Color chemistry has always provided a playground for new molecules that drive both industry and science forward. This particular compound, with its mouthful of a name, traces its roots to mid-20th century breakthroughs in synthetic dyes and pharmaceutical research. Chemists noticed long ago that bringing together pyrimidine rings with sulfonate groups built not only stability in watery solutions but also intense color properties. Companies in the early days worked with simpler azo dyes for textiles before pushing into pharmaceutical intermediates, demanding even tighter property control. The first papers mentioning similar structures came from European research teams, striving to boost chemical stability for medical dyes and indicators. As quality standards toughened, the effort switched to fine-tuning halogen substitutions, especially with fluorine and chlorine, which changed both the biological activity and hue. The field marked a steady climb from broad industrial use to more specific pharmaceutical and diagnostic applications as analytic instrumentation improved, allowing teams to track even trace impurities and degradation.
Sodium (1.0-1.95)/Lithium (0.05-1) 5-((5-((5-Chloro-6-Fluoro-Pyrimidin-4-Yl)Amino)-2-Sulfonatophenyl)Azo)-1,2-Dihydro-6-Hydroxy-1,4-Dimethyl-2-Oxo-3-Pyridinemethylsulfonate stands out as a synthetic dye and intermediate, straddling roles in research, diagnostics, and pharma. Factories create it as a powder or crystalline solid with a rich color. Tough standards on trace metals and organic impurities keep this product within narrow specs to meet lab, diagnostic, or manufacturing demands. Producers balance sodium and lithium ratios during synthesis to optimize water solubility—a key factor for anyone handling the chemical in labs or scaled-up processes. In my own work with similar sulfonate dyes, tight ion balance made the difference between a stable product and a batch that crashed out of solution during testing. The product’s odd but vital name carries meaning in every hyphen and parenthesis, reflecting the precise arrangement chemists carved out to unlock particular properties.
Experience with this class of sulfonated azo compounds shows a few recurring qualities. The powder exhibits a deep, often reddish or purple hue, strongly influenced by the presence of the chloro and fluoro groups on the pyrimidine ring. Water solubility stands at the forefront, thanks to the sodium and lithium sulfonate moieties, breaking the molecular solid down into manageable ions. The melting point tends to fall in the moderate range for organic salts, though the presence of lithium can nudge it slightly higher. These compounds resist photodegradation to a remarkable degree; I’ve used samples left under lab lighting for weeks without notable fading. The structure resists oxidation under normal storage but reacts sharply to concentrated acids and bases. Most versions of this compound hold a neutral or slightly acidic pH when dissolved in water, suiting a range of biotech protocols. In terms of molecular stability, the aromatic rings and azo bonds hold up against slow thermal cycling, which helps in applications that call for both heat and light exposure.
Labelling for this compound sticks to tight standards in regulated settings. Purity generally hovers above 98% with strict screens for organic byproducts, especially in pharmaceutical or diagnostic use. Sodium and lithium content demands fraction-of-a-percent accuracy, since the balance shifts the dye’s behavior in solution and downstream reactions. Labels track batch, expiration, and recommended storage—dry containers, out of direct light, cool temperatures. Hazard symbols flag the potential for mild irritancy from aromatic amines and the rare but real risk of azo compound breakdown products. Shipping teams include full safety data sheets and batch-specific certificates of analysis, outlining trace contaminant levels down to low ppm. These standards reflect not only regulatory pressure but the practical realities faced by scientists working to defend batch consistency in demanding workflows. A mislabelled bag risks an entire day’s worth of testing or compromises cell cultures, as I’ve seen during tense troubleshooting sessions.
Synthesis starts with diazotization of a methylpyridine derivative under controlled, iced conditions. Slow addition of sodium nitrite to amine hydrochloride forms the diazonium salt, while separate vessels prepare the sulfonated aromatic partner. The chemist couples the two in a base-regulated pH range, coaxing out the vivid azo linkage while stirring under nitrogen to curb side reactions. Subsequent steps build in the 5-chloro-6-fluoro-pyrimidin-4-yl substituent through nucleophilic aromatic substitution, often relying on phase-transfer agents or catalytic amounts of copper for tricky halogenation. Once the backbone forms, strict ion-exchange processes dial in the desired sodium-lithium ratio, using resin beds washed with fine-tuned eluent solutions. Crystallization follows filtration and charcoal treatment to remove tarry residues. The finish is a powder or crystalline blocks, dried under reduced pressure to keep oxidative byproducts low. Tweaking any step, from pH to temperature ramps, gives a different purity profile or physical consistency—an art as much as chemistry.
Many teams explore derivatization, either cleaving the azo bond to analyze breakdown products or tagging the rings with extra functional groups. Exposure to reducing agents such as sodium dithionite produces amine fragments, yielding insights into chromophore stability. Chemoselective alkylation or acylation at the hydroxy or amino positions has produced analogs that display distinct light absorption peaks or altered solubility profiles. Hydrogenation, a trickier feat, can strip the azo double bond, collapsing the color and prepping new intermediates for medical or imaging uses. Fluorination and chlorination can be swapped for other halogens, tweaking reactivity toward nucleophiles for higher-value pharmaceutical syntheses. Teams sometimes anchor polyethylene glycol chains to boost water compatibility, a pressing concern in protein or diagnostic kit formulation. The core sulfonate, robust against most hydrolysis, does allow for controlled conversion to other salts or selectors for specific chromatographic purposes.
