Bromoform: A Deep-Dive into Its Evolution, Properties, and Promise
Historical Development
Curiosity about bromoform stretches back to the 19th century, when creative chemists like Justus von Liebig sought better ways to explore halogenated compounds. Early industrial research in Europe found bromoform during efforts to produce iodine-rich salts, due to its ties with bromine extraction. At that time, scientists used labor-intensive steam distillation and river water brimming with bromide ions as starting material. Over decades, as synthetic chemistry really took shape and the periodic table became mainstream, industry picked up bromoform for its role in density measurements and analytical methods. Today, most routes use cheaper and safer feedstocks, but researchers still see bromoform as a vital link to understanding halogen chemistry and as a cautionary example from the days when safety guidelines trailed innovation.
Product Overview
Bromoform stands out among simple halomethanes, packing three bromine atoms onto a methane backbone. Unlike its better-known cousin, chloroform, bromoform shows up less in pop culture but never lost its value in laboratories and certain niche industries. Produced both as a pure chemical and within complex mixtures—especially in older fire extinguishing fluids and some specialty solvents—it persists in the toolbox for density gradient separations. Bromoform's sharp odor, potent action, and deep color make it unmistakable, which helps in both handling safety and avoiding accidental misuse.
Physical & Chemical Properties
Drop bromoform onto a glass slide, and it forms dense droplets that sink in water. Weighing in at around 2.89 g/cm³ at room temperature, it offers more heft per milliliter than nearly every common organic liquid. Colorless to pale yellow, with a sweet yet almost medicinal scent, bromoform boils at 150.2°C and freezes near 8.3°C. It shows respectable solubility in ethanol, ether, and organic solvents but barely mixes with water. That density and non-miscibility made it a go-to liquid in mineral separation labs. Its molecular structure, CHBr₃, sets the stage for a cluster of chemical behaviors. Explosive reactions with strong bases, and its reactivity with metals like magnesium, demand careful storage—far from oxidants and open heat.
Technical Specifications & Labeling
Bromoform for analytical or industrial use usually comes with a minimum assay, often above 99%. Labels note molecular weight, boiling point, and a batch number for traceability. Reputable suppliers sway toward transparent labeling—clear hazard pictograms, GHS statements, and recommended storage temperatures populate each drum and bottle. Barcodes and QR links to security datasheets mean that any operator, from an off-site contractor to a plant chemist, can quickly check safe handling protocols. Everyone—regulatory inspectors, users, and even logistics staff—demands such rigorous specification in the modern era, after costly lessons from the past.
Preparation Method
The classic synthesis paths of bromoform involve the “haloform reaction” using acetone and elemental bromine in an alkaline aqueous medium. One pours sodium hypobromite into acetone, and the mixture gives off bromoform along with sodium acetate. This method offers both high yield and straightforward separation, since bromoform, being so heavy, settles out beneath the aqueous layer for easy collection. Industrial-scale operations favor safer bromine donors and automated controlled additions to contain risk and boost throughput. Innovations over the past fifty years simplified waste handling and air emissions, which echoes demands from both environmental watchdogs and cost-conscious manufacturers.
Chemical Reactions & Modifications
In the lab, bromoform opens doors for several transformations. Grignard-like additions, dehalogenations, and halide exchange reactions all work on bromoform’s heavily brominated carbon. Some enterprising researchers push it into the realm of organometallic chemistry, yielding intermediates for pharmaceutical building blocks and materials research. Industry rarely fiddles with bromoform itself for end-use, instead coveting its role as a reagent. It falls under scrutiny for its reactivity with strong bases, which can liberate bromide gas, an occupational hazard no modern plant manager takes lightly. Handling modifications demands exhaust hoods, real-time monitoring, and rigid PPE adherence, since slight missteps could expose workers to toxic vapors.
Synonyms & Product Names
Bromoform appears under a handful of aliases in trade catalogs and technical papers, notably tribromomethane, methyl tribromide, and Methenyl tribromide. Across various applications—from density separation to coolant research—these synonyms crop up in labeling, so barcode and data sheet harmonization has grown into a compliance headache. An old bottle in a university storeroom might hide under the name “bromoforme,” a reminder that international supply chains and language drift sow confusion unless procurement and safety teams educate themselves.
