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Chemists have leaned on strong, reliable oxidizers for a long time, and 3-chloroperoxybenzoic acid, often called mCPBA, brings a story of utility shaped by years of laboratory experiment and industry adaptation. Its rise in popularity comes from its simple promise: it accomplishes tasks other peracids leave half-finished. Labs of the mid-20th century looked for manageable reagents that didn’t need tricky storage or special handling. mCPBA’s solid form and stability filled a gap. Researchers in synthetic organic chemistry popularized it for its ability to achieve epoxidation in a straightforward, repeatable way without fussing over weird byproducts. Over the decades, mCPBA moved from academic settings to more practical hands, giving pharmaceutical chemists and chemical manufacturers a backbone for making specialty compounds safer and faster.
A batch of 3-chloroperoxybenzoic acid comes as an off-white powder, sometimes a bit clumpy, but always potent. The commercial versions find a balance—active component content typically stays between 57% and 86%. A reliable portion of inert solid ensures safer handling and reasonable shelf life. Bench chemists see these tweaks play out daily. The inert chunks make scooping and weighing more consistent. Material like this hasn’t stayed in labs by accident. Demand flows from its unique tolerance. mCPBA doesn’t catch fire easily, doesn’t stink of rot, and patrols that fragile space between effectiveness and overreactivity.
mCPBA sets itself apart by packing the strong oxidative punch of a peracid in a more user-friendly solid form. It melts around 90°C, and those who’ve handled it know the faint, sharp smell in the air when a spill dries. Water barely dissolves it, but it fares better in solvents common on the bench: dichloromethane, chloroform, and sometimes acetone if you don’t mind a more sluggish mix. Importantly, the peracid group stands ready for business—highlighting the breakable O-O bond at the heart of the oxidation reaction. The presence of chlorine on the aromatic ring gives a slightly different reactivity profile compared to methyl variants. Storage usually means keeping it cool, dry, and out of bright light to prevent unpredictable degradation.
Anyone in a regulated setting knows mCPBA’s label reads like a caution note from an overprotective parent: peracid content strictly stated, inert solid content clear, hazard warnings bold. Real-world usage hovers around the median—too little active ingredient, and reactions drag on; too much, and process safety officers get nervous, recalling more than a few stories from graduate school gone wrong. Batch-to-batch uniformity requires diligent quality checks. The packet always comes with reminders about gloves, goggles, and dust control. Yet, users value the predictability. They know exactly what’s getting poured into the flask, allowing more precise calculations and preventing unwelcome surprises down the line. Good labels don’t just tick regulatory boxes; they build trust between manufacturer and operator.
On the manufacturing side, mCPBA production falls back on old principles: straightforward oxidation. 3-chlorobenzoic acid reacts with hydrogen peroxide under acidic conditions—traditionally with sulfuric acid present to steer the reaction. Each operator learns quickly that controlling temperature and dosing rate makes the difference between a safe synthesis and a runaway mess. Purification often relies on repeated washing and careful drying to reduce impurities without sacrificing too much active material. Scale-up always challenges plant technicians, as peracids can go from manageable to unpredictable if energy or mass transport lags behind ambition. This preparation approach, refined step by step, lets both academic labs and production plants generate a consistent supply without straying into dangerous territory.
mCPBA proves its mettle in synthesis time and again. Organic chemists turn to it for epoxidizing alkenes—transforming double bonds into the more strained, reactive epoxide rings that launch dozens of downstream reactions. The byproduct, often a harmless acid, simplifies purification and prevents the end-of-reaction headaches other oxidants can create. mCPBA also performs well with Baeyer-Villiger oxidations, expanding the toolkit for converting ketones into esters and lactones. Modifications spin from these basics: researchers play with variant reaction conditions, try out solvent mixes, or tinker with additives to get cleaner, higher-yield results. A hands-on approach to reaction design with mCPBA saves time, slashes waste, and trims budgets. Making these maneuvers routine expands the palette of what’s possible for the working chemist.
Across the literature and supply catalogs, mCPBA goes by a laundry list of names: m-chloroperoxybenzoic acid, 3-chloroperbenzoic acid, MCPBA. These aliases reflect differences in naming conventions or branding more than any true chemical difference. In teaching, professors sometimes slip into shorthand—mCPBA rolls off the tongue easier, becoming the household name for generations of undergraduates. Recognizing the synonyms saves headaches troubleshooting between suppliers or digging into older research that may have stuck with now-dated terminology. By keeping an eye out for these alternate labels, practitioners avoid confusion and keep experimental records matching up with published protocols or older safety data.
