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Trifluoroacetic anhydride, often called TFAA, surfaced on the radar of organic chemists as labs scrambled for more effective reagents during the rapid growth of synthetic chemistry in the mid-20th century. Its roots trace back to the expansion of fluorine chemistry, a period driven by the search for stable yet reactive compounds for industry and research. Handling fluorinated chemicals, honestly, brings its own set of hurdles, but TFAA found a place because it outperforms many agents where strong acylating power and resistance to hydrolysis matter. My own first memories with TFAA live in a cramped university lab, watching the white fumes snake out of the flask—both intimidating and impressive. The compound has not just stuck around; its role in synthesis, especially in pharmaceuticals and advanced materials, has only deepened over the years.
TFAA stands out for its tough, almost abrasive character. The sharp biting smell, the volatility, and the rapid reaction rate—it’s a tool built for speed and strength in the right hands. You don’t reach for this chemical unless you want something done fast and thoroughly. Its uses span acylation, dehydration, and at times, tweaking complex molecules that standard agents just stumble over. Not everything goes right with TFAA. Handling errors and misuse crop up regularly, forcing chemists to stay sharp and grounded in their technique. Yet, this edge is what keeps it at the forefront for research, custom synthesis, and pilot-scale industry processes. It sometimes feels like TFAA runs with a crowd of dangerous friends—ethers, strong acids, and other aggressive reagents—yet, it delivers results many others can’t touch.
Trifluoroacetic anhydride arrives as a colorless, highly corrosive liquid, often hiding under a ghostly mist. It boils at a modest temperature, below the threshold of a gentle simmer, and attacks skin, eyes, and metals with alarming intent. The strong odor announces its presence even before you spot the bottle. Chemically, TFAA exerts strong electrophilicity. Its reactivity, owed to three electron-starving fluorine atoms, lends it the kind of power necessary to slice through resistant sites on challenging substrates. Still, that same potency tears through gloves and glassware more lightweight than borosilicate. Small spills drill into benchtops and give off choking vapors—hard lessons I’ll never forget. This is not a reagent you leave uncapped or work with outside well-ventilated hoods.
Handling TFAA means wrestling with precision. Purity almost always hits pharmaceutical or analytical benchmarks—often above 99%—because stray acids or peroxides become real problems during synthesis. Its labeling relies on globally recognized symbol warnings, including corrosive, toxic, and environmental hazard icons. Experts in compliance keep an eye on storage requirements, reminding everyone that even tiny leaks cause big headaches. Packing regulations underline danger; specialized bottles with PTFE-lined caps block slow vapor escape. No one in my experience treats the arrival of a TFAA shipment lazily, and everyone double-checks secondary containment. Mistakes in labeling or tracking, in this world, are invitations for disaster.
Lab-scale batches usually build TFAA from trifluoroacetic acid, stripping out water by using strong dehydrating agents. Large-scale operations leverage proprietary processes and tighter controls, but the fundamentals don’t shift—demand for dryness, inert atmospheres, and close monitoring of temperature. In synthesis, even brief contact with moisture triggers hydrolysis and a cloud of acid fumes. In fact, entire chapters of synthetic chemistry textbooks carve out space for troubleshooting failed dehydrations or incomplete conversions. In my time handling lab prep, we simply learned to treat every surface as suspect—any speck of water ruined yield, and no amount of wishful thinking restored product lost to ambient humidity.
Most talk about TFAA centers around its acylating hunger—no functional group escapes its reach if you let your guard down. TFAA cleans up carboxylic acids into their anhydrides, caps alcohols and amines, and carries out O- and N-acetylations for tricky substrates. Sometimes, chemists use it to set up staged reactions, activating molecules in ways milder agents can’t manage in a reasonable timeframe. TFAA also pulls downwater in dehydration and cyclization strategies, fostering environments for ring closures, rearrangements, and even the build-out of specialty fluorinated intermediates. Newer fields, such as chemical biology, see researchers adopting TFAA for site-specific modifications, targeting known liabilities in peptide or protein chains. These advances ride on the backs of experts who master the balance between reactivity and control—TFAA can scorch or finesse, depending on the skill applied.
