Looking back, imidazolium-based compounds changed the way many labs worked with ionic liquids. The path to creating 1-Sulfobutyl-3-methylimidazolium inner salt traces through decades of trial and error. Chemists realized early on that imidazolium rings mixed with functional side chains opened up new chemical territories. Organic and inorganic researchers alike hopped on board in the late twentieth century, growing tired of traditional solvents that lost their edge at higher temperatures or corroded delicate glassware. Tinkering with butyl sulfonic acid groups and methyl substitutions on the imidazole core gave rise to this zwitterionic inner salt. As journals began publishing successful syntheses, academic and industrial chemical labs turned to these salts for easier handling of ionic systems, energy storage materials, and as parts of green solvent initiatives.
1-Sulfobutyl-3-methylimidazolium inner salt looks like an off-white crystalline or powdery material, dissolving well in water and some polar organic solvents. Its zwitterionic structure means it packs both a positive charge on the imidazolium ring and a negative charge from the sulfonate tail on the same molecule. That balance makes it stable, even outside the bottle. It stands out in the sea of ionic liquids and salts thanks to hardiness against hydrolysis and a knack for dissolving tricky compounds like cellulose and certain transition metal complexes. Researchers value it for use in catalysis, electrochemical systems, and biocompatible extraction protocols.
This salt tends to form a solid at room temperature, melting at a temperature usually above 200°C, though the exact point swings a bit based on purity and moisture. It avoids decomposition until higher temperatures, giving it a leg up as a heat-resistant choice compared to standard imidazolium salts that rely on counterions for stability. The robust sulfonate group keeps it from breaking down easily under acidic or basic conditions, which comes in handy for reaction setups full of surprises. Its high polarity and ability to shuttle ions without clogging up reaction pathways earned it a spot as a favored additive for synthesis, separation, and materials design.
Chemical suppliers list purity levels, usually upwards of 98%. Product labels mention the CAS number 719010-52-7, structural formula, recommended storage (dry, cool conditions), and cautions about moisture absorption. Companies provide material safety data sheets with full breakdowns of molecular weight, melting point, solubility profile, and batch-specific spectral data. Knowing the fine details — including impurity profile and water content — matters especially for researchers seeking reproducible results in sensitive experiments like high-end battery development or pharmaceutical processes.
Preparation starts by alkylating 1-methylimidazole with a sulfonate-containing butyl halide. In a stirred, heated flask, the reactants move through a nucleophilic substitution, bringing the butyl group with its sulfonate moiety onto the nitrogen. The purification steps almost always include extraction, rotary evaporation, recrystallization, and drying under vacuum. Operators often test the end material by NMR, IR spectroscopy, and elemental analysis to confirm the full switch from separate building blocks to the intended zwitterionic final compound.
Beyond the basic synthesis, the inner salt structure gets tweaked to create derivatives that change solubility or thermal properties. Researchers attach longer alkyl chains or swap in various functional groups to suit specific applications. Reactions with metals or complex organics give birth to coordination compounds that push into areas like rare earth recovery. Adding or replacing groups on the imidazolium ring can tune the chemical reactivity, making a single family of materials fit tasks across catalysis, separation, and even drug delivery.
Suppliers and researchers often call it “SBMIM inner salt,” “1-Sulfobutyl-3-methylimidazolium betaine,” or “BMIM-SO3.” Some trade names pop up in catalogs, especially from manufacturers serving the fine chemicals or biotechnology markets. These synonyms show up in patents, publications, and safety documents, so using the correct name avoids confusion between the zwitterion and other imidazolium salts carrying external anions.
Handling always deserves respect, even with well-tested lab salts. Users should wear gloves and goggles and work in a well-ventilated space, keeping the powder off skin or eyes. Fine dust causes mild, temporary irritation if inhaled or touched, according to standard safety reports. The product is not known for high flammability or acute toxicity, yet good lab practice dictates cleanup with solid absorbents and careful disposal via approved chemical waste streams, never dumping down drains or general garbage bins. Storage in tightly sealed containers with a desiccant adds a layer of protection against water uptake, clumping, or slow degradation. Facility managers often post quick access safety protocols to keep accidents rare.
