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Acetyl chloride's story stretches back to the 19th century, in a period where organic chemistry began pulling ahead from its alchemical roots. Carl Gerhardt first prepared acetyl chloride in 1852 by treating potassium acetate with phosphorus trichloride, marking a shift toward more controlled synthesis methods. In those early days, much of the equipment leaked or caught fire, and few people appreciated the toxic vapors floating around cramped laboratories. The same compound that workers once feared became essential for streamlining chemical transformations, especially for introducing acetyl groups, and this legacy gives acetyl chloride its special place among organic reagents. Over more than a century, batch processes gave way to continuous production, and safety precautions caught up with its corrosive, fuming reputation.
Acetyl chloride, with the formula CH3COCl, has established itself as both a lab staple and an industrial powerhouse. This colorless, volatile liquid releases sharply pungent fumes in the air and can go from inert container-hugger to aggressive reactant in a heartbeat. It finds itself bottled not just for research benches, but also for bulk processes in manufacturing settings. No one in a synthetic chemistry lab ignores the clear warning: this stuff doesn’t mess around. Acetyl chloride finds its way into pharmaceutical plants, fragrance factories, plasticizers workstreams, and agrochemical lines. Instead of relying on clumsy make-do reagents, chemists reach for acetyl chloride specifically because it reacts quickly with alcohols, amines, and sometimes with water, which prompts the infamous white smoke — hydrochloric acid vapor in the air.
At room temperature, acetyl chloride shows off as a colorless, mobile liquid. Don’t try smelling it directly; the fumes sting eyes and nose right away. Its boiling point sits at about 51°C — lower than water — and it tends to fume in moist air, indicating how readily it reacts with airborne water molecules. With a density of roughly 1.104 g/cm3 and a refractive index near 1.389 (20°C), it’s denser and shinier than water. Its melting point drops down around -112°C. A key trait stands out: fierce reactivity with nucleophiles. Acetyl chloride breaks down in the slightest presence of water to yield acetic acid and hydrochloric acid; that reaction, foamy and smoking, captures the imagination of students and also highlights safety concerns. As an acyl halide, it’s particularly useful as an acetylating agent in both lab-scale syntheses and industry-scale reactions.
Product specifications for acetyl chloride leave little room for ambiguity. High-purity material reaches 99% assay or better. Labels include the UN number (UN1717), hazard pictograms for corrosiveness and toxicity, and storage instructions so explicit that even the most distracted technician will pause. Safety Data Sheets don’t mince words, warning about violent hydrolysis, vapor toxicity, and the risk of contact-induced chemical burns. Experienced chemists always inspect labeling for batch number, manufacture date, and purity grade—grasping how a slip in labeling can cause misidentification and batch contamination. Trace water content and acidity can derail sensitive downstream reactions, so technical specifications aren’t a formality, but a shield against missed yields and dangerous accidents.
Most production routes rely on reaction between acetic acid derivatives and chlorinating agents. Industrial runs often treat acetic anhydride or acetic acid directly with phosphorus trichloride or thionyl chloride, with byproducts such as SO2 and HCl evolving in the process. Factories running continuous or batch processes keep water out religiously, using glass-lined reactors and elaborate vent scrubbing systems. Small-scale synthesis sometimes opts for simpler setups, converting sodium acetate with phosphorus pentachloride in a cold, dry flask. I once watched a green chemist spend an hour drying every glass joint before he dared pour the acetic acid — one careless drip of water would have sent fumes cascading through the hood. That focus on preparation underscores the line between a smooth synthesis and a serious safety spill.
Acetyl chloride reacts snappily with alcohols to form esters. Add an amine, and you get an amide. Professional chemists go for this route because it runs faster, cleaner, and with fewer side reactions than other acetylating methods. It’s a cornerstone reagent for preparing acetyl derivatives of cellulose, giving synthetic fibers like cellulose acetate their life and shape. In labs, acetyl chloride often serves as the go-to for introducing protecting groups onto molecules, or for modifying aromatic rings to yield acetophenones, a valuable building block in scent and pharmaceutical synthesis. Its ability to react with water — producing hydrochloric acid and acetic acid in a frothy, exothermic surge — is not for the faint-hearted or careless. Careful handling, ice-cold conditions, and precise dropwise additions form the rulebook for any technician worth their gloves.
