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Few molecules tie past to present chemical innovations quite like 1,3,5-benzenetricarboxylic acid, more widely known as trimesic acid. Chemists dug into aromatic carboxylic acids back in the 19th century, seeking molecules to thread through dyes, surging fuel needs, and emerging pharmaceuticals. Trimesic acid emerged from coal tar and crude oil, products that powered countries and entire industries. Early studies zeroed in on its symmetry and the way its three carboxyl (COOH) groups shaped reactivity. Chemists like to look for template molecules, and trimesic acid, with its rigid benzene ring and three evenly spaced arms, offered just that. Over the decades, it found regular mention in research focused on building blocks and frameworks, signaling a shift from basic understanding to tailored molecular design.
Trimesic acid shows up as a pure white powder, crystalline in form and readily available in chemical supply houses for labs and large-scale industry needs alike. The three carboxyl groups on the benzene core draw in both newcomers and experienced researchers, who see its potential in coordination chemistry, especially in forming complex metal-organic frameworks (MOFs). Chemists see this molecule as a scaffold with wide potential in modern chemical synthesis, not just another lab curiosity. I’ve handled this compound myself in research projects aiming to create porous materials for gas capture; its unique shape played a critical role. So, whether the aim is to produce high-performance coatings or novel drug carriers, trimesic acid often sits near the start of the story.
This compound melts at temperatures just above 340°C, stays stable up to that point, and dissolves best in polar solvents like water or ethanol at elevated temperatures. Its structure, shaped by strong hydrogen bonding between carboxyl groups, resists breakdown under ordinary conditions. In my experience, its limited solubility at room temperature can be a nuisance for those aiming for reactions in aqueous solution, but this trait also forms the backbone for its use in controlled crystal growth. Unlike more volatile acids, trimesic acid remains non-hygroscopic. Its high melting point and low volatility make it a good candidate for applications needing temperature stability. Physically, it's inert in standard laboratory air, but once heated or added to reactive chemistry, the carboxylic groups spring into action.
Specification standards for trimesic acid focus on purity, often demanding levels above 98%. Impurities like isophthalic and terephthalic acids can slip in during certain synthesis routes, changing the reactivity and sometimes fouling reactions downstream. High-purity material usually gets packed in air-tight, moisture-resistant bottles to prevent the rare, but possible, uptake of ambient water vapor. Labels stick to chemical shorthand—C9H6O6, CAS number—and hazard statements reminding handlers of its mild irritant properties. All the samples I’ve ordered came with a clear batch record and analytical profile, reflecting growing demands for traceability and responsible sourcing in chemical manufacturing. Such protocols stem from creeping regulatory oversight and an industry shift toward transparency, especially as chemicals like this support everything from industrial resins to consumer-end polymers.
Commercial and research needs led to several synthetic paths for trimesic acid. The most common method starts with oxidation of mesitylene using strong oxidants—nitric acid or potassium permanganate hold court here. Exothermic reactions, vigorous evolutions of heat and gas, punctuate the process. Acidic workups and careful filtration yield the pure, snow-white crystals that define this compound. Laboratories seeking smaller amounts often rely on catalytic oxidation, using robust metal catalysts to steer the reaction with less waste. Some green chemistry routes use enzymatic or alternative oxidation systems, but these haven’t overtaken the chemical stalwarts yet. Simple in principle, but anyone who’s scaled up this reaction knows the devil hides in managing heat and handling last traces of unreacted aromatic compounds.
The carboxyl arms of trimesic acid beg for modification, drawing in reagents ranging from basic alkylation agents to sophisticated organometallic complexes. Acid chloride formation opens the door for amide, ester, and anhydride synthesis—key steps in advanced polymer chemistry. Sharper minds than mine have used trimesic acid to build MOFs, anchoring metal ions into robust structures for gas storage and separation. In research, I’ve seen it serve as the backbone for dendrimers and supramolecular assemblies, hooking in new chemical groups at each available site. Rigidity of that benzene ring, coupled with predictable reactivity, lets scientists build up from trimesic acid like blocks in a molecular game. Reactivity with primary amines or alcohols produces a suite of derivatives, ensuring it never becomes just another bench-top relic.
