Diisopropylethylamine, known to many lab folks as Hünig’s base, found its place on the shelf at a time when synthetic organic chemistry was pushing the envelope. Researchers in the 1950s and 60s, hungry for new compounds that could sharpen yields, stumbled onto it during acid scavenging and alkylation explorations. The compound, with its crowded nitrogen center, offered shifts in basicity and hindered reactivity that mainstream amines couldn’t match. Labs looking to beat side-reactions found it worked better than bulky amines like triethylamine. Chemists saw a base that wouldn’t get in the way, and the industry picked up on it, bringing diisopropylethylamine to scale for peptide synthesis and pharma pipelines.
Diisopropylethylamine usually rolls out as a clear, pungent liquid sold in steel drums or smaller glass bottles, depending on the buyer’s needs. Chemical suppliers push its value for consistent basicity and low nucleophilicity. Typical shipments come with purity checks around 99%, since impurities trip up syntheses and lead to regulatory headaches. Most bottles carry hazard labels for flammability and skin irritation—practically a fixture on every organic chemist’s bench. Its known uses run from classical peptide couplings to stubborn esterifications, but it thrives best wherever gentle basicity and minimal side reactions matter most.
In the lab, diisopropylethylamine shows up as a colorless liquid, with a boiling point sitting near 127 to 129°C. Its density sits close to 0.742 g/cm³, showing up light and mobile in the hand, with a sharp, ammonia-like smell that warns even seasoned chemists to handle it quickly. Its low freezing point ensures storage at room temperature rarely runs into problems, while its miscibility in organic solvents like dichloromethane and acetonitrile makes it versatile in multi-step reactions. Flash point checks put it flammable, so open flames and heating mantles keep their distance when this liquid’s in play.
Every bottle or drum comes with technical data like purity, water content, and residual amine analysis as a standard check. Most manufacturers list the CAS number 7087-68-5 front and center, tagging it with warning symbols for both acute toxicity and harmful vapors. GHS-compliant labeling calls out standard hazards: H226 (flammable liquid), H302 (harmful if swallowed), and H315 (causes skin irritation). Safety data sheets hit on flash point, precautions for eye contact, and recommended PPE. Trace aldehyde content and water contamination feature in technical specs, since these throw off delicate couplings or cause batch-to-batch headaches. Vendors highlight compliance with ISO and REACH standards, making it easier for buyers doing cross-border supply.
Industrially, folks start with diisopropylamine and react it with ethyl bromide or ethyl chloride in aprotic solvents like acetonitrile or DMF. The reaction uses a base such as sodium or potassium carbonate to mop up acid as the alkylation runs. Distillation under vacuum rids the mix of byproducts and unreacted starting materials, leaving high-purity diisopropylethylamine behind. At the bench scale, the process doesn’t change much, but careful washing and drying of organics become a necessity, as small quantities amplify impurities and degrade reaction performance.
Chemists reach for diisopropylethylamine as a base in nucleophilic substitution or acylation reactions because its steric bulk shields the nitrogen from reacting. This trait prevents formation of unwanted byproducts, especially where other amines would jump into the fray and grab an acyl group or attack an electrophile. In peptide synthesis, it excels in coupling steps by accepting protons and sweeping away acid generated in the reaction. Its mildness opens up regioselective transformations and complex, multi-step syntheses seen in pharmaceutical research. Rarely does it find use as a nucleophile or reductant, showing the discipline chemists look for in a non-reactive base. The market keeps an eye out for modified amines with similar performance but improved environmental or handling profiles, and chemists still chase the perfect balance between basicity, solubility, and reactivity.
The chemical world gives diisopropylethylamine many handles: Hünig’s base, DIPEA, N,N-diisopropylethylamine, or 2,6-diisopropyl-N-ethylethanamine. Catalogs may list it as DIPEA or even under tradenames coined by specific suppliers. Synonym awareness matters in regulatory approvals and supply chain checks—mislabeling leads to everything from regulatory delays to disastrous cross-contamination. For researchers and buyers, consistency in naming helps streamline orders and avoid confusion, especially when projects jump international borders.
Working with diisopropylethylamine demands basic chemical safety, starting with gloves and splash-proof goggles. Its vapors irritate eyes and lungs, triggering quick evacuations if a spill goes unchecked. In my own experience, neglecting the fume hood means long-lasting reminders of its odor clinging to the lab coat. Fire safety enters the picture, as a careless spark near spilled liquid puts the whole team at risk of flash fires. Emergency protocols lean on eyewash stations and chemical spill kits. Storage in tightly-sealed bottles, away from strong acids and oxidizers, prevents unexpected reactions in crowded chemical cupboards. Training and safety culture dominate discussions in most labs using this base—newcomers run through handling drills to avoid mishaps that can stall ongoing research.
Pharmaceutical labs look to diisopropylethylamine for coupling reactions during drug discovery and scale-up. It streamlines peptide assembly, offering a clean alternative to less selective bases without dragging down yields. The agrochemical industry uses it for creating complex molecules that safeguard crops or boost soil health. Academic labs turn to it for organic synthesis education, teaching students about acid-base theory and reaction selectivity. Active development work pursues greener alternatives and recycling options, as environmental rules tighten on solvent and amine waste. Its signature as a sterically-hindered base keeps it featured in journals describing new synthetic pathways and total synthesis projects.
Research communities continue to probe how diisopropylethylamine interacts with new coupling reagents and flow chemistry setups. Companies chase derivatives with tweaked solubility and decreased toxicity, aiming to keep performance without the headaches of hazardous shipping. Analytical chemists track breakdown products in large-scale reactions to help manufacturers extend shelf life and reduce batch rejection. The rise of continuous manufacturing highlights its role in scalable base-driven transformations, as process chemists search for ways to minimize amine consumption without sacrificing reaction pace. Collaboration between academia and industry keeps pushing the boundaries, with dozens of recent patents outlining new uses in both pharma and specialty chemistry.
Laboratory studies on diisopropylethylamine point to hazards mostly linked to inhalation and skin contact—minor compared to heavy metals and some alkylating agents, but not trivial. Acute exposure tends to cause eye and mucosal irritation, while chronic mishandling can lead to dermatitis and headaches. Animal studies show moderate oral toxicity, but the compound is not flagged as a strong carcinogen or mutagen. Wastewater from manufacturing and labs raises concerns, as the amine can disrupt water quality and local ecosystems. Researchers develop new treatment strategies—activated carbon adsorption and advanced oxidizing protocols get plenty of attention to reduce environmental impacts. In many labs, waste stewardship programs tackle leftover base as part of broader sustainability mandates.
The future for diisopropylethylamine looks tied to regulatory shifts and green chemistry goals. Busy labs want safer, less volatile alternatives that keep the clean reaction profiles DIPEA delivers. Improvements in bulk synthesis promise lower costs and fewer impurities, benefitting contract manufacturers and small startups. Solvent-free or aqueous-based processes attract investment, as big pharma and specialty chemical players search for greener production lines. The push for sustainable chemistry means rising demand for recovery and recycling systems tailored to hindered amines. Collaboration between material scientists and synthetic chemists seeks to develop new functionalized amines that retain the perks of DIPEA while cutting environmental burdens. The story of this base keeps evolving—chemists across the globe keep learning, adapting, and searching for smarter, safer ways to drive chemical innovation forward.
Diisopropylethylamine shows up almost everywhere you look in labs focused on organic chemistry. Folks in research outfits, as well as at big pharmaceutical companies, rely on it because it does one key job better than most others: it can accept protons easily, but it won’t get in the way through other chemical reactions. It’s this blend of muscle and selectivity that pushes it to the top of every chemist’s toolkit.
The main thing you see with diisopropylethylamine is its role as a base. Not a flashy role, but a crucial one. For example, in peptide synthesis, it steps in to neutralize acids, allowing molecules to join together without breaking down. You’ll spot it in the background during steps where delicate intermediates demand an easy touch. Because it doesn’t push itself into side reactions, researchers end up with cleaner products and save time they’d otherwise spend purifying samples.
Drug makers spend years trying to trim down the time it takes to move a candidate from the bench to the clinic. In this space, diisopropylethylamine comes into play by giving chemists better control at each step. For instance, it helps build key structures in antiviral drugs or anti-cancer agents. Its ability to “stay out of the way” lets drug designers build molecules that hit their targets without racking up unwanted byproducts. That reliability lowers the cost and headache during quality checks.
Handling chemicals with strong smells and irritating vapors calls for care, and diisopropylethylamine isn’t any different. I’ve seen too many people ignore proper ventilation or forget gloves, thinking they’ll be fine for a quick synthesis. These shortcuts don’t fly when you remember how easily this chemical can irritate the eyes and the lungs. Sticking to gloves, goggles, and fume hoods keeps everyone focused on the experiment and not on a trip to the sink. In teaching labs, safety briefings that go beyond the basics make sure everyone knows the rules before a bottle gets opened.
The push for cleaner, greener chemistry stands out as one area where diisopropylethylamine sparks debates. Its low boiling point and volatility raise flags about workplace exposures and environmental footprints. Some teams experiment with less volatile bases, but most keep coming back to diisopropylethylamine for its reliability. Efforts to recycle solvents and use containment gear help cut down on emissions, but the story isn’t finished. Teams looking to lower their impact have started to compare the chemical’s overall footprint versus possible substitutes, nudged along by new rules and market pressures that reward sustainability.
Smart use of diisopropylethylamine boils down to experience and a willingness to adapt. Training, good lab habits, and a watchful eye for new research keep it valuable for years to come. Anyone working with specialty chemicals owes it to themselves and their co-workers to keep up with new safety data, stay informed on greener options, and keep best practices alive. It’s not just the reaction in the flask that counts; it’s how we choose to get there.
Every experienced chemist recognizes diisopropylethylamine from a distance. In the lab, people often call it DIPEA or Hünig’s base, a nod to its strong presence as an organic base. The chemical formula, C8H19N, may sound simple, but it tells a story familiar to anyone who has ever touched a beaker or tried to solve an organic synthesis problem without tears of frustration.
Chemical formulas answer more than just textbook questions. When handling a bottle of DIPEA, knowing C8H19N means a researcher can balance a reaction without unnecessary guesswork. The formula reveals the presence of eight carbon atoms, nineteen hydrogen atoms, and one nitrogen atom—reminding those doing a late-night titration that every molecule has the muscle to push specific chemical reactions without causing troublesome byproducts.
Several years ago, I found myself fumbling through an organic synthesis in a poorly ventilated academic lab, with DIPEA as the "fix-all" base. The formula C8H19N was scrawled on the bottle in fading marker. I knew from experience that even a slight miscalculation could result in waste or, worse, dangerous gas. The structure itself—two isopropyl groups and one ethyl stuck to a central nitrogen—makes this amine especially bulky. That kept it from swooping in and reacting where it shouldn't, earning its reputation as a non-nucleophilic, reliable partner for peptide coupling and other delicate procedures.
Real-world chemistry doesn’t leave much room for error. DIPEA’s chemical arrangement steers clear of forming unwanted bonds. No chemist wants their base to become a participant instead of an observer, and the formula C8H19N proves why DIPEA stays on the sidelines. It stands as the “go-to” whenever you need to mop up acid without making extra work. I’ve watched colleagues reach for it in pharmaceutical R&D settings more times than I can count, knowing their reactions would finish cleaner with fewer greasy side products clogging purification steps.
The same formula that brings efficiency can pose risks if respect drops. DIPEA has a sharp odor and reacts if mishandled. Simple actions—wearing gloves, using a fume hood, storing it away from incompatible chemicals—keep the lab safe. This isn’t scaremongering; it's the result of hands-on mishaps shared every semester in chemical safety talks. Understanding C8H19N, beyond the numbers, means knowing its flammability and the need for proper disposal procedures to protect both health and the environment.
There’s no shortcut to safety and performance in synthesis. DIPEA, with its formula C8H19N, reminds me that understanding the basics—the atoms, the functional groups, even the way the structure bends and twists—feeds better outcomes in research and production. Green chemistry pushes us to use the right amount, reduce waste, and choose safer substitutes if our application allows. Education bolsters this shift. Sharing real lab experience, mistakes, and lessons ensures everyone who handles DIPEA sees more than numbers on a label. Chemistry gains not just from perfect formulas, but from the careful hands and honest stories behind them.
You never really forget the sharp smell that hits your nose the moment a bottle of Diisopropylethylamine cracks open. This stuff, often called Hunig’s base, isn’t just another chemical for a back shelf. With its strong ammonia-like odor and tendency to sting the skin, Diisopropylethylamine grabs your attention. At the bench, nobody wants a trip to the ER from a preventable spill. Direct experience reminds anyone working in chemistry: the best day is a safe day.
Accidental splashes hurt. Beyond that, vapors can make you cough or worse, cause breathing problems in a badly ventilated room. If even a drop lands on bare skin, a quick burn crops up—something I learned firsthand my first summer in the lab. Eyes come out especially vulnerable. Like many organic bases, just the fumes can cause irritation. The Centers for Disease Control and Prevention flag long-term exposure risks and point to proper handling as key to protecting your lungs, skin, and vision.
Gloves matter most; nitrile usually holds up well against amines. No point in risking unknown breaks with latex. A face shield adds another layer when pouring from larger bottles, and safety goggles beat regular glasses every time. Lab coats with long sleeves shield every square inch they cover. Even for folks used to relaxed policies, closed-toe shoes become non-negotiable once you smell the vapors.
A chemical fume hood isn’t just a fancy box. I always reach for the sash, just high enough to allow my arms in, keeping fumes away from my face. Leaving a reaction open on the bench can fill a room in minutes with that sharp odor—a clear warning to never get careless.
Hunig’s base doesn’t play nice with acids. Keeping acids and amines far apart prevents anything from boiling over. I check chemical labels twice before returning bottles to their shelves. Keeping containers tightly sealed cuts down on vapor buildup and spoilage. For long-term storage, cool and dry trumps anywhere that heats up with sunlight or equipment.
If a spill happens, absorbent pads rated for solvents make cleanup straightforward. Flushing skin quickly with water made all the difference in my own mishap—no soap at first, just lots of water. Eyewash stations and showers belong within seconds of the lab bench. A reminder sign near every workstation keeps everyone alert.
Chemistry can turn dangerous fast. Relying only on old habits encourages shortcuts; up-to-date training humbles everyone to the real risks. Each year, I walk through chemical safety modules and hands-on spill response drills. New graduates and seasoned researchers share their stories to highlight lessons learned. These conversations shape a culture where protecting yourself and your coworkers beats any shortcut.
Institutions benefit by stocking the right personal protective equipment and by marking clear storage zones. Supervisors who enforce standards protect everyone. Emergency procedures make a real difference when every second counts. I’d take a day reviewing response plans over one spent in a hospital bed. Safety with Diisopropylethylamine depends on keeping hazards and solutions in plain sight, so everyone leaves the lab as healthy as they walked in.
Every chemist knows the anxiety that can come with storing odd-smelling, tricky reagents. Diisopropylethylamine (DIPEA) sits on many lab benches, usually in a glass bottle with a red cap. Some of us call it Hunig's base, but whatever the name, any misstep can lead to ruined reactions, safety scares, and wasted budgets. Most mistakes stem from skipping small details that add up over time.
DIPEA has a pungent amine smell—once you open that bottle, you never forget it. Few would call it pleasant, but its role in synthesis deservedly makes it common in both research and industry. The stuff boils at just under 130°C and stays liquid at any room temperature, but it catches fire pretty easily. That flashes warning lights for anyone handling or storing it.
So the most immediate risk is fire. Store DIPEA in a cool place, away from sunlight, heat sources, and ignition points. I’ve seen labs get lazy, stashing bases near Bunsen burners or hot plates for convenience. A single spark could turn that convenience into an accident. If you’re managing larger amounts, a flammable chemicals cabinet is non-negotiable—any safety officer will confirm this.
Moisture messes with DIPEA. It’s hygroscopic, soaking up water from the air and going bad if humidity invades the bottle. Damp DIPEA can disrupt sensitive syntheses, making yields unpredictable. Tight seals save a lot of frustration. Screw the cap down each time and use PTFE liners or septa if available. In my experience, storing a little desiccant bag inside the bottle or keeping the container in a dry box blocks most problems before they start.
Storing under an inert gas like nitrogen offers an extra layer for demanding work, such as scale-up synthesis for pharmaceuticals. While everyday bench use doesn’t always call for this, the best labs set up Schlenk lines or use glove boxes for the really critical steps.
I’ve seen DIPEA yellow and get sticky after sitting out too long. Oxygen and light can slowly degrade it, especially over months. While no one enjoys fumbling with brown bottles, they reduce light-sensitive breakdown. Label the date you open each bottle. If an old batch starts to look or smell off, don’t gamble on purity: order fresh stock or distil before use.
DIPEA’s fumes can sting your nose, eyes, and throat. I made the mistake as a grad student of opening a bottle in a poorly ventilated space. Lessons learned: handle it in a fume hood, and keep personal protective equipment on hand—goggles, gloves, even a simple lab coat. Easy access to spill kits also doesn’t hurt.
What about leftover DIPEA or used containers? Never pour it down the drain. The law’s clear, and so is the science—amines contaminate waterways and play havoc with environmental health. Find a certified hazardous waste program and follow disposal protocols. Universities and companies often have specialists for this, and their advice trumps internet shortcuts every time.
Good storage habits save money, time, and stress. DIPEA sticks around in labs and factories for solid reasons, but it pays to be proactive. Flammable liquid cabinets, dry boxes, fume hoods, and meticulous labeling all work together. Sharing tips and stories with colleagues—both good and bad—keeps everyone ahead of trouble. A little planning and respect for the basics go farther than any fancy safety sign on the wall.
Anyone who spends a bit of time at the bench learns early that chemicals bring their baggage. Diisopropylethylamine (DIPEA, often called “Hunig’s base”) holds a reputation for being pretty friendly in a variety of reactions. It’s all over peptide synthesis protocols and popped up in routines when chemists wanted a strong, non-nucleophilic base, especially where other amines got too grabby. But somehow, there’s a vibe out there suggesting it can just be thrown at anything with no issues. That would make life easy, but chemistry rarely gives out freebies like that.
It’s easy to get lulled into thinking a “universal” solvent base exists, especially after getting decent results in a few common solvents—think dichloromethane, acetonitrile, toluene, THF. DIPEA gets along well in those. Problems start cropping up somewhere in the less-traveled corners, though. Try suspending it with a protic solvent like water and trouble follows: hydrolysis can start biting. With alcohols, unexpected alkylation sometimes rears up if the reaction gets warm, and ethers take on the risk of peroxide formation. There are also those not-so-obvious moments, like finding out DIPEA gets oxidized in the open air (with the pesky smell to prove it), or that impurities in a solvent trigger reactions you didn’t even plan for.
Talking about reagents, DIPEA’s “non-nucleophilic” reputation needs some qualifying: in theory, it isn’t supposed to step in as a nucleophile in most cases, but stories emerge from crowded synthetic labs where it grabs onto acyl chlorides or forms salts unexpectedly with strong acids you thought were stable. And then certain metals—let’s say copper or silver—don’t really enjoy DIPEA’s company, as chelation or reduction starts making a mess out of intended outcomes. Some oxidizers just chew right through amines, turning the benign base into something that ruins yields. Drying agents and glassware preparation can also trace their own issues; a few minutes around strong Lewis acids, and the reaction gets noisy quickly.