Few chemicals go by as many names as acetyl chloride. Acetic chloride, ethanoyl chloride, or just plain "acetyl chloride" on shipping labels. In research settings, one might see abbreviations like AcCl. Sales catalogs use synonyms that suit import/export regulations or local nomenclature, but the CAS number, 75-36-5, cuts through that confusion. Colleagues in procurement keep a list of alternate names handy to avoid accidental substitutions—a lesson learned after one order for “acetic anhydride” created a turnaround delay nobody enjoyed.
Acetyl chloride draws respect, not just cautious glances. In my early years training in chemical plants, we heard stories about newcomers who underestimated its power. Fume hoods, thick gloves, acid-resistant aprons, and tight goggles keep people safe, but the real lessons come from hearing a hiss and knowing it’s no ordinary vapor. Acetyl chloride doesn’t just hurt on contact, it sets off a chain reaction with any trace water — on skin, in air, in glassware — releasing hot acid and blinding fumes. Standard handling procedures insist on dedicated glassware, absolute dryness, and quench stations ready for accidents. In industrial settings, all piping gets lined with tough plastics or enamel, and sensors watch for leaks. The best labs drill teams on spill response and keep calcium chloride or soda ash at hand to soak up even a hint of a leak. Storage rules keep it away from strong bases, water supplies, and direct sunlight. Nobody cuts corners more than once with acetyl chloride — the compound’s reputation for causing chemical burns and respiratory stress keeps everyone on their toes.
In the pharmaceutical industry, acetyl chloride streamlines the synthesis of analgesics, antibiotics, and intermediates. I’ve watched medicinal chemists snatch it from the shelf to acetylate salicylic acid, yielding aspirin in the blink of an eye. In fragrance and flavor factories, it helps build esters that bring bouquets to perfumes and tastes to confections. Dye manufacturing, particularly for acetate-based dyes or pigments, counts on acetyl chloride’s reactivity to provide fast, reliable acylation. In plastics and fiber production, the reaction with cellulose pushes innovation in filters, films, and nonwoven fabrics. Laboratories reach for it routinely to introduce acetyl groups into natural products, peptides, or other complex molecules as a way to modulate biological properties. The reach goes far beyond the original research lab, extending into bulk commodity chemicals and specialty item production.
The drive for greener, safer acetylation methods has triggered waves of research focusing on alternative chlorinating agents, solvent-free conditions, and better containment systems. Teams working in academic and industrial partnerships look for catalysts that cut waste and risk, whether for bulk commodity synthesis or new drug candidates. Some researchers try to tweak process conditions so acetyl chloride’s infamous fumes stay trapped in closed-loop systems. R&D also churns out new derivatives of acetyl chloride, adapting its sharp reactivity for newer pharmaceuticals or bioactive molecules. Each new project circles back to the same question: how to harness acetyl chloride’s transforming power without sacrificing worker safety or adding environmental burdens.
Scientists have tracked acetyl chloride’s toxicity for decades. Direct contact burns skin, scars corneas, and damages mucous membranes. Inhalation of vapors inflames airways and can trigger asthma in sensitive workers or chronic bronchitis with enough exposure. Animal studies uncovered its corrosive properties, and occupational safety groups list it among substances strictly limited in the workplace. Even tiny spills can generate clouds that send everyone scrambling. Toxicologists focus research on exposure symptoms, rapid detection, and effective neutralization. Improvement in local exhaust systems and medical surveillance has reduced incidents, but accidents still draw swift investigation. Many safety officers remind teams that short-term slip-ups cause more trouble than people care to admit—acetyl chloride doesn’t forgive momentary lapses.
Acetyl chloride’s role isn’t fading; trends in drug development, specialty polymers, and fine chemicals suggest demand will hold steady or increase. New manufacturing processes stress safety and efficiency, portending cleaner, more contained systems that keep the compound’s volatility in check while lowering emissions. Companies seek recycling methods for chlorine byproducts and scrubbers that cut HCl releases to meet tightening environmental rules. As synthetic biology pulls ahead, some innovators eye bio-based feedstocks for acylation, yet acetyl chloride’s reliability keeps it in the toolbox. Innovations in packaging, process automation, and remote sensor monitoring promise to boost operational safety and product consistency. No doubt, acetyl chloride will keep both chemists and safety trainers busy, balancing progress and precaution for years to come.
