© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Observing centuries of chemistry unfold, aromatic monocarboxylic acids reveal a pattern common to scientific discovery: everyday materials hid remarkable significance waiting for curious minds to dig deeper. Early chemists like Justus von Liebig and Friedrich Wöhler worked with compounds such as benzoic acid, applying newly developed distillation and crystallization methods to isolate and characterize them. For years, these acids served as mysterious crystals found in resins and plant extracts. Cracking their structures through painstaking experimentation allowed generations of scientists to understand not just their composition, but also their transformative role in chemical synthesis, preservation, and industrial production. It fascinates me that before the molecular age, careful smell, taste, and observation led to the recognition of the unique, fragrant qualities that inspired their name. Experiments in the early 1800s with gum benzoin brought forth benzoic acid, launching exploration into other aromatic relatives. Each new method, structural insight, and practical application marked a turning point that shaped organic chemistry itself.
Think about common names: benzoic acid, salicylic acid, cinnamic acid, and p-toluic acid. They share a benzene ring with one carboxylic acid group attached. The aroma often comes from their plant origins, whether in food preservatives or medicinal use. High purity is vital for their role in pharmaceuticals, so strict quality testing follows every batch. Beyond benzoic acid’s use to keep food safe from mold, salicylic acid stands out for its long history in skincare and pain relief. Production volumes climbed for both, but usage differs: one fights spoilage, the other soothes skin and joints. Understanding which acid fits a use case involves tracking reactivity, efficacy, and—most importantly—potential side effects.
Pulling a sample of benzoic acid from the lab shelf, I’m reminded of how its chalky crystals dissolve slightly in water, much better in ethanol. Many aromatic monocarboxylic acids melt between 120 and 220 degrees Celsius, and their odors reveal subtle differences depending on substitute groups attached to the benzene core. These acids resist easy breakdown, holding up well in processing and storage; they do not burn off or degrade quickly, so preservative power lasts. Chemical bonds in the aromatic ring arm these molecules with stability. That same structure lets them play in reactions ranging from nitration and halogenation to classic decarboxylations.
Looking past promotional gloss, actual users care most about solubility, melting range, purity, and residual impurities. Analytical standards include high-performance liquid chromatography (HPLC) or gas chromatography (GC) for exact quantification. Labs report the presence of tiny byproducts—like toluic acid with traces of xylenes—that affect final product performance or regulatory acceptance. Labeling needs to be precise, not only because laws demand it, but because trace residues shift risk profiles for food, medicine, and industrial use. It’s easy to gloss over these details, but any professional who’s dealt with an industrial mishap or product recall knows just how critical full disclosure and compliance can be.
Laboratory synthesis uses classic oxidative decarboxylation for certain acids, often with potassium permanganate or chromium reagents. On an industrial scale, air oxidation of toluene gives benzoic acid, a process refined steadily for efficiency, safety, and environmental impact. Older methods used animal-based sources, but plant extraction and petrochemical routes dominated by the twentieth century. Scaling up means handling significant volumes of organic solvents, so operational protocols evolved to avoid fires or releases. Waste management remains a sticking point; newer catalytic approaches pursue lower emissions and easier recovery. These are no minor updates—avoidance of heavy metals and reduction of greenhouse gases underpin current research funding and regulatory pressure.
Whether for undergraduate lab classes or big pharma, aromatic monocarboxylic acids often step into the limelight as building blocks. Chemists alter their core structure by attaching nitro, sulfonic, or amino groups, opening access to dyes, drugs, or perfumes. For example, acetylation of salicylic acid delivers acetylsalicylic acid—better known as aspirin. Esterification makes food flavorings, and coupling reactions with amines or alcohols diversify downstream chemistry. Hardly a semester goes by in any organic chemistry curriculum without students learning the Friedel–Crafts acylation or electrophilic substitution on these rings. Those basic transformations explain why they remain so widely used across industries.
Names tell stories, especially in chemistry. Benzoic acid is also known as E210 in the food world, or benzene carboxylic acid in technical discussions. Salicylic acid once went by “spiræic acid,” linking back to its willow tree roots. Cinnamic acid gained fame as natural flavor in vanilla or cinnamon substitutes. Regulatory naming sometimes creates confusion outside the lab, but product-specific identifiers help prevent costly mistakes. For health and chemical safety conversations, clarity in naming is not a bureaucratic chore—it guards against shipping errors, cross-contamination, or mistaken handling that impacts worker safety or consumer health.
It’s easy to forget how dangerous some basic chemicals can be when handled carelessly. Benzoic acid seems benign but inhaling its dust irritates airways; repeated skin contact brings dermatitis after a while. Tight PPE requirements matter as much in food plants as in chemical factories. Storage must stay cool, dry, well ventilated—especially since acids like benzoic and cinnamic can decompose with heat and light, creating off-odors and harmful byproducts. Regulatory frameworks require periodic review, yet real-life compliance hinges on on-the-ground training and accountability. Mistake-free operations depend on robust safety culture, not just technical bulletins or safety data sheets gathering dust on a wall.
For most people, contact starts in the food aisle. Benzoic acid, with its long tradition as a preservative, lines up behind every bottle of soft drink and fruit preserve that must survive weeks on a shelf. Salicylic acid keeps showing up in anti-acne products, but its soothing touch started in folk remedies for pain and fever, much before aspirin’s invention. In my work with industrial process audits, I’ve seen aromatic acids smooth the way in alkyd resin production for paints or as intermediates for dyes and perfumes. Even in rubber manufacturing, these acids prevent premature vulcanization—the sort of detail overlooked by end users but vital for performance and safety. Each new use brings closer scrutiny of long-term exposure, especially in consumer-facing products.
Research and development efforts home in on two persistent questions: How to make these acids in cleaner, more cost-effective ways, and how to reduce or redirect their impact on human health and the environment. Green chemistry pushes for bio-based synthesis or catalytic processes using less toxic reagents. Scientists track how these compounds degrade in wastewater, and look for alternatives that resist bioaccumulation or persistence. Clinical researchers, on the other hand, keep investigating the fine line between therapeutic action and toxicity, especially since even minor impurities or byproducts change how these chemicals behave in biological systems. For every major advance—a new catalyst, a discovery of a cancer-preventive property—there’s a new set of safety studies, manufacturing audits, and consumer questions to address.
Toxicologists do not take aromatic monocarboxylic acids lightly. Even though benzoic acid holds a GRAS (Generally Recognized As Safe) status for food, there’s no free pass when it comes to chronic exposure, especially in vulnerable populations. High intake of benzoic acid or its salts links to hyperactivity in children and rare allergic reactions. Salicylic acid, so valued for pain relief, brings risk of poisoning at high doses or in sensitive groups like children. Each new application triggers a fresh wave of occupational safety studies, consumer tolerance testing, and environmental impact reviews. These are not faceless checklists—they are the backbone of trust in the products we use every day. Mistakes or regulatory slip-ups carry lasting consequences for public health and corporate reputation alike.
You won’t see aromatic monocarboxylic acids replaced overnight. Their versatility stubbornly resists easy substitution, but future breakthroughs hinge on green chemistry, waste minimization, and safer product design. As consumer voices grow louder about chemical exposure, pressure increases for non-toxic preservatives and plant-based production routes. Young chemists entering the field must learn not just technical mastery but ethical decision-making, because choices made in the lab or boardroom echo across markets and communities. The push for sustainable raw materials, lower emissions, and faster product development cycles will shape where these compounds show up—from smart packaging to personalized medicine. The next wave of research tries to match consumer demand for safer, cleaner, more transparent products, without losing the benefits that centuries of chemistry have brought to daily life.
Aromatic monocarboxylic acids, like benzoic acid and its cousins, quietly play huge parts in shaping products found in medicine cabinets, grocery carts, and even your favorite gadgets. Working in research, I noticed how a simple molecule can end up driving vast segments of modern manufacturing. Benzoic acid stands out as a preservative in foods—if you enjoy a soda on a hot day, chances are the fizz and freshness owe a little debt to these compounds. Benzoic acid and its salts hop into acidic processed foods because they fight off mold, keeping things safe to eat without flavoring them like the acrid taste of some chemicals. Food scientists keep a watchful eye on quantities, sticking to regulations laid out by food safety authorities.
