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Related Concept Videos

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:
Washing, Drying, and Ignition of Precipitates00:52

Washing, Drying, and Ignition of Precipitates

After filtration, the precipitate is washed to remove coprecipitated impurities and any remaining mother liquor. Colloidal precipitates, such as silver chloride, are washed with an electrolyte (such as dilute nitric acid) to prevent the peptization of the precipitate. In the case of slightly soluble precipitates, the wash solution contains a common ion to reduce solubility. Lead sulfate, which is slightly soluble in water, is washed with dilute sulfuric acid. Similarly, wash solutions may be...
Weak Base Solutions03:21

Weak Base Solutions

Some compounds produce hydroxide ions when dissolved by chemically reacting with water molecules. In all cases, these compounds react only partially and so are classified as weak bases. These types of compounds are also abundant in nature and important commodities in various technologies. For example, global production of the weak base ammonia is typically well over 100 metric tons annually, being widely used as an agricultural fertilizer, a raw material for chemical synthesis of other...
Imperfections in Crystal Structure: Non-Stoichiometric Defects01:29

Imperfections in Crystal Structure: Non-Stoichiometric Defects

Non-stoichiometric defects refer to a type of defect in the crystal structure of a compound where the ratio of its constituent elements deviates from the ideal stoichiometric ratio. There are two main types of non-stoichiometric defects: metal excess defects and metal deficiency defects.Metal excess defects occur when there is a slight surplus of metal ions than what is required by the stoichiometric ratio of the compound. For example, heating a sodium chloride crystal in sodium vapor results...
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:
Weak Acid Solutions04:02

Weak Acid Solutions

Few compounds act as strong acids. A far greater number of compounds behave as weak acids and only partially react with water, leaving a large majority of dissolved molecules in their original form and generating a relatively small amount of hydronium ions. Weak acids are commonly encountered in nature, being the substances partly responsible for the tangy taste of citrus fruits, the stinging sensation of insect bites, and the unpleasant smells associated with body odor. A familiar example of a...

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A Microfluidic Approach for the Study of Ice and Clathrate Hydrate Crystallization
08:01

A Microfluidic Approach for the Study of Ice and Clathrate Hydrate Crystallization

Published on: August 18, 2022

Hydroxide impurity in ice.

Lukasz Cwiklik1, J P Devlin, Victoria Buch

  • 1The Fritz Haber Institute for Molecular Dynamics, The Hebrew University, Jerusalem 91904, Israel. lukasz@fh.huji.ac.il

The Journal of Physical Chemistry. A
|April 17, 2009
PubMed
Summary
This summary is machine-generated.

Hydroxide ions (OH-) in water ice I can halt proton mobility by binding to specific traps. However, proton activity resumes when these traps become saturated with sufficient hydroxide ions.

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Identification of Plant Ice-binding Proteins Through Assessment of Ice-recrystallization Inhibition and Isolation Using Ice-affinity Purification
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Identification of Plant Ice-binding Proteins Through Assessment of Ice-recrystallization Inhibition and Isolation Using Ice-affinity Purification

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Area of Science:

  • Physical Chemistry
  • Surface Science
  • Materials Science

Background:

  • Proton mobility in water ice is crucial for various chemical and physical processes.
  • Understanding the influence of adsorbates on proton transport is essential for ice science.

Purpose of the Study:

  • To investigate the role of hydroxide ions in proton mobility within water ice I.
  • To elucidate the mechanism by which base adsorbates affect proton activity at ice surfaces.

Main Methods:

  • Computational methods, specifically density functional theory (DFT) calculations on ice slabs.
  • Experimental isotopic exchange experiments on ice nanoparticles.

Main Results:

  • Base adsorbates on ice surfaces significantly influence proton activity.
  • Trace amounts of base adsorbates inhibit proton activity by trapping hydroxide ions (OH-).
  • Increased adsorbate concentration restores proton activity by saturating the hydroxide ion traps.

Conclusions:

  • Strong binding sites for hydroxide ions exist at the ice surface and interior, immobilizing them and halting proton mobility.
  • Proton activity is restored when these deep traps are saturated by a sufficient abundance of hydroxide ions.
  • Hydroxide ions exhibit a broad energy distribution when located at different lattice sites in ice.