Walk into any chemistry lab, and eventually you’ll run into a bottle of acetyl chloride. Its pungency hits the nose, and chemists instinctively check the fume hood fan. Acetyl chloride carries a well-earned reputation for reactivity. This chemical finds regular use in making acetylated compounds — for example, medicines, fragrances, and dyes.
Pharmaceutical researchers count on acetyl chloride to transform alcohols and amines into acetates and amides. These reactions crop up in drug discovery and development, especially for antibiotics, anti-inflammatories, and cancer medicines. It speeds up these jobs through its strong acylating power, handing over an acetyl group to the target molecule. Even aspirin manufacturing at an industrial scale uses chemistry closely related to acetyl chloride’s main reactions.
The value of acetyl chloride extends into making plastics and advanced materials. Some pesky intermediates in polymer production only come from acetyl chloride-based syntheses. This ties it to products that reach consumers everywhere — cell phone screens, car interiors, medical devices, and more. Fine chemicals and agrochemicals rely on the same processes.
Acetyl chloride brings risks along with its benefits. Breathing its fumes causes coughing and serious irritation. It reacts violently with water, shooting out hydrochloric acid. Even a small spill can damage equipment and harm people. Here’s where responsible handling means everything. Engineers invest in explosion-proof storage, tight process controls, and safety training. Technicians suit up with gloves, goggles, and protective clothing.
Having worked alongside teams in chemical labs, I’ve seen safety protocols turn what seems like a high-wire act into a routine process. Regular emergency drills, clear labeling, and ventilation systems separate safe operations from headlines about lab accidents. Sharing these best practices helps new researchers keep their guard up.
Disposing of acetyl chloride brings a different set of worries. Poured down the drain or released into the air, it breaks down into hydrochloric acid and acetic acid — both tough on local ecosystems. Governments set strict rules about storage, transport, and waste. In the United States, acetyl chloride falls under the Clean Air Act and hazardous waste laws. Europe, Canada, and Japan take similar steps.
Green chemistry offers better answers, like designing milder acetylation reagents and recycling leftover chemicals. Some startups and university labs now research solvents and alternative reagents that match acetyl chloride’s performance with less risk.
As long as the chemical industry keeps searching for life-saving drugs, longer-lasting materials, and smarter electronics, acetyl chloride’s place seems secure. The demands it places on safety and waste management show up in every training manual and safety audit. Relentless attention to detail keeps it from shifting from a valuable tool to a hazardous liability.
Acetyl chloride brings trouble if handled carelessly. Every time I’ve seen someone get lax with this reagent, things go wrong fast. When acetyl chloride touches water, even the humidity in the air, it hisses and spits out hydrogen chloride gas. That gas stings your throat, scorches your lungs, and leaves a taste you won’t soon forget. Most accidents happen when someone underestimates how aggressive that reaction hits. For a reactive chemical like this, cutting corners costs real suffering.
Cotton lab coats won’t cut it with acetyl chloride. I wear a chemical-resistant apron on top, eye protection with side shields, and thick nitrile gloves—and I keep a fresh pair as backup. Splashing a bit on bare skin brings sharp burning pain, even before you wash it off. My goggles have saved me from panic more than once. The fumes bite your eyes right away, so covering your face matters. It’s tempting to say a little won’t hurt, but even one drop brings trouble.
Opening a bottle in a cramped room brings immediate regret. In college, I learned the hard way: poor airflow makes acetyl chloride practically unmanageable. The fume hood is the only real option. Even then, I turn the sash as low as possible and keep chemicals far from the opening. You’ll never regret double-checking the airflow before pouring. That sharp, sour smell is the only warning you get before the gas fills your lungs. Building management needs to inspect and maintain hoods often.
Mixing acetyl chloride with water causes a fast, violent reaction. You can't even rinse equipment casually—the leftover drops can spit acid vapor if water goes in too soon. Dry all glassware fully, and use sealing stoppers, not plastic wrap or paper. Remember, moisture from the air causes trouble, so don’t work on rainy or humid days if you can avoid it. I always plan ahead—keep water-based waste and cleanup supplies far from the workspace until the job is finished and all reagents are neutralized.
