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| Names | |||
|---|---|---|---|
| IUPAC name
trichloro(deuterio)methane[1] | |||
| Other names
Chloroform-d Deuterochloroform | |||
| Identifiers | |||
3D model (JSmol) |
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| 1697633 | |||
| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.011.585 | ||
| EC Number |
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PubChem CID |
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| UNII | |||
| UN number | 1888 | ||
CompTox Dashboard (EPA) |
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| Properties | |||
| CDCl3 | |||
| Molar mass | 120.384 g/mol | ||
| Appearance | Colorless liquid | ||
| Density | 1.500 g/cm3 | ||
| Melting point | −64 °C (−83 °F; 209 K) | ||
| Boiling point | 61 °C (142 °F; 334 K) | ||
| Hazards | |||
| GHS labelling: | |||
   | |||
| Danger | |||
| H302, H315, H319, H331, H336, H351, H361, H372, H373 | |||
| P201, P202, P260, P261, P264, P270, P271, P280, P281, P301+P312, P302+P352, P304+P340, P305+P351+P338, P308+P313, P311, P312, P314, P321, P330, P332+P313, P337+P313, P362, P403+P233, P405, P501 | |||
| NFPA 704 (fire diamond) | |||
| Related compounds | |||
Related compounds |
Chloroform | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references | |||
Deuterated chloroform, also known as chloroform-d, is the organic compound with the formula CDCl3 or C2HCl3. Deuterated chloroform is a common solvent used in NMR spectroscopy.[2] The properties of CDCl3 and ordinary CHCl3 (chloroform) are virtually identical.
Preparation
Deuterated chloroform is commercially available. It is more easily produced and less expensive than deuterated dichloromethane.[3] Deuterochloroform is produced by the reaction of hexachloroacetone with deuterium oxide, using pyridine as a catalyst. The large difference in boiling points between the starting material and product facilitate purification by distillation.[4][5]
- O=C(CCl3)2 + D2O → 2 CDCl3 + CO2
NMR solvent
In proton NMR spectroscopy, deuterated solvent (enriched to >99% deuterium) is typically used to avoid recording a large interfering signal or signals from the proton(s) (i.e., hydrogen-1) present in the solvent itself. If nondeuterated chloroform (containing a full equivalent of protium) were used as solvent, the solvent signal would almost certainly overwhelm and obscure any nearby analyte signals. In addition, modern instruments usually require the presence of deuterated solvent, as the field frequency is locked using the deuterium signal of the solvent to prevent frequency drift. Commercial chloroform-d does, however, still contain a small amount (0.2% or less) of non-deuterated chloroform; this results in a small singlet at 7.26 ppm, known as the residual solvent peak, which is frequently used as an internal chemical shift reference.
In carbon-13 NMR spectroscopy, the sole carbon in deuterated chloroform shows a triplet at a chemical shift of 77.16 ppm with the three peaks being about equal size, resulting from splitting by spin coupling to the attached spin-1 deuterium atom (CHCl3 has a chemical shift of 77.36 ppm).[3]
Deuterated chloroform is a general purpose NMR solvent, as it is not very chemically reactive and unlikely to exchange its deuterium with its solute,[6] and its low boiling point allows for easy sample recovery. It, however, it is incompatible with strongly basic, nucleophilic, or reducing analytes, including many organometallic compounds.
Hazards
Chloroform reacts photochemically with oxygen to form chlorine, phosgene and hydrogen chloride. To slow this process and reduce the acidity of the solvent, chloroform-d is stored in brown-tinted bottles, often over copper chips or silver foil as stabilizer. Instead of metals, a small amount of a neutralizing base like potassium carbonate may be added.[7] It is less toxic to the liver and kidneys than CHCl3 due to the presence of a C−D bond which is stronger than a C−H bond. The C−D bond is stronger than a C−H bond, making it somewhat less prone to form the destructive trichloromethyl radical (•CCl3).[8][9]
References
- ↑ "Chloroform-d".
- ↑ Fulmer, Gregory R.; Miller, Alexander J. M.; Sherden, Nathaniel H.; Gottlieb, Hugo E.; Nudelman, Abraham; Stoltz, Brian M.; Bercaw, John E.; Goldberg, Karen I. (2010). "NMR Chemical Shifts of Trace Impurities: Common Laboratory Solvents, Organics, and Gases in Deuterated Solvents Relevant to the Organometallic Chemist" (PDF). Organometallics. 29 (9): 2176–2179. doi:10.1021/om100106e.
- 1 2 "The Theory of NMR – Solvents for NMR spectroscopy". Archived from the original on 2016-03-03. Retrieved 2014-01-23.
- ↑ Paulsen, P. J.; Cooke, W. D. (1 September 1963). "Preparation of Deuterated Solvents for Nuclear Magnetic Resonance Spectrometry". Analytical Chemistry. 35 (10): 1560. doi:10.1021/ac60203a072.
- ↑ Zaharani, Lia; Johan, Mohd Rafie Bin; Khaligh, Nader Ghaffari (2022). "Cost and Energy Saving Process for the Laboratory-Scale Production of Chloroform-d". Organic Process Research & Development. 26 (11): 3126–3129. doi:10.1021/acs.oprd.2c00260. S2CID 253071632.
- ↑ Sabot, Cyrille; Kumar, Kanduluru Ananda; Antheaume, Cyril; Mioskowski, Charles (2007-06-01). "Triazabicyclodecene: An Effective Isotope Exchange Catalyst in CDCl3". The Journal of Organic Chemistry. 72 (13): 5001–5004. doi:10.1021/jo070307h. ISSN 0022-3263. PMID 17530896.
- ↑ Teipel, Jan; Gottstein, Vera; Hölzle, Eva; Kaltenbach, Katja; Lachenmeier, Dirk W.; Kuballa, Thomas (2022). "An Easy and Reliable Method for the Mitigation of Deuterated Chloroform Decomposition to Stabilise Susceptible NMR Samples". Chemistry. 4 (3): 776–785. doi:10.3390/chemistry4030055. ISSN 2624-8549.
- ↑ Goldstein, Robin S. (2013). Toxic interactions. Hewitt, William R., Hook, Jerry B. Burlington: Elsevier Science. ISBN 978-1-4832-6970-2. OCLC 896796140.
- ↑ Ahmadizadeh, M.; Kuo, C.‐H.; Hook, J.B. (1981-07-01). "Nephrotoxicity and hepatotoxicity of chloroform in mice: Effect of deuterium substitution". Journal of Toxicology and Environmental Health. 8 (1–2): 105–111. doi:10.1080/15287398109530054. ISSN 0098-4108. PMID 7328696.