Thioacetic acid
Organosulfur compound (CH3C(O)SH) From Wikipedia, the free encyclopedia
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]
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| Names | |||
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| Preferred IUPAC name
Ethanethioic S-acid[1] | |||
| Other names
Thioacetic S-acid Thiolacetic acid | |||
| Identifiers | |||
3D model (JSmol) |
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| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.007.331 | ||
| KEGG | |||
PubChem CID |
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| UNII | |||
CompTox Dashboard (EPA) |
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| 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 | |||
Refractive index (nD) |
1.465 | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards |
May cause severe skin and eye burns. Highly flammable liquid. | ||
| GHS labelling: | |||
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| 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): | |||
LD50 (median dose) |
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).
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Synthesis and properties
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
Summarize
Perspective
Acidity
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
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
Reductive acetylation
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 from 4-nitrophenol or 4-nitroanisole.[10]
References
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