Anyone digging through literature finds this acid cropping up under several names—trimesic acid, benzene-1,3,5-tricarboxylic acid, or just BTC in shorthand. Some older chemical catalogs listed it as tricarballylic acid, but most current references steer toward the more accurate benzenetricarboxylic acid or BTC. No matter the name, its identity as a tri-functional carboxylic acid speaks loudest in both academia and industry. A variety of suppliers market it by its formal chemical identity alongside common naming conventions, reflecting evolving naming standards and global supply chains.
Trimesic acid poses limited risk under usual lab handling. Dust irritation can crop up with careless weighing or if users neglect gloves and eye protection. MSDS documents mark it as a low-hazard irritant, urging standard precautions—ventilation, modest eye and skin protection, and care in waste disposal. In my years in the lab, students only saw trouble when they treated it with the same nonchalance as table salt. Process engineers and handlers in industry work with far greater volumes, but safety moves up with scaled processes—managing heat during synthesis, preventing over-pressure during sealing, and storing away from strong reducing agents. Regulatory bodies keep the pressure on, expecting adherence to regional workplace safety protocols, mainly for bulk processors. Trimesic acid demands respect, but it rarely appears on lists of chemicals causing acute danger.
Applications run wide, with trimesic acid leading the charge in advanced materials. MOF research, a growing field, leans heavily on trimesic acid for its symmetry and stability, letting scientists design cages for carbon dioxide or hydrogen with atomic precision. From there, its influence spreads to plasticizers, specialty resins, and engineered surface coatings that need chemical resistance and thermal strength. I've seen trimesic acid derivatives improve performance in proton exchange membranes for next-generation fuel cells, an area hungry for durability and reliability. Pharmaceutical projects occasionally reach for trimesic acid scaffolds when tinkering with rigid, multi-site molecules. Dyes and pigments, though not the hotbed of innovation they once were, benefited from its reactivity in decades past. Even water treatment options pop up, where porous polymers made from trimesic acid catch unwanted metals or organic contaminants. Applications shift as new research takes hold, but trimesic acid never loses relevance.
Current trends in research push trimesic acid beyond its classic roles. MOFs made with trimesic acid now fuel studies on gas sensing, safe hydrogen storage, and selective molecular recognition. My own work in post-graduate research saw trimesic acid at the heart of self-assembled monolayers, exploring how changing pH or ionic strength can drive or disrupt nanostructure formation. Patent databases reflect a surge in trimesic acid-based materials for environmental cleanup and advanced batteries. Universities and private sector labs across Europe, Asia, and North America look to optimize synthesis, boost recyclability, or swap out harsh oxidants for greener methods. As climate and sustainability mandates steer R&D spending, molecules like trimesic acid will form the backbone for new products that bridge green chemistry and high performance.
Trimesic acid produces little acute toxicity, a far cry from many basic laboratory acids or aromatic derivatives. No chronic effects are well-documented in standard laboratory exposures, but researchers still call for caution—especially with long-term inhalation or ingestion not well studied. Environmental toxicity data suggest it decomposes under severe oxidation, posing low long-term persistence. Worker safety standards focus on accidental exposure—skin irritation, minor respiratory discomfort with dust, and rare allergic reactions. In my years mentoring students, none suffered more than brief discomfort from accidental exposure, but chemical hygiene officers always urged prompt cleanup and ventilation. Toxicological scrutiny keeps pace with its expanding use, and regulatory bodies occasionally probe for new data as inventive applications emerge.
Eyes look to trimesic acid as the demand for tailored materials and green synthesis approaches grows. The shift toward sustainable chemistry means future production could rely on biobased aromatics or alternative oxidation catalysts, chipping away at fossil fuel reliance. MOFs made from trimesic acid will play a role in carbon capture, energy storage, and emerging separations for clean water and air. My perspective, rooted in bridging academic research and industry translation, suggests trimesic acid has more futures ahead than behind. It anchors breakthrough science today, opening the door for safer, smarter, and more sustainable chemical processes. Ongoing collaboration between academic, industrial, and regulatory spheres ensures this molecule never sits idle, pushing innovation across a growing list of fields.
