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Related Concept Videos

Solubility Equilibria03:07

Solubility Equilibria

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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: 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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Solvating Effects02:12

Solvating Effects

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An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...
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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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Intermolecular Forces03:13

Intermolecular Forces

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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...
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Solubility of Hydrophobic Compounds in Aqueous Solution Using Combinations of Self-assembling Peptide and Amino Acid
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Solubility of Hydrophobic Compounds in Aqueous Solution Using Combinations of Self-assembling Peptide and Amino Acid

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The Joint Solvation Interaction.

Ali Hassanali1, Colin K Egan1

  • 1The "Abdus Salam" International Centre for Theoretical Physics, I-34151 Trieste, Italy.

Entropy (Basel, Switzerland)
|September 27, 2024
PubMed
Summary
This summary is machine-generated.

We introduce the joint solvation interaction (JSI), a thermodynamic measure of how solvents accommodate multiple solutes. This new method helps understand solute binding and solvent effects in biological processes.

Keywords:
cluster expansioncollective effectshydrophilic interactionhydrophobic effecthydrophobic interactionsolvation thermodynamics

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Area of Science:

  • Physical Chemistry
  • Computational Chemistry
  • Biophysics

Background:

  • Solvent-induced interactions (SIIs) are crucial in molecular processes.
  • Existing methods often struggle to accurately capture complex solvent-solute thermodynamics.
  • Flexible solutes present unique challenges in quantifying solvent effects.

Purpose of the Study:

  • To formally define and quantify the joint solvation interaction (JSI) for flexible solutes.
  • To develop a computational method for calculating JSI.
  • To establish JSI as a superior metric for solute binding thermodynamics compared to indirect solvent-mediated interactions.

Main Methods:

  • Formal definition of JSI using mixture expansion.
  • Demonstration of JSI equivalence to SII for rigid solutes.
  • Development of partially connected molecular dynamics for JSI computation with free energy algorithms.

Main Results:

  • The JSI is formally defined and shown to generalize hydrophobic interactions.
  • A novel computational approach (partially connected molecular dynamics) is proposed.
  • JSI is demonstrated to be more relevant than indirect solvent-mediated interactions for binding thermodynamics.

Conclusions:

  • JSI provides a more accurate thermodynamic description of solvent effects for flexible solutes.
  • The proposed computational method enables direct JSI calculation.
  • Understanding JSI is vital for self-assembly, protein aggregation, and protein folding studies.