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4-Nitroaniline takes you on a chemical journey going back to the mid-19th century. Early chemists in Europe chased new synthetic dyes and stumbled across a compound with a distinct yellow hue. As industries grew, they learned that this chemical, with its nitro and amine groups positioned across from each other on a benzene ring, opened a door into both dyes and pharmaceuticals. I’ve seen how each stage in chemical history shapes industrial priorities. Companies first sought it for colorants, then dug deeper to find more nuanced uses. Each step revealed fresh hazards or opportunities, sometimes both at once, and the research community doggedly returned to 4-nitroaniline, appreciating its versatility and risks.
Anybody who’s worked in a chemical lab has likely gripped a bottle labeled 4-nitroaniline. This yellow, crystalline powder doesn’t carry the flash of some showier molecules, but don’t let its humble appearance fool you. The two key groups hanging off the benzene core – nitro at the fourth position and an amino at the first – make for a molecule poised between reactivity and utility. It’s more than a steppingstone towards more valuable chemicals; it’s a workhorse for chemists dogged by synthesis puzzles, dye makers bent on precision, and pharmaceutical scientists on the hunt for new scaffolds. The demand for 4-nitroaniline depends on industry health, research direction, and regulatory pressure, yet it sticks around as part of the backbone of organic synthesis.
Grains of 4-nitroaniline bring a touch of pale yellow, melting between 146 and 149 degrees Celsius. Its faint odour often gives away its presence among the solids in a storeroom. Water doesn’t take to it easily, yet you find it dissolves readily in organic solvents – a blessing for synthetic work. Stability at room temperature does not erase real risks: the compound can catch fire under the wrong conditions, and it breaks down into more toxic products if mishandled. Over the years, studies have shown its weak base properties come from the electron-withdrawing nitro group sapping the amine's donating strength. This effect matters in synthesis, because reactions sometimes stall or yield odd side-products unless you account for this influence. Reliable lab results depend on measuring out quantities accurately and knowing how temperature, light, and moisture affect every step.
Buy a bottle from any reputable supplier and you’ll see purity standards cranked above 98 percent. This kind of consistency doesn't come easily, and anyone in the lab values purity — contaminants ruin experiments and drive up costs. Labels warn of toxicity, carcinogenic potential, and flammability, plus pictograms imposed by bodies like OSHA or GHS. Reading these warnings slows you down, but people forget more accidents happen when folks ignore them out of routine or impatience. The paperwork and hazard statements matter as much as the compound itself since both protect workers from the slow creep of chemical exposure. Regulation changes from one territory to the next, so experts keep their eyes on updates to avoid landing in regulatory hot water.
Old-school chemists taught me the backbone method: start with acetanilide or aniline, douse with a nitrating mixture of concentrated nitric and sulfuric acids, and monitor the temperature religiously. Yields swing wildly if temperatures run away, so thermal control isn’t just a technical detail – it’s about not blowing up your workspace. Reaction monitoring and careful work-up, including neutralization and purification, set apart successful benchwork from messier outcomes. Over time, new variations cropped up, tweaking conditions to lower waste and improve yield, or moving away from strong acids to greener alternatives. In every case, working with nitroaromatics always feels like a balancing act. As green chemistry advances, process chemists keep searching for a route that slashes waste, saves energy, and reduces the whole operation’s environmental footprint.
4-Nitroaniline opens the door to many next-step transformations. Both the amino and nitro groups act as handles for reduction, substitution, or diazotization. Experienced chemists find that the nitro group resists reduction unless faced with a determined reagent or catalytic hydrogenation. Once reduced to a diamine, the product jumps into the dye industry or forms the core of pharmaceutical active ingredients. The amino group, less hindered than in other nitroanilines, supports direct acylation, sulfonation, or can serve as a hook for coupling reactions with diazonium salts. Techs running pilot plants spend hours fiddling with reaction parameters to coax selective chemistry, minimize side-products, and lower the cost per kilo.
University textbooks and supplier catalogs crisscross terms like para-nitroaniline, p-nitroaniline, and 4-nitrobenzenamine. While synonyms can clutter a datasheet, knowledge of these aliases matters if you’re digging through patents or ordering abroad. Miss a synonym and you can end up with the wrong grade, the wrong isomer, or the wrong safety documentation. Multilingual catalogs add to the confusion, so a sharp eye and a memory for historic trade names like 1-amino-4-nitrobenzene serve a chemist well.
