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Related Concept Videos

Common Ion Effect03:24

Common Ion Effect

41.7K
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:
41.7K
Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

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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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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,...
33.6K
Factors Affecting Solubility04:01

Factors Affecting Solubility

33.4K
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:
33.4K
Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

1.5K
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...
1.5K
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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Sulfate Separation by Selective Crystallization with a Bis-iminoguanidinium Ligand
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Controlled dissolution of a single ion from a salt interface.

Huijun Han1, Yunjae Park2, Yohan Kim1

  • 1Department of Materials Science and Engineering, Ulsan National Institute of Science and Technology (UNIST), Ulsan, 44919, Republic of Korea.

Nature Communications
|March 17, 2024
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Summary
This summary is machine-generated.

Researchers manipulated a single water molecule to observe salt dissolution at the sodium chloride (NaCl) film surface. This study reveals key insights into fundamental ion-water interactions and selective anion dissolution processes.

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Area of Science:

  • Surface science
  • Physical chemistry
  • Materials science

Background:

  • Understanding ion-water interactions is crucial for complex ionic processes.
  • Salt dissolution is a fundamental endothermic process requiring entropy increase.
  • Previous single-ion level studies were predominantly theoretical.

Purpose of the Study:

  • To experimentally demonstrate salt dissolution at the single-ion level.
  • To investigate ion-water interactions and water molecule dynamics at interfaces.
  • To elucidate the mechanism of selective anion dissolution.

Main Methods:

  • Controlled manipulation of a single water molecule on a sodium chloride (NaCl) film.
  • Observation of salt dissolution at an under-coordinated site.
  • Analysis of water dipole polarization and its effect on ionic bonds.

Main Results:

  • Demonstrated salt dissolution by manipulating a single water molecule.
  • Observed water dipole polarization of anions, leading to strong anion-water interactions.
  • Showed weakening of ionic bonds within the NaCl crystal due to water interaction.

Conclusions:

  • Provides experimental insights into a fundamental step of single-ion chemistry.
  • Highlights the role of water molecule dynamics in selective anion dissolution.
  • Offers potential applications in ion-related sciences and technologies.