Synthetic chemistry keeps rewriting its own rules, and the evolution of ionic liquids tells a fascinating part of the story. In the late 1980s and early 1990s, chemists set out to challenge the dominance of volatile organic solvents by building more adaptable, less hazardous alternatives. That’s where 1-Butylsulfonic-3-Methylimidazolium Trifluoromethanesulfonate enters. This compound, a mouthful understandably shortened to BSIM-OTf, emerged as researchers in academia and industry pushed for structures combining strong ionic character, economic synthesis, and chemical sturdiness. Scientists wanted more than simple environmental gains; the search was for performance. As patents rolled out, focusing on new cation-anion pairings, the butylsulfonic-methylimidazolium core found its way into journals and pilot-scale projects, invited by its flexibility across alkylations, biotransformations, and electrochemical setups.
BSIM-OTf doesn’t come dressed up like more famous molecules. Its reputation rides on specifics—how it dissolves polar and non-polar substances, its stubborn immiscibility with some organics, and how it catalyzes or stabilizes sensitive reactions without interfering. For a long time, labs around the world hunted for a solvent or catalyst salt they didn’t have to vent into the atmosphere or monitor for flammability. BSIM-OTf’s low vapor pressure, insensitivity to open air, and strong mi-sion between cation and anion did not disappoint. In the catalog, you sometimes see synonyms such as 1-butylsulfonic acid-3-methylimidazolium trifluoromethanesulfonate and [BSMIM][OTf]. No matter the label, inside that bottle sits a deeply polar, thermally robust, virtually non-volatile liquid awaiting a chemist’s next big idea.
This ionic liquid stands out through a density that hovers around 1.5 g/cm³ at room temperature and a viscosity higher than water but lower than many fully organic salts. That viscosity gives experimentalists some breathing space during dosing or extraction steps. Its melting point sits well below ambient temperature, so flasks never clog from crystallization. Thermal stability stretches up beyond 250°C, letting reactions run hot without worry for decomposition into hazardous byproducts. Where water or traditional solvents might pick up trace metal contamination or evaporate mid-run, BSIM-OTf remains composed. It dissolves a surprising array of both organic and inorganic species—acids, bases, some transition metals, and even biopolymers in select conditions. Electrically, the ionic nature translates to respectable conductivity, offering chemists a flexible alternative to more dangerous acidic or basic reaction media.
Producers offer BSIM-OTf in purities of 98% and up, standard for both R&D and small-scale manufacturing. Most bottles arrive capped under an inert atmosphere or with desiccant packs, since the substance could otherwise hydrate and drop in purity. Labels highlight CAS numbers and batch data, along with warnings grounded in REACH and GHS guidelines. High-grade material shuns halide contamination, keeping trace impurities below one part per thousand. Some providers add specification sheets listing water content, UV absorbance, and allowable metal ion levels for clarity. For large-scale applications, drum or tote packaging comes with QR codes linking to up-to-date safety and technical documents.
Synthesizing this ionic liquid typically follows a two-step route, drawing on well-practiced organic functionalizations. The butylsulfonic acid intermediate couples to a 3-methylimidazole ring in a heated reactor, with controlled addition of trifluoromethanesulfonic acid as the final pairing agent. Teams pay close attention to water exclusion, as hydrolysis during synthesis can yield unwanted byproducts. Purification involves liquid-liquid extraction followed by vacuum drying, often watched over by FT-IR and NMR spectroscopy checks. Scale-up happens in glass-lined reactors, with safety precautions for handling strong acids and volatile intermediates. Accessibility to affordable starting materials and clearly mapped-out reaction sequences contributes to the commercial viability.
BSIM-OTf doesn’t limit itself to the role of another solvent. Chemists look to its imidazolium core for nucleophilic or electrophilic reactivity tuning by swapping alkyl chain lengths or modifying the triflate anion. Some research teams attach catalytic residues onto the sulfonic group or use the compound as a phase-transfer agent in alkylations and oxidations. The functional versatility makes it a platform for designing task-specific ionic liquids—each adapted to a narrow chemical challenge, from asymmetric synthesis to selective extraction of precious metals. Researchers regularly modify BSIM-OTf to adjust hydrophobicity or increase its coordination strength for applications in enzyme-catalyzed reactions or non-aqueous electrochemistry.