A bottle of 4-nitroaniline won’t keep anyone up at night if protocols are respected. But let safety standards slide, and risks mount — not just acutely from inhalation or skin contact, but also from slow, cumulative exposures. Long hours stocking shelves and tipping powder into flasks remind you why good gloves, goggles, fume hoods, and regular training matter. I’ve seen the consequences of lapses: fingertip numbness, hospital trips, even surprise inspections that froze whole departments. The shift toward automated handling in factories cut direct worker exposure, but even small leaks or spills can trigger incident reports and expensive clean-ups. Groups like OSHA and European ECHA keep tightening the safety net around these chemicals, demanding better storage, clear training, and reliable emergency planning. Tight regulation frequently chafes end-users, but on balance, it protects people and communities from lasting harm.
4-Nitroaniline sits squarely in key sectors like dye manufacturing and pharmaceuticals. Its strongest draw comes from its role as an intermediate — a kind of gateway compound for getting to azo dyes, which splash color across everything from textiles to plastics. Medicinal chemistry leans on its backbone for creating analgesics and antipyretics. Some folks in agriculture point to its use in synthesizing pesticides and herbicides. Direct applications are rare since regulatory bodies frown on letting nitroanilines out in consumer goods, but its chemical descendants find their way into everyday products. Research settings praise its stability, but industrial settings value it for reproducible output and clear transformation opportunities. Legacy uses in photographic chemicals or rubber accelerants have faded as alternatives rose, but research laboratories and specialty industries keep it circulating worldwide.
Right now, chemists home in on new reaction routes for 4-nitroaniline, hunting cleaner, safer, faster ways to get from raw materials to finished goods. Research papers cover catalytic systems promising higher selectivity or run on milder conditions to sidestep harsh acids and volatile waste. Environmental concerns drive thinkers in green chemistry to adapt water-based methods or look for biocatalysts capable of nitration and amination steps. Pharmaceutical researchers probe deeper into nitroaniline analogs, betting they hold keys to antimicrobial or anticancer agents. Beyond synthesis, teams examine detection methods for environmental monitoring — important if you care about clean water and accidental discharges into natural ecosystems.
Toxicological studies on 4-nitroaniline stack up by the dozens, each pointing out the dangers posed by contact or inhalation. These risks aren’t theoretical; workers in dye plants suffer headaches, cyanosis, or worse if exposed without protection. Science shows that it’s the nitro group, and its downstream metabolites, that disrupt oxygen transport in blood, producing methemoglobinemia. Long-term studies raise red flags about carcinogenicity, reproductive impact, and waterway contamination. Even small amounts leaching out from plants get attention from regulators, environmentalists, and local communities. Researchers push for better ways to predict, monitor, and neutralize these risks, but the warning remains: proper handling saves lives, and careless disregard invites trouble for both the workplace and the broader community.
Looking to what comes next, the story of 4-nitroaniline might split along two paths: either greener chemistry reinvents its manufacture and use, or competing technologies sideline it for safer alternatives. Right now, demand isn’t wilting — dye industries in Asia, for instance, still commission multi-ton batches each year. But the push for bio-based chemicals and stricter regulations keeps shaping the playing field. I see the future balancing on how quickly firms invest in safer, cleaner synthesis and waste treatment. If these change quickly, 4-nitroaniline might remain a fixture; if not, pressure from new laws or consumer activism could shrink its role. R&D is already evolving, with more advanced catalysts, process intensification, and a move to digital process monitoring reducing human risk and environmental impact. The pace and direction of these changes will decide whether 4-nitroaniline’s next chapter gets written by old-school manufacturers or by the next generation of chemical innovators.
4-Nitroaniline pops up in chemistry conversations because of its punchy yellow color and its role in producing all sorts of useful things. I first learned about this compound during my undergraduate organic chemistry classes. The yellow hue always stood out, so it’s hard to forget. It made chemistry labs look like an art project. Beyond color, though, it holds a place in a lot of manufacturing processes.