In most books and catalogs, TFAA picks up several aliases. Chemists call it by systematic names—trifluoroacetic anhydride most formal, but also perfluoroacetic anhydride or di(trifluoroacetyl) oxide. Top-tier suppliers occasionally market it under unique trade names, but in practice, TFAA or trifluoroacetic anhydride dominate conversations across academic and industrial settings. No matter the label, the hazards and power stay constant.
With every bottle of TFAA, risk shadows the workspace. Liquid splashes burn through nitrile gloves. Vapors cut at eyes and lungs. One slip and a safety shower becomes your best friend. It’s not just hyperbole—the documented cases of severe skin and airway damage pepper the literature and safety archives. Safety data demand full-face respirators if concentrations rise or if ventilation wavers. Firefighters and first responders train to recognize leaks, planning with the knowledge that water makes things worse in a spill. Labs keep antidote stations and copious calcium gluconate or specialized neutralizers within arm’s reach, and evacuation maps always factor in worst-case scenarios for volatile fluorinated agents. Regulatory authorities, from OSHA to European chemicals agencies, set strict exposure limits. In my circles, two sets of eyes review every risk assessment, and even experienced chemists call for a buddy system during larger-scale transfers. The hidden cost of lax standards carries long tails—lost time, injuries, and sometimes legal action.
TFAA won its spot in pharmaceuticals by opening synthetic doors others left closed. The precision it delivers lets chemists manufacture key intermediates for anti-cancer therapeutics, antivirals, and central nervous system drugs. Modern agrochemical discovery also leans on TFAA, using it to forge bond types in specialty herbicides or insecticides that wouldn’t hold together under rougher treatment. High-value dyes and specialty coatings trace their origins to reactions powered by TFAA, where fine control over fluorination means more weatherproof and lightfast products. Research labs and contract synthesis partners—especially those in fast-moving biotech and med-chem—keep it around for those moments where a milder process just can’t compete. Looking at the range of patents over the last decade, TFAA makes frequent appearances for building blocks in drug discovery, often used in chiral synthesis or for modifying pivotal structural motifs. Wherever chemists walk the tightrope of reactivity and selectivity, TFAA’s reputation precedes it.
TFAA stimulates ongoing research into safer, greener, and more reliable synthesis. Today’s questions dig at ways to quench side reactions or scavenge byproducts before they turn nasty. Some labs push for catalyst systems that moderate TFAA’s temper, dialing in reactivity to match the fragility of modern drug candidates. It’s rare to see a new graduate student jump into TFAA work without extra coaching—the hazards, combined with the opportunity for breakthroughs, draw seasoned researchers to mentor closely. Companies chase improved containment, automated handling, and even micro-scale reactors that limit batch size and exposure. Instrumentation specialists develop sensor tech to spot traces of TFAA in air, aiming for early detection pathways. Imagine the relief in a lab knowing escape of fumes triggers an instant shutdown rather than relying on human noses.
The dark side of TFAA’s strength lies in its acute toxicity. Inhalation, skin contact, and ingestion all trigger aggressive tissue damage, sometimes leading to systemic toxicity that demands inpatient care. Medical journals and toxicology databases document not just acute burns, but also longer-term effects on lung tissue and metabolic pathways. Research over the last ten years points to TFAA interfering with proteins and membranes at the cellular level. Environmental scientists continue to track its fate after accidental release—its acids persist in water and resist breakdown, posing threats to aquatic life and downstream users. Toxicity research funds aim to illuminate these gaps, with regulatory bodies adjusting safety thresholds as new data emerge. Labs use active monitoring and sometimes restrict TFAA access to researchers with advanced training. Even minor exposure often lands colleagues in the health center for a checkup, and no one shrugs off symptoms like chest tightness or eye irritation in the aftermath.
TFAA’s story seems bound up with the future of sustainable and high-precision chemistry. Green chemistry drives a search for reusable reagents, safer substitutes, and recycling schemes—questions not always answered by the current generation of aggressive anhydrides. Process engineers look to continuous-flow systems or solid-supported acylation agents to cut down on waste and exposure. Investments into predictive modeling hope to minimize TFAA use, allowing chemists to preview reaction landscapes before stepping foot in the lab. Regulations will likely tighten as toxicity research deepens and as environmental advocates press for more transparency about fluorinated waste. Yet, unless a rival chemical matches both reactivity and control, TFAA will remain in demand for a slice of the most demanding synthesis work. I see a future where laboratories strike a new balance—harnessing TFAA’s unique strengths, but only with more robust infrastructure and training than in past decades. Anyone betting against its continued presence in toolkits is ignoring just how persistent problems are in science, and how rare truly universal solutions become.
