Decades ago, chemical innovators opened the door to ionic liquids, those salt compounds that stay liquid below 100°C. Propyltrimethylammonium bis((trifluoromethyl)sulfonyl)imide—often abbreviated as N1113-TFSI—entered labs during the wave of curiosity surrounding ionic liquids in the 1990s and 2000s. Scientists looked for ways to replace volatile organic solvents and landed on salts like this one, designed to stay stable and non-flammable. At first, a handful of university teams in Europe and Japan began working with similar structures, driven by demands from electrochemistry and electronics. Over time, engineers refined its synthesis, targeting lower toxicity, easier handling, and higher ionic conductivity. Research journals from that era show a steady shift: what began as an academic curiosity gradually turned into an industrial asset as large manufacturers saw the benefits for safer, greener chemistry.
N1113-TFSI belongs to the family of quaternary ammonium-based ionic liquids. The product typically forms a clear or faintly yellow liquid at room temperature, behaving much like heavy mineral oil. Chemists value it for its remarkable balance between hydrophobicity and the ability to dissolve a surprising array of materials, from polymers to metal salts—a property traced to the TFSI anion's unique fluorinated structure. Bottles often arrive in amber glass, capped and sealed, to ward off moisture. The main draw, besides stability, lies in its non-flammable nature, making it attractive for high-stakes environments such as electrolytes in lithium battery research and advanced catalysis.
When poured, N1113-TFSI moves slowly—it brings a viscosity several times higher than water. Its density clocks in above 1.3 g/cm³, so it sinks in most organic solvents. Water has a hard time dissolving it, and that’s a plus for certain applications. As for chemical resistance, it shrugs off attack from acids and bases, a trait valued in both synthesis workups and industrial rinses. The ionic nature translates to high conductivity, and the thermal window stretches from below freezing to well above boiling water temperatures. Unlike most organic liquids, it seldom volatilizes, so its vapor pressure stays low even near 100°C. That means safer labs and less air contamination.
Industrial suppliers run rigorous purity checks on N1113-TFSI before sticking a label on the container. Purity often exceeds 99%, with water content typically below 0.1%. Labels list the full compound name alongside its CAS number and UN code for transport, indicating its designation as a non-classified, low-hazard chemical. Instructions guarantee users wear gloves and goggles, and storage describes cool, dry rooms far from oxidants or open flames. Barcodes and RFID tags now appear on many containers for digital tracking, making recalls or inventory headaches less likely. Analytical methods on spec sheets—like NMR and ion chromatography—prove critical for researchers who need batch-to-batch consistency.
Manufacturers prep N1113-TFSI using classic metathesis. They start with propyltrimethylammonium chloride, combine it in aqueous medium with lithium bis(trifluoromethanesulfonyl)imide, and stir vigorously. The target compound separates as an oil, heavier than water. Next, a series of water washes remove lithium chloride and other contaminants. The liquid undergoes drying under vacuum or over anhydrous magnesium sulfate to reduce trace water. Technicians fine-tune temperature and mixing speeds to avoid forming emulsions, which are notorious for lowering yields. Standalone purification steps—like passing through activated alumina—bring the ionic liquid to research grade.
Although stable, N1113-TFSI doesn’t mind a little modification. Chemists can swap out the propyl group for other alkyl chains to tweak solubility or introduce new functional groups. In work with lithium batteries, folks tested incorporating it into polymer gels, giving up some pure conductivity for added mechanical strength. TFSI’s resilience against oxidation and strong bases means the compound survives harsh electrochemical cycles and catalytic runs. Researchers sometimes react it with transition metal salts to create custom electrolytes or catalysts, each tailored for specific reaction environments.
In catalogues, the compound wears several names. Typical synonyms include N1113-TFSI, propyltrimethylammonium bis(trifluoromethanesulfonyl)imide, and its systematic IUPAC label. Some brands list it under trade names linked to their lineup of room-temperature ionic liquids. These variations sometimes stump new users, so cross-referencing CAS numbers helps avoid mix-ups. Scientists often adopt the short-hand N-alkyl ammonium TFSI series when discussing structure-activity work across different chain lengths.
Using N1113-TFSI, safety teams lock in a familiar routine. Even though the substance brings low volatility and scant odor, direct skin or eye contact earns a swift rinse. Fume hoods stay on during any scale-up, just in case. Spills get absorbed with sand; water works less well, since the liquid barely mixes with it. Disposal routes follow non-halogenated organics guidance, sending used liquid to chemical waste processors. In recent years, most big labs started including extensive documentation on handling ionic liquids, especially for new students still navigating their first reactions. Accident logs from well-run sites rarely turn up complaints; most dangerous incidents involve improper mixing or mislabeling of containers.
Practically speaking, N1113-TFSI carved a niche in electrochemistry. Tech companies investigating new battery formulations prize its stability and conductivity, especially for next-generation lithium-ion and sodium-ion cells. Its resistance to moisture helps in metal plating and microfabrication, where errant water can undo precise work. Green chemistry initiatives lift it as a replacement for toxic and volatile solvents; the ionic liquid often appears in biomass processing streams or catalytic hydrogenations. Some creative teams even deploy it for carbon capture, leveraging its affinity for CO2 absorption. Its role in pharmaceutical synthesis remains minor, as heavy fluorinated anions sometimes cause regulatory concern.
Labs worldwide continue probing N1113-TFSI’s limits. Much of the focus targets longevity in lithium-ion electrolytes at high voltage, since breakdown products from traditional solvents set stubborn safety boundaries for electric vehicles. Research money also flows toward exploring new salt structures, using N1113-TFSI as a benchmark for conductivity, toxicity, and environmental impact. More recently, scientists turned their attention to developing recyclable or biodegradable analogues, spurred by tighter green chemistry standards. Collaborative networks exchange not only results but also precise manufacturing protocols, hoping reproducibility will help cross the divide from bench to factory floor.
Safety sheets flag low acute toxicity for most quaternary ammonium TFSIs, though chronic effects tell a more complicated story. Animal tests show minimal skin and eye irritation; systemic toxicity remains a concern only at doses much higher than routine workplace exposure. Environmental persistence raises bigger anxieties: the stable TFSI anion resists breakdown in wastewater, and its accumulation could disrupt aquatic systems long after use. Toxicologists push for more real-world data on breakdown products and long-term metabolites. Trade organizations draft voluntary exposure limits, but regulators in Europe and Japan run their own independent risk assessments. Researchers call for development of more digestible anions or full cycle recycling methods to limit potential ecological impact.
Looking ahead, the future for N1113-TFSI appears intertwined with the rise in electrification, energy storage, and sustainable chemical manufacturing. New research highlights the need to balance stability with faster degradation after use, especially where disposal regulations tighten. The compound’s role as a building block for tailored ionic liquids cements its place among advanced materials; at the same time, pressure builds to account for long-term persistence and toxicity. Market demand will likely depend on breakthroughs in recycling technologies and successful lobbying for green certifications. Industry insiders watch policy developments closely, recognizing that the chemistry hasn’t finished its story—the next chapter may be written as much by environmental scientists as by electrochemists or engineers.
Peeking into the structure of Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide always brings back memories of staring at complex chemical drawings in college labs. Little clusters of lines and letters meant stable salts, oddball liquids, or the starting point in a big experiment. Let’s break down what this mouthful of a chemical really looks like, chemically speaking.
There are two main components in this salt. One is a cation: propyltrimethylammonium. The other is an anion: bis((trifluoromethyl)sulfonyl)imide. Splitting the chemical formula like this gives the structure more meaning rather than drowning in a soup of syllables.
The propyltrimethylammonium group comes first. Imagine three methyl groups (CH3) and a single propyl group (C3H7) all attached to a nitrogen atom. The nitrogen becomes a positively charged center, forming a neat little four-armed star. When I handled similar structures in school, it amazed me how just swapping one of those arms out could change physical properties or even toxicity. That nitrogen holds the fort, lending the compound a positive charge and letting it participate in some interesting ionic dances.
Now for the anion, which sounds exotic for a reason. Bis((trifluoromethyl)sulfonyl)imide means there are two sulfonyl groups (SO2) each linked to a nitrogen, with each sulfonyl soloed by a trifluoromethyl group (CF3). If the cation looks like a star, the anion is a more sprawling shape.
Both sides bring their own personality. From experience with ionic liquids in the lab, salts built from large organic cations and non-coordinating, bulky anions often stay liquid at room temperature, which can’t be said for your basic sodium chloride. This low melting point is what pushed these salts into battery and electrochemistry circles in the first place.
The propyltrimethylammonium cation isn’t bulky, but stacked with the bis((trifluoromethyl)sulfonyl)imide, it makes for a salt that usually doesn’t crystallize easily, helping maintain liquid form even at relatively cool temps. I found that these properties come back to how those big anions disrupt tight packing in a crystal lattice. In work on sustainable solvents, swapping smaller ions for bigger, more complex ones dramatically improved solubility.
What makes this combination special isn’t just its stability or solubility—it’s the fact that the size, asymmetry, and weak interactions of these ions lead to remarkable properties. Think low vapour pressure, resistance to decomposition, and sometimes even environmental benefits—though all those fluorines do raise eyebrows in green chemistry circles. Some chemists have started looking into replacements or tweaks to reduce environmental persistence, especially with persistent organic pollutants in the headlines.
Few people think about the shape of their salt when they sprinkle it onto food, but in electrochemistry, those shapes change everything. Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide shows that structure isn’t just academic; it’s the key to unlocking new battery designs, safer solvents, and a long list of tough-to-solve problems. As regulation tightens on persistent compounds, labs need to keep pushing for safer, more sustainable structural tweaks. Drawing new lines between atoms can make as much difference as a new law or recycling scheme.
Lithium-ion batteries power our phones and help electric cars travel farther than ever, but keeping these batteries stable takes more than simple salts. Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide, known in labs as a mouthful and in the real world as a next-level ionic liquid, has carved out a key spot in battery technology. Batteries running hotter and charging quicker than before don’t just need something that can hold a charge—they count on chemicals that won’t catch fire or boil away. Thanks to its low volatility and strong resistance to heat, this compound keeps a battery’s electrolyte in the right zone, stopping nasty failures and letting devices squeeze out more cycles before they call it quits.
Supercapacitors bridge the gap between batteries and standard capacitors, pushing serious energy in bursts. Electric buses hit the streets today, scooping up quick charges at every stop; in their guts, you’ll find materials like Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide. The ability to hold a charge, then release it all at once, hinges on the right ionic fluid. Some fluids break down, gumming up the works or corroding the plates—this compound keeps things moving smoothly, no matter how many stop-and-go cycles the transport demands. Most city bus operators now see these devices deliver not only faster charge times but also more years on the road, lowering both costs and headaches.
The old way of plating electronics with gold or rare metals left behind too much toxic waste. Clean, green solutions get more attention in manufacturing every year. Factory engineers swapped in Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide because it offers a stable ionic fluid that doesn’t break down under electrical current. Rather than sending homeworkers or technicians to wrangle with fumes, this compound delivers a safer working environment and precise control. Phones and circuit boards stay shiny, and the planet breathes easier.
Making pharmaceuticals or new polymers often means wrestling with solvents that burn skin or fill labs with harsh vapors. The push for green chemistry started decades ago, but only took off as soon as chemists discovered “designer solvents.” Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide stands out thanks to its friendly environmental profile and chemical neutrality. Synthesis reactions run with fewer byproducts and less risk, which speeds up not just the chemistry but the regulatory paperwork that can kill a project before it’s born.
Propyltrimethylammonium Bis((Trifluoromethyl)Sulfonyl)Imide doesn’t freeze at low temps and doesn’t evaporate under stress. Labs and production lines see it as a shortcut to safer, longer-lasting products. Industries still struggle with cost and finding the right recycling pipeline, but the health and environmental gains over legacy solvents keep outweighing the drawbacks. As new gadgets demand safer batteries and faster charge cycles, real-world chemistry gets more creative—often using this compound as the backbone for the next round of tech breakthroughs.