Safety underscores every move around mCPBA. Anyone with bench experience learns respect quickly: peracids don’t forgive carelessness. The dangers aren’t mysterious—dust inhalation causes respiratory issues, skin contact can burn or sensitize, and concentrated material has triggered explosions when left near heat or combustible substances. Storage gets priority, usually in tightly sealed containers tucked into ventilated cabinets away from metal, organic solvents, or other reducing agents. Disposal policies keep waste streams neutral and dilute, favoring slow addition to alkaline water with plenty of room for heat to dissipate. Upgraded training, clear signage, and regular checks give operators the framework to avoid mishaps. Even small exposures prompt immediate cleanup, not just for regulatory compliance but out of respect for the shared space of the lab or plant.
Real value appears where mCPBA steps beyond textbooks. Pharmaceutical companies rely on it to create key intermediates in drug synthesis. Agrochemical producers use it for specialty molecules requiring precise oxidation steps other reagents fumble. Research labs grab mCPBA when synthesizing new polymers, sensors, or catalysts, banking on predictable outcomes. Industrial plants gravitate toward its performance profile for treating wastewater, oxidizing persistent organic micropollutants, or as a test-bed for greener process routes. mCPBA transforms dreams into reality, turning hypotheses into viable products or pilot-scale demonstrations. The tool’s strength lies in adaptability, not in being a one-trick pony. Skilled operators see its possibilities not in what it forces, but in what it enables.
Ongoing studies focus on both safety and utility. Academic groups adapt the preparation to reduce byproducts, seeking greener ways to synthesize it, some turning to water as a solvent or seeking solid supports to tame the reactive peracid group. Investigation into substitutes for mCPBA aims to deliver similar efficiency with lower risks, though few candidates catch up in versatility or stability. The strongest research pushes involve continuous-flow reactors, aiming to scale up production without the danger spikes that come from batch reactions. These innovations often reach back into fundamental chemistry, challenging old dogmas and asking whether a peracid has to behave so dangerously. Industry partnerships now drive much of the funding, with project managers demanding better waste profiles, improved yields, and safer process controls. Collaboration between corporate labs and universities opens windows on emerging risks or opportunities, creating feedback loops that benefit all hands in the chemical value chain.
Toxicological studies give mixed messages, which warrants care. Animal testing has revealed potential for both acute and chronic effects; accidental exposures have produced skin irritation and respiratory distress in workers. Chronic inhalation or repeated skin contact stokes concerns for sensitization or longer-term inflammation. Regulatory agencies have flagged mCPBA for special handling partly because of these hazards. Research into environmental fate shows it breaks down relatively quickly under natural conditions, but concentrated releases will disrupt aquatic systems before decomposition finishes. Calls for more comprehensive, long-term studies echo across safety conferences and chemical health working groups. The urgency isn’t academic, either; responsible use dictates a stronger commitment to keeping exposure as low as possible, not just meeting minimum legal thresholds.
Looking ahead, it becomes clear that mCPBA’s story is nowhere near finished. Chemists crave tools that walk the line between potency and ease of use, and the industry isn’t anywhere close to giving up on peracids. Research teams stretch the possibilities of safer handling by developing encapsulated forms or less dust-prone versions, cutting risk without sacrificing function. Green chemistry will keep chipping away at older processes, with some pushing for biosynthetic approaches or solvent-free reactions. Meanwhile, demand from high-value sectors—pharma, specialty materials, fine chemicals—continues to drive incremental improvements in production, purity, and safety. Thoughtful stewardship goes hand in hand with innovation here. The challenge comes not just in scaling up or wringing out a few more percentage points of yield, but in making sure this powerful reagent continues to help, not harm, those who rely on it to push the boundaries of science and industry.