Safety & Operational Standards
Respect for bromoform’s toxicity and volatility runs deep through the chemical workforce. Short-term exposure irritates eyes, skin, and respiratory tracts, and chronic contact—especially with poor ventilation—amplifies risks of kidney and liver damage. Regulatory agencies like OSHA and NIOSH assign low workplace exposure limits, reflecting the decreased tolerance for occupational disease claims. Modern packaging emphasizes tamper-proof seals, child-resistant caps, and dual-walled drums, in part due to tighter import and export rules. Disposal guidelines continue to evolve, responding to evidence that bromoform lingers in aquatic environments and harms aquatic life. Training and regular safety drills form an everyday reality for users, who remember that just a few missteps invite regulatory action and personal harm.
Application Area
Bromoform has forged its reputation in density separation, especially within mineralogy and forensic science. Labs use it to float or sink rock and soil fragments, pinpointing mineral content that would confound less dense solvents. Environmental chemists once used it as a reference point when tracing halogenated compound pollution, teaching generations about anthropogenic chemical footprints. Beyond the lab, fire suppression foams explored mixtures containing bromoform, though modern safety and environmental rules axed most of those ideas. More recently, marine biologists track bromoform’s formation from algal blooms, triggering tighter scrutiny of its environmental transport and role as an atmospheric contaminant. Across these fields, bromoform serves less as a finished-product ingredient and more as a key tool for scientific investigation.
Research & Development
Current research around bromoform points in several directions. Synthetic organic chemists still use it to unlock new classes of reagents, mapping out routes to high-value pharmaceuticals and polymers. Analytical advances now track trace amounts in environmental samples, linking bromoform to changes in climate-related ocean chemistry and halogen cycling. R&D teams from green chemistry labs chase alternatives that match bromoform’s density properties without the same toxicity or environmental persistence. International partnerships push for improved wastewater treatment techniques, some using new catalysts or microbe-assisted breakdown to degrade halomethanes before they enter water bodies. Universities foster interdisciplinary projects, drawing in atmospheric scientists, toxicologists, and engineers to look at bromoform's wider impact and possible benign alternatives.
Toxicity Research
Toxicologists keep a critical eye on bromoform as research uncovers its links to health hazards. Animal studies link chronic exposure to heightened cancer risk, driving bromoform onto several watch lists, including the EPA’s roster of regulated drinking water disinfection by-products. The chemical’s lipophilicity means it can pass through cell membranes and accumulate in fatty tissue—a trait that caught the attention of occupational health professionals decades ago. The steady push for lower detection thresholds in environmental monitoring reveals that trace amounts wind up in groundwater near manufacturing facilities, and areas where bromoform-based fire suppressants spilled. Medical researchers keep close tabs on epidemiological studies, noting that communities around halomethane production plants sometimes report higher rates of certain cancers and organ dysfunction. Whether these levels translate directly into risk for the general population remains contentious, but nobody claims ignorance anymore.
Future Prospects
Looking ahead, the chemical industry faces tough questions about bromoform’s future. Stricter emissions standards and growing public scrutiny force a shift toward greener substitutes, whether for density separation, analytical standards, or even research reagents. The spotlight now falls on identifying alternatives that check all the same boxes as bromoform, while sidestepping the pitfalls of persistence and health concern. Investment pours into closed-loop manufacturing and new destruction technologies, so accidental releases drop dramatically. Meanwhile, demand for purity—driven by advances in nanotechnology and medical diagnostics—keeps interest in bromoform high among specialized researchers, so long as labs meet the standard for worker protection and waste handling. In my experience, change comes slow—few properties rival bromoform’s utility in mineralogy or halogen chemistry. Still, mounting regulatory pressure and ethical concerns about environmental and health legacy push everyone to contemplate life beyond halomethanes.
What Exactly is Bromoform?
Bromoform isn’t the sort of thing most people talk about at the dinner table, but it pops up in more places than you might think. Chemists know it as a clear, heavy liquid with a sweetish odor. Officially, its main use is as a laboratory reagent. In school, I remember it showing up in organic chemistry lessons. But its reach stretches far past textbooks.
Industrial Uses and Odd Jobs
Bromoform doesn’t act as a superstar in industry the way oil or copper do, but it has niche roles that matter if you look closely. Some folks use it to separate minerals due to its high density—drop a rock in a beaker of bromoform, and you can tell if it’ll float or sink, which helps sort minerals in geology labs. In old imaging and fire extinguisher fluid recipes, bromoform made quick appearances, but safer options later replaced it. You won’t find it in your old school fire alarms anymore, partly because scientists learned it could be risky for health and tricky for the environment.