This molecule goes by several trade names and shorthand labels, mostly depending on supplier catalogues or national regulatory frameworks. You’ll see it labelled 1-Butylsulfonic acid-3-methylimidazolium trifluoromethanesulfonate, BSMIM OTf, or [C4SO3H-MIM][OTf]. Some manufacturers drop the “acid” tag to emphasize its salt-like character, while others call it an “ionic liquid” to help customers spot it in solvent sections. Knowing these differences speeds up ordering and avoids costly mislabeling, especially in industries where regulatory compliance depends on precise product traceability.
Labs treat BSIM-OTf respectfully, even if it isn’t especially volatile or flammable. GHS pictograms usually highlight irritant effects for eyes and mucous membranes, with PPE recommended in both academic and industrial settings—nitrile gloves, side-shielded glasses, and effective chemical hoods. Waste streams containing this ionic liquid pass through standard neutralization and organic removal steps before reaching municipal treatment plants, in line with REACH and OECD guidelines. Transport requirements match those for other strong organic salts, with documentation ensuring compliance along the supply chain. Any team running larger test batches keeps spill kits close and emergency showers on a clear path.
BSIM-OTf serves as a molecular Swiss army knife across several industries. In pharmaceuticals, its combination of high polarity and thermal stability enhances multi-step organic syntheses and controls selectivity in challenging transformations. Battery and supercapacitor developers count on BSIM-OTf as a robust electrolyte or separator coating, reaping the benefits of low flammability and lasting performance through repeated cycles. Materials scientists testing sol-gel processes or composite formation add the ionic liquid to improve dispersion and control microstructure. Heavy industry uses it to strip metals or process fine chemicals, banking on fewer emissions than classical solvents. Some enzyme-catalysis research takes off faster thanks to this medium’s ability to both solubilize biocatalysts and moderate their activity, opening new bio-based production routes for fuels and pharmaceuticals.
Academic labs keep pushing the frontier, using BSIM-OTf as a launchpad for more effective green chemistry. Graduate students and postdocs across the globe set up reactions with this ionic liquid, chasing higher yields or safer syntheses for prized products. Peer-reviewed publications showcase advances in both organic and inorganic routes, with common threads linking back to reduced byproduct formation, easier work-ups, and lower energy needs. On the industrial side, process engineers work to scale up reactions without generating toxic waste. The hope is simple: replace volatile solvents in flagship products with a more manageable, cost-effective alternative. Trust in BSIM-OTf grows whenever a process delivers the same product—but with cleaner conditions and a better safety profile.
Every new chemical, even those billed as “environmentally friendly,” warrants a close look at its real-world impact. Initial studies on BSIM-OTf show low bioaccumulation and poor absorption through the skin, which points to modest risk under controlled conditions. Cell culture and small-animal assays suggest irritancy without mutagenic or teratogenic effects at workplace exposure levels. Regulatory scientists keep a close watch on disposal routes, especially in places where water purity and aquatic toxicity matter. Hazard summaries from leading health agencies flag the need for careful glove selection and avoidance of splash exposure, even as chronic toxicity signs remain minimal. Industry and academic consortia push for continuous data collection as more facilities plug BSIM-OTf into their operations.
Any chemical with a proven track record for stability, performance, and reduced emissions gathers momentum over time. Ongoing research centers on engineering new functional derivatives of BSIM-OTf to boost solubility, tune polarity, and expand compatibility with emerging processes such as CO2 capture or biocatalysis. Energy storage applications show special promise, with teams testing ionic liquid-based electrolytes to boost battery safety and lifespan without sacrificing electrical performance. Policy shifts toward circular chemistry count on ionic liquids to cut the ties between production and pollution, as companies search for scalable alternatives to halogenated solvents. In academic circles, rising student interest in sustainable chemistry means that molecules like BSIM-OTf will keep drawing research funding, creative new uses, and closer scrutiny for years ahead.
Sometimes, the spotlight shines on chemicals most folks have never heard of. Take 1-butylsulfonic-3-methylimidazolium trifluoromethanesulfonate—a mouthful, sure, but its impact goes far beyond its complicated name. Chemists and engineers have put it to work because it’s an ionic liquid with qualities that turn once-impossible tasks into routine jobs.
Sustainability often depends on rethinking the way we use solvents. Traditional organic solvents create waste and hazards. This ionic liquid stays liquid well below boiling water’s temperature and won’t evaporate the way common solvents do. Its unique structure makes it non-volatile and thermally stable. These features matter in green chemistry, not just because they shrink emissions, but also because they reduce flammability and toxicity risks.
The trifluoromethanesulfonate anion increases solubility for a huge range of materials. In labs and bigger reactors, scientists use this liquid to break down biomass, extract metals, and even dissolve difficult polymers. For someone like me who’s watched old-school solvents foul up delicate catalytic reactions, this compound means fewer surprise shutdowns and less post-reaction cleanup. In tasks like Fischer esterification or Diels-Alder reactions, its ability to dissolve polar and nonpolar products cuts time and energy consumption.
Batteries and fuel cells run into trouble with competing needs: safety, energy capacity, and durability. Electrolytes made from this ionic liquid tick many of those boxes. They can shuttle ions without forming dangerous vapors. Electric vehicles using lithium-ion technology benefit directly from these safer, less-flammable electrolytes. The liquid’s high ionic conductivity helps batteries hold charges longer and cycle more times without breaking down. Anyone who’s dealt with overheating or cell shorts in lithium-ion batteries can appreciate the practical advantage here—fewer recalls, longer warranties, and fewer toxic leaks into landfills.
Handling oily wastes or heavy metals used to mean large volumes of hazardous solvents and difficult disposal. This ionic liquid helps extract rare earths, copper, and other metals more selectively, using less liquid, and with easier recycling. In spill response and pollution control, cleanup teams can trap volatile organics or separate contaminants with much less secondary pollution.
High costs have slowed more widespread use. Manufacturing ionic liquids remains expensive, mostly due to raw material purity requirements. Harnessing larger-scale, smarter synthesis can bring down costs. Public support—grants, government guidance, and better incentives—can help local companies build pilot plants. Transparent toxicity studies would make regulators and workers more comfortable with these chemicals. Education for engineers, process chemists, and first responders can reduce mistakes and keep folks safe.
This compound’s track record makes me bullish about its future, especially as renewable energy and recycling take a bigger share of the global economy. Real challenges remain, but smart investments and honest research will give us the tools to solve them.
1-Butylsulfonic-3-Methylimidazolium Trifluoromethanesulfonate sounds intimidating, but it’s not a mystery when broken down. This compound brings together a unique cation and a robust anion, resulting in a salt that sits among the ionic liquids. The cation features an imidazolium ring, attached at the first position to a butylsulfonic group, and a methyl group attached to the third position. The anion, trifluoromethanesulfonate, counts as a strong, non-coordinating player.
Looking at the molecular formula:C9H17F3N2O5S2This formula gives a snapshot of how each element joins the mix, weaving together three distinct chemical backbones into one material.
Visualizing the molecule helps far more than memorizing names. The imidazolium ring, the core of so many ionic liquids, plays the anchor role. One nitrogen in the ring bonds to a methyl group (–CH3), and the other nitrogen bonds to a butylsulfonic acid side chain (–(CH2)4SO3H). The arrangement shapes both how the molecule interacts with others and how easily it dissolves or resists breaking apart.
The trifluoromethanesulfonate anion, also known as triflate, brings three fluorine atoms attached to a single carbon, which then binds through a sulfonate group (–SO3). The presence of fluorine atoms sets up incredible stability and decreases nucleophilicity, meaning it doesn’t easily jump into reactions. In practical lab work, that’s a helpful feature—it reduces surprises and leads to more predictable results.
These sorts of compounds don’t end up in news headlines or everyday writing, but their importance in chemical research and industry can’t be overlooked. People working with ionic liquids need materials that behave in reliable ways under heat, pressure, and chemical stress. The butylsulfonic-methylimidazolium core brings excellent resistance to breakdown, while the triflate counterion ensures high thermal stability and low tendency toward unwanted reactivity.
I’ve watched ionic liquids, including compounds like this, open up new territory in extraction, catalysis, electrochemistry, and even biomass processing. Factoring in their tunable ionic nature, they work where classic solvents fall flat. Researchers aim for lower toxicity and greater recyclability. In direct comparison with older chloride-based or hexafluorophosphate-based salts, triflate versions make recycling easier and waste less hazardous.
No chemical gets a free pass when it comes to safety or environmental concerns. While the triflate and imidazolium combo resists water and harsh chemicals, there is always a consideration about what happens if these compounds leak or break down. Fluorinated compounds have a reputation for persistence in the environment. Labs and manufacturers must track disposal, containment, and alternatives that may balance performance with a lower ecological footprint.
Progress on greener chemistries continues. More teams focus on improving both synthesis routes and the afterlife of these chemicals. There’s growing emphasis on finding renewable feedstocks, better recycling techniques, and degradable alternatives. For those building processes around 1-butylsulfonic-3-methylimidazolium trifluoromethanesulfonate, looking ahead means not just focusing on lab results. It means factoring in the whole pathway from lab bench to potential waste.
Working with specialized chemicals like 1-butylsulfonic-3-methylimidazolium trifluoromethanesulfonate isn’t something people decide to do on a whim. For everyone who’s worked in a lab, safety never feels overblown—it comes from hard-learned lessons. This compound falls into the family of ionic liquids, valued for its stability and negligible vapor pressure. Even so, treating it with anything less than total respect would be a mistake.
A dry, cool, and well-ventilated room wins almost every time. Humidity encourages trouble by spurring slow degradation and unpredictable reactivity. Air-tight, clearly labeled containers, glass or compatible plastics, stop unnecessary exposure to the air. Store the bottles far from direct sunlight and heat sources, since light and warmth can sometimes coax out decomposition. Unopened containers stay upright and nested away from acids, strong bases, and oxidizers because combining reactive chemicals is inviting disaster.
Chemists who have overlooked segregation in storage often discover, through ruined experiments or much worse, that small slip-ups do catch up. While this ionic liquid boasts thermal stability compared to many organic solvents, it cannot be stacked carelessly with flammables or moisture-sensitive chemicals. Manufacturers’ datasheets recommend temperatures under 25°C for extended shelf life. Containment trays catch drips that slosh out during bottle transfers—one spill can spread fast, especially on smooth floors.
Pulling on gloves and safety goggles might sound simple, but there’s no shortcut. In my own experience, nitrile gloves hold up well, with lab coats stopping the kind of accidental sleeve drags most amateurs regret later. Face shields gain new meaning if splashing feels possible, which happens surprisingly often during measuring or pouring. Chemical fume hoods offer strong protection, drawing stray vapors away and keeping personal breathing zones clear. Breathing in anything unknown never seems like a good bet.
Keeping workstations uncluttered helps, but so does good training. I once watched a colleague forget basic disposal rules and pour waste ionic liquid into a general solvent drum. The resulting headache—label changes, rushed calls to waste contractors, and panicked emails—drilled home the point. Separate and clearly labeled waste containers must sit close at hand, and disposal follows strict local hazardous waste protocols. Equipment used with this substance doesn’t get mixed back into general circulation without a thorough, chemically compatible cleaning.
None of the above substitutes for a real emergency plan. Storing a chemical spill kit close by feels nearly as important as storing the chemical itself. Absorbent pads, neutralizing agents, and disposal bags should be within quick reach. Spare gloves and a printed copy of the safety data sheet are never a wasted expense. Knowing emergency contacts and watching out for early signs of a spill or reaction matters as much as any written rule.
Safety habits draw from more than posted charts. Mentorship plays a role—junior chemists pick up best practices by watching veterans. Experience says reviewing protocols with every team newcomer cuts down on dangerous shortcuts. Every overlooked detail, every moment of carelessness from fatigue or stress, chases up real consequences in the chemical world. Thinking ahead, working clean, and always questioning: that keeps both people and projects on the right side of safe.
Some chemicals get long, unwieldy names that scare off most folks before they get to the real reason they matter. 1-Butylsulfonic-3-methylimidazolium trifluoromethanesulfonate belongs in that group, but it deserves a closer look. This compound takes shape as a colorless to pale yellow liquid under standard conditions. Unlike the flammable solvents you find in most high school labs, this ionic liquid barely evaporates, stays calm around open flames, and carries a high thermal stability. In research, this means less fiddling with special storage and safety gear.
The liquid shows strong polarity, with each molecule made of a big imidazolium ring—very stable on its own—connected to a sulfonic acid group and butyl chain, all set opposite a trifluoromethanesulfonate anion. Such a setup gives rise to its famous low volatility and resistance to breaking down. Toss in high ionic conductivity and it’s easy to see why this stuff made a name for itself in electrochemical circles.
Ionic strength goes hand in hand with solubility, and this substance pulls off both. It dissolves a wide range of substrates—both organic and inorganic—without blinking. Labs lean on it to run greener reactions, skip over nasty solvents, and keep products stable. The strong bonds inside prevent water and oxygen from breaking it apart, making this liquid hold up in harsh conditions.
The sulfonic acid group in the cation gives this liquid a little acidity, and that nudges chemical reactions in useful directions. Chemists add it to catalytic cycles to speed things up or make certain steps work better. Its chemical stubbornness stops unwanted side reactions, so yields tend to rise. In electroplating or fuel cells, its high ionic conductivity helps keep current flowing—something battery engineers crave.
