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Chemistry didn’t always have the intricate tools and clever molecules found in today’s labs. Some of the older diazonium salts, born from the pursuit of better dyes and faster color changes, set the stage for a cascade of discoveries. As more ways to modify aromatic rings rolled in, scientists began tinkering with electron-donating and electron-withdrawing tricks — not just for color, but to unlock routes in organic synthesis that hadn’t seemed feasible before. That’s exactly where compounds like 2,5-diethoxy-4-(4-toluenesulfonyl)benzenediazonium zinc chloride came into play. Long chemical names often draw groans from students, but in this case, complexity brings precision. Each group has a history — ethoxy modifications to tune reactivity, toluenesulfonyl for shifting electronics, and a zinc chloride counterion to rein in some of the chaos that free diazonium ions threaten in solution. I remember scanning through literature from the late twentieth century, seeing the slow, almost stubborn progress toward salts stable enough to ship and choke points in cross-coupling chemistry slowly clearing up, all thanks to teams who saw the potential in these tweaks.
This molecule isn’t just another blip in a catalog. You’ll rarely find it sitting unused in an academic storeroom because its structure lends itself to purposeful, clever manipulations — a trait not every diazonium salt can claim. The main appeal comes from what these tailored structures actually allow: aromatic substitutions, participation in Sandmeyer-type reactions, and smooth transfer of functional groups under tightly controlled conditions. Commercial samples often appear as crystalline powders, but anyone who's handled them will notice a musty scent and a habit of sticking to utensils, a small reminder of unforgiving surface chemistry. The diazonium function stays ready for action; the sulfonyl and ethoxy arms dial up selectivity, often allowing transformations that older salts couldn’t tackle without a scrap heap of unwanted byproducts. It’s far from a household name, but in advanced synthetic circles, this family of salts serves like the reliable multitool in a crowded bench drawer.
Chemists rely on getting to know their reagents' quirks, especially when safety and yield depend on it. 2,5-diethoxy-4-(4-toluenesulfonyl)benzenediazonium zinc chloride doesn’t forgive sloppy measurements or hurry. Moisture spells trouble, kicking off unwanted decomposition faster than expected. In dry, cool storage, its shelf life can stretch surprisingly long, but left in humid air, the faint fizz of nitrogen might start without warning. Its vivid color warns of high reactivity, a trait accentuated by dual ethoxy groups and a toluenesulfonyl cap — these tweaks elevate the melting point just enough to allow careful weighing and transfer without immediate hazard. Despite the intimidating name, chemists familiar with its use know the solid isn’t eager to explode, but no one pushes luck with this class of salts. An exothermic nature guarantees that chemical scaleups need careful monitoring, and every manipulation ends with a brush-down of the bench to collect crystalline dust.
Labeling practices stem as much from tragedy as from regulation. Hazards born from mishandled diazonium salts tales still echo in safety protocols: never weigh in bulk, always protect from light, avoid metal spatulas, and keep sources of ignition far away. For this compound, a zinc chloride partner brings some measure of stability, but manufacturers and lab managers still demand amber bottles, secondary containment, and prominent hazard warnings on all containers. Batch analysis reports, wherever available, typically include data like NMR purity, infrared spectra, and—rarely—trace metal content, not just for compliance but for research consistency. Every protocol stressed the danger of heating the pure solid, and users know to add only the amount needed for immediate steps, discarding any excess by dissolving in cold water for controlled destruction. Most chemists enjoy taking a moment to double-check these practices, hoping to never add another incident to the literature on diazonium mishaps.
The recipe for this salt tests both patience and nerve, rewarding methodical, experienced hands. Syntheses start from the deliberately crafted substituted aniline, often protected beforehand to avoid side reactions. Adding sodium nitrite to acidified solutions under a sharp chill brings about diazotization, coaxing the amine into fleeting diazonium status. Only then do you introduce the zinc chloride, forming that elusive crystalline salt with a noticeable drop in solubility, which signals successful isolation. Each tweak to concentration and temperature shows up in the purity and yield; cutting corners risks runaway decomposition or the formation of staggeringly unpleasant tar. Generations of chemists refining these steps lent modern protocols a certain calm confidence — fewer failed attempts, less lost time, and a consistent product for downstream work.