Industrial chemistry seems to spin on wheels greased by reactive building blocks. Take terephthalic acid, which sits at the core of PET plastic. Every time plastic bottles crinkle in your hands, or someone tosses a polyester shirt in the laundry, an aromatic monocarboxylic acid helped make that happen. PET’s popularity relies on its durability, cost, and ability to be recycled—qualities that trace back to the structural strength of its base ingredients.
Sodium benzoate also gets pulled out in huge quantities for a role beyond soft drinks. It can pop up in personal care products to shield against the fungi that love warm, moist places. Big brands lean on the reliability of benzoic acid derivatives because allergic reactions are rare at approved levels. Modern households usually have half a dozen products powered by these chemicals, from shampoos to toothpaste.
Doctors hand out medicines for everything from rashes to headaches, and a surprising amount trace their chemical heritage to aromatic monocarboxylic acids. Salicylic acid, a simple aromatic acid, shows up as the backbone of aspirin. Centuries of people chewed willow bark, but streamlined, pure compounds made predictable dosing possible. Creams for skin trouble like acne or psoriasis often contain a related acid, chosen for its power to break down dead skin without too much irritation.
In pharmaceutical plants, chemists shape these acids into intermediates—stepping stones leading to complex drugs. The molecular framework holds up to rugged reactions but tolerates fine-tuning, making the search for the perfect treatment faster.
Safety looms large. Most people rarely think about how chemical rules stand in the way of poor choices or unsafe products. That’s been my experience, too, and it reinforces the responsibility on scientists and regulators. Benzoic acid, for example, should stay below recommended limits because overuse can add up or cause reactions in sensitive folks. Keeping track of usage patterns with better analytics lets food and pharmaceutical companies catch problems early.
The world presses for plastics less reliant on petroleum, making biobased sources of aromatic acids a hot topic. New manufacturing techniques harness bacteria or plant matter as feedstock, shrinking the carbon footprint. Technology opens a door to greener options, but the shift needs investments—and trustworthy research to back safety and quality.
Aromatic monocarboxylic acids don’t draw much public attention, but as a scientist or consumer, the ripple from each tiny molecule touches everyday life everywhere from labs to living rooms.
Aromatic monocarboxylic acids show up in chemistry labs and some production spaces—from benzoic acid in food preservation to para-hydroxybenzoic acid in plastics and cosmetics. I’ve seen more than one incident in a university lab that started with sloppy storage: glass jars without labels, containers left uncovered, spills that were never reported. Clean-up cost us hours, and sometimes a pricey order to replace lost reagents.
Ignoring proper handling doesn’t only leave a mess. Acids in this family can cause skin and eye irritation and give off noticeable vapors if the seal breaks. I still remember the day someone left a bottle of phthalic acid near a window; by the time we noticed, sunlight had driven up the temperature inside, sending fumes through the lab. Sometimes blunders come from inexperience, but labeling and storage mistakes show up among veterans, too.
Chemicals only stay useful if you know what’s in the bottle. I’ve learned to label every container the minute I transfer an acid, with name, formula, and the date. Old markers fade—nobody wants to guess at a mysterious powder. Mistaking one aromatic acid for another could disrupt a whole experiment or, worse, cause a reaction no one expects. This holds true in industry and research. Companies and colleges have faced health and product recalls linked to misidentified chemicals.
One sensible step: develop a simple log where every opening and movement gets tracked. It’s not bureaucracy—it’s responsibility. Students sometimes grumble, but after a few scares, they see the point. Good record-keeping protects everyone in the room.
I’ve watched acids go clumpy and discolored after sitting in a humid corner. Damp air degrades purity, so dry storage counts. Any humidity draws water into the sample, affecting reactions and analysis. Benzoic acid, for example, clumps fast under damp conditions, ruining any weighing and measurement. I keep all aromatic acids in screw-cap glass bottles lined with PTFE or rubber gaskets. Glass wins over plastic for these chemicals, unless the product label specifically recommends another option.
Store them away from direct sunlight and high heat. These acids seem stable on paper, but light and temperature swings speed up decomposition and produce byproducts that mess with future syntheses. In my old lab, we kept special cabinets for acids. No more guessing—they stayed cool, dry, and locked away from materials like amines or strong oxidizers. Cross-contamination makes cleanup miserable.
