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Looking back at how organic chemicals shape the world, methoxyphenylacetic acid stands out for its simplicity and adaptability. Organic chemists working during the last century paid close attention to benzylic acids for their role in synthesizing active pharmaceutical ingredients and flavors. In labs hinging on trial and error, researchers discovered that tinkering with a benzene ring—especially by adding methoxy and acetic groups—let them tweak reactivity and solubility. This isn’t just nerdy curiosity; the push to build molecules that nature couldn’t provide has fueled advances in medicine, agriculture, and even scent chemistry. Methoxyphenylacetic acid grew out of that environment, shaped by both academic curiosity and commercial demand for versatile building blocks.
At its core, methoxyphenylacetic acid is a benzylic carboxylic acid with an extra methoxy group hanging on the aromatic ring. The classic example people mention is 4-methoxyphenylacetic acid, thanks to its use in making pharmaceuticals, flavors, and intermediates for fine chemicals. There’s a reason chemists keep coming back to this compound: it’s easy to handle, fairly shelf-stable, and opens doors to more complex structures with the right tweaks in a reaction vessel.
Taking a look at its physical side, methoxyphenylacetic acid usually shows up as a white to off-white powder. It doesn’t evaporate easily, and it dissolves well in ethanol and other polar solvents. The melting point usually tells you whether it’s pure—impurities drop that point right down. The methoxy group on the ring makes the acid ever-so-slightly less acidic than plain phenylacetic acid. That brings advantages for downstream reactions, especially where selectivity matters. Those who have handled the stuff know it’s not volatile, doesn’t stink up the lab, and it’s got just enough reactivity to behave nicely with standard protections.
Specs aren’t just for paperwork—they can change the outcome of a whole process. Chemists regularly check for purity by NMR and HPLC, because any impurity can mess with pharmaceutical syntheses or flavor creation. Good quality methoxyphenylacetic acid has low moisture content and tight control over contaminant metals, which really matters if you use it in a multi-step synthesis or analytical assay. Companies usually label the package with molecular weight, batch number, and hazard info, because no chemist wants surprises at the benchtop.
Labs use benzene chemistry as their starting point, usually working from methoxybenzene. Dialing in the right temperature and acid/base conditions, they introduce an acetic group through a Friedel-Crafts acylation, using standard reagents like chloroacetic acid and Lewis acids, or by carboxylation of the corresponding methyl arene. The hard part involves getting good yields without introducing side-products—protecting groups can help, especially if sensitive functionality tags along. People working in industry corners push for greener processes, swapping toxic solvents with water, and using recyclable catalysts, both to save money and to avoid trouble with regulators.
You throw methoxyphenylacetic acid into a flask, and it plays well with alkylation, esterification, and amidation. In practice, scientists use it to craft a long list of derivatives, including esters for flavors, amides for pharmaceuticals, and more exotic structures through metal catalysis. Some research groups use it as a starting point for antipyretics and antimicrobials, and it finds a spot in fragrance chemistry too. Its phenyl ring, buffered by a methoxy, lets it soak up conditions that would trash other acids, keeping its integrity across a lot of synthetic moves.
People might find “p-methoxyphenylacetic acid,” “4-methoxyphenylacetic acid,” or just “anisylacetic acid” on the label. Those trade and trivial names just reflect where the methoxy group lands on the ring—sometimes ortho or meta, but usually para for most practical work. Chemists pay attention to these synonyms since subtle naming differences mean big changes in downstream chemistry.
In the chemical world, safety isn’t negotiable. Methoxyphenylacetic acid doesn’t flash off toxins or eat through gloves, but it can cause irritation if handled without care. Regulatory guidelines call for goggles, gloves, and decent ventilation—simple moves that save skin and eyes from rare but real exposure risks. Waste from reactions goes into separate drums for collection, to keep waterways clean and to comply with trade and workplace regulations. There’s always a bigger push for sustainability, so green chemistry gets top billing, nudging companies to lower emissions and minimize hazardous byproducts.
This molecule draws interest from several industries at once. Pharmaceutical labs value it for making active drug intermediates involving ether and amide bonds. Chemists in fragrance and flavor houses like its backbone for new notes, while agricultural researchers see it as a lead for designing new agrochemicals. Academic labs—my old haunt—study its reactivity just as much for what it means on paper as for the next real-world application. Wherever the demand comes from, methoxyphenylacetic acid’s adaptability drives diverse projects and products.
