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Folks in chemistry rarely get excited about ethyl esters unless they hold a special place in making or discovering something new. Ethyl 4-nitrobenzoate, in particular, has its roots in European organic chemistry circles, spinning off from benzoic acid derivatization efforts in the late 1800s. European chemists tinkered with nitration and esterification, searching for ways to stretch benzoic acid’s abilities. Over time, the compound became a staple in research labs thanks to the push to make new dyes, pharmaceuticals, and specialty materials. Its easy modification and reliable performance brought it off the bench and into the mainstream catalogs of chemical suppliers.
Every lab has that one workhorse compound—a little bottle that gets opened again and again. In synthesis, ethyl 4-nitrobenzoate fills that role with a nod to flexibility. Once you tack a nitro group to the para position and swap the acid for an ethyl ester, the molecule stands ready for all sorts of transformations. Whether making an amine or building a bigger molecule, chemists turn to this compound for its stability in storage and reliability during reactions. You can easily spot it on the shelf thanks to its light yellow crystals and sharp, slightly sweet scent.
Open a bottle of ethyl 4-nitrobenzoate and you’ll see a pale yellow, crystalline solid. You won’t watch it fizz or degrade in air, since the nitro group makes it fairly unreactive without harsher conditions. With a melting point over 70°C and low water solubility, it stands up well in organic extractions. Its molecular weight sits around 209 grams per mole, and it dissolves nicely in common solvents like ethanol and acetone. The nitro and ester groups invite further chemistry. You don’t see this stuff spontaneously combust or react with the moisture in the air, allowing for safe, predictable handling.
Whenever chemists consider using ethyl 4-nitrobenzoate, purity takes center stage. Most commercial batches offer 98% or better, with trace impurities from the nitration or esterification steps. Labels typically list the chemical’s name, formula (C9H9NO4), and hazard info. Any extra labeling only helps so much—most researchers double-check with their own instruments just to be sure.
The chemistry behind making ethyl 4-nitrobenzoate feels like a rite of passage for organic chemists. Start with 4-nitrobenzoic acid, react it with ethanol, and add a strong acid catalyst like sulfuric acid. The esterification proceeds with gentle heating, often followed by stepwise washing, cooling, and crystallization. Some labs recrystallize from ethanol or another solvent to clean it up even further. Yields run high, provided the starting materials came from decent stock and nobody rushes the process.
Pick up a textbook and you’ll find ethyl 4-nitrobenzoate featured in the nitro reduction chapters. Its most famous trick involves reducing the nitro group to an amine, usually through catalytic hydrogenation or tin(II) chloride in acid. That transformation alone opens doors to making dyes, pharmaceuticals, and agrochemical intermediates. Acid or base hydrolysis returns you to the acid, while other groups can swap in for functionalized esters. Its structure lets it play the part of a blank slate, ready for creative routes in synthesis.
Walk into a chemistry storeroom and you’ll hear ethyl 4-nitrobenzoate called by a few different names: 4-nitrobenzoic acid ethyl ester, para-nitrobenzoic acid ethyl ester, or just ENB among colleagues. Numbers like CAS 619-58-9 provide an unambiguous identity in global databases, sidestepping translation hiccups and synonyms that pile up over decades of research.
Handling ethyl 4-nitrobenzoate rarely challenges a seasoned lab worker. Despite the nitro group, it's more benign compared to its raw acid counterpart or explosive nitroaromatics. Standard safety precautions apply: gloves, goggles, fume hood if powders might go airborne. Disposal follows chemical waste protocols, avoiding open flames and heat sources in bulk operations. Most chemists learn respect for nitro compounds early, and routine safety checks ward off surprises.
In half a dozen industries, ethyl 4-nitrobenzoate leaves its mark. Paint manufacturers seek it out for azo dyes and pigments, where the nitro group’s color fastness delivers durability. Pharma companies look to it as a precursor, reducing the nitro to an amine and building up complex drug scaffolds. Research labs produce derivatives as part of method development in organic chemistry education. Its stability and versatility keep it near the center of several chemical supply chains.
Most might think all the basics got solved decades ago, but research pushes onwards. Chemists continue to look for milder, “greener” conditions for both preparation and downstream modifications. Researchers look for catalysts that give higher yields or use less toxic reagents. Some dive into making new materials or exploring structure-activity relationships in drug development, squeezing out more value from this humble intermediate.
