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My time in university labs always brought a sense of connection with chemical pioneers, and the story of P-Bromoaniline Fluoroacetate ties right into this tradition of curiosity, trial, and risk. Chemists in the early and mid-20th century busily explored functional groups, testing the boundaries of aromatic amines and halogen substitution. Electro-rich aromatic rings caught the eye of industrial researchers seeking out ways to deliver fine-tuned reactivity. The introduction of a bromine atom to the para position on aniline, followed by grafting on a fluoroacetate moiety, unlocked new chemical spaces. Not simply a step in synthetic methods, but a bold entry into the chemical literature, raising eyebrows about bioactivity, safety, and reactivity. Debates rose around structure-activity relationships as toxicologists, agrochemists, and pharmaceutical scientists each saw a different promise or peril in this molecule.
Looking past the textbook entries, P-Bromoaniline Fluoroacetate stands as a sharp example of how structure shapes fate in chemicals. This compound offers more than a set of atoms; it’s a tool in the hands of anyone working with acylating agents, aromatic intermediates, and toxicological probes. Combining the electron-withdrawing power of bromine and the metabolic tripwire of the fluoroacetate unit, it ends up being both useful and risky. Chemical suppliers don’t tend to push bulk sales, often handling it with meticulous controls and limited production batches. Its role in research outpaces its use in day-to-day manufacturing, a contrast to bulk chemicals like ethanol or acetone.
Anyone who has held a vial of P-Bromoaniline Fluoroacetate would recognize it as an off-white crystalline solid, sometimes appearing faintly yellow depending on purity and storage. Its molecular heft sits at the intersection of halogenated aromatics and erases any hope of volatility common to lighter amines. Slightly soluble in organic solvents like DCM and acetonitrile, it resists easy movement in water, reducing some environmental mobility but not eliminating hazard. A melting point typically stretches above standard room temperature, evidence of the molecular rigidity and strong intermolecular forces granted by aryl bromine. Chemical stability holds up under dark, cool storage—but the story changes fast with exposure to bases, acids, or strong nucleophiles. The molecule’s construction means the aniline nitrogen is more hindered, and the fluoroacetate portion brings reactivity similar to classical haloacetates, including susceptibility to nucleophilic displacement and hydrolysis, often releasing fluoride—a point not lost on toxicologists.
Reagents like this one rarely leave the lab without a thick sheaf of paperwork. Proper labeling includes signal words such as "danger" and hazard pictograms marking it as both an acute toxin and environmental hazard. Purity typically runs above 98%, with residual aniline, bromide, and fluoroacetate carefully screened by suppliers using GC-MS or HPLC analysis. Packaging demands amber glass to block UV, sealed with PTFE liners, and outer containment to prevent accidental contact. The Safety Data Sheets read like a checklist for nasty possibilities: acute toxicity, chronic exposure risk, and strong warnings about skin and respiratory protection. It only takes a brief session with this molecule to understand why personal protective equipment isn’t a choice but a necessity—double gloving and fume hoods are the standard, with spill kits ready for rapid response in case of accidental drop or splash.
Anyone interested in synthetic chemistry eventually hears stories about multi-stage, multi-solvent reactions. P-Bromoaniline Fluoroacetate starts with selective bromination of aniline using molecular bromine or NBS (N-bromosuccinimide) to tip the balance toward the para isomer, a classic example found in undergraduate organic labs. After purification—usually by crystallization or column chromatography—the next step typically involves fluoroacetyl chloride acting on the free amine in an inert solvent under basic conditions, such as pyridine or triethylamine. The key, as every hand-on chemist learns quickly, is controlling moisture and temperature to avoid side product formation and dangerous releases of hydrogen fluoride. Once the reaction runs to completion, careful washing, repeated recrystallization, and structured drying steps take the intermediate and deliver the target compound. Each stage holds its own hazards, but the fluoroacetylation step earns special respect.
This compound offers a reactive nitrogen, though sterics and electronics slow simple alkylation or acylation. I’ve watched research groups add additional substituents to the aromatic ring, sometimes via palladium-catalyzed couplings or directed ortho lithiation, expanding the utility for custom probe design or radioisotope labeling. Hydrolysis under harsh base tears apart the ester, releasing fluoroacetate—a mechanism that has drawn the eye of both poison researchers and drug designers seeking “suicide” inhibitors. Reductive reactions cleave the aryl bromide under palladium catalysis, opening up new possibilities for downstream functionalization. Modification on the aniline or fluoroacetate side continues to intrigue, whether for forensics, metabolic labeling, or bioactivity studies.