Never put these containers close to bases or strong oxidizing agents. Acids and bases don’t mix for a reason, and even vapors from volatile substances ruin purity—or worse, create unwanted reactions inside a sealed cabinet.
Regular checks on expiration dates and conditions of storage pay off. Replace seals that start to crack. Audit stocks before ordering new chemicals—the less clutter, the less chance for accidents. I encourage anyone working with these acids to keep safety data sheets handy and read them more than once.
Some places install a separate, temperature-controlled acid cabinet, especially for larger inventories. That way, housekeeping doesn’t overlap with high-traffic areas where someone might bump into a bottle or leave it open. I still trust double-sealed, clearly marked glass bottles tucked into a low-light, low-humidity cabinet. Sweat the small stuff with laboratory acids.
Responsible storage cuts costs, limits exposure, and keeps the lab from turning into a hazardous maze. Your nose and your results will thank you.
You don’t have to work in a chemical plant to cross paths with aromatic monocarboxylic acids, especially benzoic acid and its relatives. Found in everything from food preservatives to lab reagents, they often look harmless—white crystals in a jar. But behind the label lies a list of risks that can catch the careless off guard. Skin and eyes react badly to many of these compounds. Inhaling their dust triggers irritation, cough, and worse over time. At home, I once spilled a tiny vial of benzoic acid powder and forgot gloves. The sting on my fingers became a lesson about chemical burns sooner than any textbook could warn.
Direct contact leaves lasting memories, so wearing proper gear isn’t just tradition—it’s survival. Nitrile gloves remain a steadfast barrier for hands, offering more resistance than latex with plenty of dexterity. Lab coats or aprons stop splatters from sinking into clothes and skin. Eyes demand full coverage, not just flimsy spectacles; sealed goggles keep both powder and accidental sprays out. In case of an unlucky splash, a nearby eyewash and safety shower need nothing less than full working order—checked often, used without hesitation.
Good ventilation earns its place as another top safeguard. I avoid weighing acids on open benches. Fume hoods—or even basic exhaust fans—help whisk away airborne dust and vapors before breathing them in becomes a bigger problem. In smaller labs, even a portable fan can make a difference, as long as it blows fumes away and not straight at people working nearby.
Carrying a bottle with two steady hands makes sense—spills sometimes come from simple slips. Screw caps must tighten fully after measuring out every dose. For storage, dry shelves away from heat and the lab's sunny corners work best. Many aromatic acids decompose or become hazardous when stored next to strong oxidizers or bases. Keeping incompatible chemicals a few shelves apart beats dealing with a fire or toxic gas later.
If a spill does happen, I never use a shop vacuum. Dry acid powder in the air gets everywhere and can be inhaled or settle on surfaces unnoticed. Small amounts can be gathered gently with a disposable scoop or wet wipes, then sealed in labeled waste bags. Larger spills need a proper approach—call for trained help, evacuate the room, and let emergency procedures kick in.
Any leftover acid, waste mixtures, or contaminated rags go into hazardous waste bins, not the regular trash. Flushing these compounds down the drain risks environmental harm and water contamination. In academic labs, waste disposal services pick up these materials, logging each batch for safety. Even at home or in small DIY spaces, reaching out to community hazardous waste collections shows respect for both people and the planet.
No one becomes an expert overnight. Sharing stories about mishaps, keeping updated on safety sheets, and joining training sessions make a difference. The more people know about risks and how to manage them, the stronger the safety culture grows. Talking through new situations or odd odors in the lab can spot troubles early, before they spiral into bigger issues.
Staying mindful about aromatic monocarboxylic acids isn’t just about following rules. It’s about taking care of one another, keeping mistakes small, and learning from each close call. Each safety step, from gloves to teamwork, shrinks the chance of harm in any environment where these chemicals turn up.
Walk into any college chemistry class and mention benzoic acid—watch half the room nod knowingly. Aromatic monocarboxylic acids show up in all sorts of places: food preservation, medicine, even when talking about the everyday world of fragrances. These acids all follow a clear blueprint: a benzene ring holding on to a single carboxylic acid group. This simple combination decides much about their behavior and role in so many industries.