Anybody who’s worked in an organic chemistry lab has handled a white, sometimes clumpy powder called 3-Chloroperoxybenzoic Acid, or mCPBA. At 57% to 86% active content, this stuff packs a serious punch as an oxidizer. The first thing that comes to mind is its role in transformations that simply refuse to budge with mild reagents. Teachers love to hand over reaction schemes that rely on mCPBA for epoxidation of double bonds. After watching the color fade and the TLC spot change, it’s clear something big has happened. Putting all this in a real-world frame, the molecule’s aggressive nature finds it in several gritty corners outside the classroom, too.
Take pharmaceutical research. Before a pill lands on a pharmacy shelf, it’s a tangle of chemical shapes—rings, chains, and functional groups. mCPBA serves as a type of precise scalpel for chemists, helping turn one arrangement of atoms into another. For example, its knack for forming oxirane rings—epoxides—lets drug makers slip new parts onto molecules. This single step can create advanced fever reducers, heart medicines, or designer antivirals. The 57-86% content range lines up with how much punch the researcher needs; a high-content dose slices efficiently through olefins, skipping the weeks-long grind of older, cruder oxidizers.
Every time someone uncaps a bottle of perfume and inhales a complex scent, there’s a good chance mCPBA played a role. Many flavor and aroma ingredients begin as bland petrochemicals. Chemists run selective oxidations using mCPBA to install just the right oxygen atom in the chain—add a single epoxide or tweak a sulfur atom just so, and suddenly the liquid smells like jasmine or tastes like aged cheese. In my work with food scientists, we’ve relied on mCPBA to pull off transformations where gentler agents would leave us stuck with a boring intermediate, no flavor to be found.
Synthesizing fine chemicals for industries like electronics, or producing the advanced building blocks for dyes and polymers, leans on oxidizers that work cleanly with minimal byproducts. That's one place mCPBA shines. Not every oxidizer gives you a direct road to the product without lots of leftover mess. I’ve seen projects grind to a halt because other reagents led to tar or dangerous side-products, but a fresh scoop of 80% mCPBA along with steady cooling solved it. That reliability turns it into a staple for scaling up new specialty chemicals.
Experienced hands know that mCPBA is far from just another jar on the shelf. At higher concentrations, mCPBA can ignite spontaneously or explode if mistreated. Any commentary about its use must look this challenge in the eye. Fact: the chemical must be kept cool, dry, and as diluted as possible—too many stories circulate about bottles catching fire during improper transport or disposal. Meanwhille, the byproducts, including 3-chlorobenzoic acid, need thoughtful routing through waste systems to avoid soil and water contamination.
Switching from old-school bulk handling to pre-measured packs and sealed systems helped my lab reduce accidents sharply. Pairing oxidations with in-line filtration manages both yield and waste, squeezing higher performance with smaller environmental costs. Waste treatment keeps ahead of regulators by neutralizing spent solutions and recovering valuable metals. These changes don’t just check boxes—they protect people and the towns we work in.
Like most powerful tools, mCPBA's true value shows up in the hands of those who respect both its usefulness and its risks. In fields stretching from life-saving drugs to the perfume industry, and even specialty electronics, those white crystals fuel progress—so long as we back up each reaction with safety, skill, and a careful plan for every leftover drop.
3-Chloroperoxybenzoic acid, often called mCPBA, keeps popping up in organic chemistry labs because it does a clean job oxidizing a range of substances. It’s powerful—and with that comes risk. Forget to respect it, and the consequences can range from ruined experiments to dangerous fires or even serious injuries.
Lots of chemicals ask for a cool spot, but mCPBA takes that request up a notch. The compound’s oxidizing nature gets more aggressive as temperatures climb, making it unstable and, honestly, unpredictable. Refrigeration slows its tendency to decompose, and I’ve seen problems disappear just by moving a bottle from a benchtop to a fridge. That means keeping it between 2°C and 8°C at all times. Never tempt fate by leaving it out, especially during cleanup or inventory day.
Let moisture find its way into an mCPBA container, and you’ll build the perfect recipe for decomposition—and sometimes violent reactions. Always make sure containers are airtight. Humidity might seem harmless, but I’ve had a batch turn into sludge after one careless cap left half-open. Silica gel packets tossed inside storage cabinets help fend off ambient moisture.
Light, especially from the sun or those old fluorescent tubes, can set off slow and steady decomposition. Storing mCPBA in amber bottles helps, but they can't protect the compound entirely. Find a dark cabinet or drawer meant just for light-sensitive and dangerous chemicals. Good chemical hygiene means following through on common sense: don’t stack these materials near a window, and cover labels that start to fade or peel.