Researchers and suppliers tag this molecule with more than one name. The systematic IUPAC name points clearly: 4-Bromoaniline fluoroacetate. Trade and catalog names sometimes stick with para-Bromoaniline fluoroacetate, 4-Bromo-phenylamino fluoroacetate, or simply PBAFA. Lab books may abbreviate further for speed, though cross-referencing with CAS numbers remains the most reliable way to avoid dangerous mix-ups, especially in tightly regulated labs or shipments.
Workplace safety policies for P-Bromoaniline Fluoroacetate reflect years of hard-learned lessons from chemical accidents and near-misses. Direct contact triggers severe skin and mucous membrane irritation. Inhalation can tip users into acute toxic shock due to the metabolic liberation of fluoroacetate, which disrupts the mitochondrial citric acid cycle and can lead to heart and neurological symptoms. Environmental release spells disaster for wildlife, especially mammals sensitive to fluoroacetate. Laboratories working with this compound keep exposure times short, personal monitoring robust, and emergency antidotes such as acetate and ethanol ready. Chemical hygiene plans require real-time inventory logs, restricted access storage, and clear plans for waste collection and incineration. The level of respect demanded by this molecule surpasses most other aniline derivatives, earning some facilities the reputation of having “red zones” reserved for high-toxicity work.
In the real world, P-Bromoaniline Fluoroacetate escapes the boundaries of academic curiosity and moves into niche applications. Research chemists use it as a building block for fluorinated pharmaceuticals, sometimes for cancer therapy, antiparasitic leads, or enzyme inhibitors where suicide inactivation offers a strategic advantage. Some agrochemical developers have tested it as a lead scaffold before shifting to less hazardous analogs. Biochemists studying metabolic blocking or mitochondrial sabotage find it useful for simulating poisoning or tracking metabolic fate in test systems. It doubles as a reference for environmental fate and transport studies, mapping the flow of fluorinated toxins through soils or biota. On the patent side, it has pitched its tent among designer molecules for diagnostics and metabolite probes, though regulatory hurdles often limit its advance toward mass-market application.
My years with multidisciplinary research teams taught me the difficulty of safe innovation with high-toxicity tools. Academic labs typically push for new uses of P-Bromoaniline Fluoroacetate in medicinal or synthetic chemistry, often chasing selectivity in enzyme targeting or developing new scaffolding for fluorine introduction. R&D departments in larger companies track structure-activity relationships based on the molecule’s dual halogen content. Fluorine’s unique bioisosterism and the metabolic trap set by fluoroacetate attract medicinal chemists, who monitor old stories of toxicity alongside new ideas about dosing, delivery, and metabolic shielding. Ongoing efforts focus on analogs that retain positive reactivity while dialing down the danger. Computational modeling teams work shoulder-to-shoulder with bench chemists trying to predict both reactivity and toxicity, hoping to carve out space for safe innovation. Contract research organizations see periodic demand for the compound, especially in pharmacokinetic and environmental fate studies required by regulatory authorities worldwide.
The dangers of this compound register high, with fluoroacetate-related toxicity ranking among the harshest known to mammalian systems. Acute poisoning fundamentally disrupts the Krebs cycle, slamming energy production with a metabolic block that affects every organ but especially the heart and brain. Animal model studies show rapid onset of symptoms—seizure, respiratory failure, and cardiac arrest. Antidotal therapy battles against the clock; glycolate and acetate compounds, sometimes used in high-dose regimens, work only if given early, and even then survival rates can be alarmingly low. Chronic low-dose exposure remains a blind spot in scientific understanding. Some researchers worry about accumulation and subtle long-term impacts on mitochondrial health. The compound’s regulatory profile pushes for special hazard status nearly everywhere, with strict transport and use restrictions in Europe, North America, and Australia. Investigators comb through case reports and environmental incidents, seeking data that links exposure with non-lethal outcomes, offering pointers for future antidote design or safer molecular analogs.