Bromoform and Reducing Methane from Cows
These days, the chatter about bromoform is reaching farmers. Scientists noticed that certain seaweeds—like Asparagopsis—naturally contain this compound. If cows eat a pinch of this seaweed, the bromoform inside it interrupts how their stomachs produce methane. Methane matters. Every cow releases dizzying amounts of this potent greenhouse gas through burps. Methane traps heat in the atmosphere much more efficiently than carbon dioxide, so trimming it has become a climate fight with global stakes.
I grew up on a small dairy farm. We always joked about “cow burps icing the planet,” long before anyone worried about climate change. Now, solid numbers spell it out: Livestock methane makes up about 14% of total global greenhouse emissions. Feeding bromoform-rich seaweed is one experiment with real promise. Peer-reviewed studies published in journals like Nature and Scientific Reports show methane drops by up to 80% in cows fed just a sprinkle of the seaweed.
Health, Environment, and Common Sense
It’s easy to get wrapped up in the excitement, but bromoform has a dark side. High doses are toxic. Health agencies flag it as a hazardous material, requiring strict rules around handling. Drinking water can get contaminated if waste isn’t managed, and studies on rats have tied high bromoform exposure to liver and kidney troubles. Regulators keep a close eye to make sure new farm trials don’t slip into dangerous territory.
Balancing Innovation and Caution
So where does this leave us? Bromoform’s story shows how one substance can flip from niche chemical to headline solution. If scientists crack the recipe, seaweed supplements could reshape how farms tackle emissions—if everyone pays close attention to safety. Farmers I know want solutions that don’t threaten their animals or the land. Any rollout of new feed additives needs honest research, strong oversight, and updates as new studies emerge. Companies exploring this path should partner with independent researchers. Regular testing keeps everyone accountable, and transparent reporting brings trust into the process.
Moving Forward
Bromoform won’t become a household name, but its journey from obscure lab chemical to climate helper is worth watching. Tackling problems like methane requires blending practical experience with what’s proven in peer-reviewed journals. Innovations like seaweed feed show the best ideas often grow from understanding what’s already part of the natural world, supported by careful science and a fair amount of real-world patience.
What Is Bromoform and Where Does It Show Up?
Bromoform shows up as a heavy, colorless liquid used in research labs, sometimes in chemical synthesis or as a solvent. Some people have run across it in science class, others have seen it listed on chemical inventory sheets at work. Bromoform smells sweet, a lot like chloroform, and that’s the first warning that most folks ever get—it signals, “Don’t mess with me unless you know what you’re doing.”
Why Bromoform Raises Eyebrows
Open any material safety data sheet for bromoform and the red flags start flying. High concentrations in the air can irritate the eyes, skin, and lungs. People exposed to enough of it find themselves coughing, dizzy, or short of breath. Chronic exposure—think weeks or months, not just a brief whiff—has hurt livers, kidneys, and nervous systems in animal studies. The US National Toxicology Program puts bromoform in a class of substances “reasonably anticipated to be a human carcinogen.” Even short-term handling demands respect: gloves, goggles, and a fume hood are not negotiable.
My Own Experience
I spent a couple of years shuffling through graduate chemistry labs. All of us knew the bromoform bottle stood apart from less risky solvents such as ethanol. If you cracked the seal, you’d make sure you had nitrile gloves. The lab managers drilled it into us: don’t let this stuff get on your skin. No pipetting by mouth, no uncapped vials on open benches. I remember a careless spill and the sickly-sweet odor that filled the air—the group lead hit the emergency ventilators and got everyone to step outside. Even a small amount left everyone’s eyes watering.
What the Science Says
Peer-reviewed studies support what old chemistry instructors taught: bromoform absorbs through skin and can affect your health just from breathing its vapors. The Centers for Disease Control and Prevention warn about it, and the Environmental Protection Agency keeps checking drinking water for trace amounts. Lab tests in rodents show DNA changes after heavy exposure, though the evidence in people stays less clear, mostly because so few work directly with it. It takes real safety training to keep risk in check.