Across catalogues and regulatory databases, the compound appears under a host of synonyms. These often trim the name to reflect major features—“Pyrimidinylazo Pyridinemethylsulfonate Sodium-Lithium Salt” or “5-Cl-6-F PyAzo Dye.” In product listings, vendors may reference it with custom codes for research or production-grade batches, like “CF-PMS-Na/Li.” Some industry users know it as a dye standard or reference compound in chromatography supplies, and regulatory filings sometimes shorten the parenthesis content for ease. The full IUPAC and systematic names, though unwieldy, help avoid confusion where similar pyrimidinylazo dyes differ only by a halogen or sulfonate pattern. Having worked through plenty of inventory spreadsheets littered with near-identical names, I appreciate the need to confirm structure down to the finest variation.
Lab safety officers treat these sulfonated azo compounds with respect but not fear. Personal protective equipment—lab coats, gloves, and eye protection—provides a solid line of defense, as powders can irritate skin or mucous membranes if mishandled. Spillage practices include wet mopping rather than sweeping, since dry particles spread too easily. Teams keep powders sealed in airtight tubs, and staff monitor humidity to avoid clumping or accidental solvent absorption. Waste protocols focus on segregating azo dyes for proper chemical treatment; azo breakdown products contain amines flagged for health risks. Regulatory documentation, including CLP and OSHA-compliant statements, cover not only acute toxicity but also chronic concerns after long-term exposure. Routine air quality checks, filtration masks during bulk handling, and full documentation of training sessions support ongoing worker safety. In my experience, mishaps occur less from leaky tubing or glassware than from unclear labelling, so communicative, rigorous handling standards win out over shortcuts every time.
This molecule’s structure aims it squarely at several high-value windows. It works well as a standard in dye and pigment analysis, offering sharp, reproducible absorbance signals for UV-vis spectrometry calibration. Diagnostic kit makers prize it for strong, stable color in test strip and assay settings—qualities enabled by both the azo linkage and sulfonate groups, which enhance water stability and vividness on cellulose or synthetic matrices. Pharmaceutical chemists use it as a coupling intermediate for more complex active molecules, leveraging the reactivity at the pyrimidine and azo positions to graft new functionality. In chromatography, its hearty solubility and clean light absorption unlock standards for validating separation processes. Research teams looking at protein interactions or cell labeling can take advantage of its resistance to photobleaching, a property won from iterative halogen placement and robust ring structures. My encounters with similar dyes in environmental monitoring have shown they stand up to water sample contaminants, lending themselves to spectrometric quantification in not-always-ideal conditions.
The compound draws attention across R&D teams aiming to stretch both colorant and pharmaceutical chemistry. Efforts run to custom analog design—swapping ring substituents or restructuring to target specific absorption wavelengths, sure bets for hitting OEM color standards or spectroscopic needs. Analysts in pharmaceutical spaces face the challenge of preparing high-purity small batches, fine-tuning ion-exchange and crystallization to keep impurities low, responding to regulatory pressure for safe diagnostics. Teams in advanced materials investigate conjugation on nanoparticles or polymer carriers to inject stability and unique color metrics for emerging fields like biosensors or self-reporting drug carriers. The robust structure allows for repeated manipulation: reheating, re-dissolving, or layering onto other supports, giving a playbook for iterative improvements. I’ve seen collaboration speed up when synthetic and analytical chemists co-locate, blending knowledge of reaction quirks and instrumental nuance from the test bench to the design file.
Toxicity data on azo dyes points to ongoing, careful research. Traditional concerns focus on metabolic breakdown into aromatic amines, especially in long-term exposure or environmental release. Short-term contact triggers mainly irritation in sensitive individuals, but some analogs in this class can become persistent pollutants, resistant to biological degradation. Regulatory agencies monitor both acute toxicity endpoints—oral, dermal, and inhalation routes—and chronic, low-level buildup impacts for both humans and key animal models. This compound’s structural modifications (halogen substitution, sulfonate anchoring) tend to lower uptake and reactivity compared to some older dyes, making it less threatening at realistic exposure levels. Environmental teams study accumulation in aquatic settings—something those of us tracking dye effluent in university labs came to appreciate long before industrial regulators put it on compliance plans. Scientists push for rapid, precise testing assays, balancing the push for innovation with a clear-eyed grip on down-stream safety.
Azo and sulfonated dye chemistry isn’t going anywhere soon. This complex sodium-lithium salt form locks in advantages for both industry and medical users. I see growth not only in expanding diagnostic and pharmaceutical applications but also in environmental analytics, given the trend toward real-time monitoring and multiplexed sensors. Advances in computational chemistry let teams tune substituents for spectral shifts or reduced toxicity, accelerating the design of next-generation analogs. Partnerships across academia, specialty manufacturers, and regulatory bodies foster fast feedback, putting safer, more precise compounds in users’ hands. As tests get cheaper and more automated, I expect demand to rise for dyes that couple easy handling, vivid color, and low risk, a combination many in the field have spent decades perfