Sodium (4-nitrophenyl)methanesulfonate turned heads in the mid-20th century, long after the rise of benzenesulfonate derivatives that drove cleaner dye synthesis and titration reagents. Chemists in academic and industrial labs experimented with different substitution patterns on aromatic rings. Their goal was to tune both reactivity and solubility. Early data trickling out of German and Japanese chemical repositories pointed to this specific compound as a tool for selective modifications in both organic solvents and water. Over time, folks began recognizing that nitro-substituted arylsulfonates bridged important synthetic gaps. They offered strong electron withdrawal to tune reactivity and a reliable way to introduce water-solubility into aromatic platforms, with sodium (4-nitrophenyl)methanesulfonate sitting right at the crossroads of electrophilicity and salt stability.
At a glance, this yellow-to-orange crystalline powder does not promise much. Yet under laboratory lights, it embodies precision for researchers tinkering with aromatic substitution or seeking precise sulfonate labeling. Sodium (4-nitrophenyl)methanesulfonate dissolves well in water, releases its ions without fuss, and plays well in alcoholic solvents. It allows chemists to introduce both a nitrophenyl and a sulfonate tag in one go—a trick that saves time in multi-step synthesis, especially in the world of medicinal chemistry or analytical standards. No boutique laboratory catalog feels complete without it, and even large volume facilities rely on its dependable profile for pilot studies.
Chemically, sodium (4-nitrophenyl)methanesulfonate carries the formula C7H6NO5SNa. Structurally, its benzene ring hosts a nitro group on the para position and a methanesulfonate moiety, both boosting its polarity. Most samples appear as orange-yellow powders, reflecting the strong absorption bands of the nitro aromatic system. It handles routine lab temperatures without degradation and maintains dry stability on the shelf for extended periods. Solubility stands out: water readiness comes thanks to the sodium sulfonate, and common polar solvents do not break its backbone. With a molecular weight hovering around 243 grams per mole, it balances manageability and substance—heavy enough for gravity-fed operations, light enough for volumetric preparations.
For those in procurement or laboratory quality control, specifications carry enormous weight. Analytical-grade material typically guarantees purity above 98% by HPLC, with residual solvents and byproducts listed under 0.5%. Reputable suppliers publish spectra for proton NMR, mass spectrometry, and IR, allowing end users to vet both identity and purity down to the last ppm. Labels never just offer a name; they list batch number, production or retest date, storage advice, and hazard precautions as required by GHS standards. Any deviation triggers concern in regulated sectors—pharmaceutical labs, for example, often demand full traceability down to synthetic intermediates.
Producers usually start with 4-nitrotoluene, an abundant chemical in dye and pharmaceutical production. A radical bromination exchanges its methyl group for bromomethyl, followed by nucleophilic substitution with sodium methanesulfinate. Alternatively, direct sulfonation using chloromethanesulfonic acid under basic conditions gives a robust yield. These methods avoid harsh oxidizers or metal catalysts, which means less risk in waste management and lower production costs. Scale-up is straightforward: batch reactors need only basic agitation and temperature control—no exotic glassware or inert atmospheres. This makes the compound accessible and affordable, even for facilities in parts of the world where infrastructure is limited.
Once in hand, sodium (4-nitrophenyl)methanesulfonate performs in several key organic transformations. The nitro group permits standard reduction to amines using palladium or iron catalysis. Sulfonate exchange can introduce heavier metals or other organic moieties via phase transfer catalysis. Electrophilic aromatic substitution leans on the electron-withdrawing nitro, promoting clean para-selectivity and reducing risk of polysubstitution. Its dual functionality lets medicinal chemists install both reactive scaffold and ionic handle in tandem, smoothing out purification steps and making downstream analytics easier. Those in polymer science modify the sulfonate for grafting reactions, adding chromophoric stability or tweaking solubility of big molecules.
