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Related Concept Videos

Ideal Solutions02:24

Ideal Solutions

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According to Raoult’s law, the partial vapor pressure of a solvent in a solution is equal or identical to the vapor pressure of the pure solvent multiplied by its mole fraction in the solution. However, Raoult's Law is only valid for ideal solutions. For a solution to be ideal, the solvent-solute interaction must be just as strong as a solvent-solvent or solute-solute interaction. This suggests that both the solute and the solvent would use the same amount of energy to escape to the...
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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,...
22.8K
Chemical and Solubility Equilibria02:21

Chemical and Solubility Equilibria

5.2K
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,...
5.2K
Nonideal Two-Component Liquid Solutions01:29

Nonideal Two-Component Liquid Solutions

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Nonideal liquid solutions, also known as real solutions, do not strictly follow Raoult's law. Raoult's law is a rule of thumb in physical chemistry. However, not all mixtures adhere to this law due to varying molecular interactions. For example, in an acetone/chloroform solution, the individual vapor pressures of the components are lower than expected, resulting in a total vapor pressure below that predicted by Raoult's law, causing a negative deviation.On the other hand, in an ethanol/water...
94
Entropy and Solvation02:05

Entropy and Solvation

8.8K
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...
8.8K
Intermolecular Forces in Solutions02:28

Intermolecular Forces in Solutions

41.0K
The formation of a solution is an example of a spontaneous process, 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. Such a solution is called an ideal solution. A mixture of ideal gases (or gases such as helium and argon,...
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Sedimentation Equilibrium of a Small Oligomer-forming Membrane Protein: Effect of Histidine Protonation on Pentameric Stability
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Non-Ideal Behaviour and Solution Interactions in Binary DMSO Solutions.

Amninder S Virk1, Dale J Codling1, Timothy Stait-Gardner1

  • 1Nanoscale Organisation and Dynamics Group, School of Science and Health, University of Western Sydney, Locked Bag 1797, Penrith, NSW, 2751, Australia.

Chemphyschem : a European Journal of Chemical Physics and Physical Chemistry
|October 20, 2015
PubMed
Summary
This summary is machine-generated.

Hydrogen-bonded structures in dimethylsulfoxide-alcohol mixtures were studied using NMR and MD simulations. Results show DMSO-alcohol dimers are dominant, with weaker association than DMSO-water mixtures.

Keywords:
hydrogen bondingintermolecular interactionsnon-bonded interactionsself-diffusionsolvent effects

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Area of Science:

  • Physical Chemistry
  • Supramolecular Chemistry
  • Materials Science

Background:

  • Hydrogen-bonded structures are crucial for understanding binary mixtures.
  • Self-diffusion is sensitive to molecular properties, offering insights into mixture dynamics.

Purpose of the Study:

  • To investigate hydrogen-bonded associated structures in dimethylsulfoxide-methanol (DMSO-MeOH) and DMSO-ethanol (DMSO-EtOH) mixtures.
  • To analyze the impact of composition on mixture dynamics and structure.

Main Methods:

  • Nuclear magnetic resonance (NMR) diffusion experiments.
  • Molecular dynamics (MD) simulations.
  • Analysis of self-diffusion coefficients, heat of mixing, and radial distribution functions.

Main Results:

  • Self-diffusion coefficients decreased with increasing DMSO concentration in both DMSO-MeOH (up to 15%) and DMSO-EtOH (up to 10%) mixtures.
  • These decreases indicate weaker association compared to DMSO-water mixtures.
  • Intermolecular structures remained largely unchanged upon mixing, with DMSO-alcohol hydrogen-bonded dimers identified as dominant species.

Conclusions:

  • DMSO-alcohol mixtures exhibit weaker hydrogen bonding compared to DMSO-water systems.
  • The study provides detailed insights into the structural properties and dynamics of these binary mixtures.
  • Combined experimental and simulation approaches offer a comprehensive understanding of molecular interactions.