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Related Concept Videos

Solubility03:00

Solubility

Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
In a solution, the solute particles (molecules, atoms, and/or ions)...
Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.
Solubility Equilibria03:07

Solubility Equilibria

Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation.
The...
Physical Properties Affecting Solubility02:19

Physical Properties Affecting Solubility

Solutions of Gases in Liquids
As for any solution, the solubility of a gas in a liquid is affected by the attractive intermolecular forces between solute and solvent species. Unlike solid and liquid solutes, however, there is no solute-solute intermolecular attraction to overcome when a gaseous solute dissolves in a liquid solvent since the atoms or molecules comprising a gas are far separated and experience negligible interactions. Consequently, solute-solvent interactions are the sole...
Factors Affecting Solubility04:01

Factors Affecting Solubility

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:
Solution Formation02:16

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a different solvent. A simple way to predict which substances dissolve in which solvent is the phrase "like dissolves like". This means that polar substances, such as salt and sugar, dissolve in a polar substance like water. In contrast, non-polar substances are more soluble in non-polar solvents such as carbon tetrachloride.
This selective solubility...

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Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature
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Published on: December 20, 2016

Using XPS to determine solute solubility in room temperature ionic liquids.

Debbie S Silvester1, Tessa L Broder, Leigh Aldous

  • 1Physical and Theoretical Chemistry Laboratory, University of Oxford, South Parks Road, Oxford, UKOX1 3QZ.

The Analyst
|February 28, 2007
PubMed
Summary

X-Ray Photoelectron Spectroscopy quantified bromide ion solubility in an ionic liquid. The saturated solution contained 0.90 Br atom% (746 mM) at 298 K, confirmed by chronoamperometry.

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Published on: October 10, 2016

Area of Science:

  • Analytical Chemistry
  • Electrochemistry
  • Materials Science

Background:

  • Room temperature ionic liquids (RTILs) are versatile solvents with tunable properties.
  • Understanding solute solubility in RTILs is crucial for their application in various chemical processes.
  • Bromide ion concentration is a key parameter in electrochemical studies and material synthesis.

Purpose of the Study:

  • To quantify the solubility of bromide ions in a specific room temperature ionic liquid.
  • To determine the concentration of bromide ions in a saturated solution of [C(4)mpyrr]Br in [C(4)mpyrr][N(Tf)2].
  • To validate the results using an independent analytical technique.

Main Methods:

  • Quantitative X-Ray Photoelectron Spectroscopy (XPS) was employed to determine bromide ion concentration.
  • Potential-step chronoamperometry was used as an independent method for confirmation.
  • Two samples were analyzed: one with a known concentration (0.436 Br atom%) and a saturated solution.

Main Results:

  • XPS analysis revealed the saturated solution contained 0.90 Br atom% bromide ions.
  • This concentration corresponds to 746 mM at 298 K.
  • The solubility value obtained by XPS was independently confirmed by potential-step chronoamperometry.

Conclusions:

  • The solubility of bromide ions in the studied RTIL was determined to be 0.90 Br atom% (746 mM) at 298 K.
  • XPS is a reliable method for quantifying bromide ion concentration in ionic liquid solutions.
  • The findings provide essential data for the use of this RTIL in bromide-containing systems.