Research keeps finding new chemistry from this compound. Green processes get a lot of ink, as labs search for methods that cut raw material waste and energy use—catalysts that work in water, solvents you can reuse, and strategies that dodge heavy metals. People also look at tweaking the methoxy position for new properties. In fine chemical fields, making pure, single-isomer products keeps business bustling, since next-generation drug molecules demand ever-stricter specs.
So far, studies point to low acute toxicity for methoxyphenylacetic acid. Chronic effects haven’t put up red flags, but any chemical heading toward medicine or food flavors gets plenty of scrutiny. Animal studies must rule out organ toxicity and mutagenicity before regulatory bodies clear it for wider use. Chemists still stress the usual lab routines: proper storage, accurate labeling, and good hygiene to keep accidents from slowing science or sending someone to the emergency room.
Chemists see more for methoxyphenylacetic acid than its old reputation might suggest. Automation and AI promise faster screening for new derivatives that hit biological targets or create new scents. The push for green chemistry, always in the headlines, leans on molecules like this for their ease of use and adaptability to cleaner processes. For those who’ve spent years at the bench, these trends matter not just for profit or publication but because safer, smarter chemistry leaves a legacy that benefits the environment, workers, and all the people down the line who count on the products built from these unassuming but powerful building blocks.
Most folks probably haven’t spent much time thinking about methoxyphenylacetic acid. In a lab, the white powder looks like nothing special. What really makes it fascinating is how it’s become part of several industries, especially pharmaceuticals and fragrances. Every time I’ve read a box of medicine or sniffed a high-end perfume, it wouldn't occur to me that the same compound helps make both possible.
Doctors rely on new medicines to treat complex conditions, including hypertension, allergies, and mental health disorders. Methoxyphenylacetic acid steps in as a building block for active pharmaceutical ingredients. It doesn’t cure a disease by itself, but chemists use it to help create molecules that target very specific symptoms. According to publications from the American Chemical Society, the structure of methoxyphenylacetic acid allows easy modification, so scientists can attach other groups and change its behavior. That flexibility lets researchers develop drugs with improved action and fewer side effects. With the constant race against antibiotic resistance, a readily available and versatile compound becomes valuable in the fight to create new treatments.
Take a deep breath in front of a display of designer colognes, or even notice the light scent in a shampoo, and there’s a chance methoxyphenylacetic acid played a role. Perfumers have hunted for unique compounds that can bring out sweet, floral, or musky notes. What I’ve learned is that small tweaks in chemical structure lead to huge changes in aroma. Methoxyphenylacetic acid gives that sweet, anise-like nuance some synthetic fragrances rely on. Industry sources show it helps stabilize other scent molecules, so that perfume doesn’t fade halfway through a long day.
Back during my university days, chemistry majors loved to use methoxyphenylacetic acid to test reactions that need a stable, simple molecule. Teachers appreciated that it didn't break down too easily, and it gave clear, easy-to-read results for common experiments. As it’s widely available and not overly hazardous, it’s found in bench drawers in many undergraduate chemistry labs.
With demand climbing in pharmaceuticals and fragrances, manufacturing keeps scaling up production. This poses challenges. Unsafe production can lead to chemical waste or expose workers to toxic byproducts. If producers cut corners to keep costs down, they risk harming both the environment and people. According to recent EU chemical safety reports, trace waste of organic acids like methoxyphenylacetic acid can disrupt nearby waterways and aquatic life.
One promising solution lies in greener chemical processes. Some labs have started using bio-based methods—relying on bacteria or plant enzymes to produce the acid without generating hazardous leftovers. Regulations also push for stricter waste management, which helps keep possible pollutants out of the environment. Industry watchdogs recommend shifting to closed-system manufacturing, where emissions and waste are captured and recycled within the plant.
Even small, invisible ingredients shape entire industries—from the medicines that keep people healthy, to the little luxuries found in perfumes or personal care products. Watching how methoxyphenylacetic acid connects basic science, manufacturing, and even sustainability reminds me just how much thought and effort go into the products that land on shelves. For anyone working with chemicals, attention to safety and innovation in production methods isn’t just good business; it’s what keeps science moving in the right direction—and keeps people and the planet safer.
I remember opening my first college-level organic chemistry book and flipping to a diagram of Methoxyphenylacetic Acid. At its core, this compound carries a benzene ring—a cluster of six carbon atoms arranged like a tiny hexagonal badge. One of those corners, specifically the number four spot if you count clockwise from where the tail sticks out, carries an –OCH3 group: that’s the “methoxy” portion. The side chain, which distinguishes this acid, holds –CH2–COOH, or phenylacetic acid. If you lay it out, you get C9H10O3 as its molecular formula.