Color plays a big role in industry, from clothing to plastics. 4-Nitroaniline acts as a stepping stone in making azo dyes. These are dyes with especially vivid colors—the sort that don’t easily wash out or fade. Textile manufacturers count on these dyes to create everything from everyday T-shirts to formal dresses. My friend’s family ran a textile business, and they swore by the reliability of these dyes when they needed fabrics to pop on the shelves or in sunlight.
Along the same lines, pigments made from compounds like 4-Nitroaniline turn up in plastics and even ink. Anyone who’s ever spilled printer ink knows how persistent that color can be. That staying power comes from chemical intermediates like this one.
In a world with so many illnesses, it’s fascinating how simple chemicals contribute to life-saving drugs. 4-Nitroaniline acts as a building block for several pharmaceuticals. Drug manufacturers rely on small, reactive molecules to form more complex medicines. This molecule provides the right mix of reactivity and stability, letting chemists build larger medicinal compounds that target infections and inflammation.
Care has to be taken here, because the compound poses toxicity risks. Anybody working in a pharmaceutical lab deals with strict protective measures—ventilation, gloves, sometimes even face shields. Years ago, I spent a summer internship in a lab where every workday started with a safety briefing, especially when handling things like 4-Nitroaniline. There’s no room for lax procedures, since improper use leads to environmental and health hazards.
Research labs keep 4-Nitroaniline on hand for chemical analysis and calibration. It’s used as a standard sample in spectroscopic analysis. This helps calibrate equipment to deliver more accurate, repeatable results. One colleague of mine who works in quality control always mentioned how reliable reference compounds save hours of troubleshooting.
Students across the world encounter 4-Nitroaniline when learning about chemical reactions or spectrophotometry. This practical exposure helps future chemists understand analytics and reaction mechanisms. Having hands-on experience with real chemicals gives learning more depth than staring at slides or diagrams.
There’s a flip side. 4-Nitroaniline is classified as harmful. Ingesting or inhaling it leads to serious health consequences. Waste disposal needs careful planning—no dumping down the drain and hoping for the best. The chemical lingers, and contamination impacts both water and soil. Factories have a responsibility to treat their waste before it reaches communities. The Environmental Protection Agency and similar bodies lay out strict rules, but accidents and dumps still occur, especially in countries where regulations aren’t enforced well.
Education stands out as a key solution. Chemists and manufacturers who know the risks can make better choices, both for worker safety and the environment. Developing less toxic alternatives also helps, especially as green chemistry catches on. Newer dye technologies aim to replace risky intermediates with safer options, and companies already moving in this direction help set higher standards across the field. As more organizations adopt responsible sourcing and disposal practices, society can enjoy the benefits of modern chemistry with fewer of the old risks.
Working with 4-nitroaniline puts every chemist’s safety training to the test. This bright yellow powder shows up in dyes, pharmaceuticals and research labs. One sniff or a small dust cloud, though, hints at its dangers. Years spent in lab coats taught me to never underestimate colorful powders, especially ones flagged as hazardous.
4-nitroaniline can irritate skin and eyes, and if inhaled, it may cause headaches, dizziness or even shortness of breath. Some studies show possible links to blood disorders through methemoglobinemia, a condition that limits blood’s ability to carry oxygen. If this compound spills onto skin or if its dust drifts into the air, the risk goes up fast. NIOSH lists it as a substance that can cause significant health problems if handled without care.
Here is where habits make a difference. Every workplace that runs syntheses using nitroanilines insists on gloves made of nitrile, goggles with side shields, and lab coats buttoned up tight. I remember one afternoon, fresh out of graduate school, a light breeze from the fume hood swept up a bit of yellow powder. It landed on my glove; the lesson stuck. Without double-checking my protections, I might have wiped my eye or touched my face. That’s how accidents often start.
Wearing the right gloves and goggles only stops trouble if you use them every time. The powder sticks to clothing, hair, even shoes. Dedicated lab footwear stays in the work area. Handwashing doesn’t wait until after a spill—it happens before leaving the bench, before grabbing your phone, and never gets skipped at lunch breaks.
Good ventilation means more than spinning on a ceiling fan. Every lab with 4-nitroaniline should have a certified fume hood running before containers open. I’ve seen old labs where this was an afterthought, and dust crept into every gap. These particles don’t just float—they settle and linger, making every surface a potential exposure point. Testing airflow with a strip of tissue on the sash, and having annual maintenance checks, keeps filters working.