Some labs still store everything on the same shelf for the sake of convenience. In my time, I’ve seen that lead to major headaches—plenty of close calls with oxidizers like mCPBA sitting next to solvents or acids. Chemical separation isn’t overkill. Assigning separate containment bins for strong oxidizers gives peace of mind and pulls folks back from the brink of catastrophe. Fire-resistant cabinets labelled for oxidizers make a solid investment.
Routine shouldn’t breed carelessness. When handling mCPBA, gloves and safety goggles aren’t optional. Even its dry powder can irritate eyes and skin, and accidental splashes with the solution leave burns that don’t heal quickly. Stick to protocols, and train newcomers on the same habits. Someone once forgot gloves for one transfer, and it turned into two weeks of skin irritation.
Every workplace needs an up-to-date Safety Data Sheet for mCPBA within arm’s reach. Rules mean little if people can’t double-check storage limits, clean-up guidelines, and what to do after exposure. Label containers clearly with concentration percentages too—confusion here can spark bigger mistakes once the workday picks up.
Labs evolve, but chemistry’s risks remain the same. Proper storage of mCPBA isn’t just about ticking boxes on safety checklists. It starts with a culture of respect—a practice I’ve found keeps everyone safer and experiments reproducible. Invest in education, good equipment, and attention to detail. The payoff is a lab where work yields results, not accidents.
Anyone who's ever spent time around chemicals knows a single careless move can lead to long-term regret. It takes just one hurried moment—skipping gloves or ignoring eye protection—and suddenly your day heads toward the ER. I've seen skin reactions that took weeks to heal, and stories from colleagues drive the point home. Every chemical brings its own risks. Some sting right away, others sneak up after hours or days. For folks using these products daily, short cuts just cost too much.
Gloves stand at the front line. Nitrile gloves block most solvents and acids. For harsher products, butyl or neoprene work better. I've tested cotton gloves by mistake—didn’t end well. Products seeped through, skin flared up. Chemical-resistant gloves should be a habit, not an afterthought.
Goggles shield eyes from sprays and splashes. A few drops in the eye count as a major emergency. Prescription glasses won’t cut it—wraparound goggles are the gold standard. Face shields matter if splashing feels likely: pouring, mixing, or moving large quantities.
Respirators aren’t overkill for strong fumes, dust, or vapor. Even simple dust masks get you nowhere with volatile chemicals. Cartridges rated for chemical vapors offer real protection. Fit testing and proper storage of respirators mean the difference between filtered air and wasted effort.
Aprons or coveralls stop splashes from reaching your clothes and skin. Lab coats look official, but chemical-resistant aprons or full-body suits offer better coverage where it counts.
The first thing many skip? Reading the safety data sheet (SDS). It spells out the risks and proper handling steps, no guesswork required. I know plenty of stories where ignoring the SDS meant exposures that could have been avoided.
Work in a well-ventilated space. Fumes build up fast in closed rooms, turning a small risk into a big one. A fume hood, open window, or a good exhaust fan reduces the risk of breathing toxic vapors. In crowded or cramped conditions, that difference shows up by the end of the shift—headaches, coughing, that nagging chemical taste in the mouth.
Put in place a process for spill management. Accidents are part of the job. Having spill kits close by means response time shrinks from minutes to seconds. Floor absorbents, neutralizers, and proper waste containers should live within arm's reach.
Every team needs a practice plan for emergencies. Fire, chemical burns, or inhalation exposure don’t follow schedules. Regular drills make reactions automatic and fast. An eyewash station within ten seconds’ reach can mean saving vision.
I've found that regular hands-on training beats online videos. Until you’ve fumbled with gloves or rushed for an eyewash using only muscle memory, you haven’t locked in those habits. Companies protect themselves and their people by making in-person safety drills part of the routine.
This isn’t just red tape. Following these precautionary steps and using personal protective equipment turns high-risk work into a job people can stick with for decades, not weeks. Safety doesn’t slow the job down; it just helps you get home in one piece.