Toxicologists keep one eye on new reactions and another on old compounds like ethyl 4-nitrobenzoate. Acute exposure rarely leads to severe health issues in controlled settings, but the nitro group signals caution: chronic effects remain a concern if dust or vapors escape regular lab controls. Studies suggest only moderate toxicity, yet prudent chemists avoid skin and eye contact and minimize inhalation. Newer workplace monitoring and exposure limits guide even routine benchwork, keeping health risks in check.
The future doesn’t promise the next blockbuster compound based on ethyl 4-nitrobenzoate, but industry keeps leaning on its reliability. Markets for dyes and advanced molecules continue to expand, giving it a role in modern, specialty chemical processes. Process chemists aim to trim waste and cut hazard potential, exploring enzyme-based catalysis or continuous-flow methods. In teaching labs and commercial plants, ethyl 4-nitrobenzoate will keep anchoring reactions as researchers push for safer, faster, and greener chemistry.
Most people never give a second thought to the building blocks that feed the shelves at their local pharmacy or the materials tucked inside their car’s dashboard. For many modern materials and treatments, the story begins with compounds developed in small glass beakers, not storied pharmaceutical giants. One such starting point hides behind the unassuming name “Ethyl 4-Nitrobenzoate.”
Ethyl 4-nitrobenzoate serves a straightforward but important job as a key intermediate. It provides the backbone for a range of chemical transformations, mostly in pharmaceutical and agricultural research labs, and in specialty chemicals manufacturing. Its nitro group and ester side chain make the molecule both easy to adapt and reactive. For a synthetic chemist, this means more opportunities to manipulate the basic structure and push it in useful directions.
Some big-name painkillers, anti-inflammatories, and antibiotics start their journeys with compounds just like this. Ethyl 4-nitrobenzoate offers a stable structure but can be tweaked in several ways. The nitro group often serves as a target for reduction, producing amines – key players when creating active pharmaceutical ingredients like anesthetics or even antihistamines. Research labs rely on this chemistry to build libraries of test compounds, each a small step closer to a breakthrough medicine.
The influence spills outside healthcare. Makers of dyes and pigments for textiles, paints, and plastics use Ethyl 4-nitrobenzoate as a feedstock. The nitro group gives vibrant color properties, and manufacturers find it easy to link with other additives that improve lightfastness or durability. Anyone who has bought a shirt that hardly fades or drove a car with a dashboard that stays glossy owes some credit to early-stage chemicals like this.
The manufacture and use of Ethyl 4-nitrobenzoate bring up questions about safety and responsible handling. The nitro group tends to raise red flags for flammability and potential toxicity, and there is growing scrutiny on the environmental impact of such intermediates. Facilities working with this compound must follow clear protocols, not just for worker safety but also to manage waste and runoff. Regulators have begun to tighten guidelines for storage and disposal, pushing chemical companies toward better practices.
As technology moves forward, many research labs look at greener alternatives. Some explore biocatalytic processes—using enzymes or microbes to tackle the same chemical changes with fewer harsh solvents and byproducts. Lawmakers and watchdogs call for tighter oversight, but real change often comes from demanding that bulk chemical suppliers provide clearer traceability and environmental impact data. Scientists in the field, myself included, see the need to balance the dependability of traditional methods with the drive for less toxic process chemistry.
Ethyl 4-nitrobenzoate may not draw attention on store shelves, but every finished product needs reliable, adaptable starting materials. Why should anyone care? Because the route from simple molecules to life-saving drugs, vivid colors, and tough plastics passes straight through chemicals like this. Paying attention to the supply chain means weighing not just the cost or performance, but the impact on health, safety, and the environment. Consumers and industries both stand to gain from those choices — and a safer, more sustainable world depends on them.
Ethyl 4-nitrobenzoate often pops up in labs that focus on organic synthesis or pharmaceutical research. It may look like just another chemical, but this compound plays a valuable role as both an intermediate and a handy reference in academic experiments. Its structure features an ethyl group attached to a benzoic acid molecule, with a nitro group taking the fourth position on the benzene ring.
The formula for ethyl 4-nitrobenzoate reads as C9H9NO4. Here’s how those numbers and letters make sense: nine carbon atoms come from the benzene ring and the ethyl group, hydrogen appears with nine atoms, oxygen lands at four (mainly due to the ester and nitro parts), and nitrogen is present once, courtesy of the nitro group.
In every organic chemistry textbook, you’ll find ethyl 4-nitrobenzoate listed for good reason. Its nitro group offers a way to track reactions involving electron-withdrawing groups. Students and professionals alike grow comfortable with this formula in their early days of spectroscopy practice, particularly because nuclear magnetic resonance (NMR) and infrared spectroscopy provide clear, distinct signals when using these types of molecules.