Labs that use nitroanilines always have clear signs so everyone knows what chemicals are present. Label every bottle, even if it looks obvious. Standard operating procedures should be posted where anyone can check them, as memory sometimes fails under stress or fatigue.
4-nitroaniline stays in sealed glass or plastic containers, away from sunlight and incompatible chemicals like acids and oxidizers. Locking storage cabinets helps prevent cross-contamination or accidental mix-ups. In one lab I was in, a poorly closed bottle leaked and stained the shelf bright yellow; we spent hours dealing with the residue. Using spill kits designed for chemical powders and cleaning up with disposable towels rather than sweeping reduces airborne dust.
Promptly reporting and documenting any spill matters for shared spaces. I’ve filled out incident forms for less, and always felt grateful that honesty outweighed embarrassment. Having a protocol for skin or eye contact, from rinsing at the eyewash station to seeking medical help, keeps surprises under control.
Safety with 4-nitroaniline comes down to details: double-gloving if needed, marking contaminated waste clearly, and treating empty containers with respect. Everyone benefits from regular training refreshers, and open conversations about near-misses build a safer lab culture. If you’ve handled or taught with hazardous powders, you know stories stick longer than warning labels. Those stories—of unexpected spills, gloves that tore, or lessons learned from mistakes—push us to stay careful and keep each other safe.
When you spend time around a chemistry lab, names like 4-nitroaniline pop up almost every week. Its place in many synthetic pathways isn’t just tradition—it’s practical. The structure tells you a big part of that story. Start with a benzene ring, something most people recognize from high school chemistry. Now, slap on an amino group (NH2) at the number one position and a nitro group (NO2) straight across at the four spot. Fancy chemists call this the para position, but it’s really just about putting those two groups right across from each other.
That small tweak—just swapping places on the ring—turns an ordinary compound into something far more reactive. If you look at the chemical formula, you get C6H6N2O2. Draw its structure and that arrangement jumps out: NH2 (amino) and NO2 (nitro) stuck to the ring, both tugging at the electron soup floating around those six carbons. That push and pull changes both its color—think bright yellow—and its usefulness in reactions.
4-nitroaniline tips the scale at 138.13 grams per mole. You might shrug at that figure, but in the lab, every decimal counts. This molecular weight anchors the math for yields, dilutions, or any of those delicate calculations that keep reactions predictable. Forgetting a decimal usually lands a chemist with a useless mess at the bottom of a flask, and that number saves hours of wasted effort.
Beyond calculations, the molecular weight shapes how this chemical behaves. It doesn’t float off as a vapor under normal lab conditions; it stays put, useful for precise measurements. Compare that to lighter relatives, and it stands out for stability at room temperature. Its yellow color even depends on these same atoms playing together in just the right way.
Pull out a bottle of this stuff, and chances are it’s headed for a dye, a pharmaceutical precursor, or a chemical test. In the textile industry, the bright color isn’t just welcomed, it’s essential for some dyes. In my time working on undergraduate organic labs, we used 4-nitroaniline as a reference compound for melting point calibration. It’s stubborn—won’t melt too hot or too cold, so it keeps students honest about their thermometer skills.
This molecule also steps up as a building block for certain medicines. Sulfa drugs rely on structures like this, using that interplay of amino and nitro groups to tweak biological activity. Mistakes in the molecular structure can make or break a drug candidate. As a researcher, the tiniest shift often meant starting back at square one, which eats up months if not more.
No one should ignore the risks. 4-nitroaniline, like many nitro compounds, doesn’t play nice in the wrong hands. It can be toxic if swallowed or if powders are inhaled—a hard reality I learned early on after a careless spill led to a week of headaches. Chemically, its stability helps storage, but disposal needs proper planning. Wastewater treatment plants and chemical labs must watch for contamination because nitroarene compounds don’t just break down overnight.
Modern labs have stepped up safety: sealed containers, fume hoods, and gloves are standard. Yet when high school or college classes cut corners, health gets compromised. More training—hands-on, not just lecture slides—makes a difference. Green chemistry also pushes for alternatives. Researchers look for ways to replace stubborn nitroarene compounds in favor of safer choices, but not every substitute matches the handy balance of stability and reactivity here.
