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Related Concept Videos

Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

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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.
Solubility is important in biological and environmental processes. A notable...
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Solubility03:00

Solubility

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Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
In a solution, the solute particles (molecules,...
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Liquid–Solid Solutions01:29

Liquid–Solid Solutions

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The process of a solid dissolving in a liquid to form a solution is governed by the solubility limit, which is the maximum amount of the solid substance, or solute, that can be dissolved in a specific volume of the liquid or solvent. As the solute dissolves, it reaches a point where no more solute can be dissolved at a given temperature - this is known as the saturation point. However, if further solute is added and it manages to dissolve, the solution becomes supersaturated. Supersaturated...
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Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

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Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.
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Solubility Equilibria03:07

Solubility Equilibria

60.1K
Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation.
The...
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Chemical and Solubility Equilibria02:21

Chemical and Solubility Equilibria

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The free energy change associated with dissolving a solute in a liter of solvent is called the free energy of a solution, ΔGsolution. The overall ΔGsolution is expressed as the balance of ΔGinteraction against the always-favorable free-energy of mixing, ΔGmixing. Solution formation is favorable if  ΔGsolution is less than zero, whereas it is unfavorable if ΔGsolution is greater than zero. In short, for a solution to form and complete dissolution to take place,...
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Oversolubility in the microvicinity of solid-solution interfaces.

Isabelle Bergonzi1, Lionel Mercury1, Patrick Simon2

  • 1Institut des Sciences de la Terre d'Orléans, UMR 7327 Université d'Orléans/CNRS/BRGM, 45071 Orléans Cedex, France. lionel.mercury@univ-orleans.fr.

Physical Chemistry Chemical Physics : PCCP
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Summary
This summary is machine-generated.

A micrometer-thick layer of altered water, termed vicinal water, forms at solid-liquid interfaces, challenging traditional views of sharp phase boundaries. This interfacial water exhibits unique properties, including enhanced reactivity.

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Area of Science:

  • Physical Chemistry
  • Surface Science
  • Spectroscopy

Background:

  • Macroscopic water-solid interactions are typically modeled with sharp interfaces between bulk phases.
  • This simplified model is widely applied across biology, geochemistry, and materials science.

Purpose of the Study:

  • To experimentally investigate the nature of water-solid interfaces at high resolution.
  • To challenge the conventional sharp interface model with new evidence.

Main Methods:

  • High-resolution infrared (IR) and Raman spectroscopy were employed.
  • Experiments utilized a micro-scale quartz cavity and synchrotron radiation for IR mapping.
  • Spectroscopic data were spatially analyzed to map interfacial water properties.

Main Results:

  • IR and Raman mapping revealed a 1-3 micrometer thick layer of altered water at the quartz-water interface.
  • Signatures included a dangling free-OH component and a shift in the OH-stretching band.
  • This interfacial layer exhibits distinct vibrational properties compared to bulk water.

Conclusions:

  • The findings suggest that water-solid interfaces are not sharp but involve a thick, structured interfacial layer (vicinal water).
  • Vicinal water possesses unique thermodynamic properties, potentially affecting its melting point, boiling temperature, and solvent capabilities.
  • This discovery necessitates a revision of models describing water-solid interactions in various scientific and technological fields.