1-Ethyl-2,3-Dimethylimidazolium Ethylsulfate represents a class of ionic liquids growing in popularity across modern chemical industries driven by a need for more efficient and safer alternatives to volatile organic solvents. This particular compound possesses a chemical formula of C9H18N2O4S, giving rise to a molecular weight of 250.32 g/mol. The composition arises from a symbiotic pairing between the 1-ethyl-2,3-dimethylimidazolium cation and the ethylsulfate anion. Its structure establishes an effective balance between hydrophilic and lipophilic properties, helping expand its versatility across research and manufacturing applications. Intellectually, my first impression of ionic liquids was skepticism, mostly from years of working around traditional solvents that posed flammability hazards and required cumbersome disposal processes. Encountering 1-Ethyl-2,3-Dimethylimidazolium Ethylsulfate in laboratory tests changed my outlook because of its low vapor pressure and resistance to thermal degradation.
The typical form of this material can shift with temperature and manufacturing method, showing up as colorless to pale yellow flakes, powders, crystalline solids, or sometimes as a viscous liquid. Density sits near 1.12 g/cm³ at standard room temperatures, firmly higher than water but manageable in most fluid-handling equipment. It dissolves readily in polar solvents, especially water and alcohols, and holds a surprisingly broad liquid range, remaining stable from below room temperature to over 200°C without decomposing quickly. That aspect alone brings peace of mind compared to juggling glassware full of evaporating acetone or dichloromethane. As a solid, its crystalline nature makes weighing and storage convenient, with minimal risk of clumping or caking even in humid labs.
Looking at its chemical backbone reveals an imidazolium ring substituted at the 1, 2, and 3 positions, paired ionically with the ethylsulfate group. These structural decisions tweak the molecule’s viscosity, solubility, and thermal properties, putting it in a sweet spot for numerous chemical reactions and extractions. The imidazolium core resists nucleophilic attack, and the ethylsulfate side buttresses the salt’s stability against water and mild acids. Researchers often use this class of compounds for catalysis, cellulose treatment, selective separations, and electrochemical processes, pushing the edges of what older solvents could handle. On the lab bench, this ionic liquid leaves little odor, does not fog up the workspace, and rarely requires specialized ventilation. The structure and robust ionic interaction grant this substance resilience in harsh reaction conditions without the chemical footprint of legacy solvents.
Most reputable suppliers offer the compound at purities exceeding 98%. Impurities typically include trace water or leftover reactants, usually under 1%, confirmed by standard analytical methods such as NMR, Karl Fischer titration, or HPLC. Bulk material arrives as sealed bottles, kilos of fine powder or neat liquid, labeled with UN numbers compliant with international shipping, like the Harmonized System (HS) Code 294200, which marks it as an organic compound with established regulatory status for most industrial and research uses. Safety datasheets spell out handling precautions, like gloves and goggles during mixing or pouring, but standard lab ventilation handles off-gassing well.
In my experience, 1-Ethyl-2,3-Dimethylimidazolium Ethylsulfate stands safer than most common organic solvents used for extraction or synthesis. It does not flash at low temperatures or rapidly emit harmful vapors. Toxicity is mild by ingestion or skin contact, but sensible lab routines—wearing gloves, minimizing splashes—address most exposure risks. Accidental spills on the benchtop clean up without special protocols, as long as spills do not cross into areas where strong oxidizers or acids lie. Still, it counts as a hazardous chemical for regulatory purposes, calling for storage out of reach from food, drink, or poorly labeled containers. Compared with older solvents like toluene or diethyl ether, this salt’s risk factors drop significantly. Eye and respiratory irritation becomes unlikely in most real-world lab settings. For industrial handling, good practice means spill kits, local exhaust, and documented training for personnel managing bulk quantities or waste streams.
Raw production begins with imidazole derivatives and ethylsulfate precursors, both accessible in bulk and supplied by established chemical firms. Synthesis routes use clean, high-yield steps, mostly acid-base reactions followed by crystallization and vacuum drying to strip excess water. Product consistency runs high batch-to-batch—a requirement as industries move these salts from the research scale to commercial production. The resulting product finds place in green chemistry efforts, battery electrolytes, and biopolymer solubilization. This ionic liquid’s non-flammable nature makes it attractive for sustainable technology labs, where harmlessness replaces fire risk as the primary concern. As regulations tighten on solvent emissions, materials like this ionic liquid will play an ever-larger role in shaping next-generation manufacturing. For anyone building processes that aim for safer production and less environmental impact, real-world experience shows that moving away from volatile organics toward salts like these delivers both peace of mind and technical advantage.