Holding a model of this molecule, the structure feels compact but a bit asymmetrical. The –COOH group (carboxylic acid) gives the molecule its acidity and the ability to interact with other substances. The methoxy group influences the molecule’s electronic properties. These different positions give chemists a way to tune how Methoxyphenylacetic Acid reacts, both in a lab and in a living body.
Methoxyphenylacetic Acid turns up in all sorts of research, especially synthetic organic chemistry. This kind of molecule has a knack for showing up as a building block during the creation of more complex compounds. Pharmaceutical research credits molecules like this as key starting points for designing new drugs. The combination of the aromatic ring, a methoxy group, and the carboxylic acid makes it valuable for modifications—each tweak shifts how it interacts with biological targets.
Some studies point toward derivatives of Methoxyphenylacetic Acid having anti-inflammatory or antimicrobial properties. Structure guides function; adding or shifting atoms on the molecule changes its effect in biological tests. This actually ties back to my own work in a university lab, where our team tested related acids for effects on enzyme activity. A small change—adding a methoxy group—turned something inactive into a strong inhibitor.
Creating Methoxyphenylacetic Acid in a laboratory isn’t as simple as stirring ingredients in a beaker. A typical route starts by attaching a methoxy group to a benzene ring before adding on the acetic acid tail. Controlling each step, making sure side reactions don’t spoil the batch, demands sharp skills and good planning. Purifying the end product requires patience and the right tools, especially if tiny impurities matter for drug testing or medical use.
Connections to real health or industrial value hinge on safe handling and precise manufacturing. Chemical exposure always carries risks, so labs invest in ventilation, gloves, and real training. I’ve seen experienced researchers remind new students to take these risks seriously—one splash or inhaled vapor leaves a lasting memory.
Better ways to synthesize and test chemicals such as Methoxyphenylacetic Acid depend on both funding and creative research. Green chemistry practices offer promise—using less hazardous materials, minimizing waste, and cutting energy use. Some labs now experiment with enzymes to carry out steps that once required harsh chemicals, a nod to sustainability and safety. Partnerships between universities, health agencies, and industry help move these innovations from theory to practice.
Understanding the chemical layout of Methoxyphenylacetic Acid opens doors both for curiosity and for new medicines. Breaking the process into clear, careful steps—just like drawing the structure—leads to safer lab work, better science, and real-world benefits down the line.
Some folks in labs or chemical plants might come across Methoxyphenylacetic Acid and wonder if grabbing a bag or bottle is a big deal. It pops up in certain fragrance work, pharmaceutical pieces, and maybe on a university research shelf. Safety questions make sense, especially with chemicals you can barely pronounce. No one wants their desk job to turn into a trip to the hospital.
Methoxyphenylacetic Acid sounds exotic, but the basic facts are simple. It’s a white crystalline powder, often with a faint, sweet smell. Some people see it and think “vanilla” or “almonds.” At the same time, a pretty name doesn’t mean it’s risk-free.
Safety data points out a need for eye and skin protection. Direct contact often causes irritation—think of that burning itch from accidentally brushing bleach or cleaning fluid onto your skin. Inhaling its dust triggers scratchy throat or nose issues. Anyone who’s ever cleaned out a chicken coop or dusted off old books knows that feeling—multiply it by a factor of ten, and you’re closer to what even a few airborne chemical particles can do.
Science literature hasn’t logged the chemical as a common carcinogen or linked it with chronic side effects. Still, the lack of famous risks doesn’t mean ignoring regular precautions. A little mistake can turn a boring workday into a stinging lesson.
Real-world experience backs up the official government advice. During college lab days, classmates ran into trouble chasing short cuts. Cutting corners with gloves—or skipping them to type on a laptop—turned into red hands and quick trips for eye wash. Everyone wanted to get back to work, but skin complaints slowed things down.
Methoxyphenylacetic Acid isn’t unique in that sense. Anyone handling even mild chemicals learns the habit—lab coat, safety glasses, sensible gloves, and good ventilation. Some jobs ask for a mask too. Nobody ever likes duct-taping safety posters, but there’s a reason every workspace puts them up.
The U.S. Occupational Safety and Health Administration (OSHA) and the National Institute for Occupational Safety and Health (NIOSH) lay out workplace rules. For example: store chemicals in cool, dry places; label everything; wash hands before you eat or leave. Standard stuff, but every hospital sees cases caused by skipping these basics.