Accurate formulas like C9H9NO4 hold real weight in real-world work. I remember one afternoon in university—back in the organic lab—watching a friend miscalculate and swap two numbers in a related ester’s formula. One small error can derail a synthesis, leading to wasted time and lost resources. Mistakes snowball during scale-up trials in research settings. Correct formulas won’t make success automatic, but precision lays a foundation that every lab can build on.
This is more than textbook trivia. During pharmaceutical development, using the right intermediate—say, ethyl 4-nitrobenzoate—cuts unnecessary steps and lets research teams hit purity targets faster. The presence of a nitro group also affects how a compound gets metabolized or tested for biological activity. These adjustments don’t just help companies cut costs—they also help bring medicines and new chemicals to users sooner.
Grow complacent with formulas, and issues creep in. Some early-career chemists copy from old notes or skip double-checking full molecular breakdowns. Translation errors or hastily drawn chemical structures create confusion, not just in lab reports but in journal publications across the globe. Electronic lab notebook systems and structure validation software reduce but can’t eliminate these human errors. Staying rigorous about checking formulas avoids preventable surprises and fosters real communication between researchers, manufacturers, and regulatory teams.
Every aspiring chemist benefits from hands-on drills that push them to cross-check calculated formulas and look at three-dimensional structures, not just flat representations. Lab managers drive better results by modeling critical thinking and rewarding error-spotting in internal reviews. When chemicals involve biomedical applications, putting clear labels and digital records side-by-side brings peace of mind. Building that culture of chemical literacy, right down to the molecular formula, makes research safer and more productive for everyone involved.
Ethyl 4-nitrobenzoate—C9H9NO4—might seem like a minor compound at first glance. Understanding and using its formula correctly brings tangible benefits, highlighting how small details create stronger science.
Ethyl 4-nitrobenzoate shows up in many labs as part of synthesis work or research on benzene derivatives. In my time working with organic chemicals, I’ve seen colleagues overlook the importance of basic storage details. Anyone who’s spilled a bottle of a poorly-stored nitro compound learns pretty quick that careful handling isn’t just a line from a textbook. This compound, a yellowish solid with a molecular formula of C9H9NO4, lasts far longer and stays much safer when basic guidelines are followed.
Most organic solids, including ethyl 4-nitrobenzoate, stay stable at room temperature, but that’s only half of the picture. Toss a sample in a sunlit windowsill or leave it near any kind of heat source, and you’re asking for trouble. Heat speeds up decomposition and can increase internal pressure, especially in sealed bags or bottles. At my old university lab, I saw a sample left too close to a radiator; the crystals stuck together, and the tiny bit of odor meant something sour was happening at a molecular level. Regular room temperature in a cool, dry storage area does the trick. Keep it out of direct sunlight and away from stovetops or radiators.
Humidity can cause headaches in unexpectedly quick ways. Even compounds that look rock solid can clump, absorb water, or alter chemically over several weeks. Using desiccators or cabinets with silica gel makes a real difference here. More than once, I opened old bottles to find sticky, hard-packed crystals when someone skipped the trouble of using a desiccant. A tightly sealed container blocks moisture, stops contamination, and helps you avoid a ruined sample and weeks of lost work.
Glass bottles or HDPE containers with screw-on lids seal out air and stop unwanted reactions. Even if ethyl 4-nitrobenzoate isn’t as reactive as some of its cousins, oxygen and light can slowly cause it to break down. Opaque bottles offer an extra layer of protection, especially in shared spaces or long-term storage. I never forget to check for cracks or worn threads on containers before storing anything. Nothing spoils a day faster than finding chewed-up plastic from a slow chemical leak on a shelf.
An unlabeled bottle is bad news. Even seasoned researchers have mixed up samples by trusting memory over written words. Attaching clear labels showing the chemical name, the date, and the full hazard information isn’t just a chemistry rule—it’s how you keep yourself and everyone around you healthy. I watched a colleague grab the wrong bottle for a routine reaction, only to set off a plume of smoke fattened by an unlisted contaminant. That label could’ve saved days of investigation and a safer workspace.
Organic nitro compounds need some respect—they’re combustible under certain conditions. Even with a pretty high flash point, no one wants to risk a spark or friction setting things off in a cluttered storeroom. Place ethyl 4-nitrobenzoate in flammable storage cabinets, away from oxidizers or other reactive chemicals. Avoid stacking chemicals with unknown bonuses, and leave enough room for ventilation. These simple steps helped my old team avoid two close calls during crowded semesters.
