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Related Concept Videos

Common Ion Effect03:24

Common Ion Effect

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 Châtelier’s principle. Consider the dissolution of silver iodide:
Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary cation—the calcium...
Ionic Association01:28

Ionic Association

The ionic association is the association of oppositely charged ions in an electrolyte solution to form ion pairs. Bjerrum defined ion pairs as two oppositely charged ions whose electrostatic attraction exceeds the thermal energy of the system, typically expressed as 2kT. Electrostatic attraction depends on ionic charge, separation distance, and the dielectric constant of the medium. Thermal energy, represented by kT, reflects the tendency of ions to move independently due to molecular motion.
Ions as Acids and Bases02:54

Ions as Acids and Bases

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:
Formation of Complex Ions03:45

Formation of Complex Ions

A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
Ion-Exchange Chromatography01:09

Ion-Exchange Chromatography

Ion-exchange chromatography, or IEC, is a technique for separating ions based on their affinity for the stationary phase. The stationary phase is a cross-linked polymer resin with covalently attached ionic functional groups. The functional groups can be either positively charged (cation exchangers) or negatively charged (anion exchangers). A cation exchanger consists of a polymeric anion and active cations, while an anion exchanger is a polymeric cation with active anions. The choice of...

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Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
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An ab initio approach to understanding the specific ion effect.

Marcel D Baer1, Christopher J Mundy

  • 1Pacific Northwest National Laboratory, Richland, Washington 99352, USA.

Faraday Discussions
|June 26, 2013
PubMed
Summary

Large, polarizable anions adsorb to the air-water interface. Density functional theory (DFT) calculations reveal how local hydration structure correlates with an ion's position in the Hofmeister series, impacting surface adsorption.

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Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
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Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F−
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Area of Science:

  • Physical Chemistry
  • Chemical Physics
  • Surface Chemistry

Background:

  • Large, polarizable anions adsorb to the air-water interface, but the underlying interactions are debated.
  • Previous work showed dependence of iodide adsorption on molecular interaction potentials, with DFT potentials yielding less adsorption than empirical ones.
  • DFT potentials accurately model anion solvation shells, validated by X-ray absorption fine structure (XAFS) experiments.

Purpose of the Study:

  • To investigate the local hydration structure of thiocyanate (SCN-) and iodate (IO3-) anions using DFT.
  • To compare the solvation structures of these polyatomic anions with halide anions.
  • To correlate local solvation structure with Hofmeister series classifications.

Main Methods:

  • Density functional theory (DFT) calculations were employed.
  • Local hydration structures of SCN- and IO3- were examined.
  • Solvation structures were compared to halide anions.

Main Results:

  • DFT was used to examine the local hydration structure of chaotropic and kosmotropic anions SCN- and IO3-.
  • The solvation structures of polyatomic anions were compared with halide anions.
  • A correlation was established between local solvation structure and Hofmeister series position.

Conclusions:

  • Local solvation structure is a key factor influencing anion adsorption at the air-water interface.
  • DFT calculations provide insights into the hydration of various anions.
  • The findings contribute to understanding the Hofmeister series and ion-interface interactions.