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Related Concept Videos

Ion Exchange01:17

Ion Exchange

Ion exchange chromatography separates charged molecules from a solution by reversibly exchanging them with mobile, or 'active', ions associated with the oppositely charged stationary phase. This method can be used to separate ions, soften and deionize water, and purify solutions. The polymers comprising the ion-exchange column are high-molecular-weight and chemically stable polymers, crosslinked to be porous and essentially insoluble. They are also functionalized with either acidic or basic...
Formation of Complex Ions03:45

Formation of Complex Ions

A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
Complexation Equilibria: Overview01:23

Complexation Equilibria: Overview

Complexation reactions take place when dative or coordinate covalent bonds form between metal ions and ligands. The compounds formed in these reactions are called coordination compounds. The number of bonds formed between the metal ion and the ligands is called its coordination number. Generally, most metal ions in an aqueous solution are solvated by water molecules and thus exist as aqua complexes.
The equilibrium constant of the complexation reaction is represented as the formation constant...
Complexation Equilibria: The Chelate Effect01:19

Complexation Equilibria: The Chelate Effect

In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
Electrolytes: van't Hoff Factor03:08

Electrolytes: van't Hoff Factor

Colligative Properties of ElectrolytesThe 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 dissolved...
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:

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Updated: Jun 5, 2026

Merging Ion Concentration Polarization between Juxtaposed Ion Exchange Membranes to Block the Propagation of the Polarization Zone
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Merging Ion Concentration Polarization between Juxtaposed Ion Exchange Membranes to Block the Propagation of the Polarization Zone

Published on: February 23, 2017

Equilibrium polyelectrolyte bundles with different multivalent counterion concentrations.

Mehmet Sayar1, Christian Holm

  • 1College of Engineering, Koc University, Istanbul, Turkey.

Physical Review. E, Statistical, Nonlinear, and Soft Matter Physics
|January 15, 2011
PubMed
Summary
This summary is machine-generated.

Trivalent counterion concentration significantly impacts polyelectrolyte bundle formation and size. High concentrations lead to charge neutralization and an isoelectric point, altering bundle characteristics.

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Area of Science:

  • Polymer Physics
  • Solution Chemistry
  • Computational Biophysics

Background:

  • Polyelectrolyte bundles form complex structures in solution.
  • Salt concentration is a critical factor influencing polyelectrolyte behavior.
  • Previous studies focused on salt-free conditions.

Purpose of the Study:

  • Investigate the effect of trivalent counterion concentration on polyelectrolyte bundle formation.
  • Analyze changes in bundle size, size distribution, and charge density.
  • Explore the mechanisms governing bundle formation under varying ionic conditions.

Main Methods:

  • Molecular-dynamics simulations were employed.
  • Thermodynamic equilibrium conditions were maintained.
  • Systems with varying percentages of trivalent counterion charge compensation were simulated.

Main Results:

  • Trivalent counterion concentration significantly alters bundle size and distribution.
  • Bundle formation onset shifts to lower Bjerrum lengths with increased counterion concentration.
  • At high concentrations (80-100% charge compensation), bundle net charge decreases with size.
  • A nonmonotonic change in line-charge density was observed due to competing mechanisms.
  • Excess trivalent counterions (200%) lead to diminished charge density differences and an isoelectric point.

Conclusions:

  • Trivalent counterions play a crucial role in dictating polyelectrolyte bundle morphology and properties.
  • The interplay between counterion condensation and bundle merger influences effective charge density.
  • Systems can achieve charge neutrality at specific high trivalent counterion concentrations.