Thanks to its zwitterionic nature, 1-Sulfobutyl-3-methylimidazolium inner salt bridges gaps between aqueous and organic phases. Its role as a solubilizer opens doors in pharmaceutical extraction, textile dyeing, and specialty polymers. Electrochemists turn to this salt for creating high-performing, stable electrolytes in energy storage — batteries, supercapacitors, and even in metal plating baths. Its resistance to microbial and enzymatic breakdown means it can stabilize chemical environments that would chew up regular salts. Some teams blend this compound into membranes for fuel cells, aiming to boost ionic conduction with less swelling or mechanical failure over time. Environmental chemists see a chance to use the inner salt in developing “greener” systems, replacing hazardous solvents or surfactants with something more stable and less polluting.
Several university labs and R&D companies poured resources into understanding and improving this class of salts. Projects range from scaling up production without introducing excess impurities, to exploring how modifications affect ionic movement and electrochemical window. Open literature documents thousands of experiments with SBMIM-based materials in fields like enzyme catalysis, hybrid solar cells, and nucleic acid isolation. Researchers also dive into computational modeling, looking at how microstructure impacts macroscopic behavior, whether that is in viscosity, conductivity, or compatibility with other functional materials. Every new insight seems to generate two more questions—the mark of a dynamic research landscape.
Most published data points to low acute toxicity in standard cell culture and fish embryo assays. Chronic exposure at high levels still raises unanswered questions about environmental fate, so responsible research always keeps possible long-term effects in mind. Some independent groups monitor breakdown byproducts in water and soil, checking for persistence or bioaccumulation. Labs in Europe and Asia uncovered that SBMIM inner salt breaks down more readily than older ionic liquids carrying halide anions, suggesting a lower risk to the environment if spilled in small amounts. Regulators and scientists continue to assess how repeated or large-scale use might play out, especially with expansion into consumer products.
Researchers looking years ahead point toward tailored variants for battery technologies, improved catalysts that cut out waste, and safer solvents for biomedical and green chemistry. The growth of electric vehicles and renewable energy pushes industry to explore imidazolium inner salts as durable and eco-friendly support tools. Academic groups chase questions about fundamental behavior—how does the bulky, charged zwitterion interact with proteins or nanostructured materials? Companies invest in developing hybrid formulations for smart coatings or advanced recycling systems. With more funding and cross-disciplinary efforts, new applications keep arising, keeping 1-Sulfobutyl-3-methylimidazolium inner salt at the forefront of advanced materials science.
1-Sulfobutyl-3-methylimidazolium inner salt might sound like something out of a chemistry textbook, but people who work in labs often talk about it like an old reliable friend. I’ve come across it most in the context of developing solvents and electrolytes – not just for the sake of research but because real products need to perform better in ways that count in daily life. This compound stands out thanks to its ionic liquid properties. It stays stable over a range of temperatures, carries low volatility, and handles high thermal loads without drama. These are exactly the sorts of traits that become valuable in industries looking for safer alternatives to traditional solvents.
Walk through any research group focused on batteries and you’ll probably spot a bottle of this substance somewhere on the shelf. The world keeps searching for energy storage options that don’t catch fire or lose power quickly. Lithium-ion batteries, supercapacitors, and next-generation devices each ride on the quality of their electrolytes. I’ve noticed that swapping out conventional materials for ionic liquids, like this inner salt, can mean longer battery life and decreased chances of short-circuits. Fewer accidents, more charge cycles—these are not just lab goals but needs that real people face as we ramp up electric vehicle adoption and renewable energy storage.
Anyone who’s tried purifying a stubborn chemical knows the pain of never quite getting rid of troublesome impurities. This inner salt helps with separation and extraction jobs, especially when targeting precious metals or dealing with pharmaceutical intermediates. Compared to old-school organic solvents, this class of compounds produces less toxic waste and slips more neatly into processes looking to lighten their environmental load. In my own experience, cleaner separations mean less downtime and safer working conditions, which every plant worker or lab technician can appreciate.
