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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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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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Entropy and Solvation02:05

Entropy and Solvation

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The process of surrounding a solute with solvent is called solvation. It involves evenly distributing the solute within the solvent. The rule of thumb for determining a solvent for a given compound is that like dissolves like. A good solvent has molecular characteristics similar to those of the compound to be dissolved. For example, polar solutions dissolve polar solutes, and apolar solvents dissolve apolar solutes. A polar solvent is a solvent that has a high dielectric constant (ϵ...
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Solubility Equilibria03:07

Solubility Equilibria

59.8K
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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Solubility Equilibria: Ionic Product of Water01:16

Solubility Equilibria: Ionic Product of Water

2.0K
Pure water is a weak electrolyte; only a small amount ionizes into hydrogen and hydroxide ions. At any given temperature, the concentration of undissociated water is almost constant, so the ionic product of water is the product of the hydrogen and hydroxide ion concentrations, denoted as Kw. The square root of Kw gives the individual ion concentrations.
The ionic product of water varies with temperature, and its value is 1.0 x 10−14 at standard experimental conditions. Per Le...
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Solution Formation02:16

Solution Formation

38.7K
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...
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Related Experiment Video

Updated: Mar 13, 2026

Unraveling Entropic Rate Acceleration Induced by Solvent Dynamics in Membrane Enzymes
09:42

Unraveling Entropic Rate Acceleration Induced by Solvent Dynamics in Membrane Enzymes

Published on: January 16, 2016

9.4K

Differential Solvation.

Georg Schreckenbach1

  • 1Department of Chemistry, University of Manitoba, Winnipeg, MB, R3T 2N2, Canada.

Chemistry (Weinheim an Der Bergstrasse, Germany)
|October 12, 2016
PubMed
Summary

Differential solvation impacts chemical reaction equilibria. This study uses electrostatic models, like the Born and Kirkwood-Onsager equations, to explain how solvent interactions stabilize reactants or products based on charge and size. This provides insights into chemical reactivity.

Keywords:
Born equationqualitative interpretationreaction equilibriasolvent effectsthermodynamics

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Area of Science:

  • Physical Chemistry
  • Chemical Thermodynamics
  • Electrostatics

Background:

  • Solvation effects significantly influence reaction equilibria through differential solvation, where solvents preferentially stabilize either reactants or products.
  • Understanding these effects is crucial for predicting and controlling chemical reactions across various domains.

Purpose of the Study:

  • To propose a qualitative interpretation of solvation effects on reaction equilibria using fundamental electrostatic concepts.
  • To demonstrate the applicability of the Born and Kirkwood-Onsager equations for understanding these phenomena.

Main Methods:

  • Application of simple electrostatic principles.
  • Utilizing the Born equation for charged species in solution.
  • Employing the Kirkwood-Onsager model for neutral species with dipole moments.
  • Analysis of scenarios involving differences in charge, size, and dipole moments between reactants and products.

Main Results:

  • Developed a framework to qualitatively interpret differential solvation effects based on electrostatic interactions.
  • Showcased how charge, size, and dipole moment differences dictate preferential stabilization of reactants or products.
  • Illustrated the concepts with diverse chemical examples, including redox potentials.

Conclusions:

  • Simple electrostatic models provide a powerful tool for understanding complex solvation effects on chemical equilibria.
  • The proposed approach offers a qualitative yet insightful method for chemists to predict and rationalize solvent influences on reactions.
  • This work bridges fundamental electrostatic theory with practical chemical observations.