At the core sits the benzene ring, a tight-knit circle of six carbon atoms, sharing electrons and making the structure steady and hard to break apart—what chemists call aromaticity. Hook a carboxyl group (-COOH) onto one of those carbon atoms, and this arrangement opens the door to a whole family of compounds. The basic formula? C6H5COOH. That carboxylic acid group brings an acidic part to an otherwise stable ring, letting the molecule step into countless chemical reactions.
Take benzoic acid—nature’s simplest aromatic monocarboxylic acid. No fuss, just a benzene ring with a carboxyl group. Add a nitro, methyl, or hydroxy group to the benzene backbone and you get variations like para-aminobenzoic acid or salicylic acid (the key ingredient in aspirin and acne creams). The ring’s stability lets all sorts of substitutions happen, explaining why scientists can “tune” these compounds for different uses without breaking the core structure.
Now, these molecules don’t just look good on paper. Benzoic acid keeps food safe by cutting down on mold. Salicylic acid calms inflamed skin. Pharmaceuticals lean on these structures to deliver targeted effects with minimal side reactions, thanks to the predictability of that aromatic ring. I remember struggling to grasp why a simple formula like C6H5COOH makes such a difference, but it’s this foundation that lets scientists design everything from antifungal treatments to long-lasting preservatives.
Food safety teams trust benzoic acid and its relatives because these compounds stop yeast and bacteria from growing in acidic foods. The molecular structure holds up well under pressure from heat and pH swings, so shelf life stretches out. Dermatologists recommend creams and cleansers packed with aromatic monocarboxylic acids, counting on both their effectiveness and safety from years of research.
Even straightforward chemicals raise questions. Environmental researchers raise fair points about buildup in water or soil, especially as these acids see increased use in industrial and pharmaceutical settings. It’s critical to keep tabs on breakdown rates and changes in the environment to avoid long-term harm. Supporting initiatives that encourage greener synthesis and better waste treatment protects water supplies and soil, making everyday products safer in the long run.
As more companies focus on sustainable chemistry, options like biodegradable aromatic acids and smarter purification methods deserve attention. These innovations don’t just clean up the lab—they ease worries about what ends up downstream. Open collaboration between scientists, regulators, and producers creates a safer future for everyone who uses or encounters these compounds daily.
Aromatic monocarboxylic acids might not look flashy, but their structure packs a punch. The benzene ring and carboxyl group create a family of compounds trusted for stability, versatility, and reliability. Their chemical structure underlies a huge range of uses and brings up honest questions about safe use and disposal. Paying attention to both the science and the impact keeps these acids serving their purpose without letting hidden costs pile up.
Aromatic monocarboxylic acids, like benzoic acid and its close relatives, play a big part in both industrial processes and daily products. From preservatives in food to base chemicals in factories, these acids show up in places most people never notice. Still, their story doesn’t end with production. The talk about impurities never gets old for those who rely on consistent quality, whether you’re working at the bench or supervising bulk supply.
Making these acids rarely goes as cleanly as textbooks promise. Real-world batches often turn up with leftovers and unintended extras. A big offender is unreacted starting material. In benzoic acid preparation, for example, you find bits of benzaldehyde that didn’t join the party all the way.
Trace organic solvents are tough to avoid since most syntheses use them to dissolve, extract, or crystallize the acid. Even after processing, solvents like diethyl ether or toluene can tag along if the drying step cuts corners. And old glassware? It leaves its mark. You’ll see dust, tiny silica, or even residues from strong acids used in cleaning.
Another classic impurity: related isomers. Paratoluic acid, for instance, rarely comes pure from early-stage processes—there’s always a bit of ortho-toluic acid or meta-toluic acid mixed in. If you work in pharmaceuticals, even a small dose of the wrong isomer might throw the recipe off, meaning purity translates directly to patient safety.
I’ve seen batches of supposedly high-grade benzoic acid get rejected because spectroscopic analysis dug up an unexpected absorbance—a telltale sign of an extra carbonyl group. For food science, these mishaps mean health risks or regulatory trouble. Even a few ppm of certain aromatic ketones can produce off flavors, raise toxicity flags, or make it impossible to meet legal thresholds.
