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Common Ion Effect03:24

Common Ion Effect

46.2K
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:
46.2K
Precipitation of Ions03:11

Precipitation of Ions

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Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
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Intermolecular Forces in Solutions02:28

Intermolecular Forces in Solutions

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The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external source.
When the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change. Such a solution is called an ideal solution. A mixture of ideal gases (or gases such as helium and argon,...
39.0K
Electrolyte and Nonelectrolyte Solutions02:21

Electrolyte and Nonelectrolyte Solutions

71.4K
Substances that undergo either a physical or a chemical change in solution to yield ions that can conduct electricity are called electrolytes. If a substance yields ions in solution, that is, if the compound undergoes 100% dissociation, then the substance is a strong electrolyte. Complete dissociation is indicated by a single forward arrow. For example, water-soluble ionic compounds like sodium chloride dissociate into sodium cations and chloride anions in aqueous solution.
71.4K
Ions as Acids and Bases02:54

Ions as Acids and Bases

26.3K
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:
26.3K
Chemical Reactions in Aqueous Solutions03:03

Chemical Reactions in Aqueous Solutions

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Chemical substances interact in many different ways. Certain chemical reactions exhibit common patterns of reactivity. Due to the vast number of chemical reactions, it becomes necessary to classify them based on the observed patterns of interaction.
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Related Experiment Video

Updated: Jan 25, 2026

Dynamic Electrochemical Measurement of Chloride Ions
07:32

Dynamic Electrochemical Measurement of Chloride Ions

Published on: February 5, 2016

12.0K

Ion Association in Lanthanide Chloride Solutions.

Aaron R Finney1, Sébastien Lectez2, Colin L Freeman1

  • 1Department of Materials Science and Engineering, Sir Robert, Hadfield Building, University of Sheffield, Sheffield, S1 3JD, UK.

Chemistry (Weinheim an Der Bergstrasse, Germany)
|April 25, 2019
PubMed
Summary

Understanding lanthanide (Ln) salt solution chemistry is key for materials and waste management. New molecular dynamics simulations reveal how Ln ions associate with chloride, showing a shift from dissociative to associative ion pairing based on cation size.

Keywords:
ion pairinglanthanidesmolecular dynamicspotential of mean forcerare-earth elements

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Area of Science:

  • Solution chemistry
  • Lanthanide chemistry
  • Computational chemistry

Background:

  • Understanding lanthanide (Ln) salt solution chemistry is crucial for diverse applications, including materials processing and waste management.
  • Despite extensive research, the mechanisms and thermodynamics of Ln(III) association with anions in aqueous solutions remain poorly understood.
  • Current knowledge gaps hinder the development of sustainable processing routes for critical rare earth elements.

Purpose of the Study:

  • To elucidate the solution chemistry of lanthanide chloride (LnCl3) in water.
  • To investigate the mechanisms and thermodynamics of Ln(III) ion association with chloride anions.
  • To provide a computational framework for studying complex cation-solution interactions.

Main Methods:

  • Employed molecular dynamics (MD) simulations with a newly developed force field.
  • Validated the force field against density functional theory (DFT) calculations for Nd3+, Gd3+, and Er3+.
  • Utilized adaptive-bias MD simulations to study ion pairing mechanisms and thermodynamics.

Main Results:

  • The developed force field accurately reproduces lanthanide ion structures and dynamics in water.
  • Ion pairing mechanisms transition from dissociative to associative exchange with increasing cation size.
  • At low concentrations, weakly bound solvent-shared and solvent-separated ion pairs dominate over contact ion pairs.
  • Thermodynamic stabilities of inner and outer sphere complexes are comparable, with anion binding kinetics influencing speciation.

Conclusions:

  • The study provides novel insights into lanthanide chloride solution speciation, reconciling conflicting literature observations.
  • The findings highlight the importance of weakly bound ion pairs and kinetic factors in solution chemistry.
  • The computational approach offers a versatile framework for investigating complex aqueous cation systems.