1-Butylsulfonic-3-Methylimidazolium Trifluoromethanesulfonate belongs to the class of ionic liquids, a group of salts that remain liquid at room temperature. Each molecule possesses a core structure made up of a methylimidazolium ring—a stable, nitrogen-containing five-membered ring that features both methyl and butylsulfonic groups on the carbon and nitrogen atoms. Attached to this imidazolium cation is the trifluoromethanesulfonate anion, usually recognized in chemical shorthand as CF3SO3−. This unique pairing delivers a set of physical and chemical features that stand out when compared to conventional solvents, as well as other types of raw materials.
The full molecular formula of the compound looks like this: C8H15N2O4S2F3. The imidazolium core acts as the base, with a butylsulfonic side chain offering more stability and increased solubility in a variety of solvents. The trifluoromethanesulfonate side, one of the classic “triflate” groups, boosts both the chemical's oxidation resistance and resistance to moisture, which is a big deal for labs handling water-sensitive syntheses.
It doesn’t fall into a single shape or texture. Depending on preparation methods and purity, the material shows up as colorless to slightly yellow crystals, a sticky liquid, or sometimes as fine powder or pearl-like granules. Its melting point hovers around room temperature, often coming in as a viscous oil or sticky flakes in cooler labs. Density typically ranges near 1.4-1.5 g/cm3, though exact measures swing a bit with changing water content or co-dissolved impurities. It forms clear, stable solutions when mixed with many polar solvents. As a raw material, 1-Butylsulfonic-3-Methylimidazolium Trifluoromethanesulfonate resists evaporation and keeps its touch of slickness even after sitting open on a bench—an everyday advantage over volatility-prone organics.
The chemical lands under the Harmonized System (HS) Code segment for organic chemicals and ionic solutions. Most suppliers reference codes in the 2934 range, aligning with other previously synthesized imidazolium and triflate salts. Certificates of analysis usually detail purity above 97%. A top-tier lab synth will test for moisture content, keeping it below 0.2% to avoid hydration problems later in application.
Despite being less volatile, this salt remains a chemical that’s best handled with real care. Direct contact with skin or eyes causes irritation for most users. Its dense and sticky character encourages gloves and splash-resistant goggles when pouring or mixing. Though the compound does not readily form fumes, longer storage in unsealed containers gradually attracts water from the air, sometimes dulling its effectiveness in water-sensitive reactions. Standard ventilation procedures for chemicals help avoid buildup of airborne particles, especially from powders or after grinding. The triflate anion, stubborn against most breakdown routes, shows up in aquatic systems if accidental spills hit wastewater—so laboratory drains shouldn’t see this material. Waste streams ought to run into proper chemical collection—taking zero shortcuts helps keep triflate pollution in check.
Across industries working on green chemistry, advanced synthesis, and catalysis, this material’s ionic liquid characteristics open pathways for improved solvating power and easier product separation. It stands out from other solvents or salts, since its low vapor pressure directly cuts down on inhalation exposure concerns. Working in an electrochemical cell, I’ve seen how it stabilizes tricky intermediates during oxidative reactions. Chemists focusing on energy storage, smart polymers, or fuel cell design frequently choose 1-Butylsulfonic-3-Methylimidazolium Trifluoromethanesulfonate for its ability to conduct ions while resisting chemical wear and tear over long cycles.
The growth of ionic liquid use throws up big questions about lifecycle safety, toxicity, and final waste management. Studies indicate that although the butylsulfonic and triflate parts don’t rapidly degrade, their low volatility does reduce accidental exposure in the lab. Long-term risks from persistent residues in water or soil after disposal spark concerns about aquatic environment buildup. Greater emphasis on collection and incineration at specialized facilities can cut down on environmental persistence. Manufacturers who shift to “cradle-to-cradle” stewardship make it easier to track and reclaim these specialty chemicals at the end of their useful lives. Building up safety data with independent toxicology trials and encouraging broad data sharing go a long way in strengthening trust between users, suppliers, and regulators. If producers and end-users lean into more transparent, circular raw material systems, the promise of ionic liquids as safer, more sustainable chemical tools will keep pace with technology’s march forward.