The future for P-Bromoaniline Fluoroacetate probably won’t see broad industrial application, not with its current risk profile. Researchers expect more derivatives and analogs to emerge, each offering tweaks in toxicity, metabolic fate, or target selectivity that could move the needle on risk-benefit analysis. Medical research eyes use as a diagnostic challenge agent or targeted therapeutic in tightly controlled settings, especially as knowledge about controlled-release forms and in-body detoxification expands. Calls grow louder for more intelligent molecular design—harnessing the benefits of the fluoroacetate group with better off-switches in the molecule, enabling selective action with rapid neutralization in non-target tissues. Environmental chemists hope for new tools to track and neutralize any residues, especially in water-rich or agriculture-heavy regions. Training, real-time monitoring, and chemical literacy remain at the front line, not just protecting lab staff but reassuring communities living near advanced research and production centers.
P-Bromoaniline fluoroacetate doesn’t make headlines, though it plays an often-overlooked role in scientific circles. Chemically speaking, it pairs a modified aniline ring with a potent fluoroacetate group. The combination sparks the curiosity of chemists for good reason. By tweaking molecules like this, researchers can develop building blocks for all sorts of laboratory work. My own time helping set up undergrad organic chemistry experiments gave me a real sense for how these reagents shape bigger discoveries.
The main action for p-bromoaniline fluoroacetate happens inside research labs. Small tweaks to molecular structures can make or break a reaction. This compound steps in for synthetic research, often as a test piece in the development of new pharmaceuticals or advanced materials. By using the bromine and fluoroacetate groups, chemists can probe reaction mechanics or generate tiny amounts of new candidate molecules. It’s this sort of behind-the-scenes work that eventually fills pharmacy shelves or changes how engineers design polymers.
A few years back, I talked with a friend who runs custom synthesis at a biotech startup. Compounds like this were staples in his glassware. They’re not the heroes seen on packaging but instead sit in quietly labeled bottles, supporting everything from testing enzyme activity to creating drug intermediates. Without chemical intermediates like p-bromoaniline fluoroacetate, the pace of pharmaceutical progress would slow to a crawl.
There’s an important catch: fluoroacetates don’t come without danger. As a class, they have a history of serious toxicity. Years ago, sodium fluoroacetate found infamy as a rodent poison. That history drives strict regulation higher across the supply chain. Researchers receive careful training on personal protection and disposal, and hazmat teams treat spills with the utmost seriousness. I’ve gone through hazmat training myself, and the lessons stick—you respect anything labeled ‘fluoroacetate.’
Many compounds in the lab demand similar caution, but fluoroacetates raise the stakes. Their ability to disrupt metabolic pathways in living organisms means that missteps can have grave consequences. Awareness and education protect both the scientists and the communities around manufacturing sites.
Today, green chemistry trends are shaping how researchers handle hazardous chemicals. There’s a push to develop alternatives or refine protocols for older compounds like p-bromoaniline fluoroacetate. My experience in university labs saw a new generation of synthetic routes emerge, cutting down on toxic reagents and hazardous waste. Regulatory frameworks have tightened up, requiring detailed hazard communication and better chemical tracking from shipment to storage.
Institutions partner up for information sharing, so incidents get analyzed and protocols improve. Industry groups foster responsible purchasing and disposal, reducing risk for lab workers and communities. A more transparent, collaborative approach in academia and industry helps keep progress moving while protecting health and the environment.
Chemicals like p-bromoaniline fluoroacetate may fly under the radar for most people, but they matter to anyone who cares about safer medicines, better materials, or even pollution control. Better education for scientists, strong protective measures, and smarter chemical design all add up. My hope is that a more informed public conversation about these compounds fuels support for research, regulation, and innovation that keeps everyone safe.
P-Bromoaniline fluoroacetate shows up in labs where folks tinker with pharmaceuticals, agrochemicals, and a handful of specialty polymers. It’s a reactive compound, and not one to take lightly, especially with both a bromine and a fluoroacetate group in play. Now, fluoroacetate brings an outsized risk since it can gum up key cellular processes in the human body. Even small exposures cause real harm—think nervous system, heart, and respiratory trouble. In lab work, respect pays off.
Personal experience taught me early on: gloves alone never cut it. Nitrile gloves guard against accidental skin contact, but protection needs layers. Safety goggles and splash-resistant face shields form a reliable outfit. Good lab coat, long pants, and closed shoes finish the job. Every chemical leaves its mark differently—fluoroacetate compounds call for vigilance.
Never open a bottle inside a cramped space. Every time I set up to weigh, transfer, or dilute this compound, I use a certified chemical fume hood. Respirable dust or vapors? It takes only a whiff to send things south. The right local exhaust system handles those risks.
I once watched a minor powder spill go wrong because one of us tried to sweep without wetting it first—airborne dust everywhere. For fluoroacetate compounds, that’s a gamble nobody needs. If a spill happens, soak absorbent pads in water before wiping. Use tools, not bare hands. Double-bag everything and label it sharp. Everyone present should know the emergency drill by heart.
In a shared lab fridge, segregate this kind of reagent. I use sealed, chemical-resistant containers and never stack P-Bromoaniline fluoroacetate beside strong acids or bases; you risk a nasty reaction. I label containers with date, chemical name, and hazard class big enough for anyone to spot with nervous eyes.
Temperature and humidity take their toll on chemical stability. I keep a log of storage dates, and a dry box or desiccator gives peace of mind, especially in humid climates.
Waste handling means double-checking every label and container. Specialized incineration should be the target for disposal, not your ordinary lab trash. Unused or expired compounds wait in a locked cabinet, and disposal schedules stay firm—no holdovers. Lab members get proper training, and I push for refreshers every six months. One slip turns a safe lab into a tragedy.
Trust never grows from shortcuts. Each member must show up for glove and goggle fitting, hood training, and chemical-specific safety classes. I keep printed safety data sheets in plain sight and run hands-on drills more than just once a year. Mistakes shrink when everyone feels good about asking questions and flagging risks.
This stuff won’t forgive mistakes. Diligence in protective gear, engineered controls like hoods, and swift spill response let you focus on the science, not the worry. I’ve seen labs where these habits get second nature, and not once have they regretted the extra step.
Local, state, and federal guidelines shape most routines, and following that roadmap makes life easier all around. If new folks join, show them the ropes. That commitment to doing things right makes the difference, every time.
P-Bromoaniline fluoroacetate brings together two recognizable chemical groups. Picture a benzene ring with an amino group attached to one end and a bromine atom placed on the opposite side—this forms p-bromoaniline. Then, tack on a fluoroacetate group, which comes from fluoroacetic acid. In the molecule, the basic structure of p-bromoaniline contains an aromatic ring carrying a bromine atom at the para position and an amino group at the other para position. The fluoroacetate segment, as the name suggests, latches on through a classic ester or salt linkage, depending on the preparation.
The full name really just means: para-bromoaniline meets fluoroacetic acid, creating an ester. Drawing it out, you’d see a benzene ring, NH2 group, Br atom, and then a two-carbon chain with a fluorine and an ester bond. Not something you bump into at the grocery store, but each piece plays a big role in organic chemistry and pharmaceutical design.
A molecule like p-bromoaniline fluoroacetate feels more than just theoretical. Researchers choose it if they want to explore the effects of electronegative substituents on molecular reactivity, or to screen for new biologically active compounds. Chemists working with these chemicals keep a careful eye on the safety sheets. The fluoroacetate part isn’t something to treat lightly—it’s related to compounds known for their toxicity. Proper handling methods matter a great deal, including ventilation, gloves, and protective eyewear.
What really draws attention is how substituents on the benzene ring shake up electron density and bonding patterns. Adding a bromo or an amino group doesn’t just swap out a hydrogen atom—it changes how the molecule reacts with acids and bases, how it partners with other reagents, and even how it fits into more complex molecules built for medicine or industry.
Getting the structure right is what lets researchers predict how chemicals will behave. P-bromoaniline adds bulk and electron-drawing power, and the amino group makes it flexible for coupling or other synthetic steps. The fluoroacetate chain adds polarity and introduces the element of fluorine, a feature that can boost metabolic stability or biological activity in new molecules. Pharmaceutically, tweaks at these positions can lead to major differences in absorption, distribution, and interaction with enzymes or receptors in the body.
From my own lab years, every time a molecule came in with a new halogen or amino group, there was a bit of anticipation—and caution. Labs running syntheses on derivatives of aniline often compare modifications by their reactivity, color, and sometimes by their smell if protocols required mouth pipetting (not a safe practice, but it happened in the older days). Safety data gets triple-checked because working with fluoroacetate-related compounds asks for respect, not shortcuts.
Handling structures like p-bromoaniline fluoroacetate safely and smartly starts with training and clear safety protocols. Many universities and research companies regularly update their safety manuals and run workshops so everyone understands the latest best practices. It helps to keep up with literature updates, since advances in chemical analysis or detoxification might come from the corner of the world you hadn’t thought of.
For people pushing forward in synthesis or drug discovery, sharing safety insights and detailed procedures with the community goes a long way. Not every bright student walks into a lab knowing what p-bromoaniline fluoroacetate can do—or how dangerous a spill could get. By fostering habits of caution, publication transparency, and open collaboration, researchers reduce risk and set the ground for genuine insight. Chemical structure isn’t just a drawing; it’s a story about potential and responsibility.
Drawing from my own days working in research labs, attention to detail has always proved more than just helpful. A single oversight can snowball into much bigger problems, especially if you’re dealing with compounds like P-Bromoaniline fluoroacetate. Hearing stories of bottles melting or labels smudging, and seeing peers rush to correct careless storage errors, really drove home that safety isn’t just a rulebook—it's the difference between routine research and emergency procedures.
P-Bromoaniline fluoroacetate doesn’t play nice with moisture or direct sunlight. Exposure to the wrong conditions means higher chances of decomposition, and breakdown can leave lab techs with toxic fumes or dangerous by-products. If anyone doubts the seriousness, reports of exposure incidents should be enough to send them searching for storage guidelines. This isn’t fear-mongering—it’s basic self-protection, both for health and for the integrity of research data.
Researchers, suppliers, and safety experts agree on the basics for handling compounds like this. Store the chemical in airtight, clearly labeled containers. Glass with a proper sealing cap works better than plastic for many hazardous organics, especially when you want to avoid reaction with the container. Labels shouldn’t fade—regular checks keep staff updated on chemical identity and expiry dates, which aren’t just bureaucratic details.
Temperature matters. Consistent, cool storage—usually between 2 to 8°C—slows down rate of decay and minimizes risk of dangerous reactions. Fume hoods don’t only protect during experiments; keeping volatile materials close to ventilation during transfer or inspection stops accidental inhalation.
Dryness proves essential. Any moisture let in through a poorly-sealed cap or careless decanting can trigger unwanted hydrolysis, sending lab workers scrambling. Silica gel or activated alumina in storage cabinets acts as extra insurance by keeping humidity down.
Reading the label never tells the whole story. In-person training fills in the gaps, especially if the team includes students or interns without strong chemistry backgrounds. Mock drills for spills or exposures, with real instructions and step-by-step clean-up, turn safety protocols from abstract concepts into muscle memory.
I’ve seen lab managers make checklists covering inspection, labeling, and temperature logging. While some roll their eyes, daily habits like these guard against the kind of surprises no one wants. Morning routines—open the storage fridge, check condensation, look for leaks—take two minutes but can save lives.
Getting the right equipment always beats improvising. Investing in ventilated chemical storage cabinets, clear signage, and regular audits doesn’t just comply with regulations—it makes the workplace less stressful. Funding rarely stretches far, so the best labs pool resources or press suppliers for better packaging.
Encouraging teams to speak up about shortages or problems means mistakes surface before they turn dangerous. I’ve found that when staff know they won’t be blamed for asking “dumb” questions, overall awareness spikes. Trust and education always work together to create safer environments for everyone.
Looking out for high-risk chemicals like P-Bromoaniline fluoroacetate brings responsibility. Staying alert, learning from small lapses, and keeping chemical storage solid isn’t just good science—it’s real care for colleagues and for yourself or anyone who works in the same space.
P-Bromoaniline fluoroacetate rarely makes headlines, but it carries dangers that go beyond lab walls. Growing up near a chemical plant taught me early about the difference between chemicals on paper and the risk they carry in real life. With P-Bromoaniline fluoroacetate, the story feels familiar: new chemistry, not enough attention to safety.
Acute toxicity tops the list with this compound. Its structure holds the keys to trouble, combining a halogenated aniline with a fluoroacetate. Fluoroacetates already raise concern from past poisonings—think about tragedies from small-town pest control gone wrong, where trace exposure left communities shaken. This chemical can slip into the same toxic pathway. Once inside the body, it interferes with energy production at the cellular level, blocking the Krebs cycle. Organs starved for energy often turn south quickly, ending with organ failure if exposure climbs too high.
Skin contact brings its own problems. Chemical burns, blisters, and deep tissue irritation come fast. Breathing in dust can trigger burning in the lungs, coughing, and constricted airways. Someone getting careless without proper gloves or masks could find themselves facing a medical emergency before they realize what hit them.