Catalysis sounds highbrow, but it intersects with daily life more than most people realize. Making plastics, pharmaceuticals, even basic consumer chemicals often hinges on finding the right environment for reactions to happen efficiently. The versatility of 1-sulfobutyl-3-methylimidazolium inner salt lets chemists fine-tune those reaction conditions rather than crossing their fingers with harsher acids or bases. Besides making the process safer, this approach eats up less energy—a welcome improvement when utility bills seem to surge every year.
Real change takes more than introducing a single new molecule. While this inner salt brings plenty to the table, industry and research leaders weigh costs, supply chain reliability, and potential surprises in long-term use. I’ve seen projects stall due to sourcing issues or undiscovered breakdown products, which underlines the need for good partnerships across manufacturing, regulatory agencies, and academia. Companies pursuing safer, cleaner processes find compounds like these worth a closer look, but they succeed only by making sure new materials fit into existing systems without hidden costs.
Trust grows from open data, careful peer review, and practical field trials. Credible sources, including peer-reviewed journals and manufacturers with transparent safety records, point toward the potential of this compound in reducing environmental harm and improving workplace safety. The best results come from keeping lines of communication open—across supply chains and between researchers and users. My own experience in new material adoption shows the most successful solutions start with real needs and honest feedback, not just the promise of a miracle chemical.
1-Sulfobutyl-3-methylimidazolium inner salt isn’t something you spot on a grocery store shelf, but its structure draws steady interest from chemists working on modern solvents and ionic liquids. This compound belongs to the world of imidazolium derivatives—molecules essential to advanced materials research, especially where green chemistry stands front and center.
At the heart of this molecule lies an imidazolium ring, a five-membered ring packed with three carbons and two nitrogens. On one side, a methyl group hangs off the third position, which already pushes the molecule toward increased stability and low melting point—a feature that gives ionic liquids their reputation for versatility. The real story, though, happens at position one, where a butyl chain attaches to the ring.
Now, rather than ending that four-carbon chain with another typical group, chemists finish things off with a sulfonic acid anchoring point. The sulfo group carries a notable negative charge, and the imidazolium ring brings the positive. Instead of letting these opposites attract as separate ions, this molecule keeps both groups chained within the same molecule, forming what chemists call a “zwitterion”—or, more specifically, an inner salt. Cross-sections of its structure look like this: C1=N-C3(–CH3)-N-C5(–CH2CH2CH2CH2SO3–), giving each section a clear identity and function.
Ionic liquids get their unique qualities by mixing hefty, unevenly paired charges in a liquid state at room temperature. The inner salt form packs a positive and a negative group right in the same molecule. The result? Unexpected benefits, including better ionic conductivity, increased thermal stability, and a strong shot at reducing environmental harm compared to many conventional solvents. University labs and startups both dig into these compounds while aiming to cut out volatile organic solvents—a growing concern for those keeping an eye on health and climate.
From personal experience working in a graduate chemistry lab, synthesizing zwitterionic imidazolium compounds isn’t a walk in the park. Keeping moisture out, chasing pure samples, and dealing with their sticky, sometimes oily textures require a fair bit of skill. Still, the outcome justifies the hassle. The unique structure encourages researchers to test them as electrolyte additives, safe cleaners, or even as bases for drug delivery methods. Having both charges within a single molecule also helps reduce issues with ion exchange and leaching—problems that have plagued traditional ionic liquids in real-world applications.
Chemical innovation always faces practical roadblocks—scaling up precise reactions, keeping processes eco-friendly, and making sure materials meet safety standards. For 1-sulfobutyl-3-methylimidazolium inner salt, questions remain about raw material sourcing and long-term environmental effects. The good news: researchers continue to test these salts in fields ranging from battery technology to biomedicine, aiming to find sweet spots between performance, recyclability, and safety.
Sure, it’s a molecule with a mouthful of a name, but its design shows what happens when chemistry shaves off the rough edges and aims for cleaner, smarter solutions. The next time you read about ionic liquids replacing old-school solvents or powering better batteries, there’s a strong chance a cousin of this quirky inner salt played a part along the way.
Anyone who’s worked in a lab or a chemical storeroom knows what happens when you take proper storage for granted. I’ve seen a few bottles leak during summer, and cleaning up isn’t fun or safe. So, the way we handle and store chemicals like 1-Sulfobutyl-3-methylimidazolium inner salt can mean the difference between safe working conditions and disaster.
