Aqueous Phase
Aqueous Phase - Related Videos
10:11
Cell Co-culture Patterning Using Aqueous Two-phase Systems
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Cited by 32 •
2013
Aqueous two-phase systems were used to simultaneously pattern multiple populations of cells. This fast and easy method for cell patterning takes advantage of the phase separation of aqueous solutions of dextran and polyethylene glycol and the interfacial tension that exists between the two polymer solutions.
09:58
Robotic Production of Cancer Cell Spheroids with an Aqueous Two-phase System for Drug Testing
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Cited by 37 •
2015
A protocol for robotic printing of cancer cell spheroids in a high throughput 96-well plate format using an aqueous two-phase system is presented.
03:03
Chemical Reactions in Aqueous Solutions
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2020
Chemical substances interact in many different ways. Certain chemical reactions exhibit common patterns of reactivity. Due to the vast number of chemical reactions, it becomes necessary to classify them based on the observed patterns of interaction. Water is a good solvent that can dissolve many substances. For this reason, many chemical reactions take place in water. Such reactions are called aqueous reactions. The three most common types of aqueous reactions are precipitation, acid-base, and...
09:50
Measuring the Densities of Aqueous Glasses at Cryogenic Temperatures
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Cited by 4 •
2017
A protocol for determining the vitreous phase densities of micro- to pico-liter size drops of aqueous mixtures at cryogenic temperatures is described.
02:42
Aqueous Solutions and Heats of Hydration
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2020
Water and other polar molecules are attracted to ions. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. These attractions play an important role in the dissolution of ionic compounds in water. When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between them. This process...
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Hydration surrounds dissolved ions and molecules with oriented water molecules, while hydrogen bonding helps stabilize solutes. These interactions support dissociation and diffusion, allowing species to move and respond within the solution. Their behavior is also shaped by ion–ion interactions, which influence how components participate in chemical equilibria.
pH helps determine acid–base equilibria in solution, while ionic strength reflects the overall influence of dissolved ions on ion interactions. Together with composition and concentration, these variables help predict whether dissolved species remain available, change chemical form, or contribute to processes such as precipitation and complex formation.
In liquid–liquid extraction, the aqueous phase is considered alongside an organic phase rather than as an isolated solution. Comparing how compounds behave in the two phases supports phase separation and helps researchers evaluate recovery or purification. Aqueous composition, concentration, pH, and ionic strength are therefore important when interpreting the extraction outcome.
Researchers examine composition, concentration, pH, and ionic strength to characterize an aqueous phase before interpreting its chemistry. These variables provide the basis for predicting solubility, reaction pathways, phase separation, and compound recovery. Tracking them is especially useful when the solution participates in precipitation, titration, redox reaction, or extraction.
An aqueous phase can serve as the reaction medium for precipitation, complex formation, titrations, and redox reactions. Each application uses dissolved ions and molecules in a different way: precipitation separates material, complex formation changes chemical associations, and titrations or redox reactions reveal or alter solution composition. These uses make aqueous systems central to chemical investigations.
Because water supports dissolved ions and molecules, aqueous phases connect solution chemistry with biological processes as well as laboratory reactions. Their acid–base equilibria, diffusion, and ion interactions help determine how chemical species behave in biologically relevant systems. The same principles also guide recovery and purification when an aqueous phase is paired with an organic phase.