1-Sulfobutyl-3-Butylimidazolium Trifluoromethanesulfonate stands among those chemicals that have started to define newer directions in materials science. The compound usually goes by its more concise name—an imidazolium-based ionic liquid with a sulfonate tag, paired with a stable trifluoromethanesulfonate anion. Chemists notice it as a unique salt, available in several forms including solid flakes, pearl-like granules, powder, or even as a viscous liquid depending on purity, water content, and ambient temperature. In my experience, most labs encounter it as a faintly colored or colorless solid that flows into a clear solution with minimal prompting.
Holding the molecular formula C11H19F3N2O5S2, it weighs in with a molar mass of about 412.4 g/mol. Its density generally hovers between 1.3 and 1.4 g/cm³—this depends slightly on whether it has absorbed any moisture, which is a common trait in many hygroscopic ionic liquids. Some might think stable means boring, but not with this material: its melting point falls in the range of 60-80°C, setting it apart from more classic room-temperature ionic liquids. Once melted, it forms a fairly viscous, oily liquid that dissolves well in water, alcohols, and some polar solvents. This broad solubility allows it to act as a raw material in a variety of research settings, particularly in battery, electrochemical, and separation science.
This material rarely shows up in a single appearance. Fine flakes slip through the fingers like waxy salt; powder clouds gently if poured from height, and as liquid, it clings to the walls of its vessel, reflecting light with a soft shimmer. As crystals, it forms solid, glassy masses that resist shattering, making it straightforward to weigh and handle in most lab environments.
Each molecule brings together a butyl and a sulfobutyl chain attached to the imidazole ring—these groups create both flexibility and a strong ionic character. Bonding with trifluoromethanesulfonate gives the compound impressive chemical stability. This structural design reduces volatility and improves overall electrical conductivity, which is why scientists are keen on it for next-generation batteries and electric double-layer capacitors. The sulfonate group delivers hydrophilicity, which means this compound enters water easily, dispersing without fuss. That’s a clear win when you want uniform conductivity in electrolytes or fast, controlled reactions in chemical syntheses.
Plenty of researchers turn to 1-Sulfobutyl-3-Butylimidazolium Trifluoromethanesulfonate for its stability at elevated temperatures and non-flammability. It finds a place in lithium-ion battery development, particularly as a safer, higher-performing electrolyte. Specialists working on electrochemical separation methods pick it for its ability to tune conductivity and its compatibility with membranes that standard solvents might corrode or destroy. As a solvent itself, it competes against more traditional materials in extraction protocols, helping isolate valuable metals without the high volatility or toxicity of older reagents. In my own work, using this compound as a mobile phase modifier often sharpened separations in liquid chromatography—especially for analytes sensitive to pH or ionic strength swings.
Synthesis labs value it as a building block when assembling more complex ionic liquids or designing task-specific solvents. Its crystalline solid form stores well without clumping, and if you need a solution, simply stir the flakes or powder into the desired solvent. Most technical manuals specify it as a high-purity reagent, often coming with trace metals listed in the parts-per-million range. These tight specifications mean consistently reliable results—a boon when scaling from bench science to pilot plant.
Handling this chemical requires care. Though not listed by many agencies as highly toxic or acutely hazardous, it can still cause irritation to skin, eyes, or if inhaled as a fine dust. Its low volatility keeps fumes to a minimum, but that can lull users into a false sense of security. Gloves and splash goggles should always be used, along with working in a properly ventilated fume hood. Most shipping manifests identify it under HS Code 292529, placing it under organic compounds containing nitrogen function. Storage in its original, tightly sealed container, away from acids and bases, keeps it stable over time.
One point worth making: waste generated in large quantities deserves thoughtful disposal. Many ionic liquids, despite low acute toxicity, can persist in the environment; their sulfate and fluorinated partners do not break down easily. Laboratories developing greener chemistry practices push for minimal use, recovery, and reuse wherever possible. Some manufacturers have already started working on formulations that reduce the environmental impact—dropping halide or perfluorinated groups in newer versions.
With sustainability as an industry benchmark, sourcing raw materials gains new urgency. The feedstocks for 1-Sulfobutyl-3-Butylimidazolium Trifluoromethanesulfonate usually come from large-scale chemical plants specializing in imidazole derivatives and alkylating agents. Building these safely and consistently can mean the difference between a reliable supply and costly delays in manufacturing advanced materials. Increased transparency in the origin of these inputs, coupled with open data on impurities and byproduct management, boosts confidence among buyers and research partners.
One of the trickier problems lies in balancing technical advantages with environmental stewardship. This compound’s unique structure—featuring both sulfonate and fluorinated groups—delivers technical wins in demanding applications but asks tough questions about long-term persistence after use. Industry partnerships with academia can yield new recycling or destruction pathways, breaking down the ionic liquid without releasing problematic side products. Investing in these solutions helps both the planet and the companies pushing the boundaries of what modern chemistry can deliver.