In the literature, sodium (4-nitrophenyl)methanesulfonate turns up under several guises: p-nitrophenyl methanesulfonate sodium salt, sodium p-nitrobenzyl methanesulfonate, or the succinct “4-NPMS sodium.” Some catalogs abbreviate this even further, causing headaches for chemists double-checking structures before scale-up. The registry number—often referenced in publications—links directly to major database entries in chemical supply chains, smoothing out procurement for multinational teams. Wherever it appears, the structural motifs rarely change, keeping identity mix-ups to a minimum.
Lab veterans pay close attention to the fine print on sodium (4-nitrophenyl)methanesulfonate’s safety data sheet. The compound irritates skin, eyes, and mucous membranes, so gloves and goggles earn their keep. Dust can carry enough compound into the air to trigger sneezing or mild respiratory discomfort in crowded fume hoods—smart facilities keep good ventilation and train staff on spill response. Waste streams need proper neutralization and segregation. Most facilities reject casual disposal into sinks, knowing that unchecked release of nitroaromatics raises red flags during environmental audits. For rare scale mishaps, eyewash stations and showers should be close by. Emergency drills make sense even for compounds that rarely cross the kilogram mark in any one batch.
In research and manufacturing, sodium (4-nitrophenyl)methanesulfonate stands out for its flexibility. Pharmaceutical teams use it as a starting block in the design of bioactive compounds, building in both charge and aromaticity for leads targeting enzymes or receptors. Analytical chemists use its charged, UV-active properties as a marker in titration, capillary electrophoresis, and ion chromatography. Dye manufacturers working on high-stability pigments turn to the nitro/methanesulfonate combination to toughen colorfastness under ultraviolet exposure. Even polymer chemists test this compound on surfaces to tweak hydrophilicity or introduce functional nodes for future attachment. In academia, students learn sulfonate chemistry from it, cutting their teeth on real-world problems that require both mastery and a bit of creativity to solve.
Curiosity still drives research into new uses for sodium (4-nitrophenyl)methanesulfonate. Medicinal teams investigate it as an intermediate for nitrophenyl-linked drugs, or as a prodrug carrier for improved solubility. Analytical chemists develop new titrimetric protocols and sensors that benefit from its sharp chemical signals. Materials scientists fold the compound into hydrogels and scaffolds that serve in tissue engineering and environmental cleanup. Green chemistry initiatives look at optimizing synthesis with fewer byproducts, lower emissions, and safer reagents. Consortia of universities and industry partners share performance data on tailor-made derivatives, betting that new functional groups anchored off the aromatic sulfonate will unlock advances in catalysis or energy storage. Patents continue to trickle in, reflecting both the maturity and adaptability of this seemingly simple molecule.
Toxicologists in both private and public sectors continue monitoring the biological impact of sodium (4-nitrophenyl)methanesulfonate. Like many nitroaromatic and sulfonated compounds, concerns focus on potential cytotoxicity, environmental persistence, and effects on aquatic life. Most acute exposure cases involve irritation without major organ toxicity, but researchers monitor chronic exposure for subtle effects on liver and kidney function. Water treatment studies report that the compound resists rapid breakdown, especially in cold environments—something that nudges regulators to push for best practices in disposal. Risk assessments at universities and chemical companies rely on both in vitro and in vivo data to update safe handling guidelines. Ongoing studies in zebrafish, invertebrates, and select mammalian models aim to fill data gaps for long-term ecological health, especially where wastewater management falls short.
Chemists searching for robust and adaptable building blocks should keep an eye on sodium (4-nitrophenyl)methanesulfonate. As pharma and materials fields demand more modular, water-compatible reagents, the value of dual-functional compounds rises. Emerging applications—ranging from customized sensors to next-generation membrane technologies—push demand for derivatives with tuned electronics and tailored solubility. Environmental chemists work to design more biodegradable analogs that still deliver sulfonate flexibility. Automation in synthesis opens doors to faster screening and optimization of reactions that once relied on tedious benchwork. Research into safe and sustainable manufacture keeps costs down and makes compliance easier in regions with strict green chemistry mandates. In a world chasing efficiency and smarter chemistry, compounds like sodium (4-nitrophenyl)methanesulfonate will keep playing their part—quietly, but with undeniable impact.
Sodium (4-Nitrophenyl)Methanesulfonate doesn’t roll off the tongue. Most people never cross paths with it. But for lab scientists, it’s like that socket wrench you grab once in a while, the one that really gets the job done. What catches my attention about this compound is not just its badge as a reagent, but the way it fits into the long process of building new molecules. Every time I see it on a shelf, I think of the effort that goes into making complex molecules behave and react.
You usually find this compound in research chemistry, mostly in the field of organic synthesis. I remember working with a team trying to add just the right functional group onto a molecule. It's finicky, this work—too rough and you break your ends, too gentle and nothing happens at all. Sodium (4-Nitrophenyl)Methanesulfonate steps up as an activating agent. Chemists use it to tweak molecules so new parts stick where they’re supposed to. For example, this compound helps introduce sulfonate groups or set the stage for what chemists call coupling reactions—a backbone technique in making everything from pharmaceuticals to dyes.
Building new drugs often starts in a dish, with careful, calculated steps. The reliability of sodium (4-Nitrophenyl)Methanesulfonate makes it handy for these moments. A few years back, we had a project on cancer drug candidates. We leaned on this very compound to help insert chemical groups that would later attach to targeting agents. Published studies back up this use, too. Researchers use it to craft linkers and helpers that turn good medicine into great medicine by improving how drugs move through the body or bind to their targets. Without this kind of chemical tool, labs run into dead ends far more often.
It’s easy to get lost in the excitement of laboratory progress, but real stories from labs always include a discussion about safety. This compound isn’t something you splash around without training. Gloves, goggles, and good ventilation matter. Data from the PubChem database highlights potential irritant properties, reminding chemists to treat it with respect. Waste management also comes up. Over years of working in research environments, proper disposal and tracking of leftover sulfonates continue to matter both to staff and regulators. Better waste policies and safer substitutes serve labs and the planet better. Initiatives that limit run-off and promote responsible chemical use can’t come fast enough.
There’s real value in searching for greener ways to do the same jobs in the lab. My experience with engineering students showed me that curiosity drives change—some are already looking for new compounds that do what sodium (4-Nitrophenyl)Methanesulfonate does, but with a lighter footprint. Peer-reviewed journals have started to follow this conversation, and grant money is trickling toward safer, sustainable chemistry. Chemistry, like every field, moves forward in small steps, and compounds like this one set the pace. Bet on the next generation of scientists building on what’s useful about sodium (4-Nitrophenyl)Methanesulfonate while making it safer to use and easier to handle.
Chemistry runs on details, and nowhere is this more obvious than when it’s time to make or use a compound like Sodium (4-Nitrophenyl)Methanesulfonate. This molecule packs a punch—useful in research, synthesis, and sometimes as a reagent when probing biochemical pathways. Getting the molecular weight right shapes everything from preparing solutions in the lab to making sure experimental ratios hit the target.
For Sodium (4-Nitrophenyl)Methanesulfonate, the formula lines up as C7H6NO5SNa. Taking a step through the periodic table:
Add those together: 84.07 + 6.06 + 14.01 + 80.00 + 32.07 + 22.99 gives a result of 239.20 g/mol. That’s your working number. Educators like to drive this point home because a miscalculation will not just wreck a reaction—it could easily waste precious reagents and time.
People treat molecular weight as just a number to punch into a calculator. I’ve run into the wall this mindset builds. Years in the lab showed me that molecular weight builds trust—between chemists, between suppliers and buyers, and even between an experiment and its expected result. If a warehouse delivers a bottle labeled wrong by just a couple of grams per mole, the fallout ripples through experiments, publications, and clinical trials.
Fundamental data like this have to be transparent and based on reputable sources. Chemists turn to the CRC Handbook, peer-reviewed articles, and reliable suppliers like Sigma-Aldrich to confirm the numbers. Professional integrity rides on those habits. Google’s E-E-A-T principles push for information based on real experience, expertise, and transparency. My own work mirrored that—refuse to cut corners, question each source, and record every calculation so others can cross-check.
Some say a gram here or there never hurts. In real applications, incorrect weights drive up costs, spoil product batches, and sometimes trigger regulatory headaches. Many industries operate under audit or good manufacturing practice rules, where incorrect weights spell non-compliance and lost contracts. Lab techs and plant managers depend on accuracy so that what you develop at the bench can scale without surprises.
So what helps avoid these pitfalls? Start with accessible courses on basic chemistry for young scientists—make the math stick. Use checklists and require peer review before using or reporting a new chemical in the workplace. Digital calculators help, but a hand calculation now and then keeps skills sharp. Engage suppliers in conversations about batch testing and certificates of analysis to strengthen trust from both directions.
Knowing the molecular weight of Sodium (4-Nitrophenyl)Methanesulfonate—239.20 g/mol—reaches past trivia. It’s a detail wedged into the foundation of chemical science, supporting safe labs, successful research, and a reliable industry. Those numbers become a language we trust, one calculation at a time.
Sodium (4-nitrophenyl)methanesulfonate stands out as a special compound in labs because of its clear-cut behavior in water. Many researchers, especially those tackling organic synthesis or enzyme activity studies, often ask about its solubility. It turns out, this molecule mixes well in water at room temperature, thanks to its sodium sulfonate group. Chemists often see concentrations up to 100 g/L dissolve without much trouble — that’s plenty for most reactions, assay prep, or analytical work. The story shifts a bit as temperatures change, or depending on how pure the water is. Cold water slows down how quickly it dissolves, and hard water introduces variables. No big surprise — salts dissolve better in more water, warmer temperatures, and clean glassware.
Plenty of us have tried to wrangle a stubborn powder into solution, watching grains swirl long after they should have vanished. Sodium (4-nitrophenyl)methanesulfonate doesn’t frustrate as much as some hydrophobic compounds. The 4-nitrophenyl part creates some polarity, but the sulfonate group dominates, making this molecule practically jump into water given a swirl or brief sonication. Solid, dependable solubility shortens time spent prepping and cuts down on waste. You get more accurate concentrations, fewer headaches, and cleaner results in dye chemistry and bioconjugation work.
Many research stories hang on simple things: Can you make a clear solution? In enzyme assays where this sodium salt tags or labels substrates, cloudy mixtures mess up the data. Medical researchers relying on colorimetric tests count on solutions being fully clear to trust the color shifts. Unpredictable lumps or incomplete dissolution mean wasted chemicals and suspicion over results. Academic labs often stretch tight budgets, so throwing out batches due to poor prep stings even worse. The real benefit here isn’t just saving a few minutes — it protects integrity, saves resources, and helps ensure measurements reflect what’s actually in the flask.
Every so often, a supposedly water-soluble batch refuses to dissolve. That throws a wrench in the plan. This can happen when storage lets the powder clump up from humidity, or when lots of sample ends up in little water without stirring. In those moments, practical fixes matter: Use more water. Break up clumps. Warm gently if needed — but don’t boil, as decomposition might creep in. Slight pH tweaks help for some solutions; for this salt, plain pH 7 water usually does the trick. Glassware fresh from the dishwasher beats beakers crusted with old salts. It’s the same process that helps with most sodium-based organics, but worth repeating since these basics get overlooked in the rush of routine lab work.
Over time, reliable solubility builds trust in protocols. Journal articles, suppliers’ datasheets, and chemical safety documents agree: sodium (4-nitrophenyl)methanesulfonate won’t suddenly drop out of solution if prepared right. Researchers, undergraduates learning new lab skills, and safety teams all depend on this. With good solubility, less sample is needed for stocks. Clean preparation translates to clean science.
To push research further, more labs share their real-world notes on everything from solubility to shelf-life. Open data, standardized reporting, and direct supplier communication can help everyone avoid silent errors that slow discovery. With sodium (4-nitrophenyl)methanesulfonate, real improvement comes through these small, stepwise efforts. The clearer the solution, the clearer the science — and the more confident anyone can be in the answers that follow.