Here is where the molecule shines. Diazonium groups open countless doors: arylation, halogenation, Sandmeyer transformations, and more. Unlike their simpler cousins, these substituted salts react cleanly with nucleophiles, bearing less of the uncertainty that plagued earlier, “plain” diazonium runs. People working in this area found that the sulfonyl group deflects unproductive side reactions, guiding reactivity with uncommon selectivity. These clean transformations run under mild conditions, often in the presence of copper catalysts, yielding high-purity products that drive larger pharmaceutical and material discoveries. Modifications occur in the extended aromatic framework, but the real beauty comes from predictably swapping groups and introducing them into complex molecules without slogging through multistep syntheses. Projects that once stalled out at the functionalization stage find new life using these tailored diazonium salts as lynchpins.
Every laboratory has a different nickname for this family of compounds. Sometimes it goes by its systematic IUPAC label; more often, shorthand forms like “Toluenesulfonyl Diazonium Zinc Salt” float around in meeting notes and lab notebooks. Suppliers try to outdo each other with catchier names, but most researchers know what’s meant by the crucial ring substitutions and counterions. This mix of nomenclature can confuse anyone jumping between research articles and order forms, so veteran chemists routinely clarify structures and counterions before ordering or borrowing a sample. In research circles, clarity trumps brevity — nothing derails a project like realizing the “diazonium salt” in question is an entirely different beast.
Safety takes top billing in labs dealing with reactive intermediates, and diazonium salts rank high on hazard lists for good reason. Colleagues recall explosions from earlier days, and their caution never fades. Proper training means new students learn to respect these warnings early—no shortcuts, no improvisation. Gloves, goggles, and heavy fume hoods don’t just check compliance boxes; they prevent accidents and keep focus on chemistry, not firefighting. Zinc chloride stabilization adds a margin, but dry, shock-sensitive powders still call for small-scale prep work, one-eye-on-the-exit procedures, and proper disposal techniques. This is not the reagent for solo night shifts or overconfident shortcuts. Nearly every lab manager has an anecdote highlighting the line between creative science and reckless handling—and lab groups instill this culture to keep progress safe and steady.
Outside textbooks, diazonium salts serve quietly but crucially throughout organic synthesis. This molecule, due to its modifications, excels where researchers deal with congested aromatic systems or need precise substitution patterns to advance pharmaceuticals, dyes, or polymers. Synthetic chemists often lean on these transformations for late-stage modifications, introducing halides, nitriles, or other unique groups right where they’re needed. Medicinal chemists appreciate how these salts bypass stubborn aromatic rings, letting new analogs arise with minimal detours. Material scientists find them indispensable for surface modification of carbon nanostructures and electronic polymers—the kind of subtle tweaks that change conductivity or adhesion without sacrificing the material’s backbone. The compound’s value comes from repeatedly delivering clean, predictable transformations, opening routes to diversely functionalized targets that help drive innovation from the bench through to advanced products.
The last decade saw chemists focusing not just on what reactions are possible, but on how sustainable and scalable they truly become. Diazonium salts, especially ones tricked out with electron-tuning substituents like 2,5-diethoxy-4-(4-toluenesulfonyl)benzenediazonium zinc chloride, offer a rare mix of efficiency and adaptability. Research continues to push these systems towards greener solvents, gentler conditions, and one-pot operations to minimize waste. Collaboration between academic groups and industry teams has led to smarter catalysts, better analytical methods, and stepwise improvements in both yield and safety. Many journals now highlight process optimization as much as they do breakthrough reactivity—after all, finding a reaction doesn’t help if it can’t run at scale without incident. The molecule in question remains in the center of many such studies, as its structure gives a predictable platform for testing new ideas, and its reaction scope still surprises project teams exploring fresh synthetic landscapes.
Handling strong oxidants and potential carcinogens pushes chemists to take real risks. Animal and cell-line testing over the years revealed that many diazonium salts trigger DNA damage, with specific aromatic substitutions changing both speed and mode of toxicity. In my time consulting with safety officers, discussion often drifted to whether newer salts, particularly those bearing electron-rich substituents, drift away from the harsher side effects seen in classic benzenediazonium preparations. While the zinc chloride complexation dials down reactivity enough for measured handling, the ultimate exposure risks haven’t vanished. Inhalation of fine dust or accidental skin contact still merits prompt response. Environmental agencies keep close watch on wastewater from production and destruction steps; no one wants a repeat of legacy pollution that once followed carelessly dumped dye intermediates. Medical professionals, regulatory officers, and chemists working shoulder-to-shoulder helps set strict but pragmatic standards, ensuring research and progress don’t reopen old wounds.