Every lab worker develops a sense of respect for strong oxidizers like 3-Chloroperoxybenzoic Acid (mCPBA) pretty quickly. This stuff works wonders for epoxidizing alkenes or knocking out oxidations in organic syntheses, but its reputation as a skin and eye irritant, or a source of spontaneous combustion, always stands in the background. Those who have ever reached for a bottle of mCPBA from a reagent shelf know how much care goes into the simplest tasks.
Most reported accidents in research labs involving mCPBA stem from spills or splashes. The powder or crystals can turn the calmest hand jittery, knowing contact leads to burns or worse. No one forgets the sharp, chlorine-like smell either.
One time a coworker dropped a spatula of mCPBA on the bench. Nobody panicked, but you could read the tension on every face as a cloud of dust started to lift. The best thing we did in that moment? Shut down reactions, alert everyone, and clear the area. Several studies, including data from the ACS Division of Chemical Health and Safety, stress that rapid evacuation reduces accidental inhalation or spread on clothing and shoes.
Dealing with the mess called for much more than paper towels. A pile of mCPBA absorbs moisture from the air and can ignite stray solvents in an instant. We grabbed inert absorbents—think dry sand, not sawdust—and used plastic scoops, not metal, to avoid sparks. Scraping and sweeping took patience, but it worked. We collected all contaminated waste for proper disposal, then washed surfaces with diluted sodium thiosulfate to break down any residue. Forget bleach or acetone; these can react badly, sometimes explosively.
Exposure to mCPBA through the eyes or skin happens even to the cautious. Immediate rinsing with water makes a world of difference. I learned early that safety showers and eyewash stations are not just architectural requirements—they are lifesavers. Medical attention isn’t optional, and hazard forms offer a learning moment for the team afterward.
Lab coats and double nitrile gloves stay non-negotiable. After every near-miss, the checklist of lessons grows: Only open mCPBA under a fume hood, keep incompatible solvents far away, never walk away from a spill, and store the acid in a cool, dry, clearly labeled spot. The CDC and OSHA lay out much of this plainly, but culture in a lab environment cements these ideas into habits.
The safest labs build skills for spill response into regular training. Watching a demonstration, then using simulated powders, helps demystify the protocol. Written plans never replace practice. Teams should talk through near-misses, adapting protocols every semester if needed.
High school chemistry taught me early on that mistakes happen. Yet with chemicals like mCPBA, there’s no room for guesswork. Fast, informed action, supported by proper training and access to neutralizing agents, lowers risks and builds a culture that values life over rushed results. If there’s a silver lining, it’s that each accident pushes everyone toward better science and safer work spaces.
People often treat storage as an afterthought. Stack some bottles on a shelf, check the labels, and move on. I’ve seen this approach turn a routine day at work into a near-miss emergency. Mixing incompatible chemicals creates risks nobody should underestimate. Whether you’re in a lab, a factory, or even a high school science room, a little knowledge can save a lot of trouble.
Let’s use sodium hypochlorite as an example. This common disinfectant, found in household bleach, is affordable and widely used. Toss it near acids or ammonia and trouble starts. You don’t need to be an expert to see why. Mixing sodium hypochlorite and acids releases chlorine gas. Not some harmless vapor—chlorine gas can leave you coughing, gasping for breath, or worse. As evidence, the Centers for Disease Control and Prevention reports thousands of household injuries linked to these types of accidents every year. Ammonia and bleach create chloramine vapors, another danger that sends people to the ER.
Plastic seems safe. But not every type works with every chemical. Strong oxidizers like hydrogen peroxide or nitric acid may eat through some plastics or rubbers. I learned that lesson the hard way in a college chemistry lab, watching a container collapse as acid leaked across the bench. Polyethylene usually handles many corrosive chemicals better than cheap plastics. Metal containers, on the other hand, do not mix with acids—rust happens fast, and leaks follow. Some acids even attack stainless steel. That’s not just annoying, it's a fire risk or chemical spill waiting to happen.
I remember one maintenance manager who thought glass jars would stand up to anything. One day, hydrofluoric acid turned the jar cloudy, then weak, then cracked. Hydrofluoric acid eats glass. You won’t forget that smell either. Always check the chemical compatibility of a container instead of assuming the strongest material you have on hand will do the job.
Storing strong oxidizers near flammables jumps to mind. One spark and disaster follows. Separate these, use proper storage cabinets, and read safety data sheets. Corrosives such as acids and bases belong in their own zones. Combine them and heat, toxic gases, and even explosions result. Storing acids away from cyanides belongs on any checklist—if those mix, deadly hydrogen cyanide gas forms. Even seasoned professionals find themselves surprised by how quickly things go wrong in a cluttered space.
Building good habits around chemical storage goes a long way. Always label containers with full names, concentration, and dates. Skip abbreviations—nobody wants to play a guessing game when it matters. Use appropriate storage containers, and line storage areas with chemical-resistant trays or mats to contain spills. Regularly inspect for bulging, leaks, or cracked lids. Rotate chemicals so older stock gets used first, and dispose of anything past its expiration date following local guidelines.
Every lab, shop, or warehouse should keep a current inventory. Consult chemical compatibility charts available from reputable sources like the National Institute for Occupational Safety and Health or the manufacturer’s documentation. Don’t rely on memory or habits handed down from the last shift lead. Training refreshers do more than check compliance boxes—they save lives.
Over the years, I've learned that simple steps, grounded in facts and experience, build a culture where everyone goes home safe. Respect the chemicals. Store them the right way. Don't cut corners. A small investment in knowledge and planning beats racing for the eye-wash station every time.
| Names | |
| Preferred IUPAC name | 3-chloroperoxybenzoic acid |
| Other names |
m-Chloroperbenzoic acid meta-Chloroperoxybenzoic acid MCPBA peroxy-m-chlorobenzoic acid |
| Pronunciation | /ˌθriː-klɔːr.oʊ.pəˌrɒk.si.bɛnˈzoʊ.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | [937-14-4] |
| 3D model (JSmol) | 3D model (JSmol) string for 3-Chloroperoxybenzoic Acid: `CC1=CC(=CC=C1C(=O)O)Cl` |
| Beilstein Reference | 3918737 |
| ChEBI | CHEBI:52049 |
| ChEMBL | CHEMBL1567223 |
| ChemSpider | 8457 |
| DrugBank | DB14004 |
| ECHA InfoCard | 03fea114-627d-4936-8fe2-9fc4d0123eab |
| EC Number | 201-995-5 |
| Gmelin Reference | 1478025 |
| KEGG | C06614 |
| MeSH | D015555 |
| PubChem CID | 70418 |
| RTECS number | CU1400000 |
| UNII | E6FRW9Q2DH |
| UN number | 3108 |
| Properties | |
| Chemical formula | C7H5ClO3 |
| Molar mass | 156.57 g/mol |
| Appearance | White or pale yellow solid or powder |
| Odor | Pungent |
| Density | 1.53 g/cm³ |
| Solubility in water | soluble |
| log P | 2.06 |
| Vapor pressure | 0.0013 hPa (25℃) |
| Acidity (pKa) | 7.47 |
| Basicity (pKb) | 12.58 |
| Magnetic susceptibility (χ) | -6.8e-6 cm³/mol |
| Refractive index (nD) | 1.619 |
| Viscosity | 2.1 mPa·s (25 °C) |
| Dipole moment | 2.71 D |
| Thermochemistry | |
| Std enthalpy of combustion (ΔcH⦵298) | -1576 kJ/mol |
| Pharmacology | |
| ATC code | D08AX |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS07, GHS09 |
| Pictograms | GHS03,GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H271, H302, H314, H332, H335, H410 |
| Precautionary statements | P234, P221, P261, P271, P280, P220, P264, P321, P301+P330+P331, P305+P351+P338, P304+P340, P302+P352, P332+P313, P337+P313, P333+P313, P362+P364, P363, P370+P378, P405, P501 |
| NFPA 704 (fire diamond) | 3-2-1-OX |
| Flash point | 40°C (104°F) |
| Autoignition temperature | 117°C |
| Explosive limits | Explosive limits: 4.0 - 74% |
| Lethal dose or concentration | LD50 oral rat 3,900 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral (rat): > 500 - 2000 mg/kg |
| NIOSH | UN2884 |
| PEL (Permissible) | PEL (OSHA) : Not established |
| REL (Recommended) | 0.2 mg/m³ |
| Related compounds | |
| Related compounds |
3-Chlorobenzoic acid m-Chlorobenzoyl chloride Peroxyacetic acid meta-Chloroperoxybenzoic acid Benzoic acid Peracetic acid |
