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Related Concept Videos

Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

1.4K
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...
1.4K
Common Ion Effect03:24

Common Ion Effect

41.6K
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:
41.6K
Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

14.7K
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.
When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between them. This process...
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Ions as Acids and Bases02:54

Ions as Acids and Bases

23.7K
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:
23.7K
Ion Exchange01:17

Ion Exchange

588
Ion exchange chromatography separates charged molecules from a solution by reversibly exchanging them with mobile, or 'active', ions associated with the oppositely charged stationary phase. This method can be used to separate ions, soften and deionize water, and purify solutions. The polymers comprising the ion-exchange column are high-molecular-weight and chemically stable polymers, crosslinked to be porous and essentially insoluble. They are also functionalized with either acidic or...
588
Formation of Complex Ions03:45

Formation of Complex Ions

23.6K
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...
23.6K

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Updated: Jun 27, 2025

Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature
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Anionic Effects on Concentrated Aqueous Lithium Ion Dynamics.

Robert G Felsted1, Trent R Graham1, Yatong Zhao1

  • 1Pacific Northwest National Laboratory, Richland, Washington 99352, United States.

The Journal of Physical Chemistry Letters
|May 6, 2024
PubMed
Summary
This summary is machine-generated.

Lithium nitrite solutions exhibit significantly higher viscosity and altered dynamics compared to other lithium salts. This suggests nitrite anions strongly influence water-ion network interactions and solution properties.

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Area of Science:

  • Physical Chemistry
  • Solution Chemistry
  • Spectroscopy

Background:

  • Understanding the behavior of concentrated electrolyte solutions is crucial for various applications.
  • Lithium salts are widely used in batteries and other electrochemical systems.
  • The influence of specific anions on solution properties requires detailed investigation.

Purpose of the Study:

  • To investigate the dynamics, orientational anisotropy, diffusivity, viscosity, and density of concentrated lithium salt solutions.
  • To compare the effects of different lithium salts (LiCl, LiBr, LiNO2, LiNO3) on solution properties.
  • To elucidate the role of anions in structuring water-ion networks.

Main Methods:

  • Two-dimensional infrared spectroscopy (2D IR) for probing molecular dynamics.
  • Nuclear magnetic resonance (NMR) spectroscopy for structural and dynamic analysis.
  • Viscometry to measure solution viscosity.

Main Results:

  • Lithium nitrite (LiNO2) solutions showed longer correlation times, lower diffusivity, and approximately four times higher viscosity than other lithium salts at equivalent concentrations.
  • LiNO2 solutions demonstrated a significant facilitation of structure formation, strengthening water-ion network interactions.
  • Lithium nitrite and lithium nitrate solutions exhibited weakened interactions between lithium cations and the methyl thiocyanate probe molecule compared to lithium halide salts.

Conclusions:

  • Nitrite anions play a significant role in enhancing the structure of concentrated aqueous solutions, impacting bulk properties.
  • The observed differences in dynamics and viscosity are attributed to specific anion-water and anion-cation interactions.
  • These findings provide insights into the molecular mechanisms governing the properties of concentrated electrolyte solutions.