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People who work with organic chemistry know that 2,4,6-Tribromo-3-hydroxybenzoic acid didn’t arrive on the scene by accident. Its story starts in the era when scientists dug into halogenated benzoic acids, searching for new properties and uses. Back in the 20th century, researchers often wanted to add bromine to benzene rings because this altered physical and chemical behavior in big ways. Even now, starting materials like phenols and benzoic acids earn plenty of attention because they serve as building blocks for dyes, medicines, and lab tools. Many breakthroughs, especially in pharmaceuticals and specialty synthesis, trace their roots to these halogenated benzoic acids. The journey of this specific molecule includes shifts in analytical methods and safer bromination, and the acid itself keeps making appearances where stability and reactivity both matter.
2,4,6-Tribromo-3-hydroxybenzoic acid wears many hats in research. At its core, it is a benzoic acid with three bromine atoms and one hydroxy group. With this specific combination, the compound opens up possibilities in both organic synthesis and the study of natural products. Scientists working with halogenated aromatics keep this acid on their shelf for a good reason: it reacts predictably, binds well in some enzyme studies, and stands up to tough lab conditions. As a small-molecule acid, it fits into research that calls for stable, brominated, and moderately acidic substances. Its relatively straightforward preparation and recognizable structure mean it's easily tracked and characterized—details anyone who’s spent time isolating reaction mixtures can appreciate.
This benzoic acid stands out for its dense, off-white or slightly straw color. Three bromine atoms pack on some weight and give it a distinctly high melting point. The acid has decent solubility in polar organic solvents but little interest in mingling with plain water. Its hydroxy group forms strong intramolecular hydrogen bonds, changing how it dissolves and crystals form. In the lab, you don't mistake its moderate acidity or its strong bromine-driven electron-withdrawing effects. That trio of bromo groups pulls electronic density away from the aromatic ring, allowing chemists to tackle electrophilic reactions without worrying too much about unwanted side products.
Most packaging arrives with details about purity, melting point, and occasionally, spectroscopic fingerprints. Labels warn of irritant properties and note storage in cool, dry places. Some brands report the acid’s batch impurities or recommend specific storage vessels, sticking with glass or compatible plastics. For researchers, confidence comes from seeing clear labels, batch analysis data, and expiration dates. While not every bottle spells out particle size or full impurity profiles, these days reputable suppliers include chromatographic data to help buyers trust what’s inside.
Synthesis always depends on the starting materials and target yield, and anyone who has spent time in a synthetic lab will remember the sharp smell of bromine during benzoic acid bromination. Most routes begin with 3-hydroxybenzoic acid or similar precursors. Controlled bromination—often using elemental bromine in acetic acid or glacial conditions—shapes the final product. The hydroxy directing group and acidity help bromine settle at the 2, 4, and 6 positions. Filtration, washing, and crystallization follow, though more careful hands add purification by recrystallization or column chromatography for high-purity work. Modern labs sometimes use less aggressive reagents or green chemistry tweaks to cut down on hazardous waste.
In the hands of a patient chemist, 2,4,6-Tribromo-3-hydroxybenzoic acid opens up rich possibilities for coupling and substitution. The electron-poor aromatic ring resists wild reactions, so carefully chosen catalysts or nucleophiles move things forward. The acid tests well in Suzuki or Sonogashira couplings after suitable activation, thanks to the bromo atoms. Acylation, esterification, or reduction spin out new derivatives for use in specialty fields. In biochemistry, modifications at the hydroxy site provide handles for labeling or crosslinking, letting teams customize the molecule for specific assays or target screening.
In research papers, people might see the acid referred to as 3-hydroxy-2,4,6-tribromobenzoic acid, tribromo-hydroxybenzoic acid, or even using older IUPAC names. Trade names rarely surface, since this isn’t a mass-market commodity, but catalog entries stick to systematic names for clarity. These synonyms echo across chemical databases, helping researchers locate safety data, preparation notes, and references from past studies.
