Isoelectric point

The isoelectric point (pI), sometimes abbreviated to IEP, is the pH at which a particular molecule or surface carries no net electrical charge.

Amphoteric molecules called zwitterions contain both positive and negative charges depending on the functional groups present in the molecule. The net charge on the molecule is affected by pH of their surrounding environment and can become more positively or negatively charged due to the loss or gain of protons (H+). The pI is the pH value at which the molecule carries no electrical charge or the negative and positive charges are equal.

Surfaces naturally charge to form a double layer. In the common case when the surface charge-determining ions are H+/OH-, the net surface charge is affected by the pH of the liquid in which the solid is submerged. Again, the pI is the pH value of the solution at which the surfaces carries no net charge.

The pI value can affect the solubility of a molecule at a given pH. Such molecules have minimum solubility in water or salt solutions at the pH that corresponds to their pI and often precipitate out of solution. Biological amphoteric molecules such as proteins contain both acidic and basic functional groups. Amino acids that make up proteins may be positive, negative, neutral, or polar in nature, and together give a protein its overall charge. At a pH below their pI, proteins carry a net positive charge; above their pI they carry a net negative charge. Proteins can, thus, be separated according to their isoelectric point (overall charge) on a polyacrylamide gel using a technique called isoelectric focusing, which uses a pH gradient to separate proteins. Isoelectric focusing is also the first step in 2-D gel polyacrylamide gel electrophoresis.

Calculating pI values
For an amino acid with only one amine and one carboxyl group, the pI can be calculated from the mean of the pKas of this molecule.


 * $$ pI = {{pK_1 + pK_2} \over 2} $$

For amino acids with more than two ionizable groups, such as lysine, the same formula is used, but this time the two pKa's used are those of the two groups that lose and gain a charge from the neutral form of the amino acid. Lysine has a single carboxylic pKa and two amine pKa values (one of which is on the R-group), so fully protonated lysine has a +2 net charge. To get a neutral charge, we must deprotonate the lysine twice, and therefore use the R-group and amine pKa values (found at List of standard amino acids).


 * $$ pI = {{9.06 + 10.54} \over 2} = 9.80 $$

The pH of an electrophoretic gel is determined by the buffer used for that gel. If the pH of the buffer is above the pI of the protein being run, the protein will migrate to the positive pole (negative charge is attracted to a positive pole). If the pH of the buffer is below the pI of the protein being run, the protein will migrate to the negative pole of the gel (positive charge is attracted to the negative pole). If the protein is run with a buffer pH that is equal to the pI, it will not migrate at all. This is also true for individual amino acids.

Examples
In these three examples the isoelectric point is shown by the green vertical line. In glycine the pK values are separated by nearly 7 units so the concentration of the neutral species, glycine (GlyH), is effectively 100% of the analytical glycine concentration. Glycine may exist as a zwitterion at the isoelectric point, but the equilibrium constant for the isomerization reaction in solution
 * H2NCH2CO2H  H3N+CH2CO2-

is not known.

Lysine has an amino group on the side-chain, so the isoelectric point is the average of the amino group pK values. The concentration of the neutral species, lysine (LH), is a maximum at the isoelectric point, but the concentration is less than 100% because the difference in pK values is only about 1.5. Lysine may exist as a zwitterion in solution.

The third example, adenosine monophosphate is shown to illustrate the fact that a third species may, in principle, be involved. In actual fact the concentration of (AMP)H32+ is negligible at the isoelectric point in this case.

Ceramic materials
The isoelectric points (IEP) of metal oxide ceramics are used extensively in material science in various aqueous processing steps (synthesis, modification, etc.). For these surfaces, present as colloids or larger particles in aqueous solution, the surface is generally assumed to be covered with surface hydroxyl species, M-OH (where M is a metal such as Al, Si, etc.). At pH values above the IEP, the predominate surface species is M-O-, while at pH values below the IEP, M-OH2+ species predominate. Some approximate values of common ceramics are listed below (Haruta and Brunelle, except where noted). The exact value can vary widely, depending on material factors such as purity and phase as well as physical parameters such as temperature. In addition, precise measurement of isoelectric points is difficult and requires careful techniques, even with modern methods. Thus, many sources often cite differing values for isoelectric points of these materials.

Examples of isoelectric points
The following list gives the pH25°C of isoelectric point at 25 °C for selected materials in water:

Note: The list is ordered by increasing pH values.


 * tungsten(VI) oxide WO3: 0.2-0.5
 * antimony(V) oxide Sb2O5: <0.4 to 1.9
 * vanadium(V) oxide (vanadia) V2O5: 1-2 (3 )
 * silicon dioxide (silica) SiO2: 1.7-3.5
 * silicon carbide (alpha) SiC: 2-3.5
 * tantalum(V) oxide, Ta2O5: 2.7-3.0
 * tin(IV) oxide SnO2: 4-5.5 (7.3 )
 * zirconium(IV) oxide (zirconia) ZrO2: 4-11
 * manganese(IV) oxide MnO2: 4-5
 * delta-MnO2 1.5, beta-MnO2 7.3
 * titanium(IV) oxide (titania) (rutile or anatase) TiO2: 3.9-8.2
 * silicon nitride Si3N4: 6-7
 * iron (II, III) oxide (magnetite) Fe3O4: 6.5-6.8
 * gamma iron (III) oxide (maghemite) Fe2O3: 3.3-6.7
 * cerium(IV) oxide (ceria) CeO2: 6.7-8.6
 * chromium(III) oxide (chromia) Cr2O3: 7 (6.2-8.1 )
 * gamma aluminium oxide (gamma alumina) Al2O3: 7-8
 * thallium(I) oxide Tl2O: 8
 * alpha iron (III) oxide (hematite) Fe2O3: 8.4-8.5
 * alpha aluminium oxide (alpha alumina, corundum) Al2O3: 8-9
 * silicon nitride Si3N4: 9
 * yttrium(III) oxide (yttria) Y2O3: 7.15-8.95
 * copper(II) oxide CuO: 9.5
 * zinc oxide ZnO: 8.7-10.3
 * lanthanum(III) oxide La2O3: 10
 * nickel(II) oxide NiO: 10-11 (9.9-11.3 )
 * lead(II) oxide PbO: 10.7-11.6
 * magnesium oxide (magnesia) MgO: 12-13 (9.8-12.7 )

Mixed oxides may exhibit isoelectric point values that are intermediate to those of the corresponding pure oxides. For example, Jara et al. measured an IEP of 4.5 for a synthetically prepared amorphous aluminosilicate (Al2O3-SiO2). The researchers noted that the electrokinetic behavior of the surface was dominated by surface Si-OH species, thus explaining the relatively low IEP value. Significantly higher IEP values (pH 6 to 8) have been reported for 3Al2O3-2SiO2 by others (see Lewis ). Lewis also lists the IEP of barium titanate, BaTiO3 as being between pH 5 and 6, while Vamvakaki et al. reported a value of 3, although these authors note that a wide range of values have been reported, a result of either residual barium carbonate on the surface or TiO2-rich surfaces.

The farther the pH of an Amino Acid solution is from its pl the greater the electric charge on that population of molecules.

Isoelectric point versus point of zero charge
The terms isoelectric point (IEP) and point of zero charge (PZC) are often used interchangeably, although under certain circumstances, it may be productive to make the distinction.

In systems in which H+/OH- are the interface potential-determining ions, the point of zero charge is given in terms of pH. The pH at which the surface exhibits a neutral net electrical charge is the point of zero charge at the surface. Electrokinetic phenomena generally measure zeta potential, and a zero zeta potential is interpreted as the point of zero net charge at the shear plane. This is termed the isoelectric point. Thus, the isoelectric point is the value of pH at which the colloidal particle remains stationary in an electrical field. The isoelectric point is expected to be somewhat different than the point of zero charge at the particle surface, but this difference is often ignored in practice for so-called pristine surfaces, i.e., surfaces with no specifically adsorbed positive or negative charges. In this context, specific adsorption is understood as adsorption occurring in a Stern layer or chemisorption. Thus, point of zero charge at the surface is taken as equal to isoelectric point in the absence of specific adsorption on that surface.

According to Jolivet, in the absence of positive or negative charges, the surface is best described by the point of zero charge. If positive and negative charges are both present in equal amounts, then this is the isoelectric point. Thus, the PZC refers to the absence of any type of surface charge, while the IEP refers to a state of neutral net surface charge. The difference between the two, therefore, is the quantity of charged sites at the point of net zero charge. Jolivet uses the intrinsic surface equilibrium constants, pK- and pK+ to define the two conditions in terms of the relative number of charged sites:


 * $$ pK^- - pK^+ = \Delta pK = \log {\frac{\left[MOH\right]^2}{\left[MOH{_2^+}\right]\left[MO^-\right]}} $$

For large ΔpK (>4 according to Jolivet), the predominate species is MOH while there are relatively few charged species - so the PZC is relevant. For small values of ΔpK, there are many charged species in approximately equal numbers, so one speaks of the IEP.