Zeta potential is a parameter characterizing electrochemical equilibrium at interfaces. It depends on the properties of both the surface and the surrounding liquid. It plays an important role in the theory of aggregative stability, also known as DLVO theory. Electrostatic repulsion between particles is related to the value of zeta potential. The higher the zeta potential, the stronger the repulsion, and therefore the more stable the system becomes. For instance, the high zeta potential of fat droplets in milk prevents them from coalescing. Adding acid to milk, for example, reduces the zeta potential and causes the milk fat droplets to coalesce. The end result is the formation of cheese.
Zeta potential is a property of an electric structure that is usually built up at interfaces, in a region referred to as the “double layer” (DL). Simply explained, the double layer is a structure that forms on the surface of an object in a liquid. It consists of two layers: a surface charge layer of ions chemically adsorbed onto the surface, and a second layer of oppositely charged ions which are attracted to the surface by Coulomb forces.
This phenomena was described in Fundamentals of Colloid and Interface Science by J. Lyklema: “…the reason for the formation of a “relaxed” (“equilibrium”) double layer is the non-electric affinity of charge-determining ions for a surface…”. This process leads to the build-up of an electric surface charge. This surface charge creates an electrostatic field that then affects the ions in the bulk of the liquid. This electrostatic field, in combination with the thermal motion of the ions, creates a counter-charge, and thus screens the electric surface charge. The net electric charge in this screening diffuse layer is equal in magnitude to the net surface charge, but has the opposite polarity. As a result the complete structure is electrically neutral.
Distribution of the electric potential in the DL is shown in the Figure below for a positively charged surface.
Electric potential decays almost exponentially, which allows introduction of the “Debye length“ as an estimate of the DL thickness. Electric potential drops by approximately 2.7 times at the distance from the surface that equals to the Debye length. Debye length depends mostly on “ionic strength” of the liquid. It is approximately 1 nm at an ionic strength of 0.1 M, and it increases as a reciprocal of the square root of ionic strength (electrolyte concentration) becoming, for instance, 10 nm at an ionic strength of 0.001 M.
There is another characteristic distance within DL: the location of a slipping plane associated with tangential motion of the liquid relative to the surface. The liquid inside of the slipping plane remains attached to the surface, whereas the liquid beyond the slipping plane moves with the surrounding liquid. The electric potential at the slipping plane is what is referred to as “Zeta potential.” It is measured in millivolts (mV), with a maximum absolute value of 100 mV in aqueous solutions, according to International Standard ISO 13099, Parts 1: 2012 “Colloidal systems – Methods for Zeta potential determination”.
Calculation of Zeta Potential from the parameters measured by zeta potential analyzers requires appropriate theory.There are two important asymptotic cases when analytical theories exist. The most known case is that of a “thin DL”, which corresponds to particulates with DLs that are much thinner than their particle radius. The vast majority of aqueous dispersions satisfy this condition, except for very small particles and low ionic strength media. Calculation of Zeta Potential can be performed using the “Smoluchowski theory” when surface conductivity is negligible.
The opposite asymptotic case is that of a “thick DL,” which corresponds to systems where the DL is much larger than the particle radius. The vast majority of dispersions in hydrocarbon media, which inherently have very low ionic strength, satisfy this condition.
These two asymptotic cases allow one to picture, at least approximately, the DL structure around spherical particles.
There is one more important factor affecting DL structure: the so-called “overlap of DLs”. Increasing volume fraction and/or reduction of the particle size brings particles surfaces close and eventually diffuse layers would overlap. This overlap of Double Layers might become important for nano-particles, macro-molecules, proteins, etc. It is definitely important in non-polar liquids, within which double layers extend quite far and are therefore more likely to overlap. This overlap of Double Layers is also important in in porous materials.
There are more details can be found in the JUPAC report on Electrokinetic phenomena, as well as on Wikipedia. An overview of the different methods of Zeta Potential measurement can be found in our book.