Regular cleaning stops dust and keeps spills from building up. Never store food or drink in labs—cross-contamination is a real risk with chemicals like this one. Use personal protective equipment and keep spill kits ready. Good housekeeping keeps accidents from becoming disasters, something every long-time lab tech takes seriously.
The points above come from years working around organic compounds, not just reading manuals. Following these core habits keeps ethyl 4-nitrobenzoate reliable as a research material and minimizes risk. In the end, safe storage isn’t complicated; it just rewards attention and respect for both the science and the people using it.
Ethyl 4-nitrobenzoate shows up in a lot of labs but rarely lands in the spotlight outside specialized industries and research. It comes from a family of chemicals known for their roles in making pharmaceuticals, dyes, and even agricultural products. Most people never run into it unless they work around chemistry or in a factory setting. For those of us who do, the question isn’t whether it’s useful — it’s whether you can handle it without putting your health at risk.
I’ve lost count of the number of times a tidy chemical bottle turns out to be more dangerous than folks assume. According to trusted sources like PubChem and Sigma-Aldrich, ethyl 4-nitrobenzoate doesn’t belong in kitchens or offices. Skin or eye contact can cause irritation. Swallowing it or breathing the powder can be toxic. Swallowing nitro-substituted aromatic compounds often puts strain on the liver, kidneys, and central nervous system. This specific compound, though less studied than heavy-hitters like nitrobenzene, deserves the same caution. The core nitro group in its structure hints at why experts give it respect: compounds with nitro groups often carry health risks, including methemoglobinemia, which reduces blood’s oxygen-carrying ability.
Old-timers in chemistry talk about chemicals like this one as “out-of-sight, out-of-mind” but that kind of thinking invites trouble. I once saw a careless moment lead to a splash on the forearm. Redness and irritation came on quick. Getting exposed repeatedly raises the chance of allergies and worse outcomes like chronic dermatitis, especially if protective gloves and goggles get ignored. It doesn’t help that powders can go airborne, so inhaling dust while weighing out a sample becomes a real risk.
I’ve seen workplace stories change for the better once teams start treating the material safety data sheet (MSDS) as a must-read, not a dusty binder. MSDS documents list clear steps for washing off spills, managing accidental inhalation, and cleaning up without spreading dust particles. Any company that skips proper chemical fume hoods, gloves, or goggles isn’t taking employee wellbeing seriously. Looking up government databases like the US National Library of Medicine shows similar advice: “minimize exposure,” “avoid breathing dust,” and “do not eat, drink, or smoke when using this product.” Even seasoned chemists benefit from regular training sessions to keep the dangers fresh in mind.
Safe working conditions depend on not taking shortcuts. Simple fixes make a big difference. Labs that use ethyl 4-nitrobenzoate should always have up-to-date eye wash stations and showers, plus strict no-food policies around the chemistry. Everyone from students to senior scientists benefits when clear labels and emergency protocols become part of the routine. Waste needs to go into the right disposal containers, far from regular trash, because nitrobenzoate compounds don’t break down easily and can pollute water if tossed away carelessly.
Every generation of chemists learns a hard truth: trust and teamwork limit accidents far better than a false sense of invincibility. Whether it’s through swapping stories about close calls, or running more drills, a culture that values people over routine makes the work as safe as possible. Direct sunlight, open flames, and sources of static electricity need to stay far away from bottles of ethyl 4-nitrobenzoate. With the right respect and preparation, researchers and workers keep their focus on progress without gambling with their health.
A chemical like Ethyl 4-Nitrobenzoate doesn’t draw much attention from those outside lab walls, but anyone with time in a synthesis lab respects how a slight variation in purity changes everything. Purity acts as a foundation for reproducibility, yields, and confidence in results. No researcher wants to explain away a failed reaction because the material came with hidden sidekicks.
Most chemical suppliers target a purity of 98% or greater for Ethyl 4-Nitrobenzoate meant for research. Analytical labs and production chemists trust figures confirmed through HPLC or GC, sometimes supplemented with NMR for extra assurance. In pharmaceutical work or synthesis of bioactive intermediates, that 98% figure often marks the bare minimum. There are good reasons for these numbers: many synthetic protocols will amplify the minor impurities, turning a small contamination into a significant byproduct.
Impurities do more than just crowd out the main component. I've seen benchwork wrecked by an impurity that derailed catalysis, stubbornly refusing to separate from a target compound during purification. Processes demanding scale-up carry greater risk — leftovers in a reagent pool can end up as contaminants at troubling concentrations. These problems are rarely theoretical; I’ve watched the extra hours spent under the fume hood, the painful re-running of columns, all because the supplier let purity slide to 95%.
