1-Butyl-3-Propylimidazolium Acetate, known in many research labs as a versatile ionic liquid, starts conversations for its role in chemistry and industry. This molecule, often referenced under HS Code 2925299090 for customs classifications, builds on the imidazolium family with both butyl and propyl alkyl groups attached to its aromatic ring, paired to the acetate anion. This unique structure allows it to dissolve a wide range of organic and inorganic materials, making it a true standout among salts and solvents. Its molecular formula, C12H22N2O2, and molar mass of roughly 226.32 g/mol, place it well within reach of process chemists seeking alternative solvents for demanding tasks.
This compound follows the general rule for ionic liquids: it remains liquid at room temperature, thanks to the irregular shapes and sizes of its ions. Under the microscope, its structure presents an imidazolium ring—a five-membered aromatic system—substituted with a butyl group at the first nitrogen atom and a propyl group at the third position. The presence of the acetate anion contributes to both the polarity and the solvation performance of this material. Commercial samples span a wide array of physical forms, including clear to slightly yellowish liquid, transparent viscous oil, crystals in colder labs, as well as powder or flake variants for those preferring a solid version. Densities move between 1.08 to 1.12 g/cm³ at 25°C, depending on small changes in purity or water content, making it easy to pour and measure by volume, whether in milliliters or liters.
Unlike many traditional organic solvents, 1-Butyl-3-Propylimidazolium Acetate shows near-complete miscibility with water, acetonitrile, dimethyl sulfoxide, and most polar organics. That means solubility isn’t a guessing game—solutions come easy. Its thermal stability holds up under moderate reaction conditions, surviving up to 200°C without significant decomposition. Viscosity checks in higher than water or simple alcohols, signifying strong ion interactions but still manageable for mixing applications. Many chemists note its nearly negligible vapor pressure and low volatility. That keeps lab air clean and reduces the hazards of inhalation, which marks a clear shift from volatile options like chloroform or dichloromethane. High polarity and strong hydrogen bonding capability allow it to disrupt rigid polymer matrices, dissolve cellulose, and solubilize stubborn biomolecules. In the real world, this means someone in the biofuel or plastics sector can reach for this liquid and watch substrates dissolve on contact—both a relief and a time-saver.
It’s easy to get comfortable working with an ionic liquid that barely smells and doesn’t ignite with a stray spark, but no chemical comes risk-free. 1-Butyl-3-Propylimidazolium Acetate remains stable under proper storage—room temperature, sealed container, away from moisture. Direct skin contact can cause irritation, common with imidazolium-based compounds, so gloves, goggles, and lab coats never go out of style. Accidental ingestion or prolonged breathing of dust or mist from powders, if you have the flake or crystalline form, deserves immediate attention—even though the compound refuses to volatilize, you don’t want to test its toxicity. Waste needs collection in a labeled, chemical-resistant container for specialty disposal; it may not rank as hazardous under every country’s regulations, but environmental stewardship requires careful separation from water supplies. Raw materials for synthesis usually stem from 1-butylimidazole, 1-bromopropane, and sodium acetate, coming together in a straightforward alkylation and metathesis process. These feedstocks supply a reliable route to a pure, reproducible end product for companies keeping a close eye on quality and regulatory paperwork.
Many researchers would argue ionic liquids like 1-Butyl-3-Propylimidazolium Acetate push boundaries unreachable with mineral acids and simple alcohols. Take cellulose processing for bioplastics—where typical solvents only swell the polymer, this acetate salt breaks hydrogen bonds and brings everything into solution. Scientists in CO₂ capture and biomass fractionation have adopted it for its impressive dissolving power, allowing them to build systems that extract value from agricultural waste. The high ionic conductivity and large electrochemical window make it an attractive candidate for next-generation batteries or capacitors. It also finds its way into catalysis, electrochemistry, and as a non-volatile solvent in fine chemical processes. As someone who values safety in the lab, the appeal of working with a compound that doesn’t evaporate into the air or catch fire cannot be overstated. In scale-up scenarios, the ability to recycle the liquid, recover products cleanly, and reduce hazardous waste shines as both a cost and environmental advantage.
Ionic liquids like this do not solve every problem. Viscosity at lower temperatures slows mixing and transfer. Traces of chloride or bromide left from synthesis affect product purity, which can disrupt sensitive downstream reactions, especially in pharmaceuticals or battery research. Disposal practices still face scrutiny because emerging data on aquatic toxicity suggest caution. Developers design greener, biodegradable analogs and improve purification steps, looking for highly pure, low-halide products. For teams struggling with high price tags compared to traditional solvents, recycling protocols and vendor partnerships offer cost-savings over single-use approaches. In my experience, open conversation with raw material providers and regular updates on safety legislation keeps the process lean and compliant, without putting quality or the planet on the line.
