Related Experiment Video

Updated: Jul 18, 2026

Optimization of Crystal Growth for Neutron Macromolecular Crystallography
12:29

Optimization of Crystal Growth for Neutron Macromolecular Crystallography

Published on: March 13, 2021

[Solubility and phase transitions in the water-protein-salt system]

S P Rozhkov

    Biofizika
    |November 30, 2006
    PubMed

    More Related Videos

    Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers12:37

    Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers

    Published on: September 4, 2015

    Controlling the Size, Shape and Stability of Supramolecular Polymers in Water16:24

    Controlling the Size, Shape and Stability of Supramolecular Polymers in Water

    Published on: August 2, 2012

    Related Concept Videos

    Phase Transitions: Melting and Freezing02:39

    Phase Transitions: Melting and Freezing

    Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
    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...
    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)...
    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...
    Entropy and Solvation02:05

    Entropy and Solvation

    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 ≥ 15); an...
    Solubility Equilibria: Ionic Product of Water01:16

    Solubility Equilibria: Ionic Product of Water

    Pure water is a weak electrolyte; only a small amount ionizes into hydrogen and hydroxide ions. At any given temperature, the concentration of undissociated water is almost constant, so the ionic product of water is the product of the hydrogen and hydroxide ion concentrations, denoted as Kw. The square root of Kw gives the individual ion concentrations.
    The ionic product of water varies with temperature, and its value is 1.0 x 10−14 at standard experimental conditions. Per Le Chatelier's...