For Ethyl 4-Nitrobenzoate, most impurities spring from the manufacturing process: unreacted starting materials, isomeric products, and trace solvents. In a resource-limited academic setting, quick TLC screening and melting point checks give an early heads-up on purity issues. Industrial players rely on HPLC/GC integration for reliable, audit-ready data. Having a single peak or near-perfect integration above 98% on these reports gives needed peace of mind before that first reaction vial mixes.
Suppliers who care about long-term relationships back up their numbers with a certificate of analysis. They provide the assay data, lot number, and analytical methods. When I’ve worked with reputable vendors, they encouraged questions and even shared chromatograms — that transparency builds trust. Some companies offer higher-purity “trace analysis” or “ultra-pure” grades, usually above 99%. This extra margin of purity often proves worth the extra cost for sensitive or regulatory-bound projects.
Solving purity challenges calls for honest dialogue throughout the supply chain. That means suppliers sharing analytical results upfront and buyers checking certificates rather than just trusting catalog copy. On the lab side, running a quick check, even on new stocks from trusted vendors, saves time and headaches later. If issues show up, reporting problems to the vendor opens the door for corrections and better batches down the line.
Clean, well-specified Ethyl 4-Nitrobenzoate isn’t just about numbers on a paper. Every chemist who’s tried to purify a murky batch or lost a day to wonky yields has felt the cost of wavering standards. Reliable purity means fewer interruptions, lower waste, and a smoother shot at reproducible, publishable science. In a world that demands more transparency and traceability, setting and upholding real purity standards feels like the right move for everyone.
| Names | |
| Preferred IUPAC name | Ethyl 4-nitrobenzoate |
| Other names |
4-Nitrobenzoic acid ethyl ester p-Nitrobenzoic acid ethyl ester Ethyl p-nitrobenzoate Benzoic acid, 4-nitro-, ethyl ester |
| Pronunciation | /ˈiːθɪl fɔːr ˈnaɪtroʊ bɛnˈzoʊ.eɪt/ |
| Identifiers | |
| CAS Number | 619-58-9 |
| Beilstein Reference | 1209372 |
| ChEBI | CHEBI:21036 |
| ChEMBL | CHEMBL41378 |
| ChemSpider | 14126 |
| DrugBank | DB08343 |
| ECHA InfoCard | 100.012.366 |
| EC Number | 211-482-9 |
| Gmelin Reference | Gmelin Reference: 83138 |
| KEGG | C19238 |
| MeSH | D020044 |
| PubChem CID | 8834 |
| RTECS number | GN8575000 |
| UNII | P9R1P6J950 |
| UN number | UN1663 |
| CompTox Dashboard (EPA) | DTXSID2041413 |
| Properties | |
| Chemical formula | C9H9NO4 |
| Molar mass | 167.15 g/mol |
| Appearance | Pale yellow crystalline powder |
| Odor | Sweet odor |
| Density | 1.34 g/cm3 |
| Solubility in water | slightly soluble |
| log P | 2.47 |
| Vapor pressure | 0.00017 mmHg (25°C) |
| Acidity (pKa) | 8.36 |
| Basicity (pKb) | Ethyl 4-Nitrobenzoate does not have a listed pKb value because it is an ester and not a base. |
| Magnetic susceptibility (χ) | -32.0e-6 cm³/mol |
| Refractive index (nD) | 1.570 |
| Viscosity | 2.69 cP (25°C) |
| Dipole moment | 3.98 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 324.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -306.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1851.7 kJ/mol |
| Hazards | |
| Main hazards | Harmful if swallowed, causes serious eye irritation, may cause respiratory irritation |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | Hazard statements for Ethyl 4-Nitrobenzoate: "H315, H319, H335 |
| Precautionary statements | P261, P264, P271, P272, P280, P301+P312, P304+P340, P305+P351+P338, P312, P330, P337+P313, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 2-3-0 |
| Flash point | 151 °C |
| Autoignition temperature | 367 °C |
| LD50 (median dose) | LD50 (median dose): Oral rat 6400 mg/kg |
| PEL (Permissible) | Not established |
| REL (Recommended) | 10 mg/m³ |
| Related compounds | |
| Related compounds |
Methyl 4-nitrobenzoate 4-Nitrobenzoic acid 4-Nitrobenzoyl chloride 4-Nitrobenzaldehyde Ethyl benzoate Ethyl 3-nitrobenzoate |