Long experience dealing with brominated benzoic acids shows that safety isn’t something to skim over. Solid particles cause serious irritation if inhaled or if they contact skin and eyes. Standard operating procedures direct chemists to use fume hoods, gloves, and protective eyewear. Even small spills demand attention because some bromine compounds linger in air or react with surfaces. As with many halogenated aromatics, safe waste disposal calls for separate organic waste streams, never down the drain or mixed with general trash. Regulatory agencies monitor exposure limits, though this acid doesn’t see enough widespread use to trigger restrictions like some bigger-volume chemicals. Even so, good labs train every worker to handle all halogenated materials with respect—missteps here can mean serious health or environmental costs.
Researchers reach for this acid mostly in academic and industrial chemical labs. In organic synthesis, brominated benzoic acids offer a reliable route to more complex aromatic molecules. The predictable substituent pattern aids in structure-activity work—especially valuable in pharmaceutical design, agrochemical testing, and dye chemistry. Some teams use its structure as a probe or scaffold in enzyme inhibition studies or receptor binding screens. Scientists studying environmental breakdown of halogenated aromatics sometimes turn to tribromo derivatives to track persistence and reaction pathways, especially since real-world pollutants often share the same kinds of ring substitutions.
Development keeps pushing the boundaries for halogenated aromatics. Synthetic chemists test greening up the bromination process while analytical teams chase new detection and quantification methods—often using high-resolution NMR or tandem mass spectrometry for trace identification. The molecule plays its role in exploring new reaction pathways, sometimes by testing the limits of cross-coupling catalysts. In biochemistry, modifications on the structure push boundaries in enzyme assay design, driving drug screening and diagnostics. Many efforts follow the thread of making these acids safer to handle or easier to dispose of, reflecting broad concern for both worker safety and environmental stewardship.
Toxicity always shadows the use of brominated aromatics, and this acid is no exception. Most acute studies point to moderate irritant properties, with risks rising if one ignores good lab practices. Long-term or high-concentration exposure hasn’t been mapped in detail, but chemists know that halogenated aromatics can accumulate in biological tissues. Cases of bioaccumulation and slow breakdown pop up in environmental studies, especially where similar molecules show up in effluent streams or sediment samples. The challenge of establishing full toxicological profiles lingers because the acid sees niche, not widespread, industrial use. Still, every new study adds to a slow-growing database, helping safety officers and environmental scientists track its impact and guide cleanup efforts if accidents occur.
Demand for specialized halogenated acids won’t vanish—if anything, it looks set to grow as chemists design more targeted syntheses and probes. Advances in green synthesis and waste treatment can change the picture for both safety and cost, letting more labs run reactions with fewer environmental headaches. In the life sciences, chemists keep pushing the envelope, using the acid’s structure to understand protein-ligand binding and test theories around aromatic interactions. Regulation and risk monitoring will likely expand as environmental and health concerns draw more attention to persistent brominated molecules. The acid’s value comes not from commodity production but from focused, high-impact uses—where every refinement in synthesis, safety, or function means downstream benefits in pharmaceuticals, materials, and even environmental monitoring. From my own time on the bench, I see value in pushing for new reactivity, careful waste handling, and open access to safety data. Keeping an eye on both practical and ethical stakes of halogenated benzoic acids remains as important as ever.
Chemistry surprises me every time I get my hands on an aromatic compound like 2,4,6-Tribromo-3-hydroxybenzoic acid. The name looks intimidating, but once you split it up, the logic falls into place. The base of this molecule is benzoic acid, known for its presence in food preservatives and laboratory work. By looking at the name, you see three bromine atoms attached at the 2, 4, and 6 positions of the benzene ring. Hydroxy doesn't just hang around anywhere; here, chemistry students know it sits on the 3-position. Toss in that carboxylic acid group sitting on the 1-position and the structure gets real.
The chemical formula for 2,4,6-Tribromo-3-hydroxybenzoic acid comes out as C7H3Br3O3. This tells the whole story: seven carbons from the benzene ring, three hydrogens (since bromine and hydroxy replace most of the default hydrogens on the ring), three bromine atoms, and three oxygen atoms—one for the hydroxy, two from the carboxylic acid group.
