Bromoform

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Bromoform
Skeletal formula of bromoform
Stereo, skeletal formula of bromoform with the explicit hydrogen added
Spacefill model of bromoform
Names
IUPAC name
Tribromomethane[2]
Other names
Identifiers
75-25-2 YesY
Abbreviations
1731048
ChEBI CHEBI:38682 YesY
ChEMBL ChEMBL345248 YesY
ChemSpider 13838404 YesY
DrugBank DB03054 YesY
EC Number 200-854-6
49500
Jmol 3D model Interactive image
KEGG C14707 YesY
MeSH bromoform
PubChem 5558
RTECS number PB5600000
UNII TUT9J99IMU YesY
UN number 2515
  • InChI=1S/CHBr3/c2-1(3)4/h1H YesY
    Key: DIKBFYAXUHHXCS-UHFFFAOYSA-N YesY
  • BrC(Br)Br
Properties
CHBr3
Molar mass 252.73 g·mol−1
Appearance Colorless liquid
Density 2.89 g mL−1
Melting point −4 to 16 °C; 25 to 61 °F; 269 to 289 K
Boiling point 147 to 151 °C; 296 to 304 °F; 420 to 424 K
3.2 g L−1 (at 30 °C)
log P 2.435
Vapor pressure 670 Pa (at 20.0 °C)
17 μmol Pa−1 kg−1
Acidity (pKa) 13.7
1.595
Thermochemistry
130.5 J K−1 mol−1
6.1–12.7 kJ mol−1
−549.1–−542.5 kJ mol−1
Vapor pressure {{{value}}}
Related compounds
Related alkanes
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
YesY verify (what is YesYN ?)
Infobox references

Bromoform (CHBr3) is a brominated organic solvent, pale yellow liquid at room temperature, with a high refractive index, very high density, and sweet odor is similar to that of chloroform. It is a trihalomethane, and is one of the four haloforms, the others being fluoroform, chloroform, and iodoform. Bromoform can be prepared by the haloform reaction using acetone and sodium hypobromite, by the electrolysis of potassium bromide in ethanol, or by treating chloroform with aluminum bromide. Currently its main use is as a laboratory reagent.

A bottle of bromoform with some in the adjacent beaker

Uses

Only small quantities of bromoform are currently produced industrially in the United States. In the past, it was used as a solvent, sedative and flame retardant, but now it is mainly used as a laboratory reagent, for example as an extraction solvent.

Bromoform's high density makes it useful for separation of minerals by density. When two samples are mixed with bromoform and then allowed to settle, the top layer will contain minerals lighter than bromoform, and the bottom layer will contains heavier minerals. Slightly less dense minerals can be separated in the same way by mixing the bromoform with a small amount of a less dense and fully miscible solvent.

Environment and Toxicology

Natural production of bromoform by phytoplankton and seaweeds in the ocean is thought to be its predominant source in the environment.[3] However, locally significant amounts of bromoform enter the environment formed as disinfection byproducts known as trihalomethanes when chlorine is added to drinking water to kill bacteria. It is somewhat soluble in water and readily evaporates into the air. Bromoform is the main trihalomethane produced in salt swimming pools with some public swimming pools found to contain up to 1.3 ppm (parts per million) bromoform.[4] Occupational skin exposure limits are set at 0.5 ppm.[5]

The substance may be hazardous to the environment, and special attention should be given to aquatic organisms. Its volatility and environmental persistence makes bromoform's release, either as liquid or vapor, strongly inadvisable.

Bromoform can be absorbed into the body by inhalation and through the skin. The substance is irritating to the respiratory tract, the eyes, and the skin, and may cause effects on the central nervous system and liver, resulting in impaired functions. It is soluble in about 800 parts water and is miscible with alcohol, benzene, chloroform, ether, petroleum ether, acetone, and oils. Its LD50 is 7.2 mmol/kg in mice, or 1.8g/kg. Bromoform is a confirmed animal carcinogen; (ACGIH 2004). Carcinogen category: 3B; (DFG 2004).

References

  • Lua error in package.lua at line 80: module 'strict' not found. PDF
  • U.S. Department of Health and Human Services. Toxicological Profile for Bromoform and Dibromochloromethane [1]. August 2005.
  1. ↑ 1.0 1.1 Cite error: Invalid <ref> tag; no text was provided for refs named PGCH
  2. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  3. ↑ Palmer C J and Reason C J (2009), Relationships of surface bromoform concentrations with mixed layer depth and salinity in the tropical oceans (2009), Global Biogeochemical Cycles, 23, GB2014.
  4. ↑ Beech AJ et al (1980) Nitrates, Chlorates and Trihalomethanes in Swimming Pool Water. Am J Public Health, 70(1), 79-82
  5. ↑ CDC - NIOSH Pocket Guide to Chemical Hazards

External links

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