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Thioacetic acid
Skeletal formula of thioacetic acid
Ball-and-stick model of the thioacetic acid molecule
Names
Preferred IUPAC name
Ethanethioic S-acid[1]
Other names
Thioacetic S-acid
Thiolacetic acid
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.007.331 Edit this at Wikidata
KEGG
UNII
  • InChI=1S/C2H4OS/c1-2(3)4/h1H3,(H,3,4) checkY
    Key: DUYAAUVXQSMXQP-UHFFFAOYSA-N checkY
  • InChI=1/C2H4OS/c1-2(3)4/h1H3,(H,3,4)
    Key: DUYAAUVXQSMXQP-UHFFFAOYAO
  • O=C(S)C
Properties
CH3C(O)SH
Molar mass 76.11756 g/mol
Appearance Transparent, colorless to light yellow liquid[2][3]
Odor Unpleasant, strong thiol-like
Density 1.08 g/mL
Melting point −58 °C (−72 °F; 215 K)
Boiling point 93 °C (199 °F; 366 K)
−38.4·10−6 cm3/mol
1.465
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Severe skin burns and eye damage. Highly flammable.
GHS labelling:
GHS02: FlammableGHS05: CorrosiveGHS06: ToxicGHS07: Exclamation mark
Danger
H225, H301, H302, H314, H317
P210, P233, P240, P241, P242, P243, P260, P261, P264, P264+P265, P270, P272, P280, P301+P316, P301+P317, P301+P330+P331, P302+P352, P302+P361+P354, P303+P361+P353, P304+P340, P305+P354+P338, P316, P317, P321, P330, P333+P317, P362+P364, P363, P370+P378, P403+P235, P405, P501
Lethal dose or concentration (LD, LC):
75 mg/kg (mouse, intraperitoneal)
Safety data sheet (SDS) Fischer Scientific
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Thioacetic acid is an organosulfur compound with the molecular formula CH3C(O)SH. It is a thioic acid: the sulfur analogue of acetic acid (CH3C(O)OH), as implied by the thio- prefix. It is a yellow liquid with a strong thiol-like odor. It is used in organic synthesis for the introduction of thiol groups (−SH) in molecules.[4]

Synthesis and properties[edit]

Thioacetic acid is prepared by the reaction of acetic anhydride with hydrogen sulfide:[5]

(CH3C(O))2O + H2S → CH3C(O)SH + CH3C(O)OH

It has also been produced by the action of phosphorus pentasulfide on glacial acetic acid, followed by distillation.[6]

CH3C(O)OH + P2S5 → CH3C(O)SH + P2OS4

Thioacetic acid is typically contaminated by acetic acid.

The compound exists exclusively as the thiol tautomer, consistent with the strength of the C=O double bond. Reflecting the influence of hydrogen-bonding, the boiling point (93 °C) and melting points are 20 and 75 K lower than those for acetic acid.

Reactivity[edit]

Acidity[edit]

With a pKa near 3.4, thioacetic acid is about 15 times more acidic than acetic acid.[7] The conjugate base is thioacetate:

CH3C(O)SH → CH3C(O)S− + H+

In neutral water, thioacetic acid is fully ionized.

Reactivity of thioacetate[edit]

Most of the reactivity of thioacetic acid arises from the conjugate base, thioacetate. Salts of this anion, e.g. potassium thioacetate, are used to generate thioacetate esters.[8] Thioacetate esters undergo hydrolysis to give thiols. A typical method for preparing a thiol from an alkyl halide using thioacetic acid proceeds in four discrete steps, some of which can be conducted sequentially in the same flask:

CH3C(O)SH + NaOH → CH3C(O)SNa + H2O
CH3C(O)SNa + RX → CH3C(O)SR + NaX, where X = Cl, Br, I
CH3C(O)SR + 2 NaOH → CH3CO2Na + RSNa + H2O
RSNa + HCl → RSH + NaCl

In an application that illustrates the use of its radical behavior, thioacetic acid is used with AIBN in a free radical mediated nucleophilic addition to an exocyclic alkene forming a thioester:[9]

thioacetic acid application
thioacetic acid application

Reductive acetylation[edit]

Salts of thioacetic acid such as potassium thioacetate can be used convert nitroarenes to aryl acetamides in one step. This is particularly useful in the preparation of pharmaceuticals, e.g., paracetamol.[10]

References[edit]

  1. ^ International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. p. 97. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
  2. ^ "Thioacetic acid".
  3. ^ https://www.sigmaaldrich.com/GB/en/sds/aldrich/t30805
  4. ^ Jeannie R. Phillips "Thiolacetic Acid" Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley. doi:10.1002/047084289X.rt096
  5. ^ Ellingboe, E. K. (1951). "Thiolacetic acid". Organic Syntheses. 31: 105. doi:10.15227/orgsyn.031.0105.
  6. ^ Schiff, Robert (1895-08-09). "Preparation of Thioacetic Acid and its Importance for Chemical-Legal Investigations". Chemical News and Journal of Industrial Science. 72: 64. Retrieved 2016-11-02.
  7. ^ Matthys J. Janssen "Carboxylic Acids and Esters" in PATAI'S Chemistry of Functional Groups: Carboxylic Acids and Esters, Saul Patai, Ed. pp. 705–764, 1969. doi:10.1002/9780470771099.ch15
  8. ^ Ervithayasuporn, V. (2011). "Synthesis and Characterization of Octakis(3-propyl ethanethioate)octasilsesquioxane". Organometallics. 30 (17): 4475–4478. doi:10.1021/om200477a.
  9. ^ Synthesis of methyl 6-deoxy-4-O-(sodium sulfonato)-α-L-talopyranoside, its C-4 epimer and both isosteric [4-C-(potassium sulfonatomethyl)] derivatives László Lázár, Magdolna Csávás, Anikó Borbás, Gyöngyi Gyémánt, and András Lipták Arkivoc 2004 (vii) 196-207 Link
  10. ^ Bhattacharya, Apurba; et al. (2006). "One-step reductive amidation of nitro arenes: application in the synthesis of Acetaminophen" (PDF). Tetrahedron Letters. 47: 1861–1864. doi:10.1016/j.tetlet.2005.09.196. Archived from the original (PDF) on 2016-11-04. Retrieved 2016-11-02.
source: https://en.wikipedia.org/wiki/Thioacetic_acid

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