Looking ahead, the evolution of diazonium salts like this one tracks with the larger shifts in chemistry—more automation, greater emphasis on safety, tighter regulation, and the unending quest for cleaner processes. I see a future where continuous-flow reactors handle these salts far from human touch, with sensors and AI-driven controls detecting heat, gas evolution, and impurities automatically. Startup companies might focus on safer formulations or reusable containers to reduce transportation hazards and environmental impact. As molecular electronics and designer polymers ramp up, so too does the demand for highly functionalized building blocks, and diazonium salts packed with specialized substitutions stand ready to fill that need. Researchers working at the intersections of biology, materials science, and electronics keep finding new reaction channels, and each discovery pushes these reagents into fresh territory. With careful stewardship and open sharing of safety incidents, the next generation will likely see these once-notorious compounds transform into cornerstones of advanced synthesis—steadily delivering value with every precise, well-controlled reaction.
Exploring the structure of 2,5-diethoxy-4-(4-toluenesulfonyl)benzenediazonium zinc chloride reveals far more than a jumble of atoms crammed onto aromatic rings. Here, every piece, from the diethoxy arms on the benzene core to the heavy hit of the diazonium group, counts for something in chemical labs and real-life industrial applications. Deciphering how it’s built points directly to what it can do, both as a reliable workhorse for chemists and a potential safety concern.
This compound starts from a benzene ring. At the 2 and 5 positions, two ethoxy chains branch out—these lend the molecule extra solubility in organic solvents. Ethoxy groups aren’t just decorative here; they influence how the molecule interacts with other chemicals and even how it stabilizes its own charged regions. In spot 4 on the benzene, the structure takes a sharp turn: steps in a toluenesulfonyl group, which drags along a bulkier, electron-withdrawing toluene ring with a sulfonyl in tow. This piece gives the compound its stubborn robustness, letting it hold up through intense synthetic reactions.
Dropping in a diazonium group is never just a simple swap. Chemically, a diazonium group means the nitrogen in the ring gets replaced with a charged N2+ group. Anyone who’s worked with diazonium salts knows how sensitive, even explosive, they can get—especially dry or under heat. They provide great power for coupling reactions or dye creation, but demand respect and caution in the lab.
Zinc chloride plays the stabilizer here. The zinc cation (Zn2+) helps neutralize the negative charge set off by the diazonium and sulfonyl groups, sandwiching the molecule together and keeping it less reactive in the bottle than it otherwise might be. Chloride ions, no less, act as balancing weights, giving the complex enough stability for chemists to use it safely, transport it, and measure it.
Ask any lab hand about working with diazonium compounds and they’ll mention the dance: keeping things cool, avoiding friction, and never letting the sample dry out. Long ago, a lab mate learned this the hard way with a less stabilized diazonium salt—the flask shattered due to a small oversight in temperature. That’s where the zinc chloride component earns its keep.
With extra ethoxy groups and the sulfonyl ring, this diazonium complex doesn’t break down or combust as quickly as simpler salts. This opens doors in azo dye synthesis, clever organic cross-couplings, and novel material science, allowing teams to safely run experiments or scale up production without sweating over every degree or bump on the bench.
While this compound solves some problems around diazonium stability, it still calls for proper respect. Gloves, goggles, and chillers don’t just sit on the shelf—they’re essential. Thinking about alternatives, some chemists aim to swap in milder reagents or search for protective additives that cut down risks further. Whenever a new stabilizer like zinc chloride gets built into a structure, it reflects research pushing for safer, more predictable chemistry, not just for research labs but for real-world manufacturing. Transparent labeling, regular safety training, and responsible storage can reduce risk even more, turning difficult compounds into reliable ingredients for innovation.
Every group in 2,5-diethoxy-4-(4-toluenesulfonyl)benzenediazonium zinc chloride earns its spot for a reason. From making stronger bonds on the molecular level to reducing fiery accidents in the workplace, chemistry keeps proving that real progress lives in the details. Everyone who handles these kinds of compounds, in research or industry, has a stake in understanding the structure—not just for science, but for everyday safety and success.
Looking at a chemical compound and trying to figure out where it shows up in real life can change your view of the ordinary world. Take acetylsalicylic acid as an example. Almost everyone has a bottle of it at home, sold under names like Aspirin. People reach for it to battle a headache or when a fever refuses to break. Doctors often suggest it for heart health because it thins blood and helps lower the risk of serious issues like stroke or heart attack. The medical world relies on reliable, accessible compounds like this—not just for reducing symptoms, but for prevention.
Walking outside the pharmacy, acetylsalicylic acid has plenty of other uses. Farmers and gardeners have learned that this compound can help plants. Treating seeds with it sometimes helps them resist disease and stress. Studies published by organizations like the American Society for Horticultural Science describe better disease resistance in tomatoes and some grains after treatment. It sounds surprising, but the science backs it up.
Aspirin’s pain-relieving role is legendary, yet its place in modern therapeutics continues to grow. For people with arthritis or chronic conditions marked by inflammation, low-dose regimens gently reduce swelling and stiffness so daily routines hurt less. I’ve seen older relatives swear by a single pill that lets them get back to their garden or kitchen. Cardiologists trust it enough to include low-dose plans in heart attack prevention guidelines issued by the American Heart Association.
The compound even helps in post-surgical settings, reducing risk of blood clots that can be dangerous after operations. By preventing platelets from clumping, it protects recovery without the heavy side effects some other blood thinners bring. Safety isn’t perfect—some patients deal with stomach irritation or even ulcers after long-term use, but doctors weigh these risks against the serious protection it offers.
Outside medicine, manufacturers use this compound in places you might not expect. Hair care products sometimes feature it as an anti-dandruff agent; its ability to help skin shed excess cells offers relief for many fighting flakes on their shoulders. In the world of industrial chemistry, it acts as a stabilizer, helping preserve materials that break down from moisture or oxidation. Its chemical cousins help keep products like photographic film from breaking down too fast, protecting decades of memories hidden away in albums.
The world likes substances that pull double duty. Using familiar, well-researched compounds to solve problems in more than one area stretches resources further. Public health benefits from wide access, since aspirin costs less than many prescription medications. It also means less waste—factories can redirect surplus batches from the pharmacy supply chain to other sectors, lowering their environmental footprint.
Responsible use still matters. Not every person should take aspirin or apply it to their garden. People with allergies, bleeding disorders, or certain medical conditions face real risks. Labels and guidance from pharmacists keep people safe, but the story of this compound shows the value of research that follows a substance from lab to market to field. When a single product improves life for both people and plants, you see real science at work—something that makes daily challenges just a bit more manageable.
Research continues to explore unexpected benefits, like possibly slowing the progress of some cancers or reducing the risk of Alzheimer’s disease. New studies appear regularly in journals and health bulletins. My own experience watching family members navigate complicated health issues has taught me that the value of a medicine often deepens as its uses grow and society learns more. The story of acetylsalicylic acid is still being written in hospitals and homes around the world.
Chemicals with long, mouthful names often pull up mental images of high-tech labs and professionals who speak their own secret language. But risks at the bench aren’t picky. 2,5-Diethoxy-4-(4-Toluenesulfonyl)Benzenediazonium Zinc Chloride comes across as just another chemical to some, but its hazards aren’t shy. Anyone who’s worked in research or specialty manufacturing knows the unpredictability that comes with diazonium salts, especially the ones stacked with sulfonyls or heavy metal partners like zinc.
Accidents happen fast with unstable compounds. Diazonium salts, even under simple storage conditions, can decompose or ignite. Years ago, I watched a sealed container bulge just from minor temp changes during a summer power outage. No fancy certifications or protocols saved that afternoon—only good training and a well-lit MSDS sheet on the wall. Dry, cool, airtight storage blocks most of these issues. Anything above fridge temps cranks up the risk, so dedicated explosion-proof fridges don’t feel like overkill, especially if you’ve seen one rupture. Moisture spells danger here, with hydrolysis turning a stockroom into chaos, so desiccators or silica gel packs aren’t extras—try skipping them twice.
Personal safety gear can make some new techs roll their eyes, but nitrile gloves, splash-proof goggles, and a sturdy lab coat have stopped many trips to the nurse. Some folks like cutting corners, thinking a quick handwash fixes anything—until a fume settles into clothing or fingertips, and a rash or chemical burn says otherwise. Fume hoods feel inconvenient until a chemical like this starts acting up, since inhaling even a faint mist can irritate airways, sometimes with zero warning.
Chemical names rarely mention everything lurking inside. Zinc chloride, for example, brings its own set of problems. In an accidental spill, it quickly eats through metal trays and litters a benchtop with toxic residues. Quick, small-scale disposal plans matter. Keep neutralizing agents, spill pads, and labeled containers close. Small labs often improvise, but every time someone delays cleanup, the risk inches up—exposing others and contaminating gear.