Chemists swapping stories at conferences always chat about consistency. If you’re running a factory reactor overnight, you trust the raw acid won’t clog your system or spark a weird side reaction. Importers lose sleep over shipment delays and failed purity tests, because even “minor” contamination causes expensive holdups. Small business owners who make soaps, cosmetics, or processed snacks feel the pressure too. Few people realize that a failed batch doesn’t just hurt the bottom line—it erodes trust up and down the supply chain.
The best chemists I know obsess about records: source, process, and batch-to-batch tracking. Chromatography, spectrometry, and TLC plates fill their labs because every scientist learns, often the hard way, that purity reports aren’t just paperwork. Good storage makes a difference too. Acids stored in damp or sunlit conditions pick up more degradation products— things like peroxides or strange-smelling esters—compared to properly sealed, temperature-stable storage.
Manufacturers fight impurities with both improved synthetic routes and real quality assurance. Techniques like recrystallization, filtration, and careful distillation strip out a surprising number of troublemakers. Some invest in greener chemistry, designing routes that sidestep especially sticky contaminants. Those who invest in third-party analytical testing catch more batch-to-batch changes, which gives peace of mind both to suppliers and customers.
The chase for reliable monocarboxylic acids stands on more than clean glassware and good habits— it depends on know-how and vigilance at every step, from factory synthesis to finished product shelf life. Keeping tabs on impurities isn’t just about following the rules; it’s about respect for the people and processes downstream. The best partners in chemistry, I’ve learned, are the ones who watch out not only for what’s supposed to be in the bottle, but all the things that sometimes sneak in, too.
| Names | |
| Preferred IUPAC name | Benzoic acid |
| Other names |
Aromatic Carboxylic Acids Aromatic Acidic Compounds Aromatic Monoacids |
| Pronunciation | /əˌrɒmətɪk ˌmɒnəˌkɑːbɒkˈsɪlɪk ˈæsɪdz/ |
| Identifiers | |
| CAS Number | ["99-96-7", "100-09-4", "100-07-2", "74-79-3", "619-72-7", "104-87-0"] |
| Beilstein Reference | 10 |
| ChEBI | CHEBI:33559 |
| ChEMBL | CHEMBL2364649 |
| ChemSpider | 263 |
| DrugBank | DB01362 |
| ECHA InfoCard | 04c9e510-92bb-4b10-baa4-0b22e9f8acfc |
| EC Number | 2.6.1.85 |
| Gmelin Reference | Gmelin Reference: "16 |
| KEGG | C00156 |
| MeSH | D02.241.223 |
| PubChem CID | 469 |
| RTECS number | CY1400000 |
| UNII | Q81TCZ4WND |
| UN number | UN3439 |
| Properties | |
| Chemical formula | C7H6O2 |
| Molar mass | 122.12 g/mol |
| Appearance | White to off-white crystalline powder |
| Odor | Characteristic. |
| Density | 1.06 g/cm3 |
| Solubility in water | Slightly soluble to insoluble in water |
| log P | 1.96 |
| Vapor pressure | 0.001 mmHg (20°C) |
| Acidity (pKa) | 4–5 |
| Basicity (pKb) | 3-4 |
| Magnetic susceptibility (χ) | Diamagnetic |
| Refractive index (nD) | 1.554 |
| Viscosity | 1.08 mPa·s |
| Dipole moment | 1.41 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 151.0 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -385 to -430 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3220.0 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | M01AE |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin and eye irritation, may cause respiratory irritation. |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| Precautionary statements | Keep container tightly closed. Store in a cool, dry, well-ventilated place. Avoid contact with eyes, skin, and clothing. Wear appropriate personal protective equipment. Wash thoroughly after handling. Do not breathe dust, vapor, mist, or gas. |
| NFPA 704 (fire diamond) | 2-1-0 |
| Flash point | 103 °C |
| Autoignition temperature | 550°C |
| Lethal dose or concentration | LD50 (oral, rat): 1850 mg/kg |
| LD50 (median dose) | LD50 (median dose): 1,070 mg/kg (rat, oral) |
| NIOSH | NA |
| PEL (Permissible) | 10 mg/m3 |
| REL (Recommended) | 0.5 mg/m³ |
| IDLH (Immediate danger) | 50 mg/m³ |
| Related compounds | |
| Related compounds |
Aromatic dicarboxylic acids Aromatic sulfonic acids Aromatic amino acids |
