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Related Concept Videos

Solubility03:00

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)...
Solution Formation02:16

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 Equilibria: Overview01:09

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...
Solvents01:12

Solvents

A solvent is a substance, most often a liquid, that can dissolve other substances. Here, the substance being dissolved is called a solute. When a solvent and a solute combine, they form a solution - a homogenous mixture of both the solvent and the solute. Water is a universal biological solvent. Its polar structure allows it to dissolve many other polar compounds. The ability of water to dissolve is governed by a balance between water molecules binding to each other and binding to the solute.
A...
Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

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.
Chemical and Solubility Equilibria02:21

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...

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Solubility of Hydrophobic Compounds in Aqueous Solution Using Combinations of Self-assembling Peptide and Amino Acid
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Properties of compatible solutes in aqueous solution.

Jens Smiatek1, Rakesh Kumar Harishchandra, Oliver Rubner

  • 1Institut für Physikalische Chemie, Westfälische Wilhelms-Universität Münster, D-48149 Münster, Germany. jens.smiatek@uni-muenster.de

Biophysical Chemistry
|October 22, 2011
PubMed
Summary

Ectoine and hydroxyectoine, unlike urea, enhance water molecule ordering through hydrogen bonds, forming well-defined hydration spheres. Molecular Dynamics simulations reveal their superior water accumulation capabilities, validated by experimental data.

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Area of Science:

  • Biochemistry
  • Physical Chemistry
  • Computational Chemistry

Background:

  • Ectoine and hydroxyectoine are compatible solutes known for stabilizing biomolecules.
  • Understanding their hydration properties is crucial for applications in biotechnology and medicine.
  • Urea is a common osmolyte used as a benchmark for comparison.

Purpose of the Study:

  • To investigate the hydration behavior of ectoine, hydroxyectoine, and urea using Molecular Dynamics simulations.
  • To elucidate the role of molecular charge and salt concentration on hydration structure.
  • To experimentally validate simulation findings using a DPPC monolayer phase transition.

Main Methods:

  • Molecular Dynamics (MD) simulations in explicit solvent.
  • Analysis of local water structure and hydrogen bonding.
  • Investigation of varying salt concentrations.
  • Experimental study of dipalmitoylphosphatidylcholine (DPPC) monolayer phase transitions.

Main Results:

  • Ectoine and hydroxyectoine exhibit enhanced water molecule accumulation compared to urea.
  • A pronounced ordering of water molecules around ectoine and hydroxyectoine is observed due to hydrogen bonding.
  • Molecular charge significantly influences the formation of a well-defined hydration sphere.
  • Simulation results are consistent with experimental observations of DPPC monolayer phase transitions.

Conclusions:

  • Ectoine and hydroxyectoine possess superior water-structuring capabilities compared to urea.
  • The charge of osmolytes plays a critical role in their hydration properties.
  • MD simulations provide a reliable framework for understanding osmolyte-water interactions, validated by experimental data.