These days, scientists keep a sharp eye on bromo-derivatives like this one. They show up in research, often in environmental monitoring or pharmaceutical synthesis. The heavy bromine atoms change the physical behavior, often giving the compound more stubborn persistence in soil and water. In drug development, chemists value aromatic rings that carry halogens and hydroxy groups—these pieces can make a drug molecule interact better with its biological target or last longer in the bloodstream. Getting the positions right, like the 2,4,6-tribromo arrangement, influences how the molecule fits into enzymes or disrupts bacterial growth.
Back in my own undergraduate days, the lab bench would get sticky with different benzoic acid derivatives during experiments. We always wore two pairs of gloves working with the halogenated compounds. Not only do they stain skin and bench-tops, but some, like this tri-brominated acid, call for extra ventilation due to their volatility and potential toxicity. That practical memory never leaves: chemical structure guides behavior in the lab and outside it.
Adding multiple bromine atoms makes this benzoic acid less biodegradable. The environmental side of chemistry can’t avoid talking about persistence and potential for bioaccumulation. Reports from the EPA and European Chemicals Agency show that halogenated aromatics—especially those with three or more halogens—don’t break down easily. Wastewater plants often can’t scrub these compounds out, and they sometimes drift into rivers and lakes where fish and wildlife pick them up. Brominated aromatics have occasionally shown up in studies as endocrine disruptors. This happens by mimicking hormones or interfering with normal chemical signaling in animals and maybe even in humans.
Nobody wants to stop valuable research, but risks push chemists to think creatively. Substitution can play a helpful role—swapping out for less persistent halogens like chlorine, or reducing the number used. Green chemistry pushes for reagents and methods that leave behind less waste and rely on greener solvents. Labs handling these compounds need up-to-date fume hoods, disposable nitrile gloves, and strict protocols for cleanup. Governments have rolled out requirements for registering new bromo-aromatic chemicals and tracking their use, relying on public data and collaborative science to weigh benefits against hazards.
From where I stand, the formula C7H3Br3O3 is more than just numbers and letters. It signals a blend of human ingenuity, scientific responsibility, and the never-ending puzzle of balancing discovery with safety.
2,4,6-Tribromo-3-hydroxybenzoic acid sits on the shelf in many research labs, not because it’s sexy, but because it gets the job done. This compound turns up as an intermediate—think of it as a key step in the recipe book for more complex molecules. Chemists take advantage of its reactivity to create other brominated compounds, especially in the hunt for new drugs or materials.
Looking at its track record, it’s shaped the synthesis of certain antibiotics and helped with tweaking molecules for stronger antibacterial or antifungal power. Studies from journals like “Bioorganic & Medicinal Chemistry” keep highlighting how brominated phenols like this one play a role in medicinal chemistry pipelines. Sometimes the difference between a good antibiotic and a useless one is a matter of dropping in those bromine atoms at the right spots.
Environmental scientists keep an eye on this chemical, too. Some marine organisms naturally produce compounds similar to 2,4,6-tribromo-3-hydroxybenzoic acid as part of their defense system. By studying these molecules in the lab, researchers find ways to mimic nature’s way of protecting sea sponges and algae from pests and disease. It’s not just an academic exercise—this knowledge spills into searching for nontoxic ways to keep fouling off ship hulls or deal with bacterial biofilms in water systems.
Toxicology folks don’t ignore it either. The compound’s structure, with all those bromine atoms, clues scientists in on how related molecules behave in bodies and in the environment. Knowing how these acids break down, or how persistent they stay in ecosystems, opens the door for safer design of new chemicals.
Materials chemists reach for 2,4,6-tribromo-3-hydroxybenzoic acid when working on flame retardants or specialty coatings. Brominated aromatics have proven to slow down combustion. If you’ve ever noticed how modern electronics or textiles handle heat better than the ones you grew up with, it’s due, in part, to research on compounds like this one. Safer, smarter flame retardants keep people from getting hurt in home or vehicle fires. As eco-regulations start to squeeze out older, toxic formulas, the need for smarter molecular design grows.
A friend in plastics manufacturing once told me that tweaking one side group on a molecule could shave months off R&D cycles. This acid often slips into production as a building block, helping fine-tune resins or coatings for better resilience or environmental profile. Sometimes these tweaks even help reduce chemical waste in production.
