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Related Concept Videos

Solubility Equilibria: Ionic Product of Water01:16

Solubility Equilibria: Ionic Product of Water

1.2K
Pure water is a weak electrolyte; only a small amount ionizes into hydrogen and hydroxide ions. At any given temperature, the concentration of undissociated water is almost constant, so the ionic product of water is the product of the hydrogen and hydroxide ion concentrations, denoted as Kw. The square root of Kw gives the individual ion concentrations.
The ionic product of water varies with temperature, and its value is 1.0 x 10−14 at standard experimental conditions. Per Le...
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Intermolecular Forces03:13

Intermolecular Forces

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Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
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Water: A Bronsted-Lowry Acid and Base02:30

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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:
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Aqueous Solutions and Heats of Hydration02:42

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Water and other polar molecules are attracted to ions. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. These attractions play an important role in the dissolution of ionic compounds in water.
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15.1K
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Polyprotic Acids

29.5K
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:
29.5K
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The rate of acid-catalyzed hydration of alkenes depends on the alkene's structure, as the presence of alkyl substituents at the double bond can significantly influence the rate.
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Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics
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Specific Ion Properties Induce Spontaneous H2O2 Production at the Air-Water Interface.

Yoan Carreira Mendes Da Silva1, Maria Angelaki1, D James Donaldson2,3

  • 1Universite Claude Bernard Lyon 1, CNRS, IRCELYON, UMR 5256, Villeurbanne F-69100, France.

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Spontaneous hydrogen peroxide (H2O2) formation in water droplets is linked to ion identity, not just electric fields. Anions, following the Hofmeister series, significantly influence oxidant production by altering water structure at the air-water interface.

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Area of Science:

  • Atmospheric Chemistry
  • Physical Chemistry
  • Interface Science

Background:

  • Recent studies indicate spontaneous hydroxyl radical (OH) and hydrogen peroxide (H2O2) production at air-water interfaces.
  • The underlying mechanisms for this interfacial chemistry are not fully understood, with electric fields proposed as a factor.

Purpose of the Study:

  • To investigate the role of ionic composition in spontaneous oxidant formation in aqueous droplets.
  • To elucidate the relationship between ion identity, solvation properties, and H2O2 production at the air-water interface.

Main Methods:

  • Experimental analysis of oxidant formation in salt-containing aqueous droplets.
  • Correlation of H2O2 concentration with ion identity and concentration, utilizing Hofmeister series parameters.

Main Results:

  • Oxidant formation is strongly dependent on the type and concentration of ions present in the solution.
  • Anions exert a more significant influence on H2O2 formation than cations.
  • The observed effects of anions align with the Hofmeister series, indicating a role for solvation properties.

Conclusions:

  • Spontaneous H2O2 formation at the air-water interface is primarily driven by interfacial solvation properties influenced by ions, rather than solely by electric fields.
  • Anions disrupt water structure, reducing OH- solvation and promoting dissociation, thereby increasing H2O2 production.