Repeated exposure sets up a dangerous slow march. P-Bromoaniline derivatives are suspected to contribute to genetic mutations and disrupt enzymes. Workers handling this chemical day in and day out face higher risks of chronic disease. Some effects creep in quietly: fatigue, confusion, nerve problems. Studies following exposed populations link chemicals in this family to increased rates of certain cancers. Too often, companies only take action after clusters of illness appear, and prevention comes too late.
Every health hazard listed above circles back to one problem I've seen everywhere: lack of respect for proper safety protocols. Hazard communication plans sometimes gather dust in binders. Personal protective equipment sits unused in cabinets. I remember a friend who worked at a facility with lax standards, where gloves tore often and no one stopped to clean spills immediately. It took an accident and a hospital trip to get management’s attention.
Engineering controls form the backbone of real safety here. Good ventilation, closed-system transfers, and thorough barrier protection—these become non-negotiable, not optional. Safety isn't just a training requirement; it molds culture. Companies that build safety into every shift cut down on incidents and health scares.
Medical surveillance brings issues to light before they spiral. Blood and urine tests, regular check-ins, and independent monitoring all work to catch low-level exposure. Health records need careful attention so patterns don’t get lost in the shuffle.
Transparent research remains vital. Universities and private labs need clear funding for studying long-term effects, not just acute poisoning. Regulators, industry, and workers should keep communication lines open. Advocacy organizations can press for limits, labeling, and public reporting of spills or incidents. Families living close to production or disposal sites deserve access to this information, too. Sharing knowledge and learning from chemical history stands as the surest way to avoid adding new chapters to a well-known story of neglect and regret.
| Names | |
| Preferred IUPAC name | 4-bromoaniline;2-fluoroacetate |
| Other names |
p-Bromoanilinium fluoroacetate 4-Bromoaniline fluoroacetate |
| Pronunciation | /ˌpiːˈbroʊmoʊˈænɪliːn flʊəroʊˈæsɪteɪt/ |
| Identifiers | |
| CAS Number | 403-39-0 |
| Beilstein Reference | 353938 |
| ChEBI | CHEBI:132731 |
| ChEMBL | CHEMBL3918223 |
| ChemSpider | 26469844 |
| DrugBank | DB08647 |
| ECHA InfoCard | ECHA InfoCard: 100.036.706 |
| EC Number | EC 239-202-5 |
| Gmelin Reference | 8920 |
| KEGG | C19014 |
| MeSH | Fluoroacetates; Aniline Compounds; Bromobenzenes |
| PubChem CID | 21633068 |
| RTECS number | CY8400000 |
| UNII | F8Z3V7V099 |
| UN number | UN3432 |
| CompTox Dashboard (EPA) | DTXSID70863427 |
| Properties | |
| Chemical formula | C8H7BrFNO2 |
| Molar mass | 265.050 |
| Appearance | White to off-white solid |
| Odor | Odorless |
| Density | 1.7 g/cm³ |
| Solubility in water | Insoluble in water |
| log P | 1.7 |
| Acidity (pKa) | pKa = 4.6 |
| Basicity (pKb) | 8.8 |
| Magnetic susceptibility (χ) | -64.5 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.594 |
| Dipole moment | 2.89 D |
| Thermochemistry | |
| Std enthalpy of combustion (ΔcH⦵298) | Std enthalpy of combustion (ΔcH⦵298) of P-Bromoaniline Fluoroacetate: **"-4932 kJ·mol⁻¹"** |
| Hazards | |
| Main hazards | Toxic if swallowed, causes skin and eye irritation, may cause respiratory irritation. |
| GHS labelling | GHS02, GHS06 |
| Pictograms | GHS06,GHS08 |
| Signal word | Danger |
| Hazard statements | H301 + H311 + H331: Toxic if swallowed, in contact with skin or if inhaled. |
| Precautionary statements | P260, P264, P270, P271, P301+P310, P302+P352, P304+P340, P311, P330, P361, P363, P405, P501 |
| NFPA 704 (fire diamond) | 2-3-2 |
| Lethal dose or concentration | LD50 oral rat 13 mg/kg |
| LD50 (median dose) | LD50 (median dose): 19 mg/kg |
| NIOSH | Not Listed |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 mg/m3 |
| IDLH (Immediate danger) | IDLH not established |
| Related compounds | |
| Related compounds |
P-Bromoaniline Fluoroacetic acid Aniline Bromoacetic acid Fluoroaniline |
