Tetramethylammonium hydroxide

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Tetramethylammonium hydroxide
IUPAC name
tetramethylazanium hydroxide
Other names
tetramethylammonium hydroxide; N,N,N,-trimethylmethanaminium hydroxide
75-59-2 YesY
10424-66-5 (trihydrate) N
10424-65-4 (pentahydrate) N
ChemSpider 54928 YesY
Jmol interactive 3D Image
PubChem 60966
Molar mass 91.15 g·mol−1
Density ~ 1.015 g/cm3 (20-25% aqueous solution)
Melting point 67 °C (153 °F; 340 K) (pentahydrate)
Boiling point decomposes
Basicity (pKb) 4.2[1]
Safety data sheet Sigma-Aldrich MSDS for TMAH·5H2O
GHS pictograms The corrosion pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS) The skull-and-crossbones pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)


GHS signal word Danger[2]
H300, H311, H314, H318[2]
P260, P264, P270, P280, P301+310, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P322, P361, P363, P405[2]
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Related compounds
Other anions
tetramethylammonium chloride
Other cations
tetraethylammonium hydroxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Tetramethylammonium hydroxide (TMAH or TMAOH) is a quaternary ammonium salt with the molecular formula N(CH3)4+ OH, and is one of the simplest members of this class of organic compounds. This substance is known in a (relatively) stable solid form only as the pentahydrate. Commercially, the forms in which TMAH is most commonly encountered are as concentrated solutions in water or methanol. The solid and solutions are colorless, or yellowish if impure. Although TMAH has virtually no odor when pure, samples often have a strongly fishy smell from the trimethylamine which is commonly present as an impurity. TMAH has numerous and diverse industrial and research applications (see below).


It is important to note that anhydrous TMAH has never been isolated. The only relatively stable solid form in which this substance exists is as the pentahydrate, N(CH3)4OH·5H2O, and this has been assigned the CAS# 10424-65-4. A trihydrate, C4H13NO·3H2O, has also been reported, and this has been assigned the CAS# 10424-66-5. TMAH is most commonly encountered as an aqueous solution, in concentrations from ~2–25%, and less frequently as solutions in methanol. These solutions are identified by the CAS# 75-59-2.


One of the earliest preparations of TMAH reported in the literature is that of Walker and Johnston,[3] who made it by mixing tetramethylammonium chloride and potassium hydroxide in dry methanol, in which TMAH is soluble, but potassium chloride is not:

NMe4+Cl + KOH → NMe4+OH + KCl

Where Me stands for the methyl group, CH3-.

This report also provides details for isolation of TMAH as its pentahydrate, noting the existence of a trihydrate, and emphasizes the avidity which even the former exhibits for atmospheric moisture and carbon dioxide. These authors reported a m.p. of 62–63 °C for the pentahydrate, and a solubility in water of 220 g/100 mL at 15 °C.


  • TMAH undergoes simple acid-base reactions with strong or weak acids to produce tetramethylammonium salts whose anion is derived from the acid, e.g.[4]
(i) NMe4+OH + HCl → NMe4+Cl + H2O
(ii) NMe4+OH + CO2 → NMe4+HCO3
  • An aqueous solution of TMAH may be used to make other tetramethylammonium salts in a methathesis reaction with ammonium salts, whereby the anion is derived from the ammonium salt. The reaction is driven in the desired direction by evaporative removal of ammonia and water.[5] For example, tetramethylammonium thiocyanate may be made from ammonium thiocyanate, thus:
NMe4+OH + NH4+SCN → NMe4+SCN + NH3 + H2O
NMe4+OH → NMe3 + MeOH


TMAH is a very strong base.[6]


One of the industrial uses of TMAH is for the anisotropic etching of silicon.[7] It is used as a basic solvent in the development of acidic photoresist in the photolithography process, and is highly effective in stripping photoresist. TMAH has some phase transfer catalyst properties, and is used as a surfactant in the synthesis of ferrofluid, to inhibit nanoparticle aggregation.