The challenge, as always, runs deeper than mixing chemicals. Ethical chemists and manufacturers check toxicity data and honor new standards for greener chemistry. Even something that’s been on the books for decades, like this acid, gets a fresh look as scientists search for non-toxic alternatives and recycle steps in synthesis to cut down on hazardous waste.
Collaboration remains key. Universities, start-ups, and established companies swap notes on the latest uses and limitations. There’s chatter at conferences about designing new antimicrobial coatings or greener additives by learning from these brominated molecules. Some labs tap AI to map out where a single side group change—as simple as swapping out a hydroxy group—could cut human and environmental risk.
Smart chemistry, in the end, keeps us moving forward. For 2,4,6-tribromo-3-hydroxybenzoic acid, its legacy won’t just be in what it helped make, but in how it helped chemists create safer, more effective materials and medicines.
Working with chemicals brings its own set of challenges. Some folks imagine endless rows of glass bottles with skull-and-crossbones labels in the back of a dusty storeroom. Truth is, handling even the more "ordinary" compounds demands a healthy respect for details. I’ve seen well-meaning teams get caught up in the day’s demands, forgetting to double-check the basics, which never ends well. Spills, ruined batches, or a late-night panic call to an on-call manager – it’s never worth rolling the dice.
Most technical data sheets will state exact temperature guidelines, like “store between 2°C and 8°C.” But a sticker on a fridge only goes so far. I remember laboratory fridges stuffed beyond capacity where airflow became a real problem, and the back of the fridge froze solid while the front barely kept cool. Fluctuating temperatures speed up degradation. Ruined material turns into wasted money, lost time, and sometimes safety issues, especially if something decomposes in an unsafe way.
The right container separates safe practice from disaster. Certain acids begin eating through plastic after a matter of weeks, while light-sensitive compounds lose potency in clear jars. I’ve seen well-labeled materials inside improperly sealed bags leech moisture straight out of humid air, turning usable powder into useless sludge. Screw caps should shut tightly. Never skip that visual once-over before use. Investing in amber glass, HDPE, or metal cans as appropriate isn’t about fancy storage; it prevents ruined inventory and frustrated lab techs down the road.
Crowded shelves encourage mistakes. In one plant I visited, someone stored chlorinated solvents beside oxidizers because the bins were full. One dropped bottle could have caused a costly, dangerous cleanup. It sounds simple, but double-checking what’s next to what prevents unexpected chemical reactions and keeps everyone safer. Designating incompatible shelves, even if it means walking an extra few steps each day, brings lasting peace of mind.
It’s easy to think tracking inventory is just a paperwork hassle. Yet, databases showing how long a compound’s been on the shelf, and what condition it’s in, help avoid using expired or degraded material. I’ve seen situations where someone used a canister well past its best date, only to turn out the material was no longer reactive—destroying valuable results. Regular checks and digital logs go further than scribbled notes in a composition book.
Proper airflow matters. Closed-off storage without ventilation can turn a minor leak into a series of headaches. I once watched a small peroxide container swell and rupture because vapor pressure built up in a hot storeroom. Cleanup took hours. Keeping spill kits within arm’s reach and running down the emergency checklist before every project avoids scrambling when things go sideways.
No storage protocol beats a team that knows what they’re doing. Onboarding videos and posters provide reminders, but hands-on walkthroughs stick longer. In one group I joined, monthly drills made us confident—if something spilled or broke, everyone knew exactly who handled what. Mistakes dropped off, and even outside audits commented on the difference. Regular, practical training protects people and product every day, not just during inspections.
Most problems don’t need high-tech fixes. A decent thermometer in each storage room, containers matched to chemical type, inventory routines that make you double-check for expiration dates, and steady follow-through keep risks low. Good habits up front—including taking five minutes to label and shelve things right—mean less chaos later. Companies that invest in the basics rarely face costly blowups or lost batches, because they treat chemical storage as an investment in both safety and quality.
2,4,6-Tribromo-3-hydroxybenzoic acid looks like a mouthful, but break it down and you find a benzoic acid backbone loaded up with three bromine atoms and a single hydroxyl group. Brominated organics usually raise eyebrows for health and environmental reasons. This compound crops up in some niche chemistry circles, mostly as an intermediate or a building block in synthesis. You’ll see it in research labs, not the grocery store or your average cleaning products.
