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Related Concept Videos

Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

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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.
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Physical Properties Affecting Solubility02:19

Physical Properties Affecting Solubility

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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...
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Solubility03:00

Solubility

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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,...
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Factors Affecting Solubility04:01

Factors Affecting Solubility

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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:
36.4K
Common Ion Effect03:24

Common Ion Effect

44.9K
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:
44.9K
Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

2.4K
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...
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Updated: Dec 25, 2025

Development, Characterization, and Evaluation of CAGE-based Ionic Liquid Systems for Transdermal Delivery
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Development, Characterization, and Evaluation of CAGE-based Ionic Liquid Systems for Transdermal Delivery

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SO2 absorption in pure ionic liquids: Solubility and functionalization.

Lanyun Wang1, Yajuan Zhang2, Yang Liu2

  • 1School of Safety Science and Engineering, Henan Polytechnic University, Jiaozuo, 454003, China; Collaborative Innovation Center of Coal Safety Production of Henan Province, Jiaozuo, 454003, China; State Key Laboratory Cultivation Base for Gas Geology and Gas Control in Henan Polytechnic University, Jiaozuo, 454003, China.

Journal of Hazardous Materials
|March 26, 2020
PubMed
Summary

Ionic liquids show promise for sulfur dioxide (SO2) capture, with functional groups influencing absorption. Optimizing ionic liquids for SO2 capture requires balancing capacity, energy, and viscosity.

Keywords:
Absorption mechanismsFunctionalityIonic liquidsSO(2) solubilitySO(2)/CO(2) selectivity

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Area of Science:

  • Chemical Engineering
  • Materials Science
  • Environmental Science

Background:

  • Ionic liquids offer tunable properties for gas absorption.
  • Sulfur dioxide (SO2) capture is critical for environmental protection.
  • Traditional solvents face limitations in SO2 capture efficiency and regeneration.

Purpose of the Study:

  • To review SO2 solubility and absorption mechanisms in various ionic liquids.
  • To identify strategies for enhancing SO2 capture and CO2 separation.
  • To explore the potential of biocompatible ionic liquids for SO2 capture.

Main Methods:

  • Review of literature on ionic liquid functionalities and SO2 absorption.
  • Analysis of factors influencing SO2 capacity, binding energy, and separation.
  • Discussion of molecular simulation insights into absorption mechanisms.

Main Results:

  • Moderate basicity and specific functional groups enhance SO2 capacity.
  • Electron-withdrawing groups can reduce regeneration energy, but absorption enthalpy remains high.
  • Biocompatible ionic liquids show potential due to favorable environmental profiles.
  • High viscosity and desorption energy are key challenges for ionic liquid applications.

Conclusions:

  • Ionic liquids present significant improvements over traditional solvents for SO2 capture.
  • Further research is needed to overcome viscosity and desorption energy limitations.
  • Molecular simulations can guide the design of improved ionic liquids for SO2 absorption.