Spills will happen. I keep a squeeze bottle of sodium bicarbonate solution beside me every time. Baking soda works fast to neutralize acid, but you need a liquid solution for speed. If acetyl chloride leaks or splashes, every second counts. Don’t reach for tap water—use the neutralizer first, as water alone drives out more irritating fumes. I once saw someone grab a wet rag, and the burst of gas sent everyone outside fast. Preparedness protects your eyes, skin, and lungs far better than improvisation does.
I’ve watched people casually push bottles of acetyl chloride to the back of a shelf, lids half screwed. Leaks corrode shelves and contaminate air. Sealed, clearly labeled glass containers in a dry, cool cabinet work best. Those cabinets benefit from ventilation and acid-resistant liners. Don’t share space with other acids or bases—the mix can turn small mistakes into emergencies. Before every use, double-check the container and label—aging or contaminated chemicals behave unpredictably.
No one should work with acetyl chloride alone or without proper training. Regular drills and clear instructions build good habits. I’ve seen panic when newcomers get splashed or inhale a little fume. They froze under stress. Roleplaying spill response and chemical burns prepares everyone for rare, high-stakes moments. Managers and teachers can't skimp on reminders or checks. Good procedure becomes muscle memory, and that’s saved lives.
Too many labs stash dangerous chemicals out of sight with little oversight. Regular audits, access restrictions, and refresher courses do more than keep a space tidy—they prevent serious injuries. Digital tracking and incident reporting help everyone spot patterns and fix problems before someone gets hurt. Adding emergency eyewash stations, shower access, and clearly marked disposal bins in the lab makes cleaning up safer for everyone. The right policies set up a culture where acetyl chloride gets the respect it demands and no one leaves their shift with scars.
Anyone who’s glanced at a bottle of acetyl chloride knows it’s trouble in a clear container. This isn’t just another solvent waiting to be measured out in a calm afternoon lab session. Acetyl chloride bites the moment it meets water, spitting out clouds of hydrochloric acid gas. Inhaling that stuff even once will make it clear: you don’t ever want an accident with this chemical.
My first chemistry professor repeated, “Keep it dry,” almost like a chant. Some might think tossing the bottle in a chemical cabinet counts as safe, but with acetyl chloride, humidity itself spells danger. You slide it into a tightly sealed glass bottle. No plastic, since it can break down over time or start leaking. Good old glass, with a screw cap lined inside with Teflon or polyethylene, stands up to the nasty fumes and corrosiveness.
If the cap slips or moisture creeps in, the whole bottle could swell and burst. In my own grad school lab, a careless seal once caused a ring of hydrochloric acid crystals to build up around the threads. At that point, opening the bottle isn’t just risky — you’re basically rolling dice with a chemical reaction ready to go. That’s real-world proof moisture-proof bottles aren’t only a suggestion. They’re survival for anyone nearby.
Heat and sunlight coax more fumes out of acetyl chloride. If you care about air quality or the nerves of the person sitting next to you, stash the bottle in a cool, shaded cabinet designed for corrosives. Leaving it out on a sunlit bench shortens the container’s life. Fume cabinets work best because minor spills or splashes find containment right away. A separate spot marked for acid chlorides cuts down on mix-ups. Mix-ups mean cleanup, or worse, a call to emergency services.
Unmarked bottles invite disaster. A well-placed label with the full name, concentration, and the date received stops anyone from poking around or guessing at the contents. In the world of shared labs, I’ve watched new students mess with clear bottles every semester. It’s always a label — or the lack of one — that leaves people guessing. Sometimes extra precaution comes down to reading a handwritten warning before disaster strikes.
Accidents still happen, even with great storage. Ventilated cabinets suck up escaping fumes, keeping the lab’s air safer for sensitive lungs. If handling acetyl chloride, goggles, gloves, and a face shield aren’t up for debate. Once, after a splash burned through cheap gloves, only fast water and a lab coat kept it from eating into my skin. The lesson stuck: never cut corners with safety gear.
Poorly stored or expired acetyl chloride doesn’t just evaporate out of sight. Never pour leftovers down a drain. Neutralize small spills with dry sand or sodium bicarbonate in a fume hood, then pack up waste for approved disposal. If a bottle’s looking rough or oily on the outside, don’t even touch it solo — call in trained hazmat help. What starts as a tiny leak can become a roaring gas release faster than most realize.
