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Related Concept Videos

Electrochemical Systems01:24

Electrochemical Systems

Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution, the Zn metal, composed...
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:
Intermolecular Forces03:13

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
The Electrical Double Layer01:30

The Electrical Double Layer

In the region where two bulk phases meet, an intricate electric charge distribution arises due to charge transfer, ion adsorption, molecular orientation, and charge distortion. This complex distribution is commonly referred to as the electrical double layer.When a solid electrode interfaces with ions in an electrolyte solution, the speed of electron transfer dictates the rates of oxidation and reduction. The electrode acquires a charge through the escape of atoms into the solution as cations or...
Intermolecular Forces in Solutions02:28

Intermolecular Forces in Solutions

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,...
Colloidal precipitates01:09

Colloidal precipitates

The high insolubility of some precipitates can result in an unfavorable relative supersaturation. This can lead to colloidal particles with a large surface-to-mass ratio, where adsorption is promoted. For instance, in the precipitation of silver chloride, silver ions are adsorbed on the surface of the colloidal particles, forming a primary layer. This layer attracts ions of opposite charge (such as nitrate ions), forming a diffuse secondary layer of adsorbed ions. This electric double layer...

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Proof-of-Concept for Gas-Entrapping Membranes Derived from Water-Loving SiO2/Si/SiO2 Wafers for Green Desalination
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UNEXPECTED PRESENCE OF SOLUTE-FREE ZONES AT METAL-WATER INTERFACES.

B Chai1, A G Mahtani, G H Pollack

  • 1Department of Bioengineering, Box 355061, University of Washington, Seattle, WA 98195.

Contemporary Materials
|June 29, 2013
PubMed
Summary
This summary is machine-generated.

Scientists discovered unexpected solute-free "exclusion zones" next to various metals in water, with zinc creating the largest zones. These findings may offer new insights into metal-interface electrochemical processes.

Keywords:
aqueous solutioncharge separationexclusion zonesmetal-water interfacesmetalsoxidation

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Area of Science:

  • Electrochemistry
  • Materials Science
  • Surface Chemistry

Background:

  • Solute-free zones, known as exclusion zones, are commonly observed near hydrophilic surfaces in aqueous solutions.
  • The formation and characteristics of such zones at metal-aqueous interfaces are not well understood.

Purpose of the Study:

  • To investigate the presence and characteristics of exclusion zones adjacent to various metal surfaces in aqueous environments.
  • To correlate the properties of these exclusion zones with the electrochemical nature of the metals.

Main Methods:

  • Experimental observation of exclusion zones using microscopy.
  • Measurement of electrical potentials within the exclusion zones.
  • pH measurements in the aqueous regions adjacent to the metals.
  • Comparison with the galvanic series of metals.

Main Results:

  • Exclusion zones were observed next to reactive metals (e.g., zinc, aluminum, tin, lead, tungsten), but not precious metals (e.g., platinum, gold).
  • The largest exclusion zone, approximately 200 µm, was adjacent to zinc.
  • Positive electrical potentials were measured within the exclusion zones.
  • An abundance of hydroxide (OH-) ions was detected beyond the exclusion zones.
  • Exclusion zone size correlated with the metal's position in the galvanic series.

Conclusions:

  • The study reveals the unexpected formation of interfacial exclusion zones adjacent to various metals in aqueous solution.
  • These findings suggest a link between metal reactivity, electrochemical potential, and the formation of exclusion zones.
  • The existence of these zones may necessitate a re-evaluation of electrochemical processes at metal-aqueous interfaces.