium, each with the reason it gives.

• Chemical equilibriumBroader topic: Acid strengths and solution pH depend on equilibrium between protonated and deprotonated species.

• Buffer solutionNarrower topic: Buffer composition is governed by proton-transfer equilibrium.

• CarbonationRelated: It governs the acidity changes caused by dissolved carbon dioxide.

• PhosphateRelated: It determines which phosphate species predominate at a given pH.

• Liquid–liquid extractionRelated: Ionization can change a solute’s affinity for each phase.

• Sodium hypochloriteRelated: Solution pH determines the proportions of hypochlorite ion and hypochlorous acid.

• LactateNarrower topic: This equilibrium accounts for lactate predominating over lactic acid near neutral pH.

• Ion-exchange chromatographyRelated: It determines how pH changes the charge of solutes and some exchange groups.

• Solubility equilibriumCompared with: It can alter solubility, but its defining balance is proton transfer.

• Isoelectric pointRelated: The isoelectric point follows from how a molecule’s groups gain or lose protons as pH changes.

• Chemical speciationRelated: pH changes protonation states and therefore the species available for other reactions.

• Pourbaix diagramRelated: pH-dependent boundaries separate species that differ by protonation.

• Carbonated waterRelated: It describes the linked forms of dissolved carbon dioxide and their effect on acidity.

• DiazotizationRelated: Acidity controls nitrous acid formation and the protonation state of the amine.

• PhenolphthaleinRelated: Changes in proton concentration shift the forms of phenolphthalein present in solution.

• Potassium dichromateRelated: Acidity shifts equilibria among dichromate, hydrogen chromate, and chromate ions.

• Universal indicatorRelated: Indicator molecules change between differently colored forms as this equilibrium shifts.

• PhenethylamineRelated: The amino group can accept a proton, changing phenethylamine’s charge and solubility.

• Bromothymol blueRelated: The dye’s two colored forms coexist in a pH-dependent equilibrium.

• Ion chromatographyRelated: It determines analyte charge, which can change whether and how strongly an analyte is retained.

• Sodium bisulfiteRelated: Solution pH determines the balance among sulfur dioxide, bisulfite, and sulfite.

• Sodium chromateRelated: Solution acidity controls the distribution of chromate and dichromate ions.

• VanadateRelated: Solution pH shifts vanadate among protonation states and structures.

• Potassium bisulfateNarrower topic: Dissolved HSO₄⁻ establishes equilibria that determine the solution’s acidity.

• Disodium citrateRelated: The salt’s solution composition depends on proton exchange among hydrogen citrate and other citrate forms.

• GuanidineRelated: Guanidine’s basicity is expressed through its equilibrium with guanidinium ions.

• Aluminium triacetateRelated: Acetate protonation and aluminium-ion hydrolysis jointly influence solution pH.

• Ammonia solutionNarrower topic: It describes how ammonia and water generate small amounts of ammonium and hydroxide ions.

• Ammonium acetateNarrower topic: The dissolved ions exchange protons with water and with each other.

• Chromate and dichromateRelated: Adding acid shifts chromate toward protonated and condensed forms, including dichromate.

• Monopotassium phosphateRelated: Its phosphate ion can accept or donate protons depending on solution conditions.