Scientists and manufacturers have come to depend on 1,3,5-Benzenetricarboxylic Acid, also called trimesic acid, for good reason. It stands out among aromatic acids because of its three carboxyl groups arranged symmetrically on a benzene ring. That simple arrangement allows the molecule to form strong hydrogen bonds and network structures, leading to a surprising range of practical uses.
Everyday products and high-performance technology both benefit from BA3C’s unique structure. In my experience working with polymers, performance and versatility count. Manufacturers use this molecule in the production of polyesters and polyamides, where it acts as a building block that brings rigidity, heat resistance, and durability to the final material. Think about plastic films used in electronics, packaging that protects food from spoilage, and fibers woven into clothing—these materials come out tougher, more stable, and more reliable thanks to this single compound.
Engineers also turn to BA3C as a key component in the synthesis of metal-organic frameworks (MOFs). MOFs have shot up in popularity for their ability to trap gases, which plays a role in fields such as clean energy, gas storage, and even air purification. The large surface area and tunable pores in these frameworks trace right back to trimesic acid’s molecular shape and binding ability.
Pharmaceutical and research labs have found a host of uses for trimesic acid. Its ability to help build stable crystals makes it valuable in drug delivery and diagnostic tests. Labs use it as a starting material when synthesizing more complex organic compounds. There’s always a demand for purity and precision in medicine; this acid helps control reactions and yields clean products, giving people consistent results in trials and treatments.
Researchers working on separation technologies, such as chromatography, use this acid to develop better stationary phases and to modify surfaces. By doing so, they improve separation accuracy, making sure we get clean readings in biochemistry and quality control tests. Anyone who has ever had a critical medical test or works with industrial quality checks benefits, even if indirectly, from these advances.
My background in sustainable product development keeps me thinking about chemical impacts on the planet. 1,3,5-Benzenetricarboxylic Acid has potential for greener chemistry. Researchers rely on its ability to create water-stable frameworks and absorbents to filter contaminants, remove heavy metals, and capture carbon dioxide. These solutions don’t just look good on paper—they really work and create cleaner spaces for everyone.
Wastewater treatment and gas separation technologies grow year by year. As demand for sustainable solutions increases, this molecule keeps delivering. It has the right mix of stability and reactivity, so it stands up in harsh conditions and still performs its job.
Not every chemical makes its way from the lab bench to large-scale industry, but the track record of 1,3,5-Benzenetricarboxylic Acid speaks volumes. Engineers, scientists, and medical professionals count on it because it simplifies manufacturing, creates stronger products, and paves the way for cleaner technologies. As new challenges emerge—whether in sustainability, healthcare, or advanced technology—BA3C keeps finding fresh ways to matter.
1,3,5-Benzenetricarboxylic acid, also known as trimesic acid, pops up in a surprising number of chemistry discussions, thanks to its neat symmetry and stubborn stability. Looking at its chemical formula, C9H6O6, you get nine carbons, six hydrogens, and six oxygens. This arrangement isn’t there by accident. This molecule belongs to the family of aromatic carboxylic acids, drawing structure from a benzene ring that sprouts three carboxyl (–COOH) groups at the first, third, and fifth positions.
Start by picturing a benzene ring—a hexagon built from six carbon atoms, each bonded to one hydrogen. In trimesic acid, three of those hydrogens are gone. Carboxyl groups swoop in, one each at the 1, 3, and 5 spots. If you sketched this molecule, it would almost look like a three-bladed fan, each blade jutting out at even intervals around the ring. That’s symmetry in action, and it’s more than just pretty on paper. This layout gives the compound special properties, including high melting point (over 300°C) and resistance to easy breakdown.
The full chemical formula—C6H3(COOH)3—spells it out clearly. Each “COOH” stands for a carboxyl group. Line them up on a benzene ring, and you don’t just have another acid; you get a building block used in stuff like metal-organic frameworks (MOFs). These MOFs matter because they soak up gases like carbon dioxide or hydrogen, so scientists and engineers look to trimesic acid as a way to tune materials for energy storage or carbon capture.
Diving into chemistry, I’ve seen undergrads stare at these names, not realizing they’re dealing with real, useful tools. Trimesic acid has helped push forward research in advanced filtration membranes. These membranes screen out pollutants, hold on to clean water, and last longer, all thanks to tough aromatic acids like trimesic acid locking them together. The unique shape and functional groups let it grip metals, leading to frameworks with customizable spaces—almost like Lego blocks at the nanoscale.
Applications stretch into pharmaceutical synthesis, where binding to metals can spark reactions not possible with other acids. This matters for designing targeted drug delivery or fabricating sensors that pick up faint chemical signals. Environmental tech keeps moving forward because scientists use these stable, multi-armed molecules to anchor complex networks for capturing unwanted molecules from the air or water.
Most handbooks report trimesic acid as low in toxicity, but it pays to handle powders and acids with care—nobody wants random exposure in a lab. Following chemical hygiene rules stands out as the responsible approach. Watching how researchers keep finding new ways to snap these molecules together gives me optimism. Every year, journals fill up with articles tweaking the basic structure to make stronger, lighter, or smarter materials.
As interest in sustainability grows, trimesic acid’s potential to build better filters, batteries, or catalysts makes it worth understanding at a molecular level. Chemists might shrug at yet another benzene derivative, but the device in your pocket or cleaner air in your city could someday owe a debt to these six carbons, three acids, and decades of clever research.
1,3,5-Benzenetricarboxylic acid, sometimes known as trimesic acid, isn't a household term. Yet, for labs and industries working with specialty polymers or research chemicals, it’s anything but obscure. It looks like a fine crystalline powder and usually grabs attention for its usefulness in making certain plastics or dyes. Manufacturing processes can’t ignore the risks it brings if the storage or the handling gets sloppy.
Crowded shelves, mislabeled bottles, leaky caps — I’ve seen how that kind of chaos turns a simple chemical store into a safety nightmare. 1,3,5-Benzenetricarboxylic acid doesn’t explode without warning or catch fire at room temperature. Still, it reacts if it meets the wrong material. Storing it in tightly sealed glass containers, away from bases and oxidizing agents, prevents headaches nobody wants.
Moisture brings its own set of problems. Left open, this chemical will start caking, clumping, and degrading. Too much water vapor kicks off hydrolysis, which ruins the purity. Dry shelves and humidity controls protect the integrity of stock. I learned all too quickly from a ruined batch the cost of ignoring the obvious: even a day on the wrong shelf can turn expensive stock into waste.
You might think gloves and goggles do enough. That’s a start, but sliding through a dusty hood, not washing exposed skin, or leaving behind chemical traces opens the door to trouble — both for people and for research. Breathing in the dust causes irritation, so a dust mask isn’t optional when measuring or transferring. Working inside a fume hood works better than relying on open benches or basic fans.
Splashy spills rarely happen if containers fit well and stay labeled. Clear labeling, along with a tidy workspace, saves labs a lot of grief. One glance at a shelf cluttered with faded tags always makes me worry. Good labels with hazard symbols and the full name cut confusion, especially when multiple projects overlap.
Ignoring storage guidelines costs more in the long run. Bad smells, stains, or powder sticking everywhere signal bad storage practices. Clean up spills with damp disposable towels, not a dry brush, to keep powder from escaping into the air. Waste containers should sit close at hand, not across the room — I learned that the hard way one busy afternoon.
Training and regular shelf checks beat expensive fixes down the road. Posting a checklist near the stockroom helps new staff learn the ropes. Quick spot checks from a lab manager or safety officer catch small mistakes before they lead to bigger ones.
Don’t cut corners just to save time. Good shelving, tight lids, controlled humidity, and straightforward labeling protect health and the bottom line. Safe chemical handling means proper cleanup kits, clear rules, and open communication. People and production both benefit when safety protocols stay simple but strict. In the end, success depends not on fancy equipment, but on small habits done right every day.
