Back in the early 20th century, the chemical industry exploded with curiosity for new amines, as researchers chased compounds offering unique reactivity and better stability. Diisopropylamine did not initially get the same attention as its simpler cousin, dimethylamine. Once organic chemists noticed its value as a non-nucleophilic base, especially during the synthesis revolution of the 1950s and 60s, industrial use picked up. Industries handling pharmaceuticals, agrochemicals, and solvents found DIPA’s properties valuable, leading to systematized production and refinement standards. The drive for higher yields and lower byproducts during major process overhauls in the 1970s pushed producers to fine-tune the methods, favoring processes that could deliver DIPA with fewer sulfates or amine-cross contaminants. You can see the effects in patent filings, technical journals, and the way international chemical catalogs began listing DIPA as a base chemical, not just for academic research but for broad industrial applications. That adoption grew stronger in the following decades as the move toward greener chemistry called for cleaner processes and easier separation of byproducts.
The core of diisopropylamine rests on two isopropyl chains attached to a single nitrogen atom, giving it the chemical formula (CH3)2CHNHCH(CH3)2. Folks working in chemical plants or research labs can recognize its ammonia-like, but distinctly musty, odor. Nearly colorless as a liquid, DIPA flows easily and resists freezing longer than straight-chain amines. Most manufacturers sell it in steel drums or lined tank cars, highlighting its stability under ambient conditions. DIPA appears in solvents, corrosion inhibitors, and plays a key role as a base in making Grignard reagents—a must-have in the toolbox for any organic chemist who values selectivity. For those who spend hours troubleshooting puzzled-up reactions, DIPA delivers clear performance, owing to its ability to balance strong basicity with relatively low nucleophilicity compared to smaller amines.
Looking at the stats, DIPA comes with a boiling point close to 84–85 °C at atmospheric pressure, making distillation a straightforward task for most chemical engineers. Water solubility trends low, which helps when separation from aqueous solutions is needed. The flash point stands lower than some related compounds, so storage demands good ventilation and spark-resistant fixtures. Its vapor pressure keeps rising swiftly with heat, mandating solid engineering controls to prevent fume mishaps. DIPA’s moderate pKa (10.98 for the conjugate acid) gives it enough punch to deprotonate weakly acidic sites, qualifying it for solid-phase synthesis work or other delicate operations where you want control and predictability. The vapor passes through filter paper and glass wool with ease, making it straightforward to trap in cold traps or to vent through scrubbers. These properties set DIPA apart from amines with bulkier or simpler substitutions, offering a sweet spot balancing volatility, reactivity, and manageability in industrial operations.
Producers list purity benchmark at 99% or higher, sometimes indicating levels for moisture, secondary amines, and color (measured by APHA standards). Density at 20°C clocks in close to 0.72 g/cm3. Labels spell out UN Numbers (UN 1158 as a flammable liquid), GHS hazard pictograms, and handling instructions with big warnings about eye and skin contact. Each barrel comes certified for identification tests (chromatography, NMR) and usually lists maximum allowable thresholds for residual solvents and other amines. Companies in the EU and US face requirements from REACH and OSHA, which means the paperwork travels with every shipment—a necessity to build credibility and maintain trust on the part of hospitals, research centers, and chemical distributors.
The mainstream route involves alkylation of ammonia with propylene or isopropanol under pressure, using a hydrogenation catalyst (nickel, cobalt, or copper-chromite variants being common). Dialkylamine and trialkylamines pop up as side products, but tighter reaction controls with advanced catalyst beds let manufacturers dial in selectivity. In some labs or custom batches, isopropyl bromide reacts with ammonia in a closed vessel—a less efficient, but faster, process. Equipment demands corrosion resistance, as even trace amines or residual alkali can kickstart side reactions and tank wear. Plant operators looking to push greener manufacturing swap to mild hydrogenation and better heat management, showing just how determined the sector stays when responding to emissions and waste mandates.