Understanding the bones of 4-nitroaniline—its structure and heft—means fewer mistakes and healthier labs. Every chemical needs this kind of scrutiny, because in the end, smart science starts with knowing what you’re holding before the first drop lands in a beaker.
4-Nitroaniline shows up in labs and manufacturing sites for good reasons. It helps in dye production, liquid crystal displays, and research settings. This yellow, odorless solid looks harmless enough, but under the wrong conditions it turns from useful material to hazardous risk. Even after years in the lab, I’ve seen how easily people gloss over the importance of careful storage. This isn’t some abstract concern. Accidents happen when we get careless with the basics.
Embedded in its chemical structure, 4-Nitroaniline holds a toxic punch. Exposure through skin, inhalation, or accidental ingestion can harm health. Once in contact with moisture and heat, decomposition produces toxic fumes like nitrogen oxides and aniline. From my own experience, storing any chemical that can do that means a minute’s laziness can lead to a bigger mess than most want to explain in a safety report.
Shortcuts with 4-Nitroaniline only invite trouble. Dry, cool, and well-ventilated spaces beat cluttered storage closets every time. I always reach for sturdy, tightly sealed containers made of glass or chemically resistant plastic — don’t use metal, which can react and spark other problems.
Any site storing this substance needs strong labeling. I’m talking clear hazards, unmissable signs, and dates. Sketched-on tape and faded ink cause confusion later. Separate from oxidizers, acids, and flammable materials — in the lab world, mixing storage almost always leads to headaches down the road. A lost label or stray bottle on the wrong shelf can ruin a whole week.
Even the best storage plan suffers if daily routines break down. During summer, a building without climate control brings extra risk. In one job, I watched temperatures creep up; the chemical stockroom started to feel more like a sauna. That warm air speeds up decomposition, so air conditioning and backup power don’t just add comfort — they mean real safety. Avoiding direct sunlight sounds obvious, until someone stacks boxes in a rush near a window.
Legal and industry standards often require locked storage with inventory tracking, especially when theft or misuse presents real danger. Digital logs work better than paper sheets tossed in a drawer. One company I worked for switched to a barcode scanning system, and those missed bottles became much rarer. Accountability works best where it’s tracked in real time.
Many storage failures result from staff who never had thorough hands-on training. Safety sheets and chemical hygiene plans mean little if nobody actually reads them. Refresher workshops — once every year, if not each quarter — cut down the risk more than any expensive storage cabinet could. Sharing real stories about close calls does more to wake up new employees than a dry lecture.
Our daily choices shape a safe environment. Keep absorption materials like spill pillows and chemical neutralizers within arm’s reach. If possible, use personal protective equipment every single time, not just during inspections. Insist on no food or drink anywhere near chemicals, no matter how short on time. These steps add up. None of them break the budget, but each reduces risk.
Smart storage of 4-Nitroaniline boils down to respect for the substance, respect for coworkers, and respect for your own future health. The cost of good habits never comes close to the price of one avoidable accident.
4-Nitroaniline comes up in a lot of chemical production, especially for dyes, pesticides, and rubber chemicals. Workers in those industries might run into it more often than most people realize. Its yellow powder seems harmless at first look, but things get risky pretty quickly if safeguards fall short.
This substance gets into the body through skin contact, inhalation, or swallowing. Most often, people who process or work near it face exposure on their skin or by breathing in contaminated dust. Once inside, it doesn’t just quietly pass through. It can react with hemoglobin, the oxygen-carrying part of red blood cells, and block its job.
Some symptoms hit fast. Workers who handle 4-nitroaniline without decent protection may feel headaches, dizziness, shortness of breath, or gut issues soon after exposure. The blue or gray tint on skin or lips often warns of a deeper problem—methemoglobinemia. Instead of carrying oxygen, blood cells grow less efficient, and some organs may start to struggle for air. Prolonged or high exposure can push things toward confusion, unconsciousness, or worse.
Doctors have linked repeated, low-level contact to skin irritation, eye redness, or even allergic reactions. Getting it in your eyes burns and causes lasting discomfort. Swallowing even a tiny amount calls for immediate medical attention.
It’s easy to think that this compound just belongs in far-off chemical plants, out of the average person’s awareness. But 4-nitroaniline sometimes contaminates water or soil after improper disposal. From my own experience working in industrial hygiene, small accidents can sneak past even vigilant teams. That’s where communities downstream from manufacturing sites end up sharing risks they never signed up for.