Most folks outside of chemistry circles haven’t heard much about 1,3,5-benzenetricarboxylic acid. Labs often call it trimesic acid. It’s a white, crystalline powder, tucked away in bottles for research, making specialty plastics, or used as a precursor for advanced materials. Conversations on chemical safety rarely start here, but maybe they should since the name can sound more intimidating than it deserves.
Looking closely, 1,3,5-benzenetricarboxylic acid doesn’t rank high on the list of headline-grabbing hazardous substances. The European Chemicals Agency database and U.S. EPA records both lack major warnings. This acid doesn’t show acute toxicity in standard rodent tests. It isn’t mutagenic. Unlike benzene, it will not evaporate quickly, nor will it soak through skin at alarming rates. I’ve never seen an industry worker or researcher cite it as a leading chemical health risk. It doesn’t build up in organisms or soil, either.
Even so, relying purely on “not dangerous” language isn’t wise. Any fine powder can create dust that irritates eyes and the lungs. If you breathe enough in, you’ll cough and maybe feel a scratchy throat. For those with sensitive skin or allergies, there’s always a chance for a rash. The signal word on the label in most labs is “warning,” not “danger.” That describes a substance that deserves care but doesn’t threaten lives with casual exposure.
Over the years, working in university chemical storerooms and research buildings, safety protocols covered everything—trimesic acid included. The advice was simple: keep the bottle closed, use gloves when handling, and avoid blowing dust around. No one used respirators for it unless dealing with big amounts or heavy dust. Storage was easy: a cool, dry shelf alongside hundreds of other powders, no special isolation required.
Risks rarely come from toxicity; they come from shortcuts and carelessness. I’ve seen more trouble from electrical shorts or broken glass in the lab than from trimesic acid. Water spills made more memorable stories. Still, institutions train everyone to sweep and mop up spills, wear goggles, and keep chemicals labeled. No one jokes about lab mistakes. Small risks never disappear, but they shrink with respect and discipline. Odds of harm drop further when everyone takes ten seconds to read a label before opening anything new.
No reports tie trimesic acid to serious environmental damage or acute hospital visits. It doesn’t show up on EPA hazardous chemical lists. The GHS classification puts it closer to mild irritants. Fact-checking with multiple public safety databases supports this view. Even so, chemical regulations can change when new scientific evidence appears, so producers track toxicology updates and follow local waste guidelines. Labs never pour leftover acid down the drain, not just for trimesic acid, but for all solid chemicals.
Teaching lab safety still matters. Small spills, skin contact, or accidental inhalation—each one is manageable with gloves, goggles, and a bit of alertness. Goggles and nitrile gloves became my favorite uniform, no matter the chemical. People can work safely with potentially harmful powders when they keep doors open, stay aware, and practice clean habits.
The story of 1,3,5-benzenetricarboxylic acid reminds us that hazard doesn’t mean panic—just respect for the tools and materials on the bench.
1,3,5-Benzenetricarboxylic acid, better known as trimesic acid, plays a quiet but crucial part in many industries. From building advanced polymers to serving as a pivotal component in metal-organic frameworks, this compound’s influence stretches well into materials science, coatings, and pharmaceuticals. Purity stands as a main talking point whenever scientists look for a source, especially in high-performance environments. Experience working with both research teams and production lines shows that even a slight deviation here can derail an experiment or foul up an industrial batch quickly.
In most commercial and laboratory circles, trimesic acid comes in a minimum purity of 98%. Research-grade material often scales up to 99% or higher. For context, a purity level of 98% fits well into bulk synthesis and general applications. The extra percentage point — closer to 99% or above — generally enters the equation for specialty pharmaceuticals or high-end laboratory projects where trace contaminants might cause trouble. Any residual solvents, metals, or organic impurities can not only shift results but also raise safety or compliance headaches. Laboratories who conduct X-ray crystallography, for instance, push manufacturers to provide certificates of analysis, and to go beyond basic purity readings to include moisture content, residual solvents, and even particle size analysis.