DIPA jumps to the frontlines as a base for creating lithium diisopropylamide (LDA), the gold-standard base in organic synthesis. Ask any synthetic chemist—they keep LDA and its parent DIPA ready for night shifts filled with anion generation or tricky deprotonations. DIPA reacts with strong alkylating agents to make higher amines, links to sulfonyl or acyl chlorides to deliver specialty compounds, and works in the formation of enolates or directed ortho-metalation reactions. Hydrophobic and minimally nucleophilic, it refuses to interfere with broad swaths of organic groups. Most applications benefit from its ability to step aside after doing its job, as it evaporates or dissolves in nonpolar solvents without fuss. Those running pilot plants appreciate DIPA’s adaptability, which reveals itself every time novel chemistries hit the bench with unexpected side products or yield bottlenecks.
Depending on country or sector, some refer to DIPA as 2-(propan-2-ylamino)propane or N,N-diisopropylamine. Large suppliers—Sigma-Aldrich, Fisher Scientific, and others—list it as DIPA, DIPAM, or N,N-DIPA. The CAS number 108-18-9 sticks as a unique identifier. People who shop in regional markets may run across similar-sounding names in trade catalogs, though regulatory pushes keep labels consistent for customs and international shipping.
Safety needs get spelled out clearly because DIPA vapor can irritate lungs and eyes fast. Anyone working with it needs gloves, goggles, and chemical-resistant aprons. Inhalation at moderate concentrations causes headaches or dizziness, and spills on skin cause dryness and rings of redness that linger for days. Industry standards demand explosion-proof storage, closed handling systems, and regular leak inspections—no room for error. Fire departments and hazmat teams responding to chemical incidents expect robust signage and instant access to material safety data. Cooling and venting work together to stop dangerous vapor accumulations, while labs and plants use local exhaust or fume hoods to keep air clear. I remember running a pilot distillation that proved just how serious these safeguards need to stay: even a leak the size of a pinhole can set off panic if you smell amines in a supposedly clean workspace. Training, routine drills, and honest safety briefings pay off big time for those relying on DIPA for high-throughput manufacturing or daily research work.
Pharmaceutical development leans hard on DIPA—not just in LDA synthesis but also as a building block for antihistamines, antidepressants, and other high-value intermediates. Crop protection products, like fungicides and herbicides, depend on DIPA to anchor side chains, bringing desired kinetics to a whole range of agrochemical molecules. Water treatment uses come in specialty blends, adding anti-corrosive properties to keep pipes clear in power stations or refinery systems. Industrial cleaning and degreasing products take advantage of its volatility and solubilizing abilities. Research teams eye DIPA for its straightforward handling in asymmetric syntheses, clocking repeatable yields with fewer purification headaches. As more sectors push for cleaner, more efficient chemical tools, DIPA’s range seems to widen, integrating into products where specialized amines historically fell short.
Each year, major chemical firms and university labs lay out millions for R&D projects targeting better amine technology. DIPA forms the centerpiece in workstreams focused on next-generation pharmaceutical backbones. Green chemistry keeps pushing for methods that reduce or skip hazardous solvents—and DIPA’s mild hydrophobicity and thermal resilience suit it to these new approaches. Analytical chemists cite its reliable NMR signature, making it easier to troubleshoot batch runs or confirm reaction progress. Start-ups playing in advanced materials seek to hybridize DIPA structures for MOD (metal-organic decomposition) inks, laying groundwork for flexible circuits or nanocoatings. I’ve seen funding bodies prioritize grants on greener amine pathways, and the compounds that keep scoring high marks always offer broad compatibility, stable handling, and minimal hazard footprints. DIPA meets these marks, and each technical conference brings reports on new catalysts or methods coaxing out higher selectivity and even purer output.
Toxicologists look closely at acute and chronic effects, with a focus on occupational exposure. Studies on rats and rabbits document moderate toxicity levels, with irritation of mucous membranes as a consistent theme. No data ties DIPA directly to carcinogenicity, yet repeat inhalation contributes to tissue damage in animal lung models, underlining the importance of strict workplace exposure limits and medical surveillance. Environmental health reports highlight persistence in air and water, though standard processing tools (carbon filtration, catalytic oxidation) clear spills quickly at industrial sites. Research reviews published in peer-reviewed journals converge on one thing: control exposure and invest in real-time monitoring, because even low-level leaks accumulate risk over long shifts. Responsible labs fit their benches and reactor halls with sensors tuned for low amine concentrations, and big plants schedule annual biomonitoring for workers near the distillation suites or bulk storage pads.
