Precipitation (chemistry)

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The process by which a dissolved chemical species comes out of solution as a solid is called precipitation. It is often employed in bioseparation applications for protein purification and concentration, although it may be used to isolate other compounds, such as nucleic acids and other cell components. Precipitation is achieved by altering the solubility of a target protein in a solution to cause it to become insoluble and thus precipitate, allowing for this concentrated solid to be more easily separated from the liquid phase (supernatant).

File:Http://en.citizendium.org/images/c/c9/Precipitation outline.png

Example of a typical precipitation process, proceeding from an initial homogenous solution to final separation of the target solute. Andrei Georgescu 08:40, 14 December 2010 (UTC)

Solubility of Macromolecules

Solubility is the property of a substance (solute) – in either gas, liquid, or solid phases – that determines the extent to which it dissolves in a liquid (called the solvent) and form a homogenous (single-phase) solution. It is based on factors such as temperature, compatibility between the solute’s net charge and the solvent’s polarity, the formation of hydration layers, the presence and concentration of other solutes dissolved in the solvent, and solvent’s ionic strength and dielectric constant.

Macromolecules (such as proteins and nucleic acids) are typically present in aqueous solvents. They are able to dissolve as a result of assuming a stable conformation in the solvent and then being surrounded by hydration layer(s). When placed in an aqueous solution, the macromolecules adopt a structure in which most hydrophobic (nonpolar) portions of the molecules gather inwards, and most hydrophilic (charged/polar) portions surround the exterior, guided to a final conformation that has the lowest Gibbs free energy. The attraction between the hydrophilic surface of the macromolecule and the polar water molecules creates an interface in which similarly-oriented water molecules associate with, and surround, the solute’s surface to form a highly ordered layer, called the hydration layer (also called the interfacial double layer). The formation of hydration layers enhances the solubility of macromolecules by greatly reducing inter-macromolecular dipole-dipole attraction and thus preventing their association with other solutes.

Effects of Solute Net Charge

In an aqueous solvent solutes with a higher net charge are more soluble, due to their enhanced ability to associate with water molecules and create a hydration layer, and their lessened inter-solute interactions as a result of increased repulsion from like-charges.

Effects of Solvent Ionic Strength

Increasing a solvent’s ionic strength (the concentration of ions in solution) decreases the availability of unassociated water molecules, which are required for the formation of hydration layers. This increases intermolecular attraction between solutes and promotes coalescence, thus decreasing the solute’s solubility.

Common Methods of Precipitation

Salting Out

A common method of protein precipitation is called salting out, and is achieved by increasing an aqueous solvent’s ionic strength by dissolving a salt. Increases in salt concentrations steadily decrease the solubility of proteins in the solution, until the proteins become insoluble and precipitate out of solution. Since proteins generally differ in their solubility, slowly adding salt allows for selective precipitation of dissolved proteins in order of lowest to highest solubility. This process is described empirically by the Cohn equation:
$ln(S)=\beta -K_{s}^{'}*I$
where $S$ is the solubility of the protein in mol/L, $\beta$ is the solubility at zero ionic strength in mol/L, $K_{s}^{'}$ is the protein’s characteristic salting-out constant (unitless), and $I$ is the concentration of ions in solution in mol/L.

The most commonly used salt for this procedure is ammonium sulfate, (NH₄)₂SO₄ due to its high solubility, lack of buffering capacity, minimal cost, and the low density of the resulting solution relative to other salts, which aids in centrifugation separation.

Isoelectric Precipitation

At its isoelectric pH, called the pI, a macromolecule possesses no net charge and thus no like-charge repulsion occurs between solutes. This results in weaker interactions with water molecules and makes the macromolecule more hydrophobic, increasing its affinity for combining with other solutes, and thus allowing for precipitation. Isoelectric precipitation is the process by which the pH of the solution is manipulated to reach the solute's pI to achieve this effect.

Alcohol Precipitation & Other Changes in Solvent

The addition of a nonpolar solvent like ethanol to a solution typically decreases solubility of highly charged solutes, and is commonly used in nucleic acid precipitation. The nonpolar alcohols compete with water for association with the dissolved solute and destabilize the hydration layer, increasing the solute’s ability to form hydrophobic interactions with other solutes, and decreasing its solubility as a result.

Flocculation

Flocculation is a process by which particles of an insoluble, dispersed (but not dissolved), and colloidal substance join together to form flaky aggregations called flocs. Typically, most biological particles suspended in a solution possess a negative charge reference. This creates repulsion between the particles, which is counteracted by a mutual attraction due to van der Waals forces. Although at short range the van der Waals forces are much more powerful, they decay rapidly with distance and as a result, inter-particle repulsive forces – which act a greater range – typically prevent particles from achieving this required approach distance.

Flocculation is achieved by minimizing the contribution of repulsive forces in order to maximize the effect of the van der Waals force, to an extent that allows the particles to move sufficiently close to permit the van der Waals force to drive particle aggregation. The most common process to produce this effect is to increase the ionic strength of the solution by dissolving a salt, whose charged ions interfere with inter-solute repulsion.

Precipitate Formation

When the concentration of a solute is greater than its equilibrium solubility, it is termed supersaturated. The process of precipitation begins in a supersaturated solution first by nucleation, in which ultramicroscopic clusters of particles are generated. Following nucleation, diffusion-limited growth of the particles occurs until the particles reach a diameter limited by the shear field of the fluid. The rate at which particles aggregate may be described by the following rate equation:
$-{\frac {dN}{dt}}=8{\pi }DL_{mol}N^{2}$
where $N$ is the number of the ultramicroscopic clusters initially created by nucleation, $D$ is the diffusivity, and $L_{mol}$ is the diameter of the particles. Integrating the equation gives:
${\frac {N}{N_{0}}}={\frac {1}{1+N_{0}K_{A}t}}$
where $N_{0}$ is the initial number of particles. After reaching their critical size, the clusters undergo a flocculation process in which their continued growth is governed by fluid motion, which causes them to collide and stick together. This growth is described by the equation:
${\frac {N}{N_{0}}}=exp(-{\frac {2{\alpha }L^{3}NGt}{3}})$
where ${\alpha }$ is the fraction of collisions that result in permanent aggregates, $N$ is the number of particles, $t$ is time elapsed, $L$ is the diameter of the particles, and $G$ is the shear rate. The flocs reach a stable size after a period called the “aging” time elapses.

History

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Invention and early development

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Recent developments

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Design and Operation

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Applications

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Examples

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