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

Ideal Solutions02:24

Ideal Solutions

19.0K
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...
19.0K
Solution Formation02:16

Solution Formation

31.1K
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...
31.1K
Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

610
Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...
610
Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

579
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...
579
Solubility Equilibria03:07

Solubility Equilibria

51.9K
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...
51.9K
Chemical and Solubility Equilibria02:21

Chemical and Solubility Equilibria

4.0K
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,...
4.0K

You might also read

Related Articles

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

Sort by
Same author

A Buffered Hexacyanoferrate Electrolyte for Thermogalvanic Heat Harvesting across Symmetric and Asymmetric Electrode Configurations.

ACS nano·2026
Same author

Nanoscale Compositional and Strain Gradients Enable High-Speed and Amplitude-Resolved Pyroelectric Sensing.

Advanced materials (Deerfield Beach, Fla.)·2026
Same author

A large-scale dataset and physics-informed neural network for viscosity prediction in many-component aqueous and organic solutions.

The Journal of chemical physics·2026
Same author

A needle-form 3-omega sensor for thermal conductivity measurements of soft materials and biological tissues.

Scientific reports·2025
Same author

On a Continuous Aqueous Thermogalvanic Redox Agent with Anomalous Thermopower.

Nano letters·2025
Same author

On the equilibrium limit of liquid stability in pressurized aqueous systems.

Nature communications·2024

Related Experiment Video

Updated: May 26, 2025

High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems
05:46

High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems

Published on: January 24, 2014

13.4K

A size-dependent ideal solution model for liquid-solid phase equilibria prediction in aqueous organic solutions.

Spencer P Alliston1, Chris Dames1, Matthew J Powell-Palm2,3,4

  • 1Department of Mechanical Engineering, University of California, Berkeley, CA 94720.

Proceedings of the National Academy of Sciences of the United States of America
|February 21, 2025
PubMed
Summary

Predicting phase equilibria in aqueous organic solutions is enhanced by a modified ideal solution theory. Accounting for molecular size differences significantly improves predictions of liquidus and eutectic points.

Keywords:
entropyphase diagramspredictive synthesissolution theorythermodynamics

More Related Videos

Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers
12:37

Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers

Published on: September 4, 2015

12.2K
Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy
10:08

Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy

Published on: October 24, 2017

9.1K

Related Experiment Videos

Last Updated: May 26, 2025

High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems
05:46

High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems

Published on: January 24, 2014

13.4K
Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers
12:37

Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers

Published on: September 4, 2015

12.2K
Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy
10:08

Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy

Published on: October 24, 2017

9.1K

Area of Science:

  • Physical Chemistry
  • Solution Thermodynamics
  • Materials Science

Background:

  • Predictive modeling of aqueous organic solutions is crucial for industrial chemistry and cryopreservation.
  • Current models struggle with accurate prediction of liquid-solid phase equilibria using only bulk properties.
  • Direct measurement or simulations are often required, limiting practical applications.

Purpose of the Study:

  • To develop an improved analytical model for predicting phase equilibria in aqueous organic solutions.
  • To enhance the predictive power of ideal solution theory by incorporating molecular size effects.
  • To provide a simpler, more accurate method for phase diagram prediction.

Main Methods:

  • Modified ideal solution theory incorporating Flory-style entropy of mixing.
  • Inclusion of mole and volume fractions for size-dependent calculations.
  • Prediction of binary phase diagrams for water and ten organic solutes.

Main Results:

  • Size-dependent model significantly outperforms the ideal solution model.
  • Reduced average error in liquidus temperature prediction by 59% (to 5.6 K).
  • Reduced average error in eutectic temperature by 45% (to 9.7 K) and composition by 43% (to 4.7 mol%).

Conclusions:

  • Molecular size effects, specifically mixing entropy, play a dominant role in aqueous organic solution phase behavior.
  • The modified model offers a simple yet powerful approach to predicting phase equilibria.
  • This work highlights the underappreciated impact of entropic effects in solution thermodynamics.