In colloidal and surface chemistry, the critical micelle concentration (CMC) is defined as the concentration of surfactants above which micelles form and all additional surfactants added to the system will form micelles.[1]
The CMC is an important characteristic of a surfactant. Before reaching the CMC, the surface tension changes strongly with the concentration of the surfactant. After reaching the CMC, the surface tension remains relatively constant or changes with a lower slope. The value of the CMC for a given dispersant in a given medium depends on temperature, pressure, and (sometimes strongly) on the presence and concentration of other surface active substances and electrolytes. Micelles only form above critical micelle temperature.[citation needed]
For example, the value of CMC for sodium dodecyl sulfate in water (without other additives or salts) at 25 °C, atmospheric pressure, is 8x10−3 mol/L.[2]
| Surfactant | CMC (molarity) | Category |
|---|---|---|
| Sodium octyl sulfate | 0.13 | anionic surfactant |
| Sodium dodecyl sulfate | 0.0083 | anionic surfactant |
| Sodium tetradecyl sulfate | 0.0021 | anionic surfactant |
| Decyltrimethylammonium bromide | 0.065 | cationic surfactant |
| Dodecyltrimethylammonium bromide | 0.016 | cationic surfactant |
| Hexadecyltrimethylammonium bromide | 0.00092 | cationic surfactant |
| Penta(ethyleneglycol)monooctyl ether | 0.0009 | neutral surfactant |
| Penta(ethyleneglycol)monodecyl ether | 0.0009 | neutral surfactant |
| Pentaethylene glycol monododecyl ether | 0.000065 | neutral surfactant |
Description
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Upon introducing surfactants (or any surface active materials) into a system, they will initially partition into the interface, reducing the system free energy by:[citation needed]
- lowering the energy of the interface (calculated as area times surface tension), and
- removing the hydrophobic parts of the surfactant from contact with water.
Subsequently, when the surface coverage by the surfactants increases, the surface free energy (surface tension) decreases and the surfactants start aggregating into micelles, thus again decreasing the system's free energy by decreasing the contact area of hydrophobic parts of the surfactant with water.[4] Upon reaching CMC, any further addition of surfactants will just increase the number of micelles (in the ideal case).[citation needed]
According to one well-known definition, CMC is the total concentration of surfactants under the conditions:[5]
- if C = CMC, (d3 /dCt3) = 0
- = A[Cs] B[Cm]; i.e., in words Cs = [single surfactant ion] , Cm = [micelles] and A and B are proportionality constants
- Ct = Cs NCm; i.e., N = represents the number of detergent ions per micelle
Measurement
editThe CMC generally depends on the method of measuring the samples, since A and B depend on the properties of the solution such as conductance, photochemical characteristics, or surface tension. When the degree of aggregation is monodisperse, then the CMC is not related to the method of measurement. On the other hand, when the degree of aggregation is polydisperse, then CMC is related to both the method of measurement and the dispersion.[citation needed]
The common procedure to determine the CMC from experimental data is to look for the intersection (inflection point) of two straight lines traced through plots of the measured property versus the surfactant concentration. This visual data analysis method is highly subjective and can lead to very different CMC values depending on the type of representation, the quality of the data and the chosen interval around the CMC.[6] A preferred method is the fit of the experimental data with a model of the measured property. Fit functions for properties such as electrical conductivity, surface tension, NMR chemical shifts, absorption, self-diffusion coefficients, fluorescence intensity and mean translational diffusion coefficient of fluorescent dyes in surfactant solutions have been presented.[7][8][9] These fit functions are based on a model for the concentrations of monomeric and micellised surfactants in solution, which establishes a well-defined analytical definition of the CMC, independent from the technique.