I’ve spent enough time around chemical labs and storage rooms to know how even small lapses in chemical storage can lead to expensive accidents. Sodium (4-Nitrophenyl)Methanesulfonate is the sort of compound that rewards careful habits. It looks plain enough—pale yellow powder, not volatile at a glance. But let a little ambient moisture creep in, or leave the jar near a heat source, and you’ll invite problems you didn’t see coming.
From my own experience, humidity finds the tiniest cracks. Salts like sodium (4-nitrophenyl)methanesulfonate draw in water from the air. Once you start getting clumps or caking, you’re looking at compromised quality and some unpredictable chemistry in your next batch or experiment. Dry chemicals belong in seal-tight containers—ideally with a desiccant packet for backup. Forget the old jam jars with screw tops. Use proper glass containers with good seals. Listen for that faint click or vacuum sound as you close it; it means you locked out the air.
Temperature swings tire out many chemicals. Sodium (4-nitrophenyl)methanesulfonate prefers a cool, stable environment. In my years working in labs without climate control, I’ve seen how summer heat can accelerate decomposition in some sulfonate salts, while cold snaps risk condensation inside containers. Ideally, store it at room temperature—but keep it away from direct sun, heating vents, or exposed lab equipment. Mid-20s Celsius keeps it happy and reliable.
This compound doesn’t crave the spotlight. Prolonged light exposure sometimes leads to discoloration or slow breakdown in aromatic nitro compounds. Keeping bottles in opaque cabinets, or at the very least, out of the sun keeps things stable. In our storage space, we mark flammable or reactive stuff with red stickers, and we keep all nitro or sulfonate chemicals away from acids and reducing agents. Spills can escalate when incompatible substances get too close. I once watched a spill migrate across a poorly organized shelf and react with something it should never have touched.
Labels can save lives. Accurate names, concentration, hazard notes, and the date everything went on the shelf—these aren’t just for busybodies or the next shift. Even though I keep my own handwritten log, labels on containers let anyone walking in know what’s at stake. In shared spaces, this often gets skipped, but the day a mystery jar goes missing is the day you appreciate a good paper trail.
Proper storage of sodium (4-nitrophenyl)methanesulfonate is a daily practice, not a one-off job. Dry, dark, cool, and clearly marked—that’s the short list. I check our shelves monthly, hunting for signs of bad sealing or creeping dampness. I know to avoid storing this alongside strong acids or reducers, and I keep a record of batch shelf-life according to the supplier’s sheet. Risks drop, and waste slows down, when storage follows good habits. The best advice doesn’t change: keep it sealed, dry, cool, and in the dark, and it’ll stay trustworthy for the next experiment.
Working in a lab introduces you to hundreds of different compounds. Some are as mild as dish soap, others can send you to the eyewash in a hurry. Sodium (4-Nitrophenyl)Methanesulfonate lands somewhere in between: not exactly benign, not quite a villain either. Some curiosity about its hazards keeps us on our toes, and for good reason.
The chemical structure packs a nitrophenyl group, which often raises eyebrows. Nitroaromatic compounds have a reputation for being less friendly to human cells, especially if inhaled or absorbed through the skin. While this specific compound hasn’t triggered major headlines for toxicity, reaching for gloves and goggles isn’t just habit—it’s good judgment. Spill a few grams, and the yellow powder might not puff up in clouds, but keeping your nose out of the way makes sense. Some users report mild irritation from repeated contact, which lines up with what safety data sheets mention. This chemical’s low volatility means fumes aren’t rushing to fill the room, but dust shouldn’t be ignored.
People ask about environmental impact next. The nitro group can persist, which makes treatment plants less likely to handle it with ease. Anyone who’s cleaned up after a spill knows the hassle of proper waste disposal. Waterways don’t need more synthetic organics, so handling with care safeguards more than the immediate workspace.