Problems in the Real World
Industry uses bromoform only for niche work these days, but risks don’t just stay in a research lab. Bromoform sometimes forms as a byproduct when chlorine meets bromide in water treatment plants. Some municipal water systems have found measurable levels, though the EPA regulates it under limits for total trihalomethanes. For most, running tap water isn’t a big concern, but workers at treatment plants or in some chemical factories see greater risk. These jobs call for good ventilation, personal protective equipment, and regular safety audits. Too often, companies skip steps to save money or time—one mistake can put workers in the hospital.
Smarter Approaches: Prevention Works Better Than Cleanup
Labs can substitute less-toxic solvents for many tasks. Where that’s impossible, investing in ventilated workstations and proper spill gear pays off. Training does more than just keep the regulators happy; it keeps people out of danger. Every safety culture—whether in a big plant or a tiny university lab—depends on people speaking up if shortcuts creep in. Management has to get serious about maintaining equipment, auditing their processes, and rotating staff so no one ends up overexposed.
Bromoform: Not for Amateurs
Given the known dangers, bromoform never belongs in home settings or in the hands of folks who haven’t handled hazardous chemicals before. It’s one of those substances that rewards careful respect, experience, and the right gear. Anyone working with it should know the risks, demand safe conditions, and refuse unsafe shortcuts. Handling bromoform safely starts with people who remember how much is at stake.
Understanding Bromoform
Bromoform may sound unfamiliar, but it’s not entirely out of reach for daily life. This heavy, colorless liquid forms during the chlorination of water, turning up in some swimming pools, tap water, and even certain manufacturing sites. The sharp, sweet smell hangs in the air when this chemical shows up, and behind that scent sits a set of health risks worth knowing about.
Health Risks That Come With Bromoform
My years working at a pool as a teenager meant long hours inhaling chlorinated air. Later, in college, I learned that the stuff irritating my nose and eyes came not just from chlorine, but also from byproducts — including bromoform. Most people experience it in tiny concentrations. Even so, those who work near treated water or industrial sites may run into higher doses.
Short-term contact with bromoform can lead to headaches, dizziness, fatigue, and an irritated throat or eyes. These symptoms often show up right after exposure, especially in places where ventilation misses the mark. Some swimmers mention skin rashes, a real annoyance after an afternoon in the pool. Animal studies used higher doses and saw more dangerous reactions: liver and kidney damage, irregular heart rhythms, even trouble breathing.
Long-term exposure raises bigger flags. Scientists studied workers in plants or people living close to heavily chlorinated water, and found links between ongoing bromoform contact and injury to the liver, kidneys, or central nervous system. The U.S. Environmental Protection Agency (EPA) ranks bromoform as a possible human carcinogen. That label means enough warning signals have piled up, especially from animal studies, even though proof in humans hasn’t closed the case. But it’s tough to ignore: cancer risk sits in the background for anyone who handles a lot of this substance.
Where Exposure Happens Most
Water treatment changes tap water worldwide. That process uses chlorine to kill harmful germs, but it also creates byproducts. Bromoform lands in drinking water, shower steam, pool air, and places where folks handle chemicals for work. Swimmers, cleaners, and plant workers face higher doses, but anyone can run into bromoform through everyday water use. Houses and apartments built near chemical plants or wells bring added risks. Families there might drink, bathe, and cook with water holding more than safe levels.
Keeping Yourself and Others Safe
The solution starts with solid basics. Filtering water with activated carbon strips out bromoform and related contaminants. Water treatment plants keep a close eye on bromoform levels, but testing at home helps, especially in neighborhoods with older pipes or frequent boil notices. Good pool management makes a difference. Better ventilation, regular water changes, and careful monitoring of chemical use all help keep air and water safer for swimmers and staff.
At work, wearing gloves, goggles, or masks and following safety rules shields employees from higher exposures. Companies must watch levels, train staff, and act fast at spill reports. For families near plants or water sources flagged for chemical spikes, bottled water or high-quality filtration can block daily intake.
Moving Toward Healthier Water
Public pressure keeps water quality on the radar for officials. Tougher standards for chemical byproducts, investments in plant modernization, and clear communication help people stay informed and safe. Our experience tells us that prevention outpaces cleanup every time — and with bromoform, a little knowledge and action lower the risk for all.