Better labeling stands out as a first line of defense. “White powder” is about as useful as a blank page. Clear signs—chemical name, handling notes, and hazard levels—cut down confusion. Extra training helps too. New workers or volunteers might not recognize risky smells, textures, or spills, so regular safety refreshers make sense. More eyes and educated workers spot mistakes before anyone gets hurt.
Better ventilation gets advocates every year. Fans, hoods, or even just open windows move stray particles away from your nose and eyes. Most accidents turn small if you flush spills fast, and know where the emergency water is before work begins.
It doesn’t take an expert to see why respect for chemicals pays off. Handle Methoxyphenylacetic Acid sensibly, keep basic protections in place, and ask questions if unsure. Trust real data, practice good habits, and chemical safety becomes another smooth part of the day—never the headline.
Methoxyphenylacetic acid sits among the more sensitive organic reagents found in research laboratories. Its preservation relates directly to purity. Contamination often means ruined batches, wasted investment, and repeating experiments from scratch. Years spent in chemistry labs taught me that stable, clean storage matters just as much as the synthesis itself. Losing product to heat, air, or careless transfers becomes costly fast.
This compound stays stable at moderate ambient temperatures, typically around 20 to 25 degrees Celsius. Exposing it to higher temperatures can accelerate degradation. A lab shelf close to a sunny window may not seem risky, but small thermal spikes can make impurities creep in sooner than expected. On the other hand, full refrigeration isn’t always practical—a reward for diligence lies in simple, constant room-temperature storage away from direct heat sources or sunlight.
Even without visible signs, moisture in the air can work its way into bottles and erode sample quality. Desiccators serve as the gold standard in most labs, acting as a shield against humidity. Growing up in regions with high seasonal humidity, we learned to throw in an extra silica gel packet, especially during monsoons. This hands-on trick proves cheap and reliable. Seal bottles tightly, double-check after each use, and add a fresh desiccant regularly.
Some folks get careless, leaving a vessel open “just for a minute” during weighing or mixing. Oxygen in ambient air reactively nips at methoxy groups, forming unwanted byproducts. On top of that, bright lab lighting—for all its utility—can skew reaction rates for sensitive aromatic acids. My routine always involved storing these bottles in amber glass, away from open benches. This small step reduces both the light and oxygen exposure risk.
Labeling goes beyond the basic chemical name. Add the date received, the expiration date recommended by the supplier, and the initial purity percentage. Mixing up containers wastes time and can spoil a project. Store methoxyphenylacetic acid away from oxidizers, acids, and volatile bases. It’s not just theoretical safety advice—minor spills happen, and incompatible neighbors magnify emergencies. I’ve seen powder caking and odd smells when similar-sounding reagents sat together, creating a hazard or ruining both lots.
The catalogues from Sigma-Aldrich and Thermo Fisher consistently recommend cool, dry, and dark environments for methoxyphenylacetic acid. Experiences from university research groups and industrial QA teams back this up, linking careless storage to batch inconsistencies and the need for additional purification. Most wasted budgets come from poor housekeeping, not flawed chemistry. Inspecting storage areas weekly may not excite anyone, but that discipline preserves both your materials and your reputation.
Clean containers and careful handling top the list of must-haves. Replace caps immediately after every use, and never scoop directly from the source bottle with potentially contaminated implements. These practices add mere seconds to the workflow but can save hours in troubleshooting. Investing in smaller vials for daily use—leaving the main stock untouched—proves especially worthwhile for those working with sensitive or expensive chemicals.
Every good lab notebook or production record reflects a respect for material integrity. Keeping acid pure and potent isn’t just a matter of following supplier suggestions—it becomes a mark of personal and institutional reliability. Consistency in storage safeguards both scientific credibility and economic sense, earning client and regulatory trust the long way.
Methoxyphenylacetic acid, known to chemists as 2-methoxyphenylacetic acid or o-methoxyphenylacetic acid, packs a molecular weight of 166.18 grams per mole. This figure isn’t just a trivia detail for flashcards—it makes a real difference in the lab, the classroom, and even in the world of pharmaceuticals.
Back at university, nothing seemed more frustrating than trying to get a reaction to run, but ending up with not enough product. In organic synthesis, it always came back to the basics: weigh out the exact amount. Get the math wrong, the whole reaction could flop or create skewed data. The molecular weight isn't just a number on paper. It’s the conversion bridge between grams and moles—the units that chemists use every day to talk about the amount of stuff in a beaker.