Most folks outside of the chemistry world never see a bottle labeled Trifluoroacetic Anhydride (TFAA). In research settings, TFAA shows up as a critical tool for scientists working on tough transformations. TFAA lands on the bench when chemists want to make better medicines, improve crop protection, or even upgrade materials for everyday products.
From my own academic days, I remember glassware lined up with strange acronyms — TFAA usually marked the start of something big. In medication discovery, chemists rely on TFAA to tweak the structure of molecules. They use the chemical to introduce a trifluoroacetyl group, which can change the way a drug performs in the body. That little tweak often boosts a compound’s stability, or makes it less likely to break down before reaching its target. Without this step, promising new treatments for things like cancer or infection would often stall in the lab.
If you eat bread, drink orange juice, or hoping your tomato plants survive the summer, crop protection matters to you. TFAA steps up again — not to spray on crops, but to help chemists create new herbicides and insecticides. When a pesticide molecule lasts just long enough in the field, it protects crops but doesn’t stick around to hurt the environment. TFAA enables safer, more selective production of these molecules, so farmers can use less chemical while still fighting off weeds or bugs.
TFAA reaches beyond medicine and farming. Electronics, batteries, and special plastics sometimes require fluorinated building blocks. TFAA joins other chemicals to build molecules that survive harsh conditions, such as high heat or caustic cleaning cycles. Some lab coats, non-stick cookware, and smartphone screens owe their resilience to chemicals born through reactions using TFAA.
Safety calls for constant vigilance in any lab setting. TFAA brings unique hazards—its fumes hurt eyes and lungs, and it reacts fiercely with water. Every chemist I’ve known respects TFAA, suiting up with goggles and gloves and working only under the fume hood. Over the years, a few close calls in academic and industrial labs have underscored the need for good training and reliable safety gear, not just policies on paper.
Even small-scale use raises eyebrows in the sustainability conversation. The story around fluorinated chemicals keeps growing: some are tough to break down, showing up in water, air, and wildlife. Research teams worldwide scramble for new ways to recover, treat, or substitute for these chemicals. Green chemistry prizes innovation, so teams have started exploring TFAA replacements that don’t carry long-term risks, and improved recycling methods that reduce chemical waste.
A lot rides on getting the right tools in the right hands. The debate over TFAA isn’t about ignoring science’s progress — it’s about thinking straight: can we keep pushing toward safer, smarter discovery, without sacrificing public health or our planet? Many in the field believe the answer lies in ongoing education, investments in green chemistry, and a dose of honest, open conversation between scientists and the wider public.
TFAA, or Trifluoroacetic anhydride, brings some real challenges to the table. It’s not just another bottle on the shelf. Keeping workers, labs, and the environment safe means knowing exactly what you’re working with. TFAA reacts with water, releases heat, and doesn’t play nicely with skin, eyes, or lungs. It can trigger fires if it contacts moisture or combustibles. Anyone handling it should respect those risks every step of the way.
From experience, nobody likes a surprise leak or fire in the lab. Once, a poorly stored acid caused a midnight evacuation—lost research, ruined samples, a panicked scramble. These events stick with you and shape your views on why safety isn’t just another box to tick.
Keeping TFAA safe starts with the right container. Only corrosion-resistant bottles, usually glass or PTFE-lined, shut tight with secure caps, keep the chemical contained. Forget about storing it near water sources; leaks and spills can lead to nasty chemical reactions.
A properly ventilated storage cabinet makes a real difference. Chemical storage cabinets, marked for corrosive or reactive substances, reduce the risk of vapor buildup. Flammable cabinets help if fire might break out, but remember, TFAA produces corrosive fumes as well as a fire hazard. Secure each container upright to cut the chance of spills. Store far from loose papers, wood, or organic chemicals—TFAA chews through more than most realize.