A quick dig through chemical safety databases tells a familiar story for halogenated aromatics. Animal studies with similar compounds point to a range of toxic effects. Irritation to skin, eyes, and the respiratory system lands at the top of that list. Brominated compounds often hang around in the environment, accumulating in living tissues over time. This process raises concerns for both workers and wildlife. Inhalation or swallowing can stress out organs like the liver and kidneys, and cause central nervous system symptoms, particularly if exposure runs high.
Evidence for specific hazards with this compound isn’t as deep as for more famous brominated chemicals (like PBDEs in flame retardants), but that doesn't offer much comfort. The structure of 2,4,6-tribromo-3-hydroxybenzoic acid sets up the same possible pitfalls: potential for persistence, chance of bioaccumulation, and a risk window if it gets handled without care.
I’ve handled my share of specialty chemicals in several lab setups. Gloves, goggles, and a working fume hood count as the basics—those rules never take a day off. I remember seeing a skin rash on a lab mate who underestimated a brominated compound; it taught the rest of us to treat any skin contact as a worry, and airflow became something you check before uncapping bottles. SDS sheets for 2,4,6-tribromo-3-hydroxybenzoic acid match what my group saw, calling for strong caution: avoid dust, keep it away from open skin, and never eat or drink near the workbench.
This compound probably won’t end up in household waterways or on your hands at home, which keeps risks down for the average person. That said, industrial run-off or careless disposal can still bring brominated acids into rivers or lakes. Even in small amounts, these chemicals don't break down quickly. Wildlife—think fish and amphibians—can't defend against toxins that build up in their tissue. Over time, this disrupts ecosystems and puts more strain on communities relying on safe water and healthy environments.
To lower risk, focus on control and containment long before any accident. Labs and facilities using chemicals like this should run closed systems, with proper ventilation and protocols for spills. Disposal needs special handling through licensed waste firms, never poured down drains. Researchers and regulators could push for alternatives, either less persistent or less toxic, especially when these chemicals serve as intermediates that can be replaced.
Open information channels matter, too. Safety data sheets, regular training, and incident response drills help people remember what's at stake. Chemical companies ought to invest in greener chemistry, shedding reliance on heavy halogenation where possible. Together, stronger safeguards and smarter choices protect health and the environment without halting progress in research.
The level of purity in a product says a lot more than just what percentage shows up on a label. Purity shapes the outcome for scientists, manufacturers, and even end consumers. Anyone who’s worked in a lab or run a production line knows contamination isn’t just a nuisance—it can wreck an entire batch or compromise safety. For me, once you experience a single delayed project thanks to a questionable shipment, you understand why folks ask about purity first.
Most chemical ingredients, raw materials, or precision additives won’t go out the door unless purity checks meet tight standards. It’s common to see specifications at 98%, 99%, or for pharmaceutical applications, 99.9% and above. Those few decimal points mean a world of difference if your outcome depends on a single compound. Quality controls rely on third-party analysis, certificates of analysis, and, quite often, customer testing. If a supplier is fuzzy about purity data, that’s a red flag. You want suppliers who provide transparent results with every delivery, showing exactly what’s in the drum or bag—no guessing games.
Mention packaging size, and the default thought is—how much comes in one container? It's easy to shrug this off, until you start thinking about handling, storage space, transport costs, and safety regulations. Over the years, I have seen industries gravitate toward options based on how they use the product. R&D labs often look for small bottles or jars, sometimes 100 grams or 250 grams. Larger production floors handle kilo packs, 25-kilogram bags, or barrels holding hundreds of liters—sometimes even 1000-liter IBC totes or tanker shipments for industrial volumes.
Too big a container, and you’re wasting money on unused product or risk it sitting too long before use. Too small, and the process stops for another order sooner than expected. In the real world, companies consider reactivity and shelf life before deciding on a size. Sensitive materials call for vacuum-sealed packs, inert gas blanketing, or even double packaging if the stakes are high. Shipping regulations—especially for hazardous products—dictate the choice between steel drums, HDPE containers, glass bottles, or those individually-wrapped ampoules.
