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Related Concept Videos

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...
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:
Solvating Effects02:12

Solvating Effects

An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...
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...
Polyprotic Acids03:38

Polyprotic Acids

Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
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:

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Achieving Moderate Pressures in Sealed Vessels Using Dry Ice As a Solid CO2 Source
06:26

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Published on: August 17, 2018

Significant cation effects in carbon dioxide-ionic liquid systems.

Oldamur Hollóczki1, Zsolt Kelemen, László Könczöl

  • 1Wilhelm-Ostwald-Institut für Physikalische und Theoretische Chemie, Universität Leipzig, Germany.

Chemphyschem : a European Journal of Chemical Physics and Physical Chemistry
|January 3, 2013
PubMed
Summary
This summary is machine-generated.

This study reveals that cations play a significant role in carbon dioxide solubility within ionic liquids. Dispersion interactions between cations and carbon dioxide offer a new way to design solvents for enhanced CO2 capture.

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Area of Science:

  • Physical Chemistry
  • Materials Science
  • Chemical Engineering

Background:

  • Carbon dioxide-ionic liquid systems are crucial for CO2 capture technologies.
  • Current understanding suggests anions dominate solute-solvent interactions.
  • The cation's role in CO2 solvation is considered minimal or secondary.

Purpose of the Study:

  • To challenge the prevailing view of cation's role in CO2 solvation.
  • To investigate the contribution of cation-solute interactions in CO2-ionic liquid systems.
  • To identify novel sites for tuning CO2 solubility.

Main Methods:

  • Theoretical approach utilizing computational chemistry.
  • Analysis of intermolecular interactions between CO2 and ionic liquid components.
  • Comparison with established solute-solvent interaction models (e.g., benzene-CO2).

Main Results:

  • Dispersion interactions are identified between the CO2 solute and the ionic liquid cation.
  • The cation's role in solvation is demonstrated to be significant, not secondary.
  • This finding contradicts previous assumptions about CO2-ionic liquid interactions.

Conclusions:

  • The cation is a key interaction site for CO2 in ionic liquids.
  • Tailoring cation structure can effectively tune CO2 solubility.
  • This research opens new avenues for designing advanced CO2 capture solvents.