Preparation beats panic. Chemical-resistant gloves and splash goggles are a must. Don’t trust thin nitrile or vinyl gloves—these break down. Neoprene or butyl gloves stop TFAA from working its way through. Lab coats and closed-toe shoes create another line of defense. I’ve watched new staff realize, after just one spill, why sturdy shoes matter: that stuff eats through sneakers fast.
Fume hoods aren’t just for show. They clear vapors before anyone can breathe them in. Work outside a fume hood and someone’s throat burns, chest tightens, or eyes water within minutes. TFAA mixers need training before the first job: not just a safety briefing, but hands-on practice with cleanup kits and eye-wash stations.
Even great labs face accidents. Having calcium carbonate or sodium bicarbonate handy helps neutralize spills. Neutralization should go slowly—TFAA reacts fast and hot. Never send TFAA residue down the sink; designated hazardous waste lines are the rule, not the exception. I once saw improper disposal lead to a blocked drain and a surprise acid bath for the custodial team. Good planning avoids horror stories.
Any accident should launch a response. Everybody, even visitors, deserves clear routes to eyewash stations and safety showers. Quick reaction keeps minor emergencies from turning into ER visits. Training isn’t a one-off event—refreshers keep everyone sharp.
Labs that treat TFAA with a routine, checklist-driven approach see fewer accidents and keep staff healthy. Experienced chemists know there’s no shortcut—it’s about habits, training, and respect for the bottle on the shelf. Firms should push for audits and invest in ongoing education. Spending money on better cabinets, gloves, and training proves cheaper than coping with medical bills or shutdowns. Anyone working with energetic chemicals learns quickly: one mistake can erase years of research in minutes.
A lot of folks in the lab world recognize trifluoroacetic anhydride by its abbreviation, TFAA. The compound answers to the CAS number 407-25-0 and carries the molecular formula C4F6O3. That numbering system, managed by the Chemical Abstracts Service, makes it possible for anyone to check a database and instantly find technical details—no matter what local name a chemist uses. I remember searching for information on strange reagents in grad school, and having reliable reference numbers saved hours in the stockroom.
TFAA shows up in lots of labs—synthetic chemists reach for it during acylation reactions, especially when they need a strong, reactive agent. Its strong electron-withdrawing trifluoromethyl groups help drive tough reactions to completion. More than once, I’ve seen TFAA used to prepare acid anhydrides or introduce trifluoroacetyl groups, especially for pharmaceuticals and advanced materials. The speed of certain syntheses sometimes hangs entirely on such a reagent.
While textbooks might list all sorts of details, seeing TFAA in action on the bench gives you real respect for its punch. Tap some into a reaction, and it wakes up even sluggish nucleophiles. It's possible to work with alternatives, but few deliver quite the same punch or consistency across different scenarios. That reliability makes a difference in research and manufacturing.
Lab safety officers always remind their teams that trifluoroacetic anhydride falls in the category of corrosive and moisture-sensitive chemicals. It reacts sharply with water or basic materials. The vapor can be rough on eyes and lungs, so fume hoods aren’t optional here. Nobody wants to learn that lesson the hard way. Proper labeling, storage in tightly sealed containers, and quick clean-up after spills lower the odds of a lab day derailing due to one missed step.
Environmental concerns come up often today. Waste containing TFAA needs attention—never down the drain, always captured for approved chemical disposal. Regrettably, some stories still surface about improper disposal leading to lasting environmental harm. That’s why accredited labs stick to protocols, respecting both air quality and water supplies.
TFAA’s streamlined molecular structure makes it a tool of choice in creative organic chemistry and process development. Its reactivity speeds up research, but only teams who handle it knowingly see full benefit without risk. Supporting staff with strong training keeps accidents low and businesses competitive.
Long-term, some researchers search for “greener” alternatives with similar efficiency but lower hazard profiles. That drive pushes the field forward. Industry groups, academic labs, and even hobbyists now share their experience more freely, offering tips on containment and neutralization. Regulations on chemical use and reporting keep tightening—and that raises the bar for everyone, including suppliers, producers, and chemists in the field.
As someone who’s spent years coaxing stubborn molecules into place, I see TFAA as a prime example of how chemical knowledge, attention to detail, and real-world discipline work together. The CAS number 407-25-0 and the formula C4F6O3 help everyone stay on the same page, no matter where they work. The best outcomes come from skill, curiosity, and respect for guidelines—traits the next generation of scientists should keep close at hand.