Those charting the future for DIPA see promise in sustainability pivots—cheaper, cleaner synthesis that avoids legacy issues like metal-catalyst residues or high-pressure hydrogenation risk. Chemical engineers focus on continuous-flow reactors and recoverable catalyst beds, both of which bring down energy costs and limit hazardous byproducts. Green solvents and less wasteful downstream work stand out in current patent filings. The pharmaceutical sector, pushed hard by generic production demands and new drug modalities, imagines better integration of DIPA-derived intermediates into large-scale platforms. As electrification changes how chemical plants operate—think renewables-powered operations and more automation—DIPA’s versatility positions it as a mainstay, with easy scalability and cross-sector value. Regulatory standards will likely become stricter, so anyone building DIPA into their processes needs to stay nimble, ensuring they keep every batch and environment safer for workers, customers, and the areas surrounding big production sites.
If you walk through a chemical plant or chat with a refinery worker, you’ll hear about diisopropylamine, or DIPA, much more often than on the evening news. This stuff shows up in places you’d never guess. My time working around industrial laboratories taught me—nothing gets used without a reason. DIPA makes a difference where it counts: helping keep our fuels cleaner and supporting the complex process of making products we use every day.
Everyone worries about air quality, but few think about where it starts. When crude oil and natural gas get pulled from the ground, they come loaded with contaminants like hydrogen sulfide and carbon dioxide. Too much of either one in your gas line leads to corrosion, costly repairs, and environmental harm down the pipe. Refineries rely on chemicals to pull these pollutants out. DIPA often lands in the center of this work. Its chemical makeup lets it grab unwanted gases and trap them, so what’s left behind goes on to be cleaner-burning fuel. Scrubbing plants will often swap between different amines, but the mildness and selectivity of DIPA makes it popular for sour gas treatment, especially with high acid gas concentrations. Ask anyone in the industry—few want to imagine this job without reliable amines.
Look at the glue on your desk or cleaners under the sink. Most folks count on products like these, rarely thinking about the chemical steps it takes to get there. DIPA turns up as an intermediate in creating herbicides, pharmaceuticals, rubber chemicals, and dye-stuffs. In my own university research days, we tried running syntheses without certain amines; results dropped off fast. DIPA’s balanced reactivity means it helps reactions reach completion without unleashing wildside byproducts—critical for consistent, safe outputs.
Everything beneficial can bite you back if ignored. DIPA can irritate the skin, eyes, or lungs, and in higher concentrations, it needs proper handling. Industrial sites set up training, spill containment, and ventilation to stop minor mistakes from turning into hospital visits. When I worked on hazard assessments, folks who skipped on gloves and goggles ended up regretting it. Manufacturers also follow clear transport guidelines since DIPA is flammable and forms hazardous vapors, especially in enclosed spaces. Safety is a real story here—not just something to check off for a lab compliance sheet.
In the chemical industry, we need new solutions all the time. DIPA’s usefulness leads to a lot of production and transport, and with that, a higher risk of leaks or accidents if sites grow complacent. Regulators and companies have pushed toward better containment systems, stricter exposure limits, and more robust fire protection standards. Research has started looking for amine alternatives with lower toxicity but similar performance. These early studies lay the groundwork for safer workspaces and less environmental impact down the line.
People may not see DIPA on supermarket shelves, but it’s hooked into the supply chain that keeps the world running. Understanding how this chemical works and where it fits helps industry keep pace with safety, responsibility, and the push for a cleaner environment—straight from the wellhead to the final product in your hand.
Diisopropylamine takes its place in many labs and factories as a useful building block. Its role in chemical synthesis can’t be dismissed, but neither can its safety challenges. I’ve stood in busy storage rooms where the faint whiff of amines hinted at poor habits, and I’ve watched coworkers learn the hard way about skipping protective gear. The risks are real. Splash or inhalation, even brief, leads to irritation—burns, breathing trouble, headaches. Shortcuts have consequences.
Every safety sheet screams for gloves and goggles. These aren’t empty slogans. My hands have felt the difference between thin latex and thick nitrile gloves after accidental splashes. Chemical-resistant gloves—think nitrile or butyl—hold up better during long tasks. Safety goggles, not plain glasses, actually block splashes and vapors. Simple lab coats only do so much, so I reach for chemical aprons with sleeves. Closed shoes, not sandals, guard against drops and spills.