Unlike standard salts or organic solvents, 1-Sulfobutyl-3-methylimidazolium inner salt often appears nearly odorless and stable at room temperature. Even though it has a neutral charge overall, it combines ionic and organic features, making it useful in ionic liquid applications and catalysis. But don’t let appearances fool you: it still brings risks that improper storage can increase, especially in humid or unregulated conditions.
Temperature control plays a big role here. From experience, any chemical that spends too much time in hot or fluctuating temperatures can start to degrade or clump up. Room temperature, somewhere between 20°C and 25°C, usually keeps the salt stable. Avoiding direct sunlight prevents unnecessary heating and keeps the bottle label readable for next time.
Moisture is another enemy. 1-Sulfobutyl-3-methylimidazolium inner salt can absorb water from the air, which messes with experiments and can change the product’s behavior in reactions. Airtight containers and desiccators offer reliable solutions. Labs with high humidity will want to check their seals and silica gel packets regularly. I’ve seen chemical powders turn sticky overnight when someone left the jar unsealed, resulting in lost material and wasted time drying it back out—or throwing it away if purity suffered.
Accidents usually start with unclear labels. Clear, legible writing and a proper hazard symbol on every bottle mean fewer mix-ups. People lose track of stock or even mistake one salt for another when someone gets lazy with the label. Experienced chemists always double-check and keep a logbook or digital inventory up to date. From my own lab days, a quick look at the chemical log saved me from using the wrong batch more than once.
This inner salt stays stable under normal conditions, but it’s smart to keep it separated from strong oxidizers or acids. This isn’t paranoia; accidental mixing can release dangerous fumes or cause unintended reactions. I once saw a storage shelf that kept all reactive components in a separate, locked cabinet—no incidents there for years.
Disposal can become complicated if storage goes wrong. Take care of spills or expired product using a container suited for ionic compounds, and follow local regulations. Rinsing the mess down the sink doesn’t just break rules—it risks harming equipment and the environment. My old supervisor insisted on dedicated waste containers, which kept hazardous waste manageable and safe.
A clean, organized storage system leads to fewer accidents, less waste, and longer-lasting supplies. It’s common sense, but easy to forget during a busy day. Building these habits keeps everyone safe, saves money, and protects hard work from careless mistakes.
I’ve run into 1-Sulfobutyl-3-Methylimidazolium inner salt during a stretch in an academic research lab. The long name throws many for a loop, but folks in chemistry circles just call it an ionic liquid—one in a growing family. Some call it “green” chemistry, because these materials help swap out more traditional organic solvents. The safety story, though, isn’t as clear-cut.
Pull up an SDS from reliable suppliers and the odd thing about this compound jumps out—there’s not much information. No piles of horror stories or gory animal test data, but that blank space isn’t comforting. Companies hedge their bets, recommending gloves, goggles, maybe even a fume hood. Because you never really know. The shortage of data doesn’t mean this inner salt is safe; it means scientists haven’t had enough time or money to run every test.
The chemical structure offers a few clues. It features a chunky imidazolium ring and a sulfonate group—both known to interact with cells in ways that could disrupt regular biochemistry. Peer-reviewed toxicology reports don’t suggest it’s as rough as hydrogen fluoride or old-school solvents like benzene, but skin and eye irritation come up every time. I’ve splashed similar ionic liquids on my hand. That tingling and dryness that follows always makes me jump for the sink and soap. Lingering worry sets in about long-term exposure.
Other ionic liquids have taught us not to get too comfortable. A lot of these compounds promise lower volatility, so you smell or breathe less compared to regular solvents. While that feels safer at first, it also means spills and residues are harder to catch. Low vapor doesn’t mean it can’t seep through skin, or that it breaks down cleanly. Several studies show that even “non-volatile” liquids still end up in wastewater or soil, sticking around longer than the manufacturer planned. Some can harm aquatic life even at low levels.