Storing Bromoform Safely Isn’t Just Regulation—It’s Common Sense
Bromoform stands out because of its unique, heavy liquid profile. It can look innocent in a bottle, but anyone who’s spent time in a lab knows a tiny spill lets off that sharp, sweet smell, followed by a feeling of worry. Over the years, cases of skin irritation and more serious symptoms from exposure have piled up in workplace safety records. Breathing in its fumes over time and even handling it without proper protection can leave a mark on health.
Lots of guides call for storage in cool, well-ventilated areas. That’s not just over-cautious advice. Chlorinated solvents like bromoform can break down under sunlight or heat, releasing gases and creating pressure inside containers. Storing it away from sunlight, in solid amber glass bottles with airtight lids, protects both people and the chemical integrity. A chemical safety cabinet with a clear hazard label on the front keeps things organized and cuts down on mix-ups. Long-sleeved lab coats, nitrile gloves, and protective eyewear become essential when handling the bottles—these steps grow out of real accidents where simple splashes have caused chemical burns or more complicated cases of organ damage.
Disposal: Beyond the Drain
Disposing of bromoform brings its own set of precautions. Dumping it down a drain means bad news for soil, water, and aquatic life. Bromoform ranks as a hazardous waste, and stories of contamination trace back to small lapses—an outdated bottle going to a landfill or a forgotten sink rinse in a school lab. Wastewater treatment systems aren’t built to handle complex organohalogen contaminants. Studies have linked bromoform in water sources to harmful effects on fish and other wildlife, and there’s enough data showing risks for humans, especially when it seeps into groundwater.
Segregating bromoform waste from other solvents is just as important as storing it correctly. Sealing it in compatible containers—preferably the original one if it’s still intact—means there’s less chance for chemical reactions. Absorbents and spill kits tackle small accidents, but for full containers, a registered hazardous waste handler should step in. Professional handlers use incineration at high temperatures to break down the compound into harmless forms before disposal, and this keeps harmful byproducts from drifting back into the environment.
Accountability Starts From the Bench
In real lab practice, keeping a detailed inventory, logging every use and disposal, limits confusion and accidental storage of forgotten bottles. Safety training doesn’t just check a box for regulations; it reaches the folks who step into the lab for the first time. Posters, digital reminders, and good communication build a culture where no one passes off the job of safe chemical management.
Institutions can invest in waste minimization programs—buying only what’s needed, sharing excess stock, and promoting micro-scale experiments. These efforts save money, reduce risks, and foster responsibility. Lab workers, environmental managers, waste contractors—all play a role in keeping bromoform’s hazards out of homes, rivers, and dinner plates.
In the end, knowledge and consistency shape safer handling of bromoform. Understanding the real, lived impacts of mishandling—from skin blisters to polluted water—grounds scientific curiosity in responsibility. There’s no shortcut to keeping people and the planet safer.
Getting Acquainted With Bromoform
Bromoform has a simple formula: CHBr3. Picture a methane molecule where three of the hydrogens have been swapped out for bromine atoms. What’s left is a dense, colorless liquid, carrying a distinct sweet odor that people compare to chloroform. Bromoform comes from the trihalomethane family and shares traits with its cousins, chloroform and iodoform. Its molecular weight checks in at about 252.73 g/mol, and in the lab, it’s known for its high density—almost two and a half times denser than water—so drops of it plummet to the bottom in a beaker of water.
A Closer Look at Physical and Chemical Properties
One of the standout features of bromoform is its impressive density, about 2.89 g/cm3. This makes it useful in mineralogy, especially when separating minerals by flotation. Its boiling point sits just below 151°C, while it freezes solid at around 8°C, which means it stays liquid at room temperature most places in the world. It’s only slightly soluble in water but mixes easily with a whole lineup of organic solvents—think alcohol, ether, and chloroform. I remember watching crystal-clear layers of bromoform drop through water back in chemistry class, leaving nothing behind but a slow-moving bubble at the bottom of a test tube.
Bromoform’s reactivity can turn into a problem, especially under light or in the presence of air and bases. It decomposes, releasing potentially harmful gases, including bromine and phosgene. In some water treatment plants, bromoform pops up as an uninvited guest—disinfection processes involving chlorine and organic debris can make trace amounts show up in tap water.