The CMC is the concentration of surfactants in the bulk at which micelles start forming. The word bulk is important because surfactants partition between the bulk and interface and CMC is independent of interface and is therefore a characteristic of the surfactant molecule. In most situations, such as surface tension measurements or conductivity measurements, the amount of surfactant at the interface is negligible compared to that in the bulk and CMC can be approximated by the total concentration. In practice, CMC data is usually collected using laboratory instruments which allow the process to be partially automated, for instance by using specialised tensiometers.[citation needed]
Practical considerations
editWhen the interfacial areas are large, the amount of surfactant at the interface cannot be neglected. If, for example, air bubbles are introduced into a solution of a surfactant above CMC, these bubbles, as they rise to the surface, remove surfactants from the bulk to the top of the solution creating a foam column and thus reducing the concentration in bulk to below CMC. This is one of the easiest methods to remove surfactants from effluents (see foam flotation). Thus in foams with sufficient interfacial area are devoid of micelles. Similar reasoning holds for emulsions.[citation needed]
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The other situation arises in detergents. One initially starts off with concentrations greater than CMC in water and on adding fabric with large interfacial area, the surfactant concentration drops below CMC and no micelles remain at equilibrium. Therefore, the solubilization plays a minor role in detergents. Removal of oily soil occurs by modification of the contact angles and release of oil in the form of emulsion.[citation needed]
In petroleum industry, CMC is considered prior to injecting surfactant in reservoir regarding enhanced oil recovery (EOR) application. Below the CMC point, interfacial tension between oil and water phase is no longer effectively reduced.[10] If the concentration of the surfactant is kept a little above the CMC, the additional amount covers the dissolution with existing brine in the reservoir. It is desired that the surfactant will work at the lowest interfacial tension (IFT).[citation needed]
See also
editReferences
edit- ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "critical micelle concentration". doi:10.1351/goldbook.C01395
- ^ Dominguez, Ana; Fernandez, Aurora; Gonzalez, Noemi; Iglesias, Emilia; Montenegro, Luis (October 1997). "Determination of Critical Micelle Concentration of Some Surfactants by Three Techniques". Journal of Chemical Education. 74 (10): 1227–1231. doi:10.1021/ed074p1227. ISSN 0021-9584. Archived from the original on 13 March 2023. Retrieved 2 June 2023.
- ^ Holmberg, Krister (2019). "Surfactants". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 1–56. doi:10.1002/14356007.a25_747.pub2. ISBN 9783527306732. S2CID 242339510.
- ^ Hakiki, Farizal; Maharsi, Dara Ayuda; Marhaendrajana, Taufan (31 December 2015). "Surfactant-Polymer Coreflood Simulation and Uncertainty Analysis Derived from Laboratory Study". Journal of Engineering and Technological Sciences. 47 (6): 706–725. doi:10.5614/j.eng.technol.sci.2015.47.6.9. Archived from the original on 20 August 2016. Retrieved 1 July 2016.
- ^ Phillips J. The energetics of micelle formation. Transactions of the Faraday Society 1955;51:561-9
- ^ Mukerjee, P.; Mysels, K. J. In Critical Micelle Concentrations of Aqueous Surfactant Systems; NIST National Institute of Standards and Technology: Washington D.C. USA, 1971; Vol. NSRDS-NBS 36
- ^ Al-Soufi, Wajih; Piñeiro, Lucas; Novo, Mercedes (15 March 2012). "A model for monomer and micellar concentrations in surfactant solutions: Application to conductivity, NMR, diffusion, and surface tension data". Journal of Colloid and Interface Science. 370 (1): 102–110. doi:10.1016/j.jcis.2011.12.037. hdl:10347/17083. ISSN 0021-9797. PMID 22265231.
- ^ Lucas Piñeiro, Sonia Freire, Jorge Bordello, Mercedes Novo, and Wajih Al-Soufi, Dye Exchange in Micellar Solutions. Quantitative Analysis of Bulk and Single Molecule Fluorescence Titrations. Soft Matter, 2013,9, 10779-10790, DOI: 10.1039/c3sm52092g
- ^ "Concentration-model for surfactants near the cmc | QBFE -USC". usc.es. Archived from the original on 4 April 2017. Retrieved 18 December 2023.
- ^ Hakiki, Farizal (2014). "A Critical Review on Microbial Enhanced Oil Recovery Using Artificial Sandstone Core: Mathematical Model". Archived from the original on 5 November 2022. Retrieved 5 November 2022.