Lab work shapes habits for life. I’ve seen people skip steps, sit out training, and treat chemicals as nothing but science project props. It always catches up to them. Keeping acetyl chloride stored right saves health, money, and reputations. It sets a tone for the lab that helps everyone breathe easier — literally. For me, handling acetyl chloride hammered home that in chemistry, one careless moment can haunt you for years.
Acetyl chloride looks simple on paper, but its impact reaches far in chemistry. Its formula, CH3COCl, packs a punch in every lab it enters. The single carbon atom, a pair of oxygen and chlorine, and a few hydrogens make it one of those chemicals you notice by its strong, biting smell long before seeing the label. Once, a bottle broke in our freshman organic lab, and the sting to my nose reminded everyone why proper handling is a non-negotiable rule.
Looking at CH3COCl, you see a small structure playing a big role. The methyl group (CH3), the carbonyl carbon, and the chloride all team up with a distinct personality. That chloride group does the heavy lifting, turning acetyl chloride into a sharp, reactive acylating agent. Reactions run fast and often exothermic—enough to cause trouble for anyone who doesn’t respect lab safety. From textbooks to lab benches, this combination fuels many organic transformations.
Most people may not know it, but products they use daily, like pain relievers and fragrance ingredients, often start life in a vat that includes acetyl chloride. Chemists value it for making esters, amides, and acetates—each reacting quickly, sometimes producing clouds of acidic gas if water sneaks in. Once, working on acetaminophen synthesis, the whole process paused because a flask absorbed moisture, and acetyl chloride responded with a hiss and white smoke. Manufacturers appreciate speed and efficiency, yet that same power brings safety risks to every step.
Handling acetyl chloride means freight trains of safety information. Its reaction with water makes hydrochloric acid fumes, toxic to eyes, lungs, and even some metals nearby. During my own years of chemistry teaching, the moment a fume hood failed, everyone learned quickly not to underestimate substances with such a simple formula. Labs must keep dry, use gloves, safety goggles, and always vent the workspace. Industrial sites build waterless systems and finely-tuned air-handling just to manage it.
Looking past personal experiences, the facts show widespread vigilance. According to OSHA, skin contact leads to severe burns. The CDC points to respiratory damage after inhaling vapors. Countries set strict storage and transport rules because a spill or leak leads to fast escalation and dangerous cleanups. For waste handling, nobody just rinses glassware—neutralization and fume capture come first, every time.
Creating safer lab environments and better chemical stewardship starts with training. Too many accidents in academic and industrial labs come from rushing or skipping procedures. Science education must focus on hazard recognition and slow things down for careful set up. Further, research continues into greener, less reactive acylating agents. Some chemists have started using enzymatic alternatives or solid-supported reagents, cutting down on hazardous waste.
Acetyl chloride proves the saying that a little goes a long way. Its chemical formula, CH3COCl, represents a chemical that can transform, build, and even harm all in one flask. With the right respect for its hazards and continued push for safer methods, science moves forward—one reactive molecule at a time.
Acetyl chloride comes across as a small, sharp-smelling liquid used mostly in organic labs. Its formula, CH3COCl, tells a story of high reactivity. In many college chemistry labs, the bottle sits under a fume hood, marked with all kinds of warnings. People remember what happens if you add water to it—smoke, hissing, vapor. That reaction sticks in memory for good reason.
No lab book ever calls acetyl chloride water-soluble in the usual sense. As soon as a single drop touches water, it snaps apart. The molecule breaks down, creating acetic acid and hydrochloric acid instantly. The vapors can sting your nose and eyes. This makes acetyl chloride dangerous to store anywhere near water. Even a whiff in the air can make you cough.
Once, during an undergraduate lab, a peer accidentally left a vial open. The next five minutes became a textbook example of what not to do—hissing, sniffles, and a crowd of people scrambling away from the bench. The instructors were right to stress that acetyl chloride and water should never meet in a careless way. It isn’t about dissolution; it’s about rapid, aggressive decomposition.