Suppliers committed to quality don’t just state a number for purity and call it a day—they demonstrate consistency over time. Documentation isn’t just paperwork. Look for batch numbers matched with purity results, material safety data sheets, and fresh test results to back them up. Practical experience tells me the suppliers who get repeat business pay attention to the details—each shipment, each time. They’re open about where their product comes from and what packaging suits your storage setup best.
Honesty up front saves headaches. If you ever get a vague answer about an item’s purity (or if the supplier tries to brush off packaging questions), it pays to push for specifics. Most companies that value long-term partnerships offer a menu of packaging—sometimes even custom sizes—which shows they’re paying attention to what customers actually need instead of forcing a one-size-fits-all solution. This flexibility often improves lab productivity, reduces waste, and lowers safety risks down the line.
Insisting on clear purity data and sensible packaging options isn’t being picky; it’s the foundation for cost savings, safety, and peace of mind. The businesses that last ask better questions, compare documentation, and work with partners who treat these details with respect. It cuts surprises, improves product results, and lets people on the ground focus on their real work—without second-guessing what’s inside the box.
| Names | |
| Preferred IUPAC name | 3-hydroxy-2,4,6-tribromobenzoic acid |
| Other names |
2,4,6-Tribromo-3-hydroxybenzoic acid 3-Hydroxy-2,4,6-tribromobenzoic acid 2,4,6-Tribromo-m-hydroxybenzoic acid 2,4,6-Tribromo-3-hydroxybenzoesäure |
| Pronunciation | /tuː, fɔːr, sɪks traɪˈbroʊmoʊ θriː haɪˈdrɒksi benˈzoʊɪk ˈæsɪd/ |
| Identifiers | |
| CAS Number | 18991-98-5 |
| 3D model (JSmol) | `3D model (JSmol)` string for **2,4,6-Tribromo-3-hydroxybenzoic Acid**: ``` COC1=CC(Br)=C(C(=C1Br)Br)C(=O)O ``` or as a SMILES (which JSmol accepts for 3D rendering): ``` OC(=O)c1c(Br)cc(Br)c(O)c1Br ``` |
| Beilstein Reference | 1759249 |
| ChEBI | CHEBI:52318 |
| ChEMBL | CHEMBL262141 |
| ChemSpider | 73616 |
| DrugBank | DB04135 |
| ECHA InfoCard | 03c64578-1cf8-474c-808b-059c2b7d9568 |
| EC Number | 3.1.1.59 |
| Gmelin Reference | Gmelin Reference: 104703 |
| KEGG | C06535 |
| MeSH | D017968 |
| PubChem CID | 13241717 |
| RTECS number | CB8925000 |
| UNII | W76J19F82K |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | DTXSID10141245 |
| Properties | |
| Chemical formula | C7H3Br3O3 |
| Molar mass | 360.87 g/mol |
| Appearance | White to off-white solid |
| Odor | Odorless |
| Density | 2.35 g/cm³ |
| Solubility in water | Slightly soluble in water |
| log P | 1.93 |
| Vapor pressure | 2.78E-8 mmHg at 25°C |
| Acidity (pKa) | 2.5 |
| Basicity (pKb) | 11.64 |
| Magnetic susceptibility (χ) | -5.27e-5 cm^3/mol |
| Refractive index (nD) | 1.694 |
| Viscosity | 1,008 Pa·s (25 °C) |
| Dipole moment | 3.5507 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 309.6 J⋅mol⁻¹⋅K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -259.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -2191.6 kJ/mol |
| Pharmacology | |
| ATC code | D01AE21 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes skin irritation. Causes serious eye irritation. |
| GHS labelling | GHS02, GHS07, GHS09 |
| Pictograms | GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P261, P280, P305+P351+P338, P337+P313 |
| Flash point | 196°C |
| Lethal dose or concentration | LD50 oral rat 3220 mg/kg |
| LD50 (median dose) | LD50: 5000 mg/kg (rat, oral) |
| NIOSH | TY9625000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 10 mg |
| IDLH (Immediate danger) | Not listed |
| Related compounds | |
| Related compounds |
2,4,6-Tribromobenzoic acid 2,4,6-Tribromophenol 3-Hydroxybenzoic acid 4-Bromo-3-hydroxybenzoic acid 2,6-Dibromo-3-hydroxybenzoic acid |