It’s tempting to open a bottle in open air. That moment’s convenience risks long-term harm. A fume hood pulls away vapors before they reach eyes or lungs. I remember a fellow tech who tried mixing compounds at a crowded bench—his eyes watered for an hour, and the smell lingered for days. Ventilation protects not only the user but everyone nearby. Any container or reaction involving this amine goes straight into the hood.
Pouring or measuring diisopropylamine takes focus. Spills soak into wood, carpets, and even skin if you’re distracted. Real discipline means reading the container twice before opening, wiping drips, and capping bottles immediately. Clean scoops, dry glassware, and clear labels matter more than fancy tracking apps. Storage in a cool, shaded cabinet—away from acids or oxidizers—cuts down the danger of reactive mishaps. Flammable cabinets exist for a reason, not to gather dust.
I once got a call when a bottle tipped, leaving a slick puddle on linoleum. Absorbent pads soaked up some, but the smell stayed for hours. The lesson: keep spill kits close. Use pads that neutralize amines, not just any paper towel. Get down on hands and knees if you must, ventilate the room, and wash surfaces with soap and water. Hands washed fast feel better at the end of the day.
Everyone trusts their routine until something slips. Training shouldn’t stop at the first month on the job. I’ve attended refresher courses every year, and always pick up something new—a trick for checking glove integrity, a tip for using the eyewash. Sharing stories and close calls brings the instructions to life.
Diisopropylamine isn’t the enemy. Neglect and hurry are. Respecting its hazards keeps more than compliance officers happy. It keeps skin smooth, lungs clear, and workdays free of accidents. That, from honest experience, means more than any checklist ever will.
DIPA pops up in a lot of scientific discussions, especially in labs dealing with synthesis, resins, or even pharmaceuticals. DIPA stands for Diisopropylamine. Thanks to its simple structure and reliable properties, it’s earned a steady role in many chemical processes. Many chemists reach for DIPA when they need a base that won’t complicate their reactions. Its ability to absorb protons can steer a reaction right where you want it. Years spent working with chemicals showed me how certain compounds make or break a project. DIPA’s clear utility and straightforward profile offer real value when stakes are high.
Getting the formula right is more than just rote memorization. It’s about knowing exactly what’s involved so you can predict reactions, avoid safety mishaps, and buy or store the correct amount. Diisopropylamine has the chemical formula C6H15N. That tells you it contains six carbon atoms, fifteen hydrogens, and a single nitrogen. The two isopropyl groups attached to the nitrogen define its structure and practical behavior. The symmetry grants DIPA some steric bulk, which helps limit where and how it reacts. In my experience, this bulk makes it less likely to cause unwanted side reactions, which means fewer headaches with purity down the line.
Anyone working with chemicals cares about molecular weight. It decides dosing, mixing ratios, and storage plans. DIPA’s molecular weight clocks in at 101.19 g/mol. That number comes from adding up the atomic weights of every atom in its formula. I’ve watched techs struggle with batches when they underestimate how much a specific compound weighs—even experienced hands slip if they don’t double-check. Commercial supply chains rely on this number to plan shipments, prevent losses, and meet legal limits. Without the right value, quality and safety both take a hit.
I’ve handled DIPA while making intermediates for medications and specialty resins. It behaves as a colorless liquid with a distinctive ammonia-like odor. Its moderate boiling point, around 84 °C, means it needs careful handling and well-ventilated storage. Folks in the industry prize its solubility in organic solvents because it blends well without gumming up the works. Handling DIPA calls for respect. Skin contact causes irritation, and vapors can sting the nose and eyes. I always recommend gloves, goggles, and fume hoods—hard lessons taught by spilled flasks and close calls.
DIPA has real value, but not every facility makes safety its top priority. Careless storage or disposal leads to leaks, which can spoil air and nearby groundwater. Years in the lab taught me that open containers or poor labeling create accidents. Regulators set exposure limits for a reason: repeated exposure leads to headaches, nausea, or chronic respiratory issues. I encourage everyone in a lab setting to stick with proper storage, personal protection, and regular safety reviews. For disposal, work with chemical waste partners who handle amines responsibly so they don’t wind up where they don’t belong.