Standard practice in chemistry labs involves nitrile gloves and shatterproof goggles. Skipping these comes back to bite, even if you’ve worked with tougher stuff before. Fresh out of college, plenty of us learned the hard way how a simple splash can ruin your day. The habit sticks because compounds like this don’t show mercy just because nothing dramatic happened last week. A bit of compound on your fingers, an absent-minded rub of the eye, and irritation follows. Over the years, habits make safety second nature, not a tiresome checklist.
Inhalation sounds like an overblown worry, but dust exposure builds up. Short stints with the powder on open benches rarely lead to problems, but frequent use—without ventilation—could irritate airways. Fume hoods give breathing room, literally. It’s not about fear; it’s about respect for things we can’t always see or feel right away. Sharper minds than mine set up these protocols after sifting through decades of incident reports.
Labeling bottles clearly, logging their movements, and reviewing SDS details become team habits. It’s not bureaucracy—think of it as keeping score on risks. One slip from lack of communication, and the next user could walk right into trouble. In reviews of lab accidents, most come down to someone underestimating risk, not the unpredictability of the substance itself. Experience teaches that chemical safety thrives on information sharing, not denial or guesswork.
Routine maintains safety better than anxiety. Routine means storing this material tightly sealed, using fume hoods, keeping a spill kit close, and reinforcing the basics before every new batch of students enters the lab. Management supports this by maintaining clear inventory and restocking PPE before it runs out. Waste gets packaged based on regulatory code, not wishful thinking. If a junior member asks about extra steps, encourage them. The one who asks the most questions keeps everyone safer.
| Names | |
| Preferred IUPAC name | sodium 1-[(4-nitrophenyl)sulfonyl]methanide |
| Other names |
Sodium (p-nitrophenyl)methanesulfonate Sodium 4-nitrobenzylsulfonate 4-Nitrobenzyl methanesulfonate sodium salt p-Nitrobenzylsulfonic acid sodium salt |
| Pronunciation | /ˈsəʊdiəm fɔːr ˌnaɪtrəʊˈfiːnɪl ˌmeθeɪnˈsʌlfəneɪt/ |
| Identifiers | |
| CAS Number | [36384-90-4] |
| 3D model (JSmol) | `[NH4+].[O-]S(=O)(=O)Cc1ccc([N+](=O)[O-])cc1` |
| Beilstein Reference | 1635952 |
| ChEBI | CHEBI:132731 |
| ChEMBL | CHEMBL3723496 |
| ChemSpider | 23443984 |
| DrugBank | DB07755 |
| ECHA InfoCard | 03d9a910-cfa2-484d-8ed2-9b2a6e2e2e25 |
| EC Number | NA |
| Gmelin Reference | 114212 |
| KEGG | C19221 |
| MeSH | D017368 |
| PubChem CID | 11434967 |
| RTECS number | PB6125000 |
| UNII | 5X99KX1H4S |
| UN number | UN2811 |
| Properties | |
| Chemical formula | C7H6NO5SNa |
| Molar mass | 269.21 g/mol |
| Appearance | Light yellow powder |
| Odor | Odorless |
| Density | 1.43 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -2.3 |
| Acidity (pKa) | -2.0 |
| Basicity (pKb) | 9.54 |
| Magnetic susceptibility (χ) | -89×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.605 |
| Dipole moment | 4.33 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 265.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -491.2 kJ/mol |
| Pharmacology | |
| ATC code | Not assigned |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS07, GHS09 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P280, P305+P351+P338, P337+P313 |
| NFPA 704 (fire diamond) | NFPA 704: 2-3-1 |
| Flash point | > 175°C |
| Lethal dose or concentration | LD50 Oral Rat 3240 mg/kg |
| LD50 (median dose) | LD50 (median dose): >2000 mg/kg (rat, oral) |
| NIOSH | NA9290000 |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | 50 mg |
| Related compounds | |
| Related compounds |
Benzenesulfonic acid 4-Nitrobenzenesulfonic acid Methanesulfonic acid Sodium benzenesulfonate Sodium 4-nitrobenzenesulfonate Sodium methanesulfonate 4-Nitrobenzyl chloride |
