Chloroform, or trichloromethane, stands out as a clear, colorless liquid with a faintly sweet aroma. Its chemical formula, CHCl₃, points to a molecule built from one atom of carbon, one of hydrogen, and three of chlorine. As a well-known solvent, chloroform finds a place in research labs, industry, and sometimes the pharmaceutical world, although regulations have limited its use over the years due to safety and health concerns. People probably recognize it from stories about its use in anesthetics, but its real story runs much deeper—playing a role in the production of refrigerants, dyes, and pesticides, and as a raw material in organic synthesis. The HS Code for chloroform usually falls under 29031300, identifying it among halogenated derivatives of hydrocarbons.
A closer look at chloroform reveals a liquid that weighs more than water, with a density of roughly 1.49 g/cm³ at room temperature. It remains liquid under normal conditions, showing little tendency to convert to flakes, powder, crystals, or pearls. It exhibits low solubility in water but mixes well with a range of organic solvents. The boiling point sits near 61 °C, which makes it more volatile than some familiar household chemicals. Chloroform doesn’t have a strong color or taste, but its distinctive odor alerts people to its presence long before they might accidentally ingest or inhale a dangerous amount. When poured into a liter flask, chloroform’s weight and clarity become obvious—heavier than expected, with no hint of cloudiness or sediment.
The structure of chloroform sets it apart from many other industrial chemicals. The molecule holds a central carbon atom bonded to three chlorine atoms and a single hydrogen atom—making CHCl₃ a textbook case of a polar solvent with strong dissolving power for lipids, alkaloids, and many fats. Reactivity stays fairly low under typical storage, but the substance can decompose under strong light or heat, releasing hazardous phosgene, hydrogen chloride, or chlorine gas. The molecular weight comes in at about 119.38 g/mol, and the molecule’s linear symmetry lets chemists predict how it’ll interact in chemical reactions. Chloroform does not appear as a solid, flake, or crystalline material at room temperature. Instead, it offers a stable liquid with specific gravity high enough to sink in water.
Quality specifications for chloroform tie directly to its purity and absence of stabilizers or contamination. Industrial supply drums or laboratory bottles often guarantee more than 99% purity. Material distributed to chemical plants or research institutions usually avoids particulates, as even small solids can interfere in precision syntheses or cause unwanted reactions. Producers describe chloroform by its physical state—clear, volatile liquid—and note its compatibility as a solvent for oils, fats, waxes, alkaloids, and certain resins. Product specifications highlight density, boiling point, refractive index, and absence of stabilizers unless noted, as unstabilized chloroform can degrade more quickly.
Exposure to chloroform brings real risk, both in routine use and in the event of a spill or accidental inhalation. The substance acts as a CNS depressant—overexposure leads to dizziness, nausea, headaches, or worse. Extended contact can damage liver, kidneys, and even affect the heart. Storage demands a cool, ventilated space, away from open flames and direct sunlight. Lab workers use fume hoods during small-scale procedures and wear splash-resistant goggles, gloves, and protective coats. In larger settings, engineering controls and proper labeling become essential. Emergency protocols cover rapid evacuation, as well as the use of breathing apparatus for fire or hazardous vapor situations.
Chloroform brings challenges for both people and the natural world. Waste disposal deserves careful planning, never dumping down drains or into soil, because chloroform easily evaporates and contaminates both air and groundwater. Inhaled or ingested, the vapor harms wildlife just as it does humans. The EPA and similar agencies regulate concentration limits, pushing industry and research to control accidental releases and to improve ventilation and control systems. Workers and communities near production sites monitor local air and water, since accidental leaks can linger long after a spill.
Modern laboratories and factories look for ways to minimize chloroform’s hazards. Closed-system handling keeps vapor out of the air and reduces direct skin contact. High-efficiency filters and local exhaust systems limit exposure when open operations can't be avoided. Substitutes take the place of chloroform in applications where possible, but sometimes the unique solvent power of chloroform can't be matched. Routine training, updated safety sheets, and stricter handling rules help lower misuse or accidents. Scientific research moves toward greener chemistry, though the gap between ideal practice and industrial reality remains wide. Meanwhile, improvements in containment, real-time monitoring, and advanced personal protective equipment keep risks in check for those still working with this potent and persistent chemical.