TMAH is the commonest reagent currently used in thermochemolysis, an analytical technique involving both pyrolysis and chemical derivatization of the analyte.[8]

Wet anisotropic etching[edit]

TMAH belongs to the family of quaternary ammonium hydroxide (QAH) solutions and is commonly used to anisotropically etch silicon. Typical etching temperatures are between 70 and 90 °C and typical concentrations are 5–25 wt% TMAH in water. (100) silicon etch rates generally increase with temperature and decrease with increasing TMAH concentration. Etched silicon (100) surface roughness decreases with increasing TMAH concentration, and smooth surfaces can be obtained with 20% TMAH solutions. Etch rates are typically in the 0.1–1 micrometer per minute range.

Common masking materials for long etches in TMAH include silicon dioxide (LPCVD and thermal) and silicon nitride. Silicon nitride has a negligible etch rate in TMAH; the etch rate for silicon dioxide in TMAH varies with the quality of the film, but is generally on the order of 0.1 nm/minute.[7]


The tetramethylammonium ion [9] affects nerves and muscles, causing difficulties in breathing, muscular paralysis and possibly death.[10] It is structurally related to acetylcholine, an important neurotransmitter at both the neuromuscular junction and autonomic ganglia. This structural similarity is reflected in its mechanism of toxicity - it binds to and activates the nicotinic acetylcholine receptors, although they may become densensitized in the continued presence of the agonist. The action of tetramethylammonium is most pronounced in autonomic ganglia, and so tetramethylammonium is traditionally classed as a ganglion-stimulant drug.[11] The ganglionic effects may contribute to the deaths that have followed accidental industrial exposure, although the "chemical burns" induced by this strong base are also severe. There is evidence that poisoning can occur through skin-contact with concentrated solutions of TMAH.[12]

A more detailed discussion of the pharmacology and toxicology of tetramethylammonium ion may be found in the Wikipedia entry for Tetramethylammonium.

See also[edit]


  1. ^ http://othes.univie.ac.at/15008/1/2011-06-10_0500634.pdf
  2. ^ a b c d Sigma-Aldrich Co., Tetramethylammonium hydroxide pentahydrate. Retrieved on 2015-04-06.
  3. ^ Walker, J.; Johnston, J. (1905). "Tetramethylammonium hydroxide". J. Chem. Soc., Trans 87: 955–961. doi:10.1039/ct9058700955. 
  4. ^ a b Lawson, A. T.; Collie, N. (1888). "The action of heat on the salts of tetramethylammonium". J. Chem. Soc., Trans 53: 1888. 
  5. ^ Markowitz, M. M. (1957). "A convenient method for preparation of quaternary ammonium salts". J. Org. Chem. 22: 983–984. doi:10.1021/jo01359a605. 
  6. ^ Stewart, R.; O'Donnell, J. P. (1964). "Strongly basic systems: III.The H_ function for various solvent systems". Can. J. Chem. 42: 1681–1693. doi:10.1139/v64-251. 
  7. ^ a b Thong, J. T. L.; Choi, W. K.; Chong, C. W. (1997). "TMAH etching of silicon and the interaction of etching parameters". Sensors and Actuators A: Physical 63: 243–249. doi:10.1016/S0924-4247(97)80511-0. 
  8. ^ Shadkami, F.; Helleur, R. (2010). "Recent applications in analytical thermochemolysis". J. Anal. Appl. Pyrol 89: 2–16. doi:10.1016/j.jaap.2010.05.007. 
  9. ^ Note that studies of the pharmacology and toxicology of TMA have typically been carried out using TMA halide salts - the hydroxide ion in TMAH is too destructive towards biological tissue.
  10. ^ Anthoni, U.; Bohlin, L.; Larsen, C.; Nielsen, P.; Nielsen, N. H.; Christophersen, C. (1989). "Tetramine: Occurrence in marine organisms and pharmacology". Toxicon 27: 707–716. doi:10.1016/0041-0101(89)90037-8. 
  11. ^ Bowman, W.C. and Rand, M.J. (1980), "Peripheral Autonomic Cholinergic Mechanisms", in Textbook of Pharmacology 2nd Ed., Blackwell Scientific, Oxford 10.21
  12. ^ Lin, C.C.; et al. (2010). "Tetramethylammonium hydroxide poisoning". Clin. Toxicol. (Phila) 48: 213–217.