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Related Concept Videos

Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

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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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Common Ion Effect03:24

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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 Châtelier’s principle. Consider the dissolution of silver iodide:
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Electrolytes: van't Hoff Factor03:08

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Colligative Properties of Electrolytes
The colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one...
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Solubility Equilibria: Overview01:09

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When a substance such as sodium chloride is added to water, it dissolves, forming an aqueous solution. The extent of dissolution is called solubility. The process of dissolution can exist in equilibrium, just like other chemical processes. Solubility equilibria are also called precipitation equilibria because the process of solubility can be reversible. The reverse of the solubility process is called precipitation.
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Aqueous Solutions and Heats of Hydration02:42

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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.
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Intermolecular Forces in Solutions02:28

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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.
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Updated: Jun 7, 2025

Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy
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Direct and indirect salt effects on homotypic phase separation.

Matt MacAinsh1, Souvik Dey1, Huan-Xiang Zhou1,2

  • 1Department of Chemistry, University of Illinois Chicago, Chicago, United States.

Elife
|November 12, 2024
PubMed
Summary

The low-complexity domain of hnRNPA1 (A1-LCD) undergoes salt-dependent phase separation, promoted by high salt concentrations. This atypical behavior is driven by ion charge neutralization and bridging, alongside strengthened π-interactions at higher salt levels.

Keywords:
molecular biophysicsmolecular dynamics simulationsnonephase separationsalt dependencesalt effectsstructural biology

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Area of Science:

  • Biophysics
  • Molecular Biology
  • Computational Biology

Background:

  • Intrinsically disordered proteins (IDPs) undergo liquid-liquid phase separation (LLPS), a crucial process in cellular organization.
  • The low-complexity domain of hnRNPA1 (A1-LCD) exhibits unusual salt-dependent phase separation, unlike typical IDPs.

Purpose of the Study:

  • To investigate the atypical salt effect on A1-LCD phase separation.
  • To elucidate the molecular mechanisms underlying salt-promoted LLPS of A1-LCD.

Main Methods:

  • All-atom molecular dynamics (MD) simulations were employed.
  • Simulations were conducted on multiple A1-LCD chains across a range of NaCl concentrations (50–1000 mM).

Main Results:

  • NaCl ions directly neutralize the protein's net charge and bridge between A1-LCD chains, promoting condensation.
  • High salt concentrations indirectly enhance π-π, cation-π, and amino-π interactions by reducing water shielding.
  • Low salt prevents phase separation via charge repulsion; intermediate and high salt concentrations promote it through charge neutralization, bridging, and strengthened π-interactions.

Conclusions:

  • Atypical salt-promoted phase separation of A1-LCD is governed by a combination of direct ion-mediated interactions and indirect effects on non-covalent forces.
  • The study predicts four classes of salt dependence for IDP phase separation based on amino acid composition.