Schools and companies both benefit from training that doesn’t skimp on the why and how of safe chemical management. Making sure anyone handling DIPA knows its weight, formula, and hazards sets a solid baseline. Labels, tracking sheets, and checklists aren’t just red tape—they catch mistakes before they snowball. More community education about chemical use and risks keeps everyone safer and makes life easier for first responders if things ever go wrong. DIPA will stay a staple for labs, but keeping its risks in check means everyone wins in the long run.
Anyone who's spent time in a lab or industrial setting knows that diisopropylamine isn’t just another bottle on the shelf. Its strong smell, flammability, and volatility earn it plenty of respect. Having worked with volatile amines, it’s clear that improper handling isn't just careless—it’s risky. Stories circulate about spills that cleared rooms, vapors that set off alarms, or worse, fires from a static spark. So, storage boils down to more than ticking regulatory boxes. It’s about looking out for people, assets, and even the next shift picking up your work.
Diisopropylamine catches fire easily. The flash point sits alarmingly low—right around room temperature. I’ve watched coworkers switch off every heat source in the area just to be safe. Any vapor in a closed space could ignite with a single spark. To keep things safe, always store this amine away from open flames, heaters, or hot surfaces. A cool, well-ventilated area makes a huge difference. Good ventilation means vapors don’t build up, and fewer headaches at the end of the day.
Plastic doesn’t always cut it. Over time, some plastics soften or crack, especially when storing strong organics. Metal containers—preferably steel or a compatible alloy—keep leaks at bay and stand up to knocks. Make sure the lid seals tightly; even a tiny gap lets vapors out. I’ve seen labs use self-closing safety cans, which don’t take much to operate even with gloves and give everyone on the floor some peace of mind.
Mixing diisopropylamine with acids or oxidizers creates trouble fast. The reaction goes exothermic, releasing dangerous gases or even starting fires. Even old hands in the lab double-check labels before putting anything close together on a shelf. Separate amines from strong acids, chlorine compounds, and peroxides. It helps to stick to color-coded or labeled shelving. Keeping things organized isn’t just tidy—it’s smart.
Clear labels prevent accidents. All it takes is one misread label or a faded sticker to set up a bad situation. Strong, readable labels with the chemical name and hazard warnings stay legible even if splashed. It sounds basic, but I’ve seen too many chemical cabinets where bottles go unmarked or markers wear off. A few extra seconds to redo a label goes a long way.
Proper goggles, gloves, and long sleeves aren’t just for show. Even retrieving a container can end badly if a seal’s weak or you've got the wrong gloves. Make sure personal protective equipment meets chemical-resistance standards, not just dust protection. Rubber or nitrile gloves hold up much better.
Stuff happens, no matter how careful you try to be. Emergency eyewash stations and spill kits nearby aren’t luxuries—they’re basic safety. Everyone in the area should know exactly where to reach the nearest eyewash and how to use an absorbent kit. I’ve seen fast, calm responses keep a minor spill from turning into a disaster.
Taking these storage steps seriously helps prevent fire, fumes, and unwanted exposure. It shows respect for everyone sharing the workspace and for the environment outside. By storing diisopropylamine correctly, you keep work running smoothly and send everyone home safe, every day.
Every day, chemicals like diisopropylamine show up in places people usually ignore—chemistry labs, factories, agriculture, even the products under the kitchen sink. Diisopropylamine helps make herbicides, rubber, pharmaceuticals, and fuel additives. Not many outside of those industries spend much time thinking about it, but there are reasons to care. From personal experience with chemical labs, even “routine” chemicals often bring more baggage than headlines suggest.
Handling diisopropylamine without working fume hoods or good gloves never turns out well. The stuff gives off strong fumes. Take a whiff, and you understand right away this isn’t just a regular solvent. Inhaling its vapors or getting it on the skin irritates eyes, nose, and throat. Spills or splashes sting on contact and leave redness or blisters. Chronic exposure makes things worse. Workers in plants with poor ventilation can face persistent coughs, headaches, and trouble breathing. The U.S. National Library of Medicine lists mucous membrane irritation and lung issues as common risks. High doses can push the body’s pH out of balance—a hit to the blood’s chemistry that takes real medical attention.