I’ve seen suppliers offer trimesic acid packaging anywhere from 25-gram glass bottles up through 25-kilogram fiber drums or lined plastic containers. On a research bench, a 100-gram jar often lasts weeks; scaling up to pilot plants, those 5-kilogram and 10-kilogram buckets start to look small. Larger batches run out of metal cans or fiber drums, usually with moisture-barrier liners to keep the product dry during long shipping journeys. Some chemical warehouses even decant custom sizes to suit a particular production cycle. Delivery in vacuum-sealed bags comes up every so often, especially for those working in moisture-sensitive syntheses or high-purity workflows.
Purity and size aren’t just technical details — they shape budgets, timelines, and even product quality. A colleague in the coatings industry recently shared how one batch of trimesic acid containing slightly elevated metal impurities led to unpredictable catalyst behavior, wasting both time and material. In pharmaceutical research, purity variations can affect reproducibility or regulatory sign-off. Even packaging can change everything: absorbing a few grams of water from a warehouse shelf, a poorly sealed drum can alter reaction stoichiometry or flow behavior in automated dispensers. Packaging transparency matters. The best suppliers document batch analyses, offer moisture and contaminant testing, and know how to package for climate and transport.
Purchasing teams do best by building long-term relationships with reputable chemical manufacturers. Go beyond just the safety data sheet — ask for current certificates of analysis, request packaging suited for your lab or plant, and consider an audit when working with high-stakes projects. For multinational firms, regional warehousing helps minimize temperature or humidity swings in transit. Smaller teams may find value in specialty chemical distributors who can break down and repack bulk shipments into bench-sized containers, while still providing traceability and handling reports. These extra steps save hassle in the long run, feeding into both smoother experiments and safer workplaces. The right mix of purity and smart packaging keeps projects on track and keeps teams confident in their results.
| Names | |
| Preferred IUPAC name | Benzene-1,3,5-tricarboxylic acid |
| Other names |
Trimesic acid Benzene-1,3,5-tricarboxylic acid 1,3,5-Tricarboxybenzene |
| Pronunciation | /waɪˈtrɪ.sɪk.lɪk bəˈziːn traɪˌkɑːr.bɒk.sɪl.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 554-95-0 |
| Beilstein Reference | 1361871 |
| ChEBI | CHEBI:16558 |
| ChEMBL | CHEMBL1407 |
| ChemSpider | 15060 |
| DrugBank | DB03238 |
| ECHA InfoCard | 03f98c2f-5597-40eb-af1d-967d8498a2d8 |
| EC Number | 205-504-9 |
| Gmelin Reference | 10419 |
| KEGG | C01584 |
| MeSH | D001587 |
| PubChem CID | 70996 |
| RTECS number | WW7875000 |
| UNII | KGF39LC8AS |
| UN number | UN1325 |
| CompTox Dashboard (EPA) | DTXSID5048569 |
| Properties | |
| Chemical formula | C9H6O6 |
| Molar mass | 210.14 g/mol |
| Appearance | white powder |
| Odor | Odorless |
| Density | 1.4 g/cm³ |
| Solubility in water | slightly soluble |
| log P | 1.1 |
| Vapor pressure | 1 mmHg (25°C) |
| Acidity (pKa) | 2.94, 3.89, 4.60 |
| Basicity (pKb) | 3.40 |
| Magnetic susceptibility (χ) | -6.6·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.664 |
| Viscosity | Solid |
| Dipole moment | 2.6 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 336.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1241.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1387.2 kJ/mol |
| Pharmacology | |
| ATC code | A16AX11 |
| Hazards | |
| Main hazards | Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS07, GHS09 |
| Signal word | Warning |
| Hazard statements | H319: Causes serious eye irritation. |
| Precautionary statements | Precautionary statements: P261, P280, P305+P351+P338, P304+P340, P310 |
| NFPA 704 (fire diamond) | 1,2,0 |
| Flash point | > 385 °C |
| Autoignition temperature | 685 °C (1265 °F; 958 K) |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 7,000 mg/kg |
| NIOSH | CV8400000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 100 mg |
| Related compounds | |
| Related compounds |
Phthalic acid Isophthalic acid Terephthalic acid Trimellitic anhydride Benzoic acid |