The Environmental Protection Agency covers 4-nitroaniline in its Toxic Substances Control Act. It’s classified as hazardous, and workers have a right to know if it’s present. Yet small businesses, informal sectors, or under-regulated importers often don’t follow every letter of the law. Years in the safety field show gaps like this often leave people and their families exposed with little warning until symptoms appear.
Proper training changes the game. People handling 4-nitroaniline need strong personal protective equipment: gloves, goggles, lab coats, and good ventilation. Spill kits and emergency showers can mean the difference between a scare and serious harm. It’s not just about workplaces. Local governments and regulators can help by pushing for transparent reporting on chemical use and disposal.
Hospitals near chemical industries need updated protocols for chemical poisoning, especially for rare but serious exposures like 4-nitroaniline. Communities near manufacturing hubs can ask tough questions, push for public testing, and demand accountability from polluters. My experience suggests many safety issues come down to human errors and rushed procedures—not just bad luck. Open training sessions, easy-to-understand warning labels, and regular health screenings for anyone at risk might keep a routine job from turning dangerous.
Science alone isn’t enough. Real health protection happens when chemical knowledge meets a culture that values worker and community safety. Honest reporting about problems, lessons learned from mishaps, and open forums for community voices all drive safer workplaces and neighborhoods. Earning trust means showing real steps to keep people safe around chemicals like 4-nitroaniline—every day, not just on paper.
| Names | |
| Preferred IUPAC name | 4-nitrobenzenamine |
| Other names |
4-Nitroaniline p-Nitroaniline 1-Amino-4-nitrobenzene p-Nitroanilide para-Nitroaniline |
| Pronunciation | /ˈfɔːrˈnaɪtroʊˌænɪliːn/ |
| Identifiers | |
| CAS Number | 100-01-6 |
| Beilstein Reference | 635923 |
| ChEBI | CHEBI:50436 |
| ChEMBL | CHEMBL1542 |
| ChemSpider | 6320 |
| DrugBank | DB13367 |
| ECHA InfoCard | 100.007.413 |
| EC Number | 202-816-1 |
| Gmelin Reference | 82100 |
| KEGG | C01593 |
| MeSH | D009603 |
| PubChem CID | 981 |
| RTECS number | AU1400000 |
| UNII | 7GR28W0FQJ |
| UN number | 1661 |
| Properties | |
| Chemical formula | C6H6N2O2 |
| Molar mass | 138.13 g/mol |
| Appearance | Yellow to orange crystalline powder |
| Odor | Odorless |
| Density | 1.437 g/cm³ |
| Solubility in water | 0.7 g/L (20 °C) |
| log P | 0.41 |
| Vapor pressure | 0.000016 hPa (25 °C) |
| Acidity (pKa) | pKa = 1.0 |
| Basicity (pKb) | 9.38 |
| Magnetic susceptibility (χ) | -52.0×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.680 |
| Viscosity | 1.23 cP (20°C) |
| Dipole moment | 3.58 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 166.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –43.7 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -1376 kJ·mol⁻¹ |
| Hazards | |
| Main hazards | Harmful if swallowed, toxic in contact with skin, causes serious eye irritation, may cause damage to blood and methemoglobin formation through prolonged or repeated exposure. |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS07, GHS09 |
| Signal word | Danger |
| Hazard statements | H302, H312, H315, H319, H317, H335, H351, H372, H400 |
| Precautionary statements | P261, P264, P270, P271, P272, P280, P301+P312, P302+P352, P304+P340, P305+P351+P338, P308+P311, P321, P330, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 3-2-2-OX |
| Flash point | > 196°C |
| Autoignition temperature | 540°C |
| Lethal dose or concentration | LD50 oral rat 750 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat 250 mg/kg |
| NIOSH | SN 0875 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for 4-Nitroaniline: "1 mg/m3 (OSHA, 8-hour TWA) |
| REL (Recommended) | REL: 3 mg/m3 |
| IDLH (Immediate danger) | 300 mg/m3 |
| Related compounds | |
| Related compounds |
Aniline p-Phenylenediamine 4-Nitrophenol 2-Nitroaniline 1,4-Dinitrobenzene 4-Bromoaniline |