Let’s take a closer look at methoxyphenylacetic acid. Its chemical formula is C9H10O3. To find the molecular weight, you add up the atomic weights:
Total: 108.09 + 10.08 + 48.00 = 166.17 grams per mole. The small decimal differences come from periodic table rounding, but for practical lab work, 166.18 g/mol is the accepted number.
Once you know this number, you stop guessing: it guides how to plan experiments, adjust enzyme concentrations, and predict how a drug might behave in the body. In pharmaceuticals, the molecular weight can hint at how well a compound might travel through the blood or slip through cell walls. Too heavy, and the body struggles to move it around. Too light, and it might get flushed out before it can do its job. For methoxyphenylacetic acid, landing at 166.18 g/mol, it’s a manageable size for both experimental synthesis and early drug development phases.
During my first research job, I weighed this exact acid by hand. I always double-checked the math, because even a small miscalculation could waste expensive chemicals or weeks of effort. Teams rely on these numbers during manufacturing, quality checks, and safety assessments. One small slip in calculating the molar mass can lead to missed targets or even hazardous spills. Clear, trusted data builds the backbone of safe, effective lab work.
While the molecular weight might seem like a footnote in a chemistry textbook, it often sets the tone for research accuracy. Accurate numbers lead to solid results, whether it’s developing a new painkiller or simply teaching students how to prepare a solution. For methoxyphenylacetic acid, that number—166.18—represents more than a statistical detail. It stands as the start of every batch, every reaction, and every analysis where this molecule plays a part.
Whether working in drug discovery, agriculture, or academia, getting this simple figure correct saves time, reduces waste, and keeps science moving forward.
| Names | |
| Preferred IUPAC name | 2-(Methoxyphenyl)acetic acid |
| Other names |
2-(4-Methoxyphenyl)acetic acid p-Methoxyphenylacetic acid 4-Methoxybenzeneacetic acid 4-Anisylacetic acid |
| Pronunciation | /ˌmɛθ.ɒk.siˌfiː.nɪl.əˈsiː.tɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 826-99-1 |
| Beilstein Reference | 1208737 |
| ChEBI | CHEBI:28662 |
| ChEMBL | CHEMBL404879 |
| ChemSpider | 5198 |
| DrugBank | DB08353 |
| ECHA InfoCard | 100.042.543 |
| EC Number | 3.1.1.78 |
| Gmelin Reference | 6135 |
| KEGG | C02126 |
| MeSH | D008715 |
| PubChem CID | 76908 |
| RTECS number | DO7525000 |
| UNII | 0LD9R8P8X9 |
| UN number | UN2811 |
| Properties | |
| Chemical formula | C9H10O3 |
| Molar mass | 166.18 g/mol |
| Appearance | White to off-white crystalline powder |
| Odor | aromatic |
| Density | 1.183 g/cm³ |
| Solubility in water | Slightly soluble in water |
| log P | 1.1 |
| Vapor pressure | 0.0000146 mmHg (25°C) |
| Acidity (pKa) | 3.77 |
| Basicity (pKb) | 14.14 |
| Magnetic susceptibility (χ) | -54.0 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.544 |
| Dipole moment | 1.90 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 380.8 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -489.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1647.0 kJ/mol |
| Pharmacology | |
| ATC code | **N02BX08** |
| Hazards | |
| Main hazards | Harmful if swallowed, causes serious eye irritation |
| GHS labelling | GHS07, GHS05 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | Hazard statements: "Causes serious eye irritation. |
| Precautionary statements | Precautionary statements: P261, P264, P271, P301+P312, P304+P340, P305+P351+P338, P312 |
| NFPA 704 (fire diamond) | 2-1-0 |
| Flash point | 99°C |
| Autoignition temperature | 240 °C |
| Lethal dose or concentration | LD50 oral rat 1620 mg/kg |
| LD50 (median dose) | LD50 (median dose): >2000 mg/kg (Rat) |
| NIOSH | BY9275000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.5 mg/m³ |
| IDLH (Immediate danger) | Not listed |
| Related compounds | |
| Related compounds |
Phenylacetic acid p-Anisic acid 4-Methoxyphenylacetonitrile 2-Methoxyphenylacetic acid 3-Methoxyphenylacetic acid p-Methoxybenzyl alcohol p-Hydroxyphenylacetic acid |
