Jove
Visualize
Contact Us
JoVE
x logofacebook logolinkedin logoyoutube logo
ABOUT JoVE
OverviewLeadershipBlogJoVE Help Center
AUTHORS
Publishing ProcessEditorial BoardScope & PoliciesPeer ReviewFAQSubmit
LIBRARIANS
TestimonialsSubscriptionsAccessResourcesLibrary Advisory BoardFAQ
RESEARCH
JoVE JournalMethods CollectionsJoVE Encyclopedia of ExperimentsArchive
EDUCATION
JoVE CoreJoVE BusinessJoVE Science EducationJoVE Lab ManualFaculty Resource CenterFaculty Site
Terms & Conditions of Use
Privacy Policy
Policies

Related Concept Videos

Entropy and Solvation02:05

Entropy and Solvation

7.0K
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...
7.0K
Intermolecular Forces03:13

Intermolecular Forces

58.2K
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...
58.2K
Solubility03:00

Solubility

17.5K
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,...
17.5K
Ideal Solutions02:24

Ideal Solutions

19.5K
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...
19.5K
Vapor Pressure Lowering03:28

Vapor Pressure Lowering

26.5K
The equilibrium vapor pressure of a liquid is the pressure exerted by its gaseous phase when vaporization and condensation are occurring at equal rates:
 
Dissolving a nonvolatile substance in volatile liquid results in a lowering of the liquid’s vapor pressure. This phenomenon can be explained by considering the effect of added solute molecules on the liquid's vaporization and condensation processes. To vaporize, solvent molecules must be present at the surface of the solution....
26.5K
Intermolecular Forces in Solutions02:28

Intermolecular Forces in Solutions

33.2K
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,...
33.2K

You might also read

Related Articles

Articles linked to this work by shared authors, journal, and citation graph.

Sort by
Same author

Hacking a Brønsted photoacid to capture and directly release a Lewis acid: application to CO<sub>2</sub> photorelease.

Chemical science·2026
Same author

Sensing the acidity of hydrogen bond networks.

Physical chemistry chemical physics : PCCP·2026
Same author

Vibrationally-Resolved Electrochemical Impedance Spectroscopy.

Journal of the American Chemical Society·2026
Same author

Unveiling Superacidity in Alcohol-BF<sub>3</sub> Complexes Using a Vibrational Probe.

The journal of physical chemistry letters·2026
Same author

Single droplet displacement infrared action spectroscopy.

Nature communications·2026
Same author

Ions as Substituents: A Supramolecular Hammett Approach for Electrostatic Control of Acidity.

The journal of physical chemistry letters·2026
Same journal

Recent progress in catalytic asymmetric synthesis of triarylmethanes.

Chemical science·2026
Same journal

GFP chromophore photophysics: ultrafast dynamics and hot ground state cooling in the neutral form.

Chemical science·2026
Same journal

Large Stokes shift fluorophores from <i>meta</i>-substituted zwitterions.

Chemical science·2026
Same journal

<i>In situ</i> glycosylation-directed H-aggregation of Type I photosensitizers for synergistic biofilm eradication and promoting diabetic wound healing.

Chemical science·2026
Same journal

Substituent engineering of dynamic covalent bonds enables simultaneous enhancement of performance and recyclability.

Chemical science·2026
Same journal

Visible-light-enabled three-component carboamidation of alkenes with aryl thianthrenium salts.

Chemical science·2026
See all related articles

Related Experiment Video

Updated: Jun 24, 2025

Proof-of-Concept for Gas-Entrapping Membranes Derived from Water-Loving SiO2/Si/SiO2 Wafers for Green Desalination
09:39

Proof-of-Concept for Gas-Entrapping Membranes Derived from Water-Loving SiO2/Si/SiO2 Wafers for Green Desalination

Published on: March 1, 2020

7.4K

Visualizing partial solvation at the air-water interface.

Kenneth D Judd1, Sean W Parsons1, Dmitry B Eremin1

  • 1Department of Chemistry, The University of Southern California Los Angeles CA 90089 USA dawlaty@usc.edu.

Chemical Science
|June 7, 2024
PubMed
Summary
This summary is machine-generated.

Researchers studied interfacial reactivity using an azide probe. They found that both electrostatic interactions and hydrogen bonding influence reactions at the air-water interface, impacting chemical processes.

More Related Videos

Studying Surfactant Effects on Hydrate Crystallization at Oil-Water Interfaces Using a Low-Cost Integrated Modular Peltier Device
06:31

Studying Surfactant Effects on Hydrate Crystallization at Oil-Water Interfaces Using a Low-Cost Integrated Modular Peltier Device

Published on: March 18, 2020

6.3K
Probing the Structure and Dynamics of Interfacial Water with Scanning Tunneling Microscopy and Spectroscopy
10:28

Probing the Structure and Dynamics of Interfacial Water with Scanning Tunneling Microscopy and Spectroscopy

Published on: May 27, 2018

8.8K

Related Experiment Videos

Last Updated: Jun 24, 2025

Proof-of-Concept for Gas-Entrapping Membranes Derived from Water-Loving SiO2/Si/SiO2 Wafers for Green Desalination
09:39

Proof-of-Concept for Gas-Entrapping Membranes Derived from Water-Loving SiO2/Si/SiO2 Wafers for Green Desalination

Published on: March 1, 2020

7.4K
Studying Surfactant Effects on Hydrate Crystallization at Oil-Water Interfaces Using a Low-Cost Integrated Modular Peltier Device
06:31

Studying Surfactant Effects on Hydrate Crystallization at Oil-Water Interfaces Using a Low-Cost Integrated Modular Peltier Device

Published on: March 18, 2020

6.3K
Probing the Structure and Dynamics of Interfacial Water with Scanning Tunneling Microscopy and Spectroscopy
10:28

Probing the Structure and Dynamics of Interfacial Water with Scanning Tunneling Microscopy and Spectroscopy

Published on: May 27, 2018

8.8K

Area of Science:

  • Physical Chemistry
  • Chemical Physics
  • Surface Chemistry

Background:

  • Reactivity at the air-water interface, particularly in microdroplets, is not fully understood.
  • Electric fields and partial solvation are suspected contributors to interfacial reactivity.
  • Understanding these factors is crucial for controlling interfacial chemical reactions.

Purpose of the Study:

  • To investigate the mechanistic nuances of interfacial reactivity.
  • To elucidate the roles of electrostatics and hydrogen bonding at the air-water interface.
  • To quantify the influence of surface charge density on interfacial reactions.

Main Methods:

  • Utilized a well-defined azide vibrational probe to measure frequency shifts at the air-water interface.
  • Independently controlled surface charge density using anionic (sulfate) and cationic (ammonium) surfactants.
  • Established the probe's response in bulk solution to electrostatics and hydrogen bonding.

Main Results:

  • The azide probe experiences an intermediate solvation environment at the interface, not fully hydrated or aprotic.
  • Anionic sulfate surfactants induced a significant blue-shift due to dominant electrostatic effects.
  • Cationic ammonium surfactants showed a balanced interplay between electrostatics and hydrogen bonding, resulting in minimal shift.

Conclusions:

  • Interfacial reactivity is governed by partial solvation, with contributions from both hydrogen bonding and electrostatics.
  • These forces can either enhance or oppose each other, influencing the polarization of interfacial species.
  • The findings provide insights for understanding and manipulating chemical reactions at interfaces.