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Over the decades, the chemistry world has seen countless molecules rise to play unsung yet pivotal roles in industry and research. 2,4,4-Trimethylpentyl 2-peroxyphenoxyacetate didn’t just appear out of thin air. Its roots reach back to the mid-twentieth century, when scientists scoured the limits of organic peroxides in search of better polymerization initiators. Peroxyesters, a broad group with numerous modifications, found their way into industry because they offered hopeful stability and tunable reactivity compared to their dialkyl and diacyl relatives. Researchers took tedious steps, testing reactions and safety limits, eventually landing on molecules like this one. Only after much careful research and a few missteps did this agent earn its place in polymer chemistry, in part because it tackled problems that earlier initiators couldn’t handle without risk or mess.
What sets this compound apart comes down to its role as an organic peroxide, more specifically, a peroxyester dissolved in a carrier solvent. Complex as its name sounds, this agent provides a reliable, highly active means to start chain reactions in polymers, which shapes material properties in everyday objects—from plastics to coatings. Users pay close attention to solution content, sticking beneath the 37% threshold. High enough to work efficiently, this value manages the delicate balance between performance and safety. Over the years, this restricted content has become critical, as mishandling pure or highly concentrated peroxides has led to accidents in labs and plants. Nobody takes the warning labels lightly.
I’ve always been a stickler for watching the little details—smell, solubility, and temperature limits, for instance—because missing a cue often spells trouble. This peroxide ester lands as a colorless to pale yellow liquid, a hallmark for many in its group. Slightly aromatic notes catch sharp noses, but the vapor isn’t usually persistent. Solvents chosen for dilution, such as phthalates, keep it flowing but buffer its volatility. It stands at a crossroads in chemical behavior: active enough to meaningfully impact free-radical processes but, in these controlled solutions, less likely to react destructively due to runaway exothermic events. Its shelf-life and storage requirements reflect a careful balance: cool, away from sunlight, and always in containers strong enough to take a hit, just in case.
Labels tell the real story. Safety and technical specs stand out on any bottle, and not just because of legal requirements—they’ve been shaped by hard-won experience. Clear hazard pictograms, signal words, and percentage caps remind handlers what’s scattered through safety reports. The compound’s catalog data unpacks: limited solution percentage, density typically near that of water, limited miscibility with polar solvents, thermal breakdown ranges, and a warning about contamination. Even professionals with decades in the industry check the label each time before use, a habit that follows years spent reviewing safety incidents in chemical plants. Temperature controls form the backbone of any safe storage plan. Too hot, and you invite creeping danger from self-accelerating decomposition. Too cold, and handling can become tricky since peroxides sometimes crystallize, risking uneven dispersion or even blockages in lines.
This molecule springs from a blend of organic synthesis steps familiar but still exacting. Manufacturers start with the core alcohol or hydroperoxide precursor, then steer it through careful esterification with phenoxyacetate derivatives. These reactions need carefully measured acid or base catalysts, precise cooling, and a lot of patience. Even tiny miscalculations lead to unwanted byproducts or unstable intermediates. Once the target molecule forms, most production lines dissolve it straight away, reducing risks and making transport feasible. In lab scale or industrial synthesis, I learned firsthand that purity checks—chromatography or simple melting point checks—catch mistakes before they snowball into costly or dangerous batches. Nobody likes a recall due to residual impurities or missed reaction steps.
Peroxyesters like this react with considerable speed under the right conditions, liberating radicals that initiate chain polymerization in vinyl and styrene-based monomers. The molecule acts as a controlled break point, fragmenting under heat or by reaction with a reducing agent, into free radicals that trigger rapid molecular growth. Modifications to its core can tune its activity or stability. For example, swapping in more hindered phenyl groups tightens the breakdown temperature, while tweaks on the alkyl backbone shift solubility. Over the years, chemists have experimented with co-initiators and additives, chasing more predictable initiation rates and less scrap. You never want your peroxide to blow off in the transport tank or during a lunch break at the plant, so these chemical modifications stay high on every manufacturer’s mind.
There’s little consistency in naming across the industry, a lesson reinforced every time I try to cross-reference peroxides for buying or regulatory review. This molecule often goes by names that highlight either the core alcohol (2,4,4-trimethylpentyl) or the peroxy linkage with phenoxyacetate. Sometimes you’ll find it labeled under trade codes that say nothing about chemistry, just numbers and letters. Among professionals the scientific shorthand wins out, but for procurement or shipping, familiarity with all the synonyms prevents ordering mistakes that could waste money or, worse, create a safety hazard through substitution.
Working with peroxyesters makes you respect risk. Stories circulate among chemists—labs lost to fires, trucks overturned, minor accidents turning fatal from simple slips in judgment or procedure. The key to running safe operations is never to depend on a single safeguard. Facilities demand redundant, robust equipment and reliable monitoring. Good training saves lives. Safety goggles, gloves, and splash shields become second nature. Storage away from incompatible chemicals—strong acids, reducing agents, combustibles—stands as law, not suggestion. Regular training drills ensure nobody forgets the right response when alarms sound or odors drift. Companies have learned the value of routine inspections and maintenance. The best-run operations foster open discussions about near-misses, not just the reported incidents, because experience grows by facing uncomfortable truths about risk.
Polymer chemistry benefits directly from this compound’s consistent performance. Every manufacturing line making PVC pipes or acrylic sheets counts on initiators like this one, which don’t just start reactions—they dictate end product quality. Initiator breakdown rates control polymer chain length, which means predictable strength and flexibility in finished goods. Even outside bulk plastics, specialty coatings and adhesives turn to peroxyesters to fine-tune how materials cure and crosslink. This selectivity drives efficiency, chipping away at waste and off-spec material. As environmental and safety standards have tightened, the search for initiators with lower toxicity and cleaner breakdown products has gotten fierce. 2,4,4-Trimethylpentyl 2-peroxyphenoxyacetate keeps finding favor because it meets the technical demands without being impossible to handle safely on a large scale.
Development labs today look beyond just polymer performance. Newer research focuses on how this initiator interacts with innovative monomers that weren’t around during the early days of plastic. Cross-disciplinary teams now test its compatibility in biocompatible and biodegradable matrices. Environmental persistence and waste stream impacts also attract scrutiny. Analytical chemists use ever more sensitive detectors to track its presence in finished goods and waste effluent. Process engineers run trials to lower residual peroxide without sacrificing throughput. Every R&D step picks at the same central question—are we making materials better and safer, or just cheaper? Growing regulatory demands and consumer skepticism around chemical additives mean industry researchers can’t stop at old data and old assumptions.
In university and industry settings, toxicology reports have taught us to err on the side of caution with peroxy compounds. Animal testing, cell cultures, and environmental modeling all point to real risks from unintended exposure. Concentrated peroxides can burn or sensitize skin, and peroxy fragments may irritate eyes or airways. Chronic exposure data for this particular molecule remain incomplete, but enough parallels in the peroxyester class drive strict controls on airborne levels and open handling. Environmental toxicologists study breakdown products because these sometimes linger in groundwater or industrial waste. Carefully documented workplace monitoring and cleanup protocols respond to decades of evidence that short cuts harm more than they help. Regulatory groups worldwide have built exposure limits with wide margins, reflecting a field that moves slowly once health hazards become clear.
Looking ahead, demand for safer, greener chemical initiators will only build. Tighter controls on toxicity and emissions put pressure on every peroxide producer to innovate—greener synthesis, improved breakdown products, or entirely new mechanisms for initiating polymerization. The value of a proven molecule like this hinges on adaptability. Should future regulatory bodies restrict its use, companies will need clear data to justify its continued application or pivot to next-generation alternatives. Technical progress lately comes from two directions: designing initiators compatible with bio-based materials and making existing peroxides safer during storage and handling. Collaboration between academia, industry, and regulators will shape whether 2,4,4-Trimethylpentyl 2-peroxyphenoxyacetate remains a staple or just a stepping stone to something safer and more sustainable. My own experience tells me the right mix of innovation and humility drives real improvements in safety and material science—something everyone in the field should take to heart, especially as new hazards emerge and public scrutiny grows sharper.
Anyone who’s spent time around a factory floor or looked into the guts of the plastics industry will tell you the real trick lies in getting reactions to happen just right. 2,4,4-Trimethylpentyl 2-Peroxyphenoxyacetate—let’s just call it TPPPA for simplicity—shows up in a spot where chemistry meets real-world progress: the toolbox of substances that help start and control polymerization.
Most people never dwell on how plastic shapes our day-to-day. Yet the toughness of a smartphone case, the stretch in food wrap, and even the shell of a bicycle helmet trace back to the way plastics are born from small molecules joining up, locking together. TPPPA steps in here, doing its job as an organic peroxide initiator. Rather than just floating along, it pushes monomers to link up in a chain, which gives us the polymers needed for everything from shopping bags to car parts.
You don’t see TPPPA on the label at the store, but its impact runs deep. It’s one of those unsung chemical helpers that start the reaction, then get out the way as molecules turn to something useful. Manufacturers rely on it in processes like the production of polyethylene, polystyrene, and even specialty copolymers that lend plastics certain features—more stiffness for a pipe, more gloss for a packaging film.
It isn’t just any peroxide. TPPPA carries a certain stability, which matters a lot on the production line. With some peroxides, things can heat up too fast, risking runaway reactions or uneven material. TPPPA offers a slower, more controllable break-down, so technicians avoid sudden bursts of heat and pressure. This translates into safer working conditions and less waste, which anybody invested in keeping costs down and workers safe would appreciate.
Years back, I worked with a team upgrading an extrusion line for electrical cable insulation. Handling peroxides always carried nerves, but TPPPA’s manageable nature let us dial in reactions more precisely. Less “polymer burn,” fewer machine clogs, a smoother finish on the plastic—these are the details that add up to better product and happier producers.
Like many chemicals, TPPPA comes with rules. The industry learned through hard lessons—fires, employee injuries, leaks—the danger of taking shortcuts with organic peroxides. Companies store TPPPA in controlled conditions, train staff, and pay attention to regulatory guidance from outfits like OSHA and the EPA.
There’s also pressure to keep looking for alternatives or safer blends, especially with newer environmental targets knocking at the door. Some manufacturers explore smaller doses or blend with other initiators to cut down on potential hazards. And waste handling stays in focus. No one wants to see leftover peroxide slipping into water systems.
As the push for greener production ramps up, industry experts talk about recycling streams, lower-temperature processes, and less hazardous substitutes where possible. TPPPA probably isn’t going away soon—it’s reliable, familiar, and gets results. But more labs tinker with bio-based initiators and tighter controls in hopes of one day doing the same job with less risk.
In all, the story of 2,4,4-Trimethylpentyl 2-Peroxyphenoxyacetate goes beyond chemistry texts. It reflects real-world demands for production efficiency, safety on the job, and responsible stewardship, showing just how chemistry shapes what we carry, wear, and use every day.
People notice the dangers of chemical solutions only after disasters hit the news. I worked with chemical drums during a college internship, where mistakes turned ordinary afternoons into emergencies. Store a reactive liquid next to a bathroom with a broken extractor fan, and you risk a hospital trip. Everything boils down to three words: prevent, protect, prepare.
Most chemical solutions demand sealed, labeled containers—no exceptions. Back in our lab, old jugs attracted dust, leaks, and confusion. Once, a cleaner moved a bottle onto a high shelf under sunlight. The next day, yellow vapor hovered around the cap. A splash of sun and a forgotten lid turned a stable chemical into a hazard.
Avoid putting containers near heat, direct sunlight, windows, or busy foot traffic. Concrete or tile beats carpet or wood for floors, since spills clean up fast and don't soak in. A basic steel cabinet, locked and marked, keeps bottles upright and out of children’s hands. Wood cabinets may look sharp, but solvents eat through varnish, and fires feed on them.
Room temperature works well for many chemicals, but that means more than “it feels fine inside.” Fumes build up fast when a storeroom goes above 27°C. I remember sweating through an August restock in a small storeroom—two bottles bloated and hissed. High heat almost cost us thousands in lost reagents. On the flip side, cold can trigger crystal growth. Iced bottles left near vents can break, mixing contents across shelves.
Humidity sneaks in through loose seals or leaky pipes. Rust chews up metal cans from the inside, while some chemicals react with just a whiff of moisture. If a storeroom smells sharp, chances are the atmosphere is shifting.
One of the oldest mistakes: mixing acids and bases, or oxidizers with anything flammable. I saw a burnt ceiling tile during a site visit when someone stacked bleach next to brake fluid. Even without a flame, fumes can corrode steel doors, warp shelves, and set off costly alarms.
A decent ventilation system clears lingering vapor, and smart storage grids keep incompatible chemicals on opposite walls. Use a spreadsheet or an old-fashioned chart. It keeps people honest, especially during high turnover or shift changes.
Never trust faded stickers or capped pens. Slapped on every bottle, a label needs clear names, date received, and hazard symbols. Our lab ran out of stickers one Friday, and Monday we stood around, guessing which jug held ammonia. A whiff told us, but luck runs out. Permanent ink, waterproof tape, and good handwriting prevent panics later.
Too many labs keep spill kits only for compliance checks, then never open them. Training matters more than the eye-wash station’s shine. Staff should know what to reach for when a bottle tips. Absorbent pads, neutralizers, gloves, and a direct line to the closest emergency exit all belong on the prep list.
Taking shortcuts with chemicals courts disaster. Secure storage, clear labeling, regular checks, and hands-on training mean the difference between routine work and a headline-making accident.
Over the years, I’ve handled plenty of household products that seemed pretty harmless at first. After all, a shiny label at the hardware store or supermarket rarely hints at the headaches and rashes people talk about later. With this product, the story seems familiar. Skin irritation pops up almost right away for folks who work with it directly. Redness, dryness, and itching don’t sound dramatic, but try scrubbing your hands for days just to cool off a burning sensation.
The bigger worry comes from inhaling dust or vapor, especially in small rooms where fresh air takes a back seat. Whenever fine powders or chemical sprays get released, breathing drags those small particles straight into the lungs. Over time, coughing, sneezing, and sore throats show up. Prolonged exposure paints a darker picture: according to the American Lung Association, everyday contact with chemical particulates can raise your risk of long-term respiratory problems. Asthma attacks aren’t confined to city smog or pollen—household chemicals can trigger them too.
Eyes deserve a mention. Splash some by mistake, and watery, burning eyes make work impossible. Even after a rinse, vision might stay foggy for a while. Serious burns, although rare, can happen if the product has harsh acids or alkalis. Several ER doctors I’ve talked to suggest eye injuries from cleaning products are more common than people imagine, especially in kids.
Don’t overlook accidental swallowing. Small kids love to explore cupboards, and bright bottles can look awfully similar to juice drinks. Over 300,000 cases of child poisoning get reported in the U.S. every year, and cleaning and household chemicals land near the top of the list.
A wise neighbor once told me—rubber gloves are cheap, hospital bills are not. For every chemical product, gloves stop the itch before it starts. Goggles keep the stinging away from eyes, especially when things splash or spray. Washing hands well after finishing the job brings peace of mind.
Good air solves problems before they begin. Keeping windows open or fans running clears out the fumes, limiting what you breathe in. Working outside beats being stuck in a closed room, but not everyone has that option. Face masks work for fine powders or strong-smelling chemicals; the CDC recommends N95s or similar rated masks for heavier jobs.
For safe storage, lock cabinets make sense—especially with curious kids. Keeping products in original packaging guards against mix-ups and accidental poisonings. Emergency numbers belong on a sticker inside the kitchen cabinet: poison control, local hospital, and family doctor. Time matters when dealing with swallowed chemicals or splashed eyes.
Most of us throw away instructions thinking we know better. The truth is, reading that little label saves more pain and money than any shortcut down the line. Look for hazard signs, check for recommended dilution, and never mix products unless the label says it’s safe—bleach and ammonia mix-ups still send people to the ER every year, often with lasting lung damage.
Whether fixing up an old house, cleaning up after pets, or just handling a simple DIY job, remembering the risks helps us pick practical safety steps that fit real life. Keeping a kit stocked with gloves, goggles, and some patience goes a long way. For the sake of your skin, lungs, and family, a little planning and care around these products pays off every single time.
All kinds of substances land on factory floors, shop benches, and in backroom storage—a little bad luck or a rushed move, and a spill sneaks its way into the day. Spills rarely fit schedule, and nobody likes cleaning them. But downplaying them or slapping on too simple a response creates headaches nobody asked for, long after the smell fades. At a plastics plant I once worked in, a clumsy drum-handling moment turned a small leak of acetone into an evacuation and a health check for everyone unlucky enough to be on the shift.
Most shops keep chemical safety data sheets on a wall or folder. They're not just there to keep inspectors happy. They spell out what you’re up against with any substance on site: fire risk, health risk, impacts on drains and drains. Water reacts with some stuff, sends off toxic fumes with others. Once, we had a rookie mop oil-based paint thinner and water together–ended up with a hallway full of coughing workers and a fire marshal visit. Knowing the specific hazard stops slapdash mistakes and keeps things from getting worse before backup arrives.
Fast action can stop a bad situation from snowballing. Something hits the floor, you grab absorption pads, booms, or even a bag of cat litter if that’s all that’s handy, and start building a border. In smaller places, simple sandbags or spill socks block the substance from reaching drains or sensitive equipment. Every minute wasted means more cleanup, bigger bills, and a tougher time tracking contamination. I’ve seen quick work with a broom and sacks save the guts of an expensive compressor from a fate nobody wanted to explain to a manager later on.
It’s tempting to charge in and “just get it done,” but skin, eyes, lungs—they hold grudges. Gloves, goggles, and breathing masks save more than just company cash. I still remember old-timers bragging about “toughing it out,” and those are the same ones comparing inhalers and doctor bills in later years. OSHA records tell a grim story: thousands end up in emergency rooms every year simply because they skipped the basics.
With the immediate mess contained, safe cleanup calls for the right supplies. Industrial spills demand the right neutralizers, absorbents or chemical cleaners—no shortcuts with kitchen mops or garden hoses. Oils head to designated absorbent pads; corrosives might need a neutralizing powder, never plain water. Solid waste from the cleanup gets sealed up, tagged, and set aside for hazardous pickup—not tossed with lunchroom trash. Every company deals with regulators, and fines for sloppy disposal come expensive and fast.
Cleanup doesn’t end with a clean floor. It means logging every detail: time, date, substance, risks, who responded, methods used. These records tell the next crew how things went sideways, and help create better training. The National Response Center in the US tracks releases over regulatory limits—failure to report guarantees bigger problems. Each incident, big or small, improves future safety if people take the paperwork seriously.
Training trumps bravado—teaching everyone on site how to handle slips, where supplies live, and who calls emergency services. Regular drills pay off: practice with fake spills lowers panic and sharpens response when the real mess hits. Relying on luck runs out sooner or later. Smart workers and careful storage mean fewer spills, less clean-up, and more people getting home with little more to complain about than empty lunch boxes.
Few folks pick up a chemical container and think much beyond what it’s used for. But 2,4,4-Trimethylpentyl 2-Peroxyphenoxyacetate doesn’t land in the trash like food scraps or broken glass. This compound falls under organic peroxides, which means it brings fire risks and toxic effects to people, animals, and the environment.
Over the years, I’ve stepped foot in enough industrial workspaces to spot the difference between something you sweep onto the shop floor and something you handle with nitrile gloves. This peroxyacetate takes the safety game up a notch—fumes irritate lungs, spills attack skin, and simple sunlight or heat sends its molecules into overdrive. One small spill in a drain could spark federal fines, contaminated soil, or even hospital visits.
Underlying all those precautions lies the lack of forgiveness from the environment and the law. In the US, the Environmental Protection Agency puts strict controls on organic peroxides. California dress code wasn’t as stressful as those hazmat rules. Dumping into municipal waste or sewers spreads the problem. Streams, plant roots, and fish never chose to be test subjects. Each town or state rolls out its own rules, but the federal Resource Conservation and Recovery Act supplies the backbone: treat this as hazardous waste.
Once, a friend tried a shortcut and thought excess peroxide just vanished in household bleach. His story ended with a scorched garage and a sheepish call to local hazmat responders. Professionals don’t take chances like that for a reason.
Here’s the proven route: keep the solution in its original container, clearly labeled, with the lid tight. I always double-check labels and never mingle it with random chemicals. That alone dodges half the accidents. Then comes storage: cool, out of sunlight, no sparks or heat nearby.
Licensed hazardous waste contractors know their stuff. They show up, check documentation, and cart the whole lot to treatment plants. Thermal destruction (high-temperature incineration) wipes out the risk and handles the toxic by-products safely. A handful of large companies even encourage suppliers to take back excess product for destruction.
I’ve seen local governments team up with regional labs for periodic chemical collection days. Painters, mechanics, and hobby chemists can drop off leftovers, no questions asked. That beats secret back-alley dumps or slow leaks in household drains. Simple outreach—posters, emails, even a quick safety seminar—helps keep disposal in the right hands.
EPA guides, OSHA fact sheets, and state environmental agencies don’t just exist to tie up time with paperwork. Their recommendations align with years of data on fires, poisonings, and environmental slip-ups. Data from the American Chemical Society suggests strong links between irresponsible disposal and groundwater contamination. Nearby water sources can pick up these traces, harming more than just the folks handling the bottle.
Switching to less hazardous alternatives always sits on the table, but not every process offers a safer substitute—at least for now. Ignorance or quick fixes cut corners, but the costs show up one way or another. As someone who’s cleaned up one too many spills, following proven disposal steps and leaning on certified pros doesn’t just check boxes—it shields people, neighborhoods, and future water supplies.
| Names | |
| Preferred IUPAC name | 2,4,4-Trimethylpentyl 2-[(phenoxycarbonyl)peroxy]acetate |
| Other names |
2-Phenoxyacetic acid, 2,4,4-trimethylpentyl ester, peroxide Peroxyphenoxyacetic acid, 2,4,4-trimethylpentyl ester 2,4,4-Trimethylpentyl peroxyphenoxyacetate |
| Pronunciation | /tuː fɔːr fɔːr traɪˈmɛθɪlˌpɛntɪl tuː pəˌrɒksɪˈfiːnɒksiˌæsɪteɪt/ |
| Identifiers | |
| CAS Number | ["31547-46-3"] |
| 3D model (JSmol) | `/carbon(OC(Cc1ccccc1O[O])=O)C(C)(C)CC` |
| Beilstein Reference | 1081444 |
| ChEBI | CHEBI:131538 |
| ChEMBL | CHEMBL572497 |
| ChemSpider | 38384650 |
| DrugBank | DB11370 |
| ECHA InfoCard | 03ad5a66-b51d-42ad-89c8-c2ae1ed7e0a9 |
| EC Number | 61788-23-0 |
| Gmelin Reference | Gmelin Reference: "1485240 |
| KEGG | C19669 |
| MeSH | D000068975 |
| PubChem CID | 136621164 |
| RTECS number | YO8225000 |
| UNII | 331FDT8W0F |
| UN number | UN3109 |
| CompTox Dashboard (EPA) | DTXSID00942998 |
| Properties | |
| Chemical formula | C16H24O4 |
| Molar mass | 318.41 g/mol |
| Appearance | Colorless transparent liquid |
| Density | 1.06 g/mL at 20 °C |
| Solubility in water | Insoluble |
| log P | log P |
| Vapor pressure | Negligible |
| Magnetic susceptibility (χ) | χ = -62.0e-6 cm³/mol |
| Refractive index (nD) | 1.468 |
| Viscosity | 5.07 mPa·s at 20 °C |
| Dipole moment | 3.72 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 482.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -577.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -7510 kJ/mol |
| Pharmacology | |
| ATC code | D18AD11 |
| Hazards | |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS02,GHS07,GHS08 |
| Signal word | Warning |
| Hazard statements | Hazard statements: H242, H302, H315, H319, H335, H411 |
| Precautionary statements | P210, P220, P221, P234, P235, P280, P370+P378, P403+P235, P411+P235, P420, P501 |
| NFPA 704 (fire diamond) | 2,4,4-Trimethylpentyl 2-Peroxyphenoxyacetate [In Solution, Content ≤37%] NFPA 704: 2-4-3 |
| Flash point | 70°C |
| Autoignition temperature | 90 °C (194 °F) (Solution, Content ≤37%) |
| Lethal dose or concentration | Lethal dose or concentration: LD50 Oral Rat 5300 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat oral 4700 mg/kg |
| NIOSH | NA1989 |
| REL (Recommended) | REL (Recommended): 6 mg/m³ |
| Related compounds | |
| Related compounds |
2,4,4-Trimethylpentyl 2-peroxyphenoxyacetate 2,4,4-Trimethylpentyl peroxide Phenoxyacetic acid Trimethylpentanol Phenoxyacetate esters |
