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Sodium dodecyl sulfate

Sodium dodecyl sulfate
IUPAC name Sodium dodecyl sulfate
Other names Sodium monododecyl sulfate; Sodium lauryl sulfate; Sodium monolauryl sulfate; Sodium dodecanesulfate; dodecyl alcohol, hydrogen sulfate, sodium salt; n-dodecyl sulfate sodium; Sulfuric acid monododecyl ester sodium salt;
CAS number 151-21-3
Molecular formula NaC12H25SO4
Molar mass 288.38 g mol−1
Density 1.01 g/cm³
Melting point

206 °C

Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Sodium dodecyl sulfate (or sulphate) (SDS or NaDS) (C12H25SO4Na), is an anionic surfactant that is used in household products such as toothpastes, shampoos, shaving foams and bubble baths for its thickening effect and its ability to create a lather. The molecule has a tail of 12 carbon atoms, attached to a sulfate group, giving the molecule the amphiphilic properties required of a detergent.

It is prepared by esterification of sulfuric acid with dodecanol (lauryl alcohol, C12H25OH) followed by neutralization with sodium carbonate. It is used in both industrially produced and home-made cosmetics.

Like all detergent surfactants (including soaps), it removes oils from the skin, and can cause skin and eye irritation.

SDS can be converted by ethoxylation to sodium laureth sulfate (also called sodium lauryl ether sulfate; SLES), which is less harsh on the skin, probably because it is not as much of a protein denaturant as is the unethoxylated substance.

It is probably the most researched anionic surfactant compound.

It has recently found application as a surfactant in gas hydrate or methane hydrate formation reactions, increasing the rate of formation as much as 700 times.[1]


Biochemical applications

In laboratories, SDS is commonly used in preparing proteins for polyacrylamide gel electrophoresis (SDS-PAGE). SDS works by disrupting non-covalent bonds in the proteins, thereby denaturing them, causing the molecules to lose their native shape (conformation). Also, anions of SDS bind to the main peptide chain at a ratio of one SDS anion for every two amino acid residues. This effectively imparts a negative charge on the protein that is proportional to the mass of that protein (about 1.4 g SDS/g protein). This new negative charge is significantly greater than the original charge of that protein. The electrostatic repulsion that is created by binding of SDS causes proteins to unfold into a rod-like shape thereby eliminating differences in shape as a factor for separation in the gel.

Safety concerns relating to SDS

When handling SDS in its solid form use extreme caution, the compound easily particlizes into the air. If inhaled can cause a serious choking hazard. It is strongly advised that a dust mask and vacuum hood be used when working with the compound to minimize exposure.

A number of health concerns about SDS have been raised in published reports.[2][3][4] These studies indicate that:

  • SDS may cause a number of skin problems (for which the non-specific term is dermatitis), with some people being affected more than others.[4][5][6]
  • SDS may cause aphthous ulcers, commonly referred to in some countries as "canker sores".[7][8]


  • The critical micelle concentration in pure water at 25°C is 0.0082 M, and the aggregation number at this concentration is usually considered to be about 50. The micelle ionization fraction (α) is around 0.3 (or 30%).[9]
  • The Optical refractive index increment of a pure aqueous solution at wavelength 532 nm is about 0.1070 ml/g.[citation needed]

See also


  1. ^ Kazuyoshi Watanabe, Shuntaro Imai and Yasuhiko H. Mori. Surfactant effects on hydrate formation in an unstirred gas/liquid system: An experimental study using HFC-32 and sodium dodecyl sulfate. Department of Mechanical Engineering, Keio University, 3-14-1 Hiyoshi, Kohoku-ku, Yokohama 223-8522. Japan.Chemical Engineering Science. Volume 60, Issue 17, September 2005, Pages 4846-4857. Abstract
  2. ^ Agner T. Susceptibility of atopic dermatitis patients to irritant dermatitis caused by sodium lauryl sulphate. Acta Derm Venereol. 1991;71(4):296-300. PMID 1681644
  3. ^ A. Nassif, S. C. Chan, F. J. Storrs and J. M. Hanifin. Abstract: Abnormal skin irritancy in atopic dermatitis and in atopy without dermatitis. Arch Dermatol. November 1994;130(11):1402. Abstract
  4. ^ a b Marrakchi S, Maibach HI. Sodium lauryl sulfate-induced irritation in the human face: regional and age-related differences. Skin Pharmacol Physiol. 2006;19(3):177-80. Epub 2006 May 4. PMID 16679819
  5. ^ CIR publication. Final Report on the Safety Assessment of Sodium Lauryl Sulfate and Ammonium Lauryl Sulfate. Journal of the American College of Toxicology. 1983 Vol. 2 (No. 7) pages 127-181.
  6. ^ Loffler H, Effendy I. Skin susceptibility of atopic individuals. Department of Dermatology, University of Marburg, Germany. Contact Dermatitis. 1999 May;40(5):239-42. PMID 10344477
  7. ^ Chahine L, Sempson N, Wagoner C. The effect of sodium lauryl sulfate on recurrent aphthous ulcers: a clinical study. Compend Contin Educ Dent. 1997 Dec;18(12):1238-40. PMID 9656847
  8. ^ Herlofson BB, Barkvoll P. The effect of two toothpaste detergents on the frequency of recurrent aphthous ulcers. Acta Odontol Scand. 1996 Jun;54(3):150-3. PMID 8811135
  9. ^ Barney L. Bales, Luis Messina, Arwen Vidal, Miroslav Peric, and Otaciro Rangel Nascimento. Precision Relative Aggregation Number Determinations of SDS Micelles Using a Spin Probe. A Model of Micelle Surface Hydration. J. Phys. Chem. B. 1998 102(50)10347-10358. Abstract
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Sodium_dodecyl_sulfate". A list of authors is available in Wikipedia.
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