In wastewater, diisopropylamine brings problems to rivers, soil, and aquatic life. The chemical breaks down in soil and groundwater, but not always quickly. It spreads in water and can kill fish at high enough concentrations. Even in smaller amounts, studies show fish exposed to this group of amines face stunted growth or even reproductive problems. In soil, it doesn’t move fast, but it sticks around long enough to disrupt bacteria communities plants rely on. As someone who spent time volunteering at local river cleanups, I’ve seen fish kills and frog deformities that scientists traced back to chemical leaks not unlike diisopropylamine.
Companies who manufacture or use this chemical must keep strict safety measures. OSHA and similar agencies put down rules about fume hoods, respirators, gloves, and quick spill response. Still, accidents happen. Proper training keeps workers from taking shortcuts, which often cause the biggest problems. My own experience in labs taught me that even skilled people get complacent. Real protection comes from double-checking systems, teaching new staff well, and holding regular drills. Curious workers ask questions and learn early about what to do during a spill or exposure. Leadership that listens to concerns sets the tone.
Once diisopropylamine escapes into the environment, cleanup grows complicated. It only takes one storm drain to send runoff to a whole creek. Emergency crews rely on neutralizers and absorbents, not just mops and soap. Companies shifting toward closed-loop systems and regular leak checks cut down the risk. On a community level, zoning helps—keeping chemical plants away from houses, rivers, and schools. Engineers designing equipment with double-containment tanks stop many releases before they start. I’ve seen firsthand how basic public reporting gives neighbors the facts they need to monitor for contamination and push for improvements.
Diisopropylamine plays a role in many modern products and processes, but it’s not something to shrug off. A little care—right from the supplier all the way to disposal—cuts the chance of harm. Sharing real information with workers and the public keeps everyone safer, from the plant floor to the neighborhood creek.
| Names | |
| Preferred IUPAC name | N-Propan-2-ylpropan-2-amine |
| Other names |
N-isopropylpropan-2-amine
N,N-Diisopropylamine DIPA Diisopropylamine |
| Pronunciation | /daɪˌaɪsəˈprəʊpɪləˌmiːn/ |
| Identifiers | |
| CAS Number | 108-18-9 |
| 3D model (JSmol) | `3D model (JSmol)` string for **Diisopropylamine (DIPA)**: ``` CCNC(C)C ``` |
| Beilstein Reference | 997938 |
| ChEBI | CHEBI:85144 |
| ChEMBL | CHEMBL153354 |
| ChemSpider | 11422 |
| DrugBank | DB14016 |
| ECHA InfoCard | ECHA InfoCard: 100.003.168 |
| EC Number | 203-558-5 |
| Gmelin Reference | 8057 |
| KEGG | C02339 |
| MeSH | D013731 |
| PubChem CID | 8054 |
| RTECS number | JZ9100000 |
| UNII | Y14515J364 |
| UN number | UN1158 |
| CompTox Dashboard (EPA) | DTXSID9020423 |
| Properties | |
| Chemical formula | C6H15N |
| Molar mass | 129.25 g/mol |
| Appearance | Colorless transparent liquid |
| Odor | Ammonia-like |
| Density | 0.722 g/mL at 25 °C (lit.) |
| Solubility in water | Soluble |
| log P | 1.37 |
| Vapor pressure | 3.16 kPa (at 20 °C) |
| Acidity (pKa) | 36.0 |
| Basicity (pKb) | 3.05 |
| Magnetic susceptibility (χ) | -7.53×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.387 |
| Viscosity | 0.78 mPa·s (at 20°C) |
| Dipole moment | 1.29 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 311.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -175.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -4160 kJ/mol |
| Pharmacology | |
| ATC code | C04AX23 |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H302, H311, H314, H332 |
| Precautionary statements | P210, P261, P280, P302+P352, P305+P351+P338, P310 |
| NFPA 704 (fire diamond) | 1-3-0-🛢️ |
| Flash point | 52 °C |
| Autoignition temperature | 373 °C (703 °F; 646 K) |
| Explosive limits | 1.1% - 8.1% |
| Lethal dose or concentration | LD50 (oral, rat): 523 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat 520 mg/kg |
| NIOSH | WS4550000 |
| PEL (Permissible) | PEL: 5 ppm |
| REL (Recommended) | 200 mg/L |
| IDLH (Immediate danger) | 200 ppm |
| Related compounds | |
| Related compounds |
Dicyclohexylamine
Dipropylamine Diethylamine Dimethylamine N-Methylisopropylamine Sec-butylamine Triethylamine |
