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Related Concept Videos

Strong Acid and Base Solutions03:22

Strong Acid and Base Solutions

37.4K
A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial concentration of acid. For example, 0.20 M hydrobromic acid will dissociate completely in water and produces 0.20 M of hydronium ions and 0.20 M of bromide ions.
37.4K
Ions as Acids and Bases02:54

Ions as Acids and Bases

27.2K
Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
27.2K
pH Scale02:41

pH Scale

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Hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes. Two different solutions can differ in their hydronium or hydroxide ion concentrations by a million, billion, or even trillion times. A common means of...
82.5K
Polyprotic Acids03:38

Polyprotic Acids

33.7K
Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
33.7K
Water: A Bronsted-Lowry Acid and Base02:30

Water: A Bronsted-Lowry Acid and Base

61.2K
The reaction between a Brønsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
61.2K
Factors Affecting Solubility04:01

Factors Affecting Solubility

38.0K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
38.0K

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Related Experiment Video

Updated: Mar 19, 2026

Activating Molecules, Ions, and Solid Particles with Acoustic Cavitation
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Protons and Hydroxide Ions in Aqueous Systems.

Noam Agmon1, Huib J Bakker2, R Kramer Campen3

  • 1The Fritz Haber Research Center, Institute of Chemistry, The Hebrew University of Jerusalem , Jerusalem 91904, Israel.

Chemical Reviews
|June 18, 2016
PubMed
Summary
This summary is machine-generated.

This review details advances in understanding proton and hydroxide ion behavior in water. It covers their structure, dynamics, and transport in various environments, including biological systems and hydrophobic interfaces.

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Area of Science:

  • Physical Chemistry
  • Biophysical Chemistry

Background:

  • Proton and hydroxide ions are crucial in acid-base chemistry and biological processes.
  • Despite extensive research, fundamental properties of these ions remain an active area of study.

Purpose of the Study:

  • To review experimental and theoretical progress in understanding proton and hydroxide ion behavior.
  • To highlight current debates and challenges, particularly concerning their accumulation at hydrophobic surfaces.
  • To discuss biological applications, such as proton transport in membranes and proteins.

Main Methods:

  • Review of experimental studies.
  • Review of theoretical and computational studies.
  • Analysis of findings across diverse aqueous environments.

Main Results:

  • Significant advances in characterizing ion structure, dynamics, and transport.
  • Insights into ion behavior in water clusters, bulk liquid, and at interfaces.
  • Discussion of ion accumulation at hydrophobic surfaces and associated controversies.

Conclusions:

  • Proton and hydroxide ion behavior is complex and context-dependent.
  • Further research is needed to resolve outstanding questions regarding their interfacial behavior.
  • Understanding these ions is vital for fields ranging from environmental chemistry to cellular bioenergetics.