Trifluoroacetic anhydride, or TFAA, is popular among chemists for making certain reactions work faster or cleaner. Many labs lean on it for pharmaceutical research and other synthetic chemistry tasks. Anyone who has worked in a lab long enough knows tools like TFAA can speed things up, but they come with some serious risks. Let’s take a look at the real hazards and some measures that help keep workers from getting into trouble.
TFAA packs more punch than some realize. If you haven’t had TFAA on your skin before, count yourself lucky. Even a small spill burns right away. Eyes and lungs do not fare much better. The fumes dig deep and can trigger coughing or even choke you up if the ventilation stinks. Once it reacts with water, TFAA produces corrosive acids like trifluoroacetic acid, which can rip apart tissue or metal in a hurry.
In a closed room, those vapors run wild, settling into every open surface. Over months, even fume hood panels start corroding. I once heard of a worker in an older academic lab who forgot to clean up a tiny spill under a cluttered balance—one week later, the metal underneath had pitted straight through. That type of damage gets expensive, fast. For folks with asthma or other respiratory issues, exposure can land them in a doctor’s office for days.
Safety with TFAA starts with one rule: respect the bottle. Gloves are must-have gear here. Nitrile or neoprene gloves hold up longer than latex. These chemicals sneak through thin gloves in minutes, so it pays to check for chemical compatibility before starting work.
Lab coats and face shields add a second line of defense. Splash goggles should never leave the bench when opening the bottle. A labmate once ignored this and paid the price—a near miss with a splash cost him a week off for medical checks. You only get two eyes.
Ventilation can’t get overlooked. Fume hoods must stay on and undamaged. TFAA doesn’t let you cheat airflow; even the slightest whiff alerts you, but that’s already too late. Keep your face out of the sash and stop prepping reagents in open air.
Spills happen. A good lab posts instructions by the door and keeps spill kits nearby. Neutralizers, like sodium bicarbonate, help deal with small drops. Plenty of labs fall into the trap of forgetting clear evacuation routes, so regular drills matter just as much as fresh gloves. If fumes escape, get outside and pull the fire alarm. No experiment beats your health.
Trained staff pick fewer fights with TFAA. Routine training refreshers keep even old-timers on their toes. Chemical hygiene officers earn their pay by walking through the lab, double-checking everything from storage cabinets to eyewash stations.
Switching to less hazardous alternatives makes sense where possible. Progress in green chemistry methods, including newer, milder reagents, helps reduce lab risk. Still, where TFAA remains the best tool for the job, everyone deserves a culture where safety stands well above speed or convenience.
Plenty of people see glass vials and complicated labels and picture the magic of chemistry, but behind the scenes, every research bench has its fair share of hazardous leftovers. Trifluoroacetic anhydride stands out among these with its sharp odor and corrosive bite. Having spent more than a decade in chemical labs, I’ve watched newcomers freeze up at the idea of disposing of anything this intimidating. Truth is, the real danger lies not just in handling the chemical—improper disposal leaves scars on people, plumbing, and the environment.
I’ve met colleagues who learned the hard way that shortcuts in chemical waste disposal only shift problems elsewhere. Dumping trifluoroacetic anhydride down the drain, for example, won’t just leave a nasty stench; it unleashes a cascade of violent reactions. Water and trifluoroacetic anhydride do not play nice. The compound reacts strongly, releasing corrosive vapors like trifluoroacetic acid and hydrofluoric acid. No one wants to see a fume hood fogging up with dangerous mist or feel the metallic taste of acid in the air.
Rules surrounding hazardous waste sometimes feel like bureaucratic obstacles, but my own work with environmental officers hammered home the reasons behind them. Lawmakers didn’t plaster the RCRA (Resource Conservation and Recovery Act) on every lab wall for fun. Trifluoroacetic anhydride counts as hazardous waste under these rules. Untrained hands pouring this substance into regular trash or sinks can poison water, harm wildlife, and damage community health. Even accidental traces find their way into bigger problems downstream, like rivers carrying fluorinated residues straight to fish and crops.
Disposal isn’t a backroom chore for the unlucky. I’ve seen entire departments scramble after an accident involving improper disposal—scrubbing floors, calling hazmat, dealing with administrative penalties. The reality is that ignoring safe procedures drags everyone into the problem, not just those who handled the chemical in the first place.