Mixing acetyl chloride with water does one thing: hydrolysis. The reaction gives off heat and fumes. For every molecule of acetyl chloride, the water rips off the chloride group. The byproducts, acetic acid and hydrochloric acid, both hang in the air as pungent vapors. Not only does the substance not “dissolve”—it doesn’t even get the chance before changing form. That’s a real hazard for anyone working in a tight or unventilated space.
In larger quantities, things spiral quickly. The solution becomes acidic, corrosive, and the fumes can bite through both sinuses and safety liners if you are not careful. The hydrolysis produces concentrated hydrochloric acid, which carries its own risks—corrosive to metal, skin, and lungs. For anyone who works in a lab, even a small spill demands prompt response, eye protection, and a working hood fan. All these risks speak louder than any technical label about “solubility.”
Anyone handling reactive chemicals must understand more than just labels. Training that covers what really happens—smoke, burns, coughing—is worth more than a technical note about water solubility. Acetyl chloride requires dry glassware, dry solvents, and steady hands. Some labs use it to acetylate alcohols or amines, and even experienced chemists get nervous when the humidity picks up. Keeping a chemical dry feels simple, but condensation, sweaty gloves, or even a wet stirring rod could spell trouble.
Lab safety comes down to good habits. Double-check the dryness of your tools. Label everything clearly, and train new colleagues to respect substances like acetyl chloride. Good ventilation and clear protocols matter as much as any piece of fancy equipment. Many safer reagents now offer similar reactivity without the risk of fuming acids, and research teams increasingly prefer these alternatives. It’s a relief to watch new manuals put a red flag over acetyl chloride. Fewer accidents mean more trust, both among scientists and from the public. Respecting reactivity and swapping in safer options—these steps make science a safer space for everyone involved.
| Names | |
| Preferred IUPAC name | Ethanoyl chloride |
| Other names |
Ethanoyl chloride Acetylchlorid Acetic chloride |
| Pronunciation | /əˈsiːtɪl ˈklɔːraɪd/ |
| Identifiers | |
| CAS Number | 75-36-5 |
| 3D model (JSmol) | `Acetyl chloride` (JSmol 3D model string): ``` CC(=O)Cl ``` |
| Beilstein Reference | 1718736 |
| ChEBI | CHEBI:37573 |
| ChEMBL | CHEMBL1357 |
| ChemSpider | 548 |
| DrugBank | DB11445 |
| ECHA InfoCard | 100.001.054 |
| EC Number | 200-865-6 |
| Gmelin Reference | Gmelin Reference: 765 |
| KEGG | C14191 |
| MeSH | D000082 |
| PubChem CID | 176 |
| RTECS number | Ak0400000 |
| UNII | WUO2968TG6 |
| UN number | UN1717 |
| Properties | |
| Chemical formula | CH3COCl |
| Molar mass | 78.50 g/mol |
| Appearance | Colorless to slightly yellow liquid |
| Odor | Pungent, irritating |
| Density | 1.104 g/mL at 25 °C (lit.) |
| Solubility in water | Reacts violently |
| log P | 0.94 |
| Vapor pressure | 24.7 kPa (20 °C) |
| Acidity (pKa) | pKa ≈ -2.9 |
| Basicity (pKb) | -6.1 |
| Magnetic susceptibility (χ) | -65.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.394 |
| Viscosity | 0.406 mPa·s (20 °C) |
| Dipole moment | 2.90 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 216.9 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | −216.9 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -572.7 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | D21AF02 |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS02,GHS05 |
| Signal word | Danger |
| Hazard statements | H314, H331, H335, H410 |
| Precautionary statements | P210, P222, P261, P280, P301+P330+P331, P303+P361+P353, P305+P351+P338, P304+P340, P310, P363, P405, P501 |
| NFPA 704 (fire diamond) | 3-2-2-W |
| Autoignition temperature | 192 °C (378 °F; 465 K) |
| Lethal dose or concentration | LD₅₀ oral rat 1410 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50: 910 mg/kg |
| NIOSH | NIOSH: AM5425000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Acetyl Chloride: 1 ppm (3 mg/m3) as an 8-hour TWA (OSHA) |
| REL (Recommended) | 14°C |
| IDLH (Immediate danger) | 200 ppm |
| Related compounds | |
| Related compounds |
Acetyl fluoride Acetyl bromide Acetyl iodide Acetic anhydride Acetic acid |