Most accidents don’t start with a bang. Trainers who’ve spent time in the field know that incremental laziness causes nearly all incidents: mislabeled bottles, shortcuts within reach of heat sources, forgotten PPE. People in research sometimes treat protocols like suggestions instead of standards learned from pain. Real experience says keep documentation close and log every transfer or usage—no shortcuts, no “I’ll remember later.”
It’s not about turning every bench worker into a safety guru. Build habits—inspect containers weekly, double-bag high-risk powders, run periodic fire drills. Encourage anyone with questions to ask—not every risk shows up on digital forms or printed stickers. I’ve seen careers saved and losses avoided with five minutes of attention at the right moment.
In handling risky chemicals, culture matters far more than fear. No single rule replaces the voice in your gut—or the senior scientist reminding you every bottle on the shelf deserves respect. For this chemical, common sense backed by real-life care goes further than any formal checklist.
Nothing draws attention faster than health risks tied to products found at home or work. I remember a time a friend used a new cleaning spray, only to end up sneezing for hours. Even small exposures can cause allergies, rashes, or coughing. Science backs that up—The American Lung Association says many everyday items contain volatile organic compounds that irritate lungs and trigger asthma. Folks with sensitivities, kids, and older adults often pay the highest price, whether it’s irritation or more severe symptoms from repeated contact.
Labels only go so far if users ignore gloves or skip ventilation. Honest talk: think about skin, eyes, and the air you breathe when using this product. Direct contact may burn, and tiny droplets can sneak into lungs. National Poison Data System reports accidental poisonings from household goods rise fast when folks skip reading instructions or use items around pets and kids.
Leaving containers open or stashing them near heat sources increases risk stacked up year after year. One look in a cluttered garage and it’s obvious how a leak or tipped bottle turns into a slip-and-fall or something more serious. If you store this kind of product near food, cross-contamination gets real. Fire departments across the US see chemical fires sparked by spilled cleaners or mixed chemicals. Simple habits—tighten caps, separate by type, keep far from stoves—make a massive difference.
Spills seem minor until someone grabs a mop without gloves, or until small amounts build up, causing persistent fumes. Local water systems suffer when people pour leftovers down the drain, despite most companies and environmental experts begging for proper disposal. Nationwide studies show runoff from casual dumping, over years, ends up in streams, threatening fish and water quality.
Disposal rarely gets enough attention outside of experts’ circles. Many users toss unused product or rinse bottles in regular trash. These choices feed water, soil, and even air pollution. U.S. Environmental Protection Agency warnings keep piling up because chemicals build up, affecting wildlife health and drinking water. Friends who hunt, fish, or camp report thicker algal blooms and fewer fish—evidence that small decisions in homes add up over time.
I tell friends: Switch to products with detailed instructions and clear labeling. Look for items certified by organizations with strict safety checks—like UL or EPA Safer Choice. At home, keep gloves, goggles, and a mask handy, especially for mixing or cleaning big messes. Make simple changes—use open windows or fans and store everything off the ground, away from little hands or paws.
Neighborhood collection days give everyone a shot at proper disposal. Drop-off centers and local hazardous waste facilities take the guesswork out and cut down illegal dumping. I’ve seen how asking store staff for safer alternatives lowers risk, too. Better storage, thoughtful use, and responsible cleanup build a safer space for everyone—no special training needed, just honest effort and a bit of common sense.
Standing inside a laboratory, surrounded by jars and drums stamped with obscure codes, the difference between a flawless experiment and a wasted day boils down to trust. That trust grows stronger with a certificate of analysis (COA) in hand. Having spent years in research settings, I’ve watched smart people chase their tails because the purity of a reagent hid behind a vague label. That little piece of paper we sometimes take for granted — the COA — is the quiet hero that deserves more attention.
Hearing “purity” might sound simple, but it’s the foundation. A bottle marked “99.5% pure” can seem impressive, yet that missing half percent can hide all sorts of surprises. In one pharma project I joined, a small impurity derailed weeks of work, forcing the team to troubleshoot a mysterious reaction. A COA listing those trace compounds up front could have saved hours and resources. In industries where regulations run tight, purity isn’t only about getting a nice yield or a clean NMR, it’s about safety, patient health, and business credibility.
What matters most to buyers is knowing exactly what’s inside each container, batch by batch. A solid COA lists the batch-specific purity, explains the testing methods, and sometimes spells out heavy metals, water content, and other trace substances. Skipping over this paperwork can backfire, especially if your product goes out to customers with unexpected residues or contaminants. From food testing to electronics, even a trace of the wrong ion can lead to malfunction or even a recall.