Compared to traditional solvents, this one stands out for safety. It stands up to heat well over 200°C, and its reluctance to light up adds peace of mind. That said, what keeps it stable—lots of fluorine—raises tricky waste problems. Breaking down trifluoromethanesulfonate groups can spit out persistent pollutants. Stringent disposal rules often arrive with large-scale use, since fluorinated molecules stubbornly stick around in soil and water.
Another point: not every lab can afford the price for high-purity ionic liquids, especially fresh, untested ones. Careful purification remains vital, since tiny changes in moisture or leftover chemicals throw off reaction outcomes. The small pool of suppliers bumps up cost, slowing down the jump from lab curiosity to industrial mainstay.
Research continues to chase safer, cheaper ways to make and recycle this ionic liquid. I’ve watched teams in renewable energy labs tinker with purification tweaks and more sustainable feedstocks. Each small advance matters—cleaner reactions reach less affluent regions, and safer solvents cut hazardous waste. More data sharing can speed up the learning curve for those just starting with unfamiliar compounds.
In the bigger picture, stricter standards and well-documented safety sheets keep newcomers safe. Knowledge exchange among chemists doesn’t solve every roadblock, but it certainly leaves fewer painful mistakes. Green chemistry needs more than a good solvent; it runs on practical know-how and open communication. As long as teams keep testing, sharing, and questioning received wisdom, progress won’t slow down.
Chemistry rarely keeps things simple, and in the realm of ionic liquids, there’s always a new pairing to scrutinize. 1-Butylsulfonic-3-methylimidazolium trifluoromethanesulfonate—quite a mouthful, but in the lab, this chemical attracts interest for its stability and ability to dissolve a wide swath of compounds. Whenever folks look for new solvents or reaction media, the question of “will it play well with others?” shows up early. Mixing up random chemicals can mean a bad day in the lab, dirty glassware, or ruined runs. So, being careful about compatibility can’t stay just a theoretical discussion.
From what’s published, this ionic liquid has built a reputation for thermal resilience and resistance to decomposition. That’s why researchers, especially in greener chemistry circles, gravitate towards it. It’s not just about finding a solvent that doesn’t boil off or react at the first sign of trouble—what really sets it apart is its adaptability. Labs have used it to dissolve salts, metal complexes, and organic molecules that would gunk up or crash out in traditional solvents.
Yet compatibility isn’t simply a checkbox—one size won’t fit all. Sometimes two liquids mix easily, sometimes one changes the behavior of the other in weird, unpredictable ways. Taking shortcuts can backfire. In my graduate days, I watched someone pair a new ionic liquid with an acid catalyst. The mix turned cloudy, pH readings went haywire, and the experiment never recovered. We saw that certain sulfonate groups can bind too tightly with metals or leach into catalytic sites, interfering with the chemistry people actually want.
Plenty of tests point out that this particular imidazolium-based ionic liquid sits pretty steady with other organic solvents and salts. Sharing a triflate anion makes it less likely to set off violent reactions or produce dangerous byproducts, as compared to pairing with chloride or acetate-based versions. Electrochemical windows show reasonable stability, which means less risk of breakdown when under electrical stress. But the story doesn’t end here.
There’s real value in checking if it latches onto or repels other chemicals in your mix. Research groups have seen changes in viscosity and solubility when water or even mild acids enter the system. Some find the liquid suddenly starts holding more water than expected. For industrial folks, that means a risk in long processes: extra water may lower product yields or clog up filters faster. That’s not just a setback; it’s wasted money and lost time.
If you’re considering this ionic liquid for electrochemistry, separation, or catalysis, start by mapping out every other chemical coming into contact with it. Running simple tests in small batches beats scaling up blind. Modern analysis—NMR, FTIR, and simple conductivity measurements—can track unwanted interactions early. Don’t just trust chemical catalogs or datasheets; lab trials catch what desk research can miss.
Collaboration across chemistry teams helps. Sharing results, even the disappointing ones, means others waste less time repeating mistakes. Look for open science databases where experimental data gets posted, not just cherry-picked success stories.
In my experience, planning helps as much as high-tech tools. Cross-check each ingredient, talk to vendors about impurities, and check how long the mixture needs to sit—some issues show up hours later. Real-world chemistry means thinking several steps ahead, not just going by the book. This mindset turns experiments into useful products, not just glossy academic reports.