Slipping into the “DIPEA works with everything” mindset burns time and material. I once watched a column become a nightmare because residual DIPEA formed a stubborn salt that just would not budge. Worse, I’ve seen products degrade overnight after DIPEA met a mild oxidant left in the system from the last run. Labs working on expensive intermediates for pharma or complex natural product synthesis feel these losses in their bottom line, not just in broken glassware. Reliable results in scale-up demand fewer surprises, and that can come to a halt if someone assumes this reagent is always compatible. Side reactions steal precious product and muddy up purification—never a great way to spend a Friday evening.
Before dropping DIPEA into a new mix, it’s worth checking the compatibility tables, running a small test batch, or digging up old literature. Looking up sources that list known incompatibilities helps. A walk through SciFinder or Reaxys reveals published landmines: unwanted reactions with oxidizers, strong electrophiles, or with specific transition metals. Experienced chemists usually rely on a scrappy checklist: watch solvents for peroxide risk, cover bases for possible acid-base or redox side chemistry, and document everything for the next person. These steps may slow things down, but they always win out over cross-your-fingers chemistry.
| Names | |
| Preferred IUPAC name | N-ethyldi(propan-2-yl)amine |
| Other names |
DIPEA
Hünig’s base N,N-Diisopropylethylamine Diisopropyl ethylamine N-Ethyl-N,N-diisopropylamine |
| Pronunciation | /daɪˌaɪsəˌproʊpɪlˈɛθɪlˌæmin/ |
| Identifiers | |
| CAS Number | 7087-68-5 |
| Beilstein Reference | 136793 |
| ChEBI | CHEBI:85258 |
| ChEMBL | CHEMBL254984 |
| ChemSpider | 5416 |
| DrugBank | DB08357 |
| ECHA InfoCard | 032-019-00-3 |
| EC Number | 202-940-0 |
| Gmelin Reference | 82161 |
| KEGG | C06086 |
| MeSH | D017766 |
| PubChem CID | 6057 |
| RTECS number | YT3225000 |
| UNII | HZG39ZF8H1 |
| UN number | UN1158 |
| CompTox Dashboard (EPA) | urn:CST:0QZ10G6S8U |
| Properties | |
| Chemical formula | C8H19N |
| Molar mass | 129.24 g/mol |
| Appearance | Colorless liquid |
| Odor | Amine-like |
| Density | 0.742 g/mL at 25 °C |
| Solubility in water | Miscible |
| log P | 2.9 |
| Vapor pressure | 0.5 hPa (20 °C) |
| Acidity (pKa) | 10.75 |
| Basicity (pKb) | 3.0 |
| Magnetic susceptibility (χ) | -44.7e-6 cm³/mol |
| Refractive index (nD) | 1.394 |
| Viscosity | 2.62 mPa·s (20 °C) |
| Dipole moment | 2.40 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 296.5 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –236.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -4785.7 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS07,GHS08 |
| Signal word | Danger |
| Hazard statements | H226, H302, H312, H314, H332 |
| Precautionary statements | P210, P261, P264, P271, P280, P301+P312, P303+P361+P353, P304+P340, P305+P351+P338, P312, P330, P337+P313, P370+P378, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 1-3-0 |
| Flash point | 40 °C |
| Autoignition temperature | 432 °C |
| Explosive limits | Explosive limits: 1.1–6.0% |
| Lethal dose or concentration | LD50 (oral, rat): 1160 mg/kg |
| LD50 (median dose) | LD50 (oral, rat): 926 mg/kg |
| NIOSH | NJ0175000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 5 mg/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Triethylamine
Diisopropylamine N,N-Diisopropylmethylamine |
