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Solution Formation

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a different solvent. A simple way to predict which substances dissolve in which solvent is the phrase "like dissolves like". This means that polar substances, such as salt and sugar, dissolve in a polar substance like water. In contrast, non-polar substances are more soluble in non-polar solvents such as carbon tetrachloride.
This selective solubility...

Solubility

Solubility

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, atoms, and/or ions)...

Energetics of Solution Formation

Energetics of Solution Formation

The formation of a solution is an example of a spontaneous process, which is 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. Formation of the solution requires the solute–solute and solvent–solvent electrostatic forces to...

Chemical and Solubility Equilibria

Chemical and Solubility Equilibria

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, the Gibbs energy change must be...

Solubility Equilibria: Overview

Solubility Equilibria: Overview

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...

Liquid–Solid Solutions

Liquid–Solid Solutions

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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High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems

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Solvation effects in near-critical binary mixtures.

Akira Onuki¹, Hikaru Kitamura

¹Department of Physics, Kyoto University, 606-8502, Japan.

The Journal of Chemical Physics

|August 5, 2004

Summary

Ginzburg-Landau theory reveals how solvation shells form around charged particles in polar fluids near critical points. Adding salt strengthens interactions between critical fluctuations and ions, influencing phase transitions.

Area of Science:

Physical Chemistry
Chemical Physics
Thermodynamics

Background:

Solvation effects are crucial in polar fluid binary mixtures, especially near critical points.
Understanding dielectric properties and their dependence on concentration is key to predicting solvation behavior.
Critical phenomena in fluids exhibit unique characteristics like critical electrostriction.

Purpose of the Study:

To investigate solvation effects in near-critical polar fluid binary mixtures using Ginzburg-Landau theory.
To analyze the formation of solvation shells around charged particles.
To explore the impact of critical fluctuations and ion addition on phase transition behavior.

Main Methods:

Ginzburg-Landau theory applied to polar fluid binary mixtures.

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Analysis of concentration dependence of the dielectric constant.

Calculation of structure factors for critical fluctuations and charge density.

Main Results:

A preferential solvation shell forms around charged particles.
Long-range Ornstein-Zernike tails indicate strong critical electrostriction near the critical point.
Strong coupling observed between critical fluctuations and ions upon salt addition.

Conclusions:

The study provides a theoretical framework for understanding solvation in critical fluid mixtures.
Critical electrostriction and ion-critical fluctuation coupling significantly influence system behavior.
The findings offer insights into the phase transition dynamics of these systems.