Every researcher I know treats new chemical formulations—especially ones like this inner salt—with healthy respect. Gloves and goggles are non-negotiable. Nobody pipettes ionic liquids by mouth, but every so often someone in a hurry does cut a few corners. Poor habits creep in when a material sits around long enough and nobody’s had an accident...yet. It’s easy to forget these liquids are engineered blends, not products with a track record stretching back to the days of chloroform or acetone. Anyone working with them becomes the test case for chronic exposure, stretching the boundaries for what a body can tolerate.
People ask: is it hazardous? It’s not radioactive or obviously carcinogenic, but it’s not sugar water either. Good lab practice shapes risk: always minimize skin contact, use ventilated areas for any work involving dishes or flasks, and seal containers right away. Keep a habit of washing hands after use. For work settings, waste disposal needs its own plan—don’t pour leftovers down the sink without checking the latest guidelines. Many universities maintain special collection bins for new classes of chemicals, and for good reason. These steps aren’t about paranoia, but about respecting new chemistry and its unknowns.
Sometimes the safest thing is simply taking a chemical for what it is: a tool that works, but one not fully mapped out yet. Waiting for decades of toxicity studies isn’t possible in the fast pace of modern labs, so trust your instincts and the gear designed to protect you. That keeps the surprises in the fume hood, not on your skin.
Anyone who’s spent hours in a lab knows the struggle: a new compound on the bench, white powder or sticky oil, and not a clue what it’ll do once it hits water. 1-Sulfobutyl-3-methylimidazolium inner salt, often called a zwitterion, usually greets water with open arms. This compound, with its split personality—a positively charged imidazolium ring and a negatively charged sulfonate tail—plays a unique game with solvents. In real-world lab tests, it slides into water right away, giving clear solutions at concentrations much higher than most organic salts even dream about.
Researchers appreciate these ionic liquids for more than their quirky names. The story of solubility starts with curiosity but ends up shaping new drug formulations, greener reaction solvents, and advanced batteries. One test with 1-sulfobutyl-3-methylimidazolium inner salt dissolving in water proved to me just how thirsty this compound gets for polar environments. Most published numbers put its solubility above 100 grams per 100 milliliters—you could call that “miscible,” or simply “it just doesn’t quit.” Drop it in, stir a moment, and watch that stubborn clump melt away. This isn't just convenient. Good water solubility slashes costs in purification, turns tricky reactions easy, and sometimes even helps recycle solvents.
Stick this zwitterion in alcohols such as methanol or ethanol, and it puts on a pretty good show there too. Not as ragingly enthusiastic as with water, but still plenty soluble. Ethanol can take a few grams per 100 milliliters without trouble. Once, out of curiosity, I tried dissolving it in acetonitrile—minimal luck. Same for acetone and most chlorinated solvents. Its love affair with polar protic solvents traces back to the charged groups in the molecule. The lesson is simple: if you need to use it in anything except water or short-chain alcohols, expect to work harder or try tricks like heating and co-solvents.
Tossing this compound into a beaker full of water is one thing. Scaling up is another. The high solubility sometimes brings headaches with crystallization and drying down. In one batch, overnight vacuum left a sticky oil that wanted to keep every drop of moisture. Turns out, its hygroscopic nature (water-loving trait) lives up to the reputation. Stick to drying under high vacuum or next to desiccant, and weigh samples quickly. Otherwise, the measured mass can creep up as it snags water from the air. Storage in tightly sealed bottles saves a lot of later frustration.
Big labs and startups both search for safer solvents and friendlier production steps. Zwitterionic liquids like this one sometimes replace harsher, less ecologically sound alternatives. But labs need to stay alert. High solubility means spills and waste can move rapidly into wastewater streams. Careful collection, handling, and waste treatment cut down risk. Some groups filter or use reverse osmosis to keep these compounds out of the drain. I’ve seen teams succeed with strict checklists and simple training, keeping things both green and compliant with regulations.
Anyone needing reliable, high solubility in water has a strong candidate here. For anything non-polar or only weakly polar, save yourself the headache and pick something else. Handling challenges—mostly the sticky, hygroscopic nature—pop up often, but nothing a careful hand and some extra preparation can’t beat. These quirks are just part of life with truly water-soluble salts in the modern lab.