Health and Environmental Concerns
Studies tied bromoform to possible toxic effects in both people and animals. Exposure to high levels can knock out the nervous system or irritate the lungs and eyes. Professional experience drills in the risks—equipment and fume hoods remain non-negotiable during experiments. Long-term studies connect trihalomethanes, including bromoform, to cancer risks, though the dangers hinge on how much and how often someone gets exposed. Regulatory agencies such as the EPA set limits for allowable concentrations in drinking water, keeping the numbers well below levels believed to raise health alarms.
Because bromoform doesn’t break down quickly and sinks into sediments, it can affect fish and aquatic life. Scientists have seen evidence of buildup in certain aquatic organisms, which can ripple through the local food web. These impacts push environmental groups to call for improved monitoring and stricter limits on industrial sources.
Practical Uses and Shifting Perceptions
For decades, people leaned on bromoform in labs for density measurements and solvent applications. Mineralogists tossed samples into vials of bromoform to sort out minerals by how quickly they sank. Modern labs, though, increasingly turn to safer substitutes, recognizing the possible health risks tied to regular bromoform contact.
Since many of these dangers show up in the workplace or lab, simple safeguards go a long way—using gloves, keeping experiments sealed, and working under exhaust fans. Some companies look for greener extraction technologies or switch to agents that offer less risk without giving up performance.
Looking Beyond the Test Tube
Society can’t just flip a switch and replace legacy chemicals overnight, and bromoform’s story highlights that challenge. Science brings solid evidence about risks, and real progress grows from steady pressure to use less hazardous methods, build better water treatment, and shift towards more sustainable chemicals. Each step forward relies on sharing knowledge and keeping an eye on new research. Anyone handling bromoform sees these cautionary lessons in practice every day.
| Names | |
| Preferred IUPAC name | Tribromomethane |
| Other names |
Tribromomethane
Methyl tribromide Methenyl tribromide Bromoformum |
| Pronunciation | /ˈbrəʊməˌfɔːrm/ |
| Identifiers | |
| CAS Number | 75-25-2 |
| Beilstein Reference | 358755 |
| ChEBI | CHEBI:3136 |
| ChEMBL | CHEMBL1357 |
| ChemSpider | 529 |
| DrugBank | DB04291 |
| ECHA InfoCard | ECHA InfoCard: 100.001.077 |
| EC Number | 200-595-1 |
| Gmelin Reference | 622 |
| KEGG | C01880 |
| MeSH | D001975 |
| PubChem CID | 6218 |
| RTECS number | EK9275000 |
| UNII | 3X3CJK66Z5 |
| UN number | UN2515 |
| Properties | |
| Chemical formula | CHBr3 |
| Molar mass | 252.73 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | Sweetish odor |
| Density | 2.89 g/cm³ |
| Solubility in water | 3.1 g/L (20 °C) |
| log P | 2.38 |
| Vapor pressure | 5.5 mmHg (25 °C) |
| Acidity (pKa) | 0.8 |
| Basicity (pKb) | 8.68 |
| Magnetic susceptibility (χ) | −68.0×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.597 |
| Viscosity | 2.24 mPa·s (20 °C) |
| Dipole moment | 1.60 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 254.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -24.6 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -143.7 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | R05DB04 |
| Hazards | |
| Main hazards | Toxic if swallowed, in contact with skin or if inhaled. Causes skin irritation. Causes serious eye irritation. Suspected of causing cancer. |
| GHS labelling | GHS02, GHS06, GHS08 |
| Pictograms | GHS06,GHS08 |
| Signal word | Danger |
| Hazard statements | H302, H315, H319, H331, H351, H372, H410 |
| Precautionary statements | P261, P280, P301+P310, P302+P352, P304+P340, P305+P351+P338, P308+P313, P337+P313, P403+P233, P405, P501 |
| Flash point | Flash point: 93°C (199°F) |
| Autoignition temperature | 537°C |
| Explosive limits | Not found |
| Lethal dose or concentration | LD50 oral rat 1140 mg/kg |
| LD50 (median dose) | LD50 (median dose): 7.2 mg/kg (intravenous, mouse) |
| NIOSH | RN8400000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) of Bromoform is "5 ppm (40 mg/m3) |
| REL (Recommended) | 0.5 ppm |
| IDLH (Immediate danger) | 250 ppm |
| Related compounds | |
| Related compounds |
Chloroform
Fluoroform Iodoform Methanol |