Clear steps for getting rid of trifluoroacetic anhydride start with neutralization. In my own graduate lab days, we always contacted our chemical hygiene officer before even opening the waste bottle. Small volumes sometimes got neutralized with dilute sodium carbonate, added slowly in a dedicated fume hood with continuous monitoring. This keeps fumes in check. Most of the time, though, our solution meant sealing the waste in a proper polyethylene container, labeling everything down to the amount and concentration, then logging it for collection.
Commercial chemical waste handlers pick up most of this material. They pack it and either take it for incineration or for advanced treatment processes approved by state and federal authorities. It’s a relief knowing someone with the right expertise and equipment remains in charge beyond the lab doors.
Some labs still wing it or use outdated methods. That has to change. Better staff training, updated waste handling manuals, and open communication with environmental health departments make a difference. None of these changes cost a fortune, and they go a long way toward preventing incidents nobody wants to see on the news.
Committing to correct disposal isn’t about checking off boxes. It’s a mark of respect for fellow workers, the community, and the world outside the lab. That respect starts with each bottle, every spill kit kept close, and every trip to the waste locker made with care.
| Names | |
| Preferred IUPAC name | 3,3,3-Trifluoro-2,2-dihydroxypropanoic anhydride |
| Other names |
Trifluoroacetic anhydride TFAA Perfluoroacetic anhydride Trifluoroacetyl anhydride Trifluoroethanoic anhydride |
| Pronunciation | /traɪˌflʊə.roʊ.əˈsiː.tɪk ænˈhaɪ.draɪd/ |
| Identifiers | |
| CAS Number | 407-25-0 |
| 3D model (JSmol) | `3D model (JSmol) string` for **Trifluoroacetic Anhydride (TFAA)**: **C(OC(=O)C(F)(F)F)(=O)C(F)(F)F** This is the SMILES string that can be used in JSmol for its 3D model: ``` O=C(OC(=O)C(F)(F)F)C(F)(F)F ``` |
| Beilstein Reference | 391873 |
| ChEBI | CHEBI:53076 |
| ChEMBL | CHEMBL1223037 |
| ChemSpider | 9693 |
| DrugBank | DB14298 |
| ECHA InfoCard | 03a12a90-93e8-440e-9f9b-21df8e2032ff |
| EC Number | 207-995-7 |
| Gmelin Reference | 63112 |
| KEGG | C07812 |
| MeSH | Trifluoroacetic Anhydride |
| PubChem CID | 6604297 |
| RTECS number | YO7350000 |
| UNII | 86P217C2K1 |
| UN number | UN2624 |
| CompTox Dashboard (EPA) | DTXSID0020521 |
| Properties | |
| Chemical formula | C4F6O3 |
| Molar mass | 282.045 g/mol |
| Appearance | Colorless transparent liquid |
| Odor | Pungent |
| Density | 1.489 g/mL at 25 °C |
| Solubility in water | Reacts |
| log P | 0.98 |
| Vapor pressure | 8.3 hPa (20 °C) |
| Acidity (pKa) | 0.23 |
| Basicity (pKb) | 1.2 |
| Magnetic susceptibility (χ) | -36.3e-6 cm³/mol |
| Refractive index (nD) | 1.295 |
| Viscosity | 0.949 cP (25°C) |
| Dipole moment | 2.5317 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 354.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1466.8 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -1510.4 kJ·mol⁻¹ |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | H314: Causes severe skin burns and eye damage. H331: Toxic if inhaled. H290: May be corrosive to metals. |
| Precautionary statements | P280, P305+P351+P338, P310, P303+P361+P353, P304+P340, P405, P501 |
| NFPA 704 (fire diamond) | 3-3-2-W |
| Flash point | 5 °C |
| Autoignition temperature | 430°C |
| Lethal dose or concentration | LD50 Oral Rat 200 mg/kg |
| LD50 (median dose) | 'LD50 (median dose)': Oral, rat: 200 mg/kg |
| NIOSH | AJ1925000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 10 mg/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Trifluoroacetic acid Acetic anhydride Trifluoroacetamide Trichloroacetic anhydride Perfluorobutyric anhydride |