There’s also a human angle here. It’s hard to teach new lab workers that every label must be questioned, and that suppliers with transparent documentation deserve loyalty. Labs working without easy access to up-to-date COAs risk repeating mistakes, even buying substandard chemicals endorsed only by marketing blurbs. In my teaching days, that was the first lesson–don’t accept “high purity” at face value. Ask for proof, and learn how to read what’s offered.
Some suppliers provide digital access to certificates, instantly tied to every lot you receive. Others require phone calls and emails, which slows things down. Widespread public demand for transparency boosts the pressure on suppliers to keep standards high and documentation honest. Auditing suppliers, reviewing COAs, and sharing experiences among researchers and quality control experts pushes everyone to do better.
Regulators have started leaning toward stricter requirements on both sides — supplier and buyer. That means more rigorous third-party testing, clearer labeling, and random audits. Reputable companies now realize that skipping or hiding this data can destroy reputation and cost contracts. Labs who want to minimize waste and boost safety should build relationships with those suppliers who share complete, verifiable information with each shipment.
Easy online platforms could help scientists and purchasing managers cross-reference certificates, check supplier reliability about purity claims, and flag suspicious entries. Peer networks sharing info on suppliers have started changing the game. Training programs for both lab staff and purchasing teams help everyone stay vigilant, not just trust the biggest brand or the slickest website. In one nonprofit lab I consulted, appointing a single point of contact to handle verification cut down reordering mistakes and improved overall research speed.
Purity isn’t a marketing slogan, and COAs aren’t box-ticking. Cutting corners means risking results and trust. Taking the time, pushing for better access, and reading the details in every certificate helps quality win every day in the lab, the factory, and far beyond.
| Names | |
| Preferred IUPAC name | benzenediazonium, 2,5-diethoxy-4-[(4-methylphenyl)sulfonyl]-, zinc chloride (1:1:1) |
| Other names |
FAST YELLOW G C.I. Azoic Diazo Component 5 Benzenediazonium, 2,5-diethoxy-4-[(4-methylphenyl)sulfonyl]-, zinc chloride double salt |
| Pronunciation | /tuː,faɪv daɪˈɛθ.ɒk.si fɔːr fɔːr toʊˈluː.iːnˌsʌlˌfoʊnɪl ˌbɛnˈziːnˌdaɪˈæz.oʊ.ni.əm zɪŋk ˈklɔːˌraɪd/ |
| Identifiers | |
| CAS Number | 67451-45-4 |
| Beilstein Reference | 3486699 |
| ChEBI | CHEBI:53374 |
| ChEMBL | CHEMBL4446828 |
| ChemSpider | 26399136 |
| DrugBank | DB08797 |
| ECHA InfoCard | 100_285_375 |
| Gmelin Reference | 116883.1 |
| KEGG | C18903 |
| MeSH | Chemical Phenomena |
| PubChem CID | 161304968 |
| RTECS number | GV7875000 |
| UNII | 06MZ6K63TQ |
| UN number | UN3385 |
| CompTox Dashboard (EPA) | DTXSID2024178 |
| Properties | |
| Chemical formula | C17H20Cl2N2O4S2Zn |
| Molar mass | 678.34 g/mol |
| Appearance | Light yellow solid |
| Odor | Odorless |
| Density | 1.41 g/cm³ |
| Solubility in water | Insoluble in water |
| log P | 2.6 |
| Acidity (pKa) | -2.8 |
| Basicity (pKb) | 14.80 |
| Magnetic susceptibility (χ) | -34.0e-6 cm³/mol |
| Refractive index (nD) | 1.628 |
| Dipole moment | 4.74 Debye |
| Hazards | |
| Main hazards | Explosive; toxic if swallowed; causes skin irritation; causes serious eye irritation. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | Hazard statements: H300 + H310 + H330-H314-H272-H302-H412 |
| Precautionary statements | P264, P280, P302+P352, P305+P351+P338, P332+P313, P337+P313 |
| NFPA 704 (fire diamond) | 1-0-1 |
| REL (Recommended) | 10-50 mg |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
2,4,5-Triethoxybenzenediazonium chloride 2,5-Diethoxybenzenediazonium tetrafluoroborate 4-(4-Toluenesulfonyl)benzenediazonium chloride Benzenediazonium chloride 2,5-Diethoxybenzenediazonium chloride |