There’s often a tendency to treat industrial products or chemicals as if they’re everyday items, especially after repeated use. But comfort can breed carelessness, which leads to injuries or damage to both people and the environment. Many years ago, I saw the aftermath of a small chemical spill—gloves weren’t worn, someone forgot eye protection, and a harmless-sounding powder ended up sending a coworker to the ER. From that day forward, I started reading labels and safety sheets before touching anything unfamiliar.
Before touching the product, look over the manufacturer’s safety instructions. Most companies outline the recommended protective gear and response steps in their Safety Data Sheets (SDS). Skipping these details can turn a routine task into a hazard.
Using the right gloves serves as the most basic defense. Nitrile or latex work for many substances, while heavy chemicals often need specialized gear. Without protection, absorbed chemicals irritate or burn skin, even if it looks like nothing happened at first. Skin contact surprises you days later, sometimes long after working with the product.
Eyes demand attention. Chemical splashes blind in seconds or send you to the doctor for weeks of irritation. Protective goggles with side shields give much better protection than glasses. I once saw a colleague brush a finger beneath a dust mask, and fine powder still made it past his eyelashes. Even workers who know better get caught off guard.
Inhaling dust or fumes is easy to overlook, but respiratory protection must match the hazard. Ventilated spaces help, but not every product signals trouble with a strong smell. A tight-fitting mask can block out harmful particles, but most people skip the fit-check, which turns it into false security. After reading several studies, I learned that long-term exposure—even to low levels—causes chronic respiratory inflammation and other health issues. These changes creep up on people after years, so prevention matters from day one.
After using the product, scrub hands and exposed skin with soap and water—no shortcuts. Products cling to skin or under fingernails where they can spread to other surfaces or food. Separate work clothes and wash them afterwards. Cross-contamination is a real risk, especially with kids or pets at home.
Store leftovers in containers with proper seals, away from heat or sunlight. Flammable or reactive materials start problems if shoved near cleaning supplies or mixed by mistake. Label all containers with the original product name and hazard warnings. A faded bottle in a shared garage turns into a guessing game that nobody wins.
Accidents fade from memory fast, but routines built on safe habits protect everyone. Training new hires to recognize hazards makes a difference, as does reminding coworkers to double-check gear before starting a job. Encouragement works better than lectures. Managers should set an example by wearing gear and handling the product the correct way.
Too often, trouble comes from ignoring the basics. Protect skin, eyes, and lungs, and treat each product with respect. Safe practices are easy to skip when routines set in, but every extra step stacks the odds in your favor.
Anyone working with specialty chemicals like Propyltrimethylammomium Bis((Trifluoromethyl)Sulfonyl)Imide knows the challenges extend beyond safe handling. Poor storage can mess up research, damage expensive tools, or risk health for the whole team. I learned the hard way back in grad school, watching a solvent break down and fill the storeroom with a headache-inducing odor because the container sat too close to a heat source. It set the tone for how I treat every compound, even these salt-like ionic liquids.
Propyltrimethylammomium Bis((Trifluoromethyl)Sulfonyl)Imide—lets call it PTMA-TFSI for brevity—draws attention in laboratories for its stability, low volatility, and hydrophobic nature. Ionic liquids like this don’t evaporate into oblivion, so you won’t find the familiar whoosh of a volatile organic compound. But that doesn’t mean they won’t absorb moisture or react if stored carelessly.
Many rely on PTMA-TFSI because it works well in electrochemistry, battery, and organic synthesis. Despite its resilience, it still demands careful stewardship. Water loves sneaking into lab spaces, riding in on humid air and contaminating months of careful planning. From my own bench work, leaving caps loose or using cracked glassware can turn a perfectly good batch into a sludgy mess. Even minor lapses open the door to expensive headaches.
Let’s talk about practical steps for storage. PTMA-TFSI thrives in a cool, dry place. Temperature control stands out—20–25°C works for short-term needs, but for anything longer you want true environmental stability, below 20°C if possible. Avoiding temperature swings stops condensation inside bottles, which is where many disasters begin.
Get the right containers. Airtight glass or high-quality plastic with robust seals keeps out atmospheric moisture. I use amber glass jars for most light-sensitive materials even though PTMA-TFSI doesn’t degrade under normal light conditions, but it never hurts to be cautious. Label every container with the open date—old stock attracts mistakes and confusion, especially in busy shared spaces.
PTMA-TFSI won’t start bubbling or smoke if it meets the air, but high humidity breaks down its purity over time. Precision research demands water content below ppm levels, and even trace absorption can throw off reactivity. Desiccators, silica gel, or a dry box create extra insurance against invisible contamination. I’ve watched an entire experiment fail because the starting salt picked up extra grams of water overnight.
Store it away from reactive chemicals or open acid bottles. Ionic liquids might look inert, but strong mineral acids or aggressive bases can still cause unwanted side reactions. Keeping incompatible chemicals segregated isn’t about paranoia—it’s about preventing slow, quiet contamination you only discover after you’ve sunk hours of effort.
Use periodic checks for visual changes or clumping in the powder. Set a regular cycle—once a month works for most of us, more often in tropical climates or under heavy use. I run Karl Fischer titration to check for water content if I suspect a problem, but even a simple inspection beats hoping for the best.
Safe storage stays a team effort. Write down every transfer, label clearly, and spend the extra few seconds making sure the cap twists tight. Good habits pay off at the bench and during safety audits.
Strong habits build confidence in results and protect the team. Investing in good storage practices for PTMA-TFSI isn’t about rule-following, it’s about respecting the science and people in your lab. Every successful synthesis or measurement starts with a dry, well-kept chemical—no shortcuts here.
Looking at chemicals like propyltrimethylammonium bis((trifluoromethyl)sulfonyl)imide, what matters most in the lab isn’t just performance. Chemical compatibility makes or breaks a research project. Years ago, I watched a team waste weeks trying to mix a novel ionic liquid with a standard organic solvent, only to realize their target compound broke down within hours. You start to appreciate how some compounds click with others and how some fights you only lose by learning the hard way.
This particular ionic liquid offers low volatility, strong thermal stability, and a knack for dissolving both polar and nonpolar materials. These features look perfect for scientists chasing higher efficiency in batteries, electrochemical cells, or green chemistry. Yet, adding it into a cocktail with other solvents or chemicals isn’t always smooth sailing. Propyltrimethylammonium bis((trifluoromethyl)sulfonyl)imide can actually cause unexpected results, especially when you toss it in with strong acids or strong nucleophiles.
Take common organic lab solvents, like toluene, acetonitrile, or dimethyl sulfoxide. Some publications, including studies in Green Chemistry and Journal of Molecular Liquids, have shown that this ionic liquid can mix well with certain solvents. They report good miscibility in acetonitrile and DMSO, for example. Yet, the story isn’t the same for alcohols or water. Water, in particular, disrupts the delicate ionic lattice, sometimes leading to unpredictable shifts in solubility or even separating out phases. That can really dull any green credentials you’re after.
Plenty of manufacturers and researchers have had to adjust their protocols after seeing reactions shut down or produce unexpected byproducts. The bulky trifluoromethylsulfonyl groups on this molecule don’t always play nice with less stable compounds. For example, halide salts or substances prone to oxidation and reduction can trigger side reactions. It only takes a small trace of moisture or an incompatible ionic partner to send things sideways.
In my own experiments, I check the literature, but bench tests tell the real story. Compatibility tests under controlled, repeated conditions reveal more than any single publication. Journals like Chemical Reviews and databases such as PubChem give detailed insight into the compatibility profiles, but every mixture reacts a little differently based on impurity sources and prep methods. Skipping a simple small-scale test run is a risk no one should take.
Cautious mixing remains key. Start with small volumes and document any color change, temperature shift, or change in viscosity. Digital resources like the ChemSpider or Sigma-Aldrich compatibility charts help, but putting eyes on the reaction—sometimes with infrared cameras or simple temperature probes—serves better than any chart. It helps to talk with peers as well. Open conversations about failures speed up progress for the whole field.
This ionic liquid isn’t just a tool for cutting-edge research—it reflects the challenges all scientists face when new materials meet old chemistries. Learning to respect the quirks of every chemical keeps work safer, faster, and less frustrating for everyone, whether you’re designing energy storage breakthroughs or scaling up for green manufacturing.
