© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
In the early twentieth century, chemists started taking a hard look at secondary alcohols like 2-butanol. Back then, industries leaned heavily on distillation and fermentation for alcohol production. Early uses of 2-butanol came from natural sources—like the mash left behind from cereal grains—until synthetic approaches took over. By the 1930s, companies in the United States and Europe adopted robust petrochemical refining to convert butenes, a simple byproduct of oil cracking, straight into 2-butanol. This shift brought about a reliable, pure product on a scale suited to manufacturing. As chemical companies competed, process tweaks made the substance cheaper and more available, bringing 2-butanol from obscure laboratory shelf to commercial staple. These advances didn’t just help big factories but also small labs and educators, eager to work with a secondary alcohol that didn’t break the bank.
Scrolling through standard lab catalogs, 2-butanol (anhydrous 99.5%) stands out thanks to its wide applications and dependable grade. This particular variant—anhydrous, meaning essentially water-free—delivers the reliability that synthetic pathways and sensitive reactions require. Removing water boosts shelf life and prevents headaches like unwanted by-products or explosions in metal-catalyzed chemistry. Whether you’re working in pharmaceuticals, coatings, or fine chemicals, a drum of high-purity 2-butanol means not sweating about extra water fouling up your preparations.
2-Butanol holds the chemical formula C4H10O and a molecular weight just above seventy-four grams per mole. At room temperature, it pours as a colorless liquid with a flammable flair. Its characteristic, sharp odor gives away a strong, volatile personality, much like rubbing alcohol but with a twist. This chemical boils just under 100°C, putting it squarely inside practical lab use for distillation. People sometimes mistake its density and viscosity as typical for an alcohol, but subtle differences—like a specific gravity near 0.81—hint at its unique placement among secondary alcohols. In water, it dissolves well enough at room temperature, though not quite as happily as its smaller cousin, ethanol. Its flash point, floating around 24°C, means storing and handling call for respect.
A bottle labeled 2-butanol (anhydrous 99.5%) doesn’t just brag purity for the sake of posterity. That number shows how well the cleaning steps squeezed out any trace of water or other alcohols. Typical bottles display an Assay of not less than 99.5%, using gas chromatography for accuracy. Impurities like isobutanol, propanol, or acetone usually show up only in parts per million—so low they don’t interfere with most reactions. Specific gravity, boiling range, and refractive index show up on the COA, lines that matter for regulatory and in-house acceptance. Correct hazard pictograms and compliance with globally harmonized labeling, plus UN packing group labeling for transport, reflect shifts in workplace safety expectations. Every lab technician and logistics worker who’s handled a leaky drum knows why these marks exist.
Modern routes for 2-butanol production use petrochemical butenes and steam. Companies feed butene gas into reactors with water, often using acid catalysts, such as sulfuric acid or resins, at elevated temperatures and pressure. This hydration process doesn’t come without its engineering problems—temperature swings matter, side reactions show up, and catalyst life keeps plant workers on their toes. After reaction, the mix goes through separation, distillation, and drying stages. Early batches often contain a stubborn trace of water, so companies use molecular sieves or azeotropic drying. Each ton pulled off the line not only reflects clever chemistry but close coordination between process engineers, quality controllers, and plant operators.
2-Butanol often stands as a workhorse starting point for synthesis. Dehydrating it using acid generates butenes, useful as intermediates in other chemical families. It reacts with strong oxidizers to form methyl ethyl ketone (MEK), a solvent valued in polymers and paints. Small tweaks in temperature and pressure can tilt reactions one way or another, opening routes to esters with carboxylic acids or chlorides with hydrochloric acid in the presence of a catalyst. In research settings, modifications using 2-butanol provide a playground for exploring stereochemistry, as the molecule has a chiral center—meaning it can exist as distinct right- and left-handed forms.
2-Butanol hides under a variety of monikers. Some call it sec-butanol; others go with sec-butyl alcohol. IUPAC formalists often insist on the whole “butan-2-ol,” rubbing shoulders with its registry numbers—CAS 78-92-2. On MSDS sheets, expect to see these synonyms cross-referenced alongside international trade names like SBA, 2-hydroxybutane, or methyl ethyl carbinol. Checking the label twice can save a heap of confusion, especially with similar-sounding chemicals in the mix.
There’s no substitute for vigilance around volatile organics like 2-butanol. Classed as a flammable liquid, it demands low-temperature storage, spark-proof equipment, and sensible PPE. Splashing it in your eyes or on skin brings out the worst in chemical burns, and breathing in vapor triggers headaches, drowsiness, or even narcosis in poorly ventilated spaces. Operational procedures matter. The Occupational Safety and Health Administration (OSHA) and EU REACH standards draw clear lines for permissible exposure, spill cleanup, and waste disposal. I’ve heard more than one story about someone propping open a chemical fridge and watching a drum of 2-butanol swell during a hot spell—constant reminders of the need to follow rules and handle with respect, not bravado. Training, labeling, and accessible MSDS data keep labs safe and work moving forward.
2-Butanol pulls weight as both a solvent and a chemical intermediate. Makers of paints, coatings, and inks turn to it for its moderate volatility, which enables smooth finishes and quick drying. In the pharmaceutical sector, secondary alcohols like this play a crucial part in synthesizing medicines and flavoring agents, where selectivity and purity make a big difference. Other uses include making plasticizers for flexible plastics, aiding extraction processes, and acting as a sample preparation agent in analytical chemistry. In the agriculture world, 2-butanol helps formulate certain pesticides and herbicides, showing up in formulations that require quick evaporation. Its utility often depends not on being the star ingredient, but on quietly enabling efficient workflows across sectors.
Research on 2-butanol keeps pushing boundaries, especially where sustainability and green chemistry come into play. Forward-looking labs now explore enzymatic or microbial production using renewable feedstocks like cellulose and agricultural waste, reducing dependency on petrochemicals. Chiral purity remains hot—scientists work to isolate and use only one enantiomer, which can change a drug from inactive to potent. In analytical chemistry, advances like more sensitive gas chromatography and mass spectrometry provide sharper answers about purity and trace contaminants. As regulatory limits tighten, research pivots to safer handling systems and automation to minimize human risk in industry settings. Each improvement in production or analytical techniques spills back into other chemicals, raising standards across the board.
Over the years, studies have addressed the health risks of 2-butanol exposure. Toxicologists point to its potential for central nervous system effects, comparing it to isopropanol and ethanol but noting a greater tendency for respiratory irritation. Chronic contact brings out skin and eye problems—so the need for gloves and face protection stands on solid ground. In animal studies, high concentrations led to intoxication and fatalities, but workers in industrial settings rarely hit those levels thanks to regulated air monitoring and ventilated workstations. Wastewater discharge guidelines date back decades after fish kills near manufacturing plants highlighted real-world risks from accidental spills. These hard lessons prompted better wastewater treatment and storage protocols, reflected today in routine environmental compliance.
Looking at the decade ahead, 2-butanol faces both challenges and opportunities. The global push for renewable and circular chemistry means companies will keep searching for greener production methods, whether through advanced fermentation or smarter catalysis. Regulations on chemical emissions keep tightening, urging plants and users to innovate in how they capture and recycle organics. Demand from coatings, pharmaceuticals, and agrochemicals looks steady, but newcomers in energy—biobutanol as a fuel blend—promise fresh markets if technical hurdles fall. Digital monitoring and automation in storage and delivery will help catch leaks and spills before they make news, tempering the risks tied to large volumes. The story of 2-butanol, like many industrial chemicals, remains one of adaptation: practical necessity balanced with ongoing responsibility to people and the planet.
Step onto the floor of any chemical plant, and the barrels marked “2-Butanol” tell a story of versatility and value. Industries need solvents that do more than just dissolve materials—they look for performance, safety margins, and consistency. With its high purity and lower water content, 2-Butanol (Anhydrous 99.5%) fits the bill for projects where even a little contamination throws everything off.
Walking through an auto body shop, the use of 2-Butanol in paint thinners stands out. Its structure helps strip old coatings and blend new ones. This approach protects surfaces during application and delivers more reliable results once the paint dries. Painters and manufacturers have leaned on it for its drying rate and the finish it leaves behind.
Batch after batch of colorant passes through equipment where 2-Butanol keeps everything moving. Printing businesses need bright, even colors. In combination with other solvents, 2-Butanol contributes to inks that dry at the right speed. This means printed books, magazines, and packaging avoid smearing and fading issues.
Behind most perfumes and processed foods, you find a web of chemical reactions. 2-Butanol steps in as an intermediate for different esters found in fragrances and artificial flavors. Production lines rely on its purity to make consistent products that meet regulatory standards. Any slip in quality might affect a whole lot of product, so producers keep a close eye on solvent grades.
Chemists in labs reach for anhydrous solvents to run controlled experiments and sample analyses. 2-Butanol, with its high purity, supports techniques like chromatography and extractions. Even the tiniest bit of water can skew data, so the value here sits in its dryness as much as its solvency.
It pays to remember that substances like 2-Butanol come with risks. Inhalation, skin contact, or swallowing could make people sick if no precautions are in place. Employers train workers on safe storage and good ventilation. Factories swap standard solvents for high-purity versions to cut down on byproducts and unwanted exposure. This attention helps build trust and safety, fewer chemicals in the air, and less mess during cleanup.
Some companies now search for replacements that don’t carry as many hazards or are less polluting. This takes investment in research and a willingness to rethink old standards. Waste management improvements and closed-system equipment also help. Making 2-Butanol cleaner and safer might not attract headlines, but small adjustments help protect workers and the wider world.
Research teams continue to push, looking for ways to cut emissions or stretch the lifespan of solvents like 2-Butanol. Equipment upgrades, creative recycling methods, and close monitoring of purity all weigh in. With every change, industry gets a bit closer to a process that serves modern needs and respects the environment.
Dealing with 2-Butanol in its anhydrous form shouldn’t feel like flipping a switch on autopilot. It’s a clear, flammable liquid with a distinct odor, and it doesn’t wait for mistakes before things go wrong. In everyday labs or industrial spaces, even seasoned professionals have had surprise spills or found themselves coughing after a forgotten sniff. It only takes one lapse in judgment or routine, and health can get put at risk.
Goggles aren’t just for show. Splashing a drop of this stuff into your eyes burns like nothing else—the pain and potential damage aren’t worth skipping protection. Lab coats and gloves form an obvious line of defense. Nitrile gloves handle butanol without breaking down quickly. Bare skin absorbs chemicals faster than people think, and a strong solvent like 2-Butanol goes right through some glove materials. There’s no comfort in thinking, "skin exposure is minimal;" those who’ve actually handled spills feel the tingling, sometimes with lingering effects.
Chemical fume hoods aren’t just for fancy research sponsorships. In small rooms, fumes from 2-Butanol build up fast. Exposure leads to headaches, dizziness, or worse. The American Conference of Governmental Industrial Hygienists (ACGIH) recommends keeping air levels below 15 ppm. People who’ve worked in poorly ventilated basements or corners soon learn the difference with their own lungs. Reliable exhaust fans, air circulation, and fume extraction save health and keep inspections headache-free.
2-Butanol takes ignition seriously. Its flash point—just 24°C—means a lighter or spark could set off a fire with little warning. It needs to be kept away from open flames, hot surfaces, and static discharge. Storage in tightly closed, grounded containers means less waking up at night worrying about potential explosions. Fire extinguishers—especially those rated for Class B fires (flammables)—should never collect dust in these spaces. Colleagues who’ve watched solvent fires up close never forget the panic and near misses.
Most people remember their first chemical spill by heart. Quick steps—evacuate the area, inform others, and grab spill kits packed with absorbent pads and neutralizers—matter more than waiting for a manager’s call. The material’s safety data sheet (SDS) explains exactly what to use. The best-trained teams regularly run practice drills, so that spills trigger action, not panic.
Pouring leftovers down the drain sounds tempting at the end of a long day, but it brings legal risk and environmental damage. Proper labeling of waste bottles, keeping incompatible chemicals separated, and using secondary containment for leaky containers is responsible and legally required. Local authorities and environmental agencies care about solvent disposal; stories of fines and costly cleanups remind everyone that shortcuts haunt more than just reputations.
Nothing replaces direct experience, but nobody needs a scar to learn respect. Routine training sessions, honest reviews of near misses, and sharing stories about what’s gone wrong can keep people on high alert. Teams that keep the conversation ongoing act faster and keep each other safe. Learning from mistakes, instead of hiding them, turns near disasters into real lessons. Respect for chemicals like 2-Butanol grows not just from rules, but from stories and teamwork.
Spending years working around laboratories, I’ve seen good storage habits make all the difference between a safe workspace and a risky one. 2-Butanol, especially anhydrous and this pure, brings its own challenges. It’s flammable. It releases vapors. It likes to draw water from the air. Treat it casually and the risks stack up: fire, health concerns, product loss.
2-Butanol anhydrous holds its grade by staying away from moisture. Exposure wrecks purity fast. In practice, good storage starts with airtight containers, preferably those made from materials resistant to solvent action, like glass or high-quality, compatible plastics. Never leave containers open—humidity sneaks in quicker than expected. Even minor moisture dents performance in industrial processes or research.
Tucking it onto just any shelf brings risk. A flammable liquid belongs in a dedicated chemical storage cabinet, one clearly labeled and approved for handling volatile organics. No exceptions. A fire-resistant enclosure, grounded and equipped with spill containment features, lowers odds of spreading a problem far beyond one bottle. Make sure storage areas offer enough ventilation, since even trace vapors build up over time. A fan that throws solvent-laden air right back into a room fails the safety test.
Many labs use hot surfaces—some heated up without anyone noticing. Flammable vapor lingers near 2-butanol, especially at room temperature or higher. One stray spark, one forgotten hot plate, and things go south. Store well away from heat sources, and keep ignition-proof equipment in close proximity. Good housekeeping habits keep spills from accumulating under shelving.
Lots of accidents start with “I thought that was water.” Clear, standardized labels pay off every single time. In fast-paced environments, people forget what’s in the flask or bottle. A clear date, concentration, and hazard symbols serve as an early warning for anyone handling storage or disposal. Safety Data Sheets belong right by the storage area—out of the filing cabinet and close to the chemicals.
Routine storage checks work best with good personal protection. Even the cleanest process risks a splash or a broken bottle. In my experience, a sturdy pair of gloves and safety goggles beat bandaids and eyewash stations every time. Anyone inspecting, moving, or distributing 2-butanol should suit up—not just leave safety gear for special jobs.
Even with perfect storage, accidents still happen. Spill kits fit for solvents, fire extinguishers suitable for flammables, and clear escape routes complete a solid storage strategy. Regular drills and honest safety talks create habits that stand up under stress.
I’ve watched labs lean on long checklists, yet real safety shows up in daily choices. Training and a sense of personal investment cut through complacency. It helps to walk the storage area with fresh eyes—ask, “Would I trust my own health to these habits?” By focusing on airtight containment, fire safety, clear labels, handy PPE, and spill readiness, you raise the odds of everyone heading home safely after a long day at work.
2-Butanol goes by a few nicknames, but what matters at the bench or in storage is what it can do. It’s a clear liquid that comes with a fairly sharp, sweet odor. Ask anyone working in a laboratory, and they’ll say you can smell its presence before seeing the label. This chemical helps in a range of syntheses and has been useful as a solvent long before digital safety data sheets made the rounds. Still, lurking in the background are genuine hazards that deserve more than a quick scan over the warning label.
Flammable means trouble in real-life settings where heat, sparks, or a careless hand can turn a small bottle into a local emergency. 2-Butanol falls squarely into this category, with a flash point in the low 20°C range. That places it right in the league of chemicals that catch fire with ease, especially at room temperature or in a poorly ventilated warehouse. The fire itself may not look as dramatic as a fuel burn, but vapors can travel, settle, and light up farther from the workbench.
A big problem comes from the fact that many people underestimate how quickly vapors from such liquids reach dangerous levels. If you’ve handled alcohols or solvents before, you know leaving the lid loose or wiping spills with a dry rag adds another risk. 2-Butanol doesn’t need much encouragement to fill a closed space with flammable fumes. It’s not picky about the source of ignition—static from a sweater or the click of a light could set things off.
Fire is only half the story. Breathing in 2-Butanol feels unpleasant—dizziness, headaches, irritation in the lungs, maybe even worse if exposure is prolonged or at high levels. Skin contact dries the skin and sometimes triggers allergic reactions. Splashing it in your eyes can get painful fast, leading to watering, redness, or lasting injury if you don’t rinse out right away. People have become too comfortable around alcohol-based solvents, often skipping gloves or letting spills linger, because the liquid doesn’t feel “heavy” or as threatening as some other industrial chemicals.
Chronic exposure to solvents, including 2-Butanol, reminds me of technicians who spend a whole shift cleaning glassware or equipment. Even with some training, it's easy to forget how many vapors drift into your lungs daily. OSHA and ACGIH keep lowering occupational exposure limits for a reason—the irritation and fatigue accumulate over time.
Offering simple, grounded fixes works better than rattling off rules. Here’s what I’ve seen change outcomes over the years: Good ventilation stops vapor buildup, not just in theory but in practice—a fan that works, an open window, or better, a fume hood. Personal protective equipment only works if people want to use it; gloves and goggles belong right next to the work area, not tucked in a locked cabinet. Clean up spills immediately and label containers—label everything, even if it’s “just for a few minutes.”
Training should skip jargon and focus on real-life accidents—tell stories, show photos, let experienced staff share lessons from mistakes. Reduce storage to the amount needed for a week. Keep fire extinguishers within arm’s reach, check them once a month, and explain their use during safety meetings.
2-Butanol stands as a familiar tool for many technicians, but its fire and health risks don’t fade over time. Over the years, I’ve watched new staff get hurt because of shortcuts and old-timers develop respect only after a close call. Treating each hazard seriously, with grounded knowledge and honest habits, keeps both people and projects safe.
Chemistry interests me because every compound has a story, and 2-Butanol offers a classic example. In basic language, 2-Butanol goes by other names like sec-Butyl alcohol. Its chemical formula is C4H10O, a simple combination of carbon, hydrogen, and oxygen. Each molecule of 2-Butanol features four carbons lined up in a row, with a hydroxyl group sticking off the second carbon—this little twist turns it from butane into an alcohol.
This compound doesn’t mix things up without reason. With that functional alcohol group, 2-Butanol interacts more easily with water compared to plain hydrocarbons. Many labs and industries tap into this property, not only for research but also for commercial-scale uses. It also serves as an intermediate for producing other chemicals—once you grasp its structure, you see why chemists find it handy.
Numbers matter in chemistry, since a tiny difference can change how a substance behaves. For 2-Butanol, you’ll find the molecular weight clocks in at 74.12 g/mol. This value arises from adding up the masses for each element—carbon weighs in at about 12 amu each, hydrogen adds about 1 amu, and oxygen brings a heavier touch with roughly 16 amu. For those of us who spent hours in labs weighing out reactants, this number saves time, reduces waste, and cuts down on mistakes.
Not everyone needs this figure for daily life, but the people blending chemicals or checking quality do. They want consistency, reproducibility, and safety, especially at purities approaching 99.5%, like the anhydrous version. Purity levels can impact how well it works in solutions or reactions, and even the smallest contamination sometimes causes headaches down the line.
My own experience tells me no one likes to guess about what’s going into a reaction vessel. Knowing the makeup saves money and keeps projects on track. Students often overlook these fine details, focusing instead on flashy experiments. Miss them and things may fizz, pop, or do nothing at all.
High-grade 2-Butanol, especially at 99.5% purity, gets used in fields ranging from pharmaceuticals to coatings and adhesives. People expect high reliability, and that all starts with understanding the basics. Contaminants pose risk to product quality, worker health, and environmental safety. In some cases, the difference between pure and impure shows up in shelf-life, bioactivity, or safety data sheets—and that's not just academic concern.
Businesses that move large volumes want transparency. Listing the chemical formula and the molecular weight upfront builds trust and helps everyone along the supply chain. Labs check their materials with gas chromatography, mass spectrometry, and other tools, driven by the demand for high standards. Public knowledge and clear communication drive safer, smoother work—something everyone in research, teaching, or manufacturing can support.
Giving people the full picture of what they’re handling—right down to C4H10O and 74.12 g/mol—keeps experiments running on time, products coming off the line, and workers protected from avoidable hazards. Those details reflect a bigger effort across science and industry: treating accuracy and honesty as foundation stones. This approach feeds into safer working conditions and better everyday outcomes, both for trained chemists and folks just curious about what goes into a simple bottle on the shelf.
| Names | |
| Preferred IUPAC name | butan-2-ol |
| Other names |
sec-Butanol 2-Butyl alcohol Butan-2-ol sec-Butyl alcohol Methyl ethyl carbinol |
| Pronunciation | /tuːˈbjuːtənɒl/ |
| Identifiers | |
| CAS Number | 78-92-2 |
| Beilstein Reference | 1361161 |
| ChEBI | CHEBI:35687 |
| ChEMBL | CHEMBL17562 |
| ChemSpider | 7152 |
| DrugBank | DB02332 |
| ECHA InfoCard | 03c6bd2b-8241-447f-8c03-954bcc155c6f |
| EC Number | **200-751-6** |
| Gmelin Reference | 73197 |
| KEGG | C01526 |
| MeSH | D001943 |
| PubChem CID | 6560 |
| RTECS number | EL5425000 |
| UNII | YGS27808LH |
| UN number | UN1120 |
| Properties | |
| Chemical formula | C4H10O |
| Molar mass | 74.12 g/mol |
| Appearance | Clear colorless liquid |
| Odor | Sweet, winy |
| Density | 0.806 g/mL at 25 °C (lit.) |
| Solubility in water | Miscible |
| log P | 0.61 |
| Vapor pressure | 15 mmHg (20 °C) |
| Acidity (pKa) | 16.1 |
| Basicity (pKb) | The basicity (pKb) of 2-Butanol (Anhydrous 99.5%) is "15.20". |
| Magnetic susceptibility (χ) | -7.26 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | n20/D 1.399 |
| Viscosity | 2.9 mPa·s (25 °C) |
| Dipole moment | 2.89 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 163.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -320.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | −2672.7 kJ/mol |
| Pharmacology | |
| ATC code | V07AB |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02, GHS07 |
| Signal word | Danger |
| Precautionary statements | P210, P233, P240, P241, P242, P243, P261, P264, P271, P280, P303+P361+P353, P304+P340, P305+P351+P338, P312, P337+P313, P370+P378, P403+P235, P501 |
| NFPA 704 (fire diamond) | 2-Butanol (Anhydrous 99.5%): 2-3-0 |
| Flash point | Flash point: 22 °C |
| Autoignition temperature | 398°C |
| Explosive limits | 2.4 - 12% (in air) |
| Lethal dose or concentration | LD50 Oral Rat 2190 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50: 2190 mg/kg |
| NIOSH | EW2800000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for 2-Butanol (Anhydrous 99.5%): 150 ppm (TWA) |
| REL (Recommended) | NIOSH REL: TWA 100 ppm (300 mg/m3) |
| IDLH (Immediate danger) | 1600 ppm |
| Related compounds | |
| Related compounds |
1-Butanol tert-Butanol Isobutanol Methanol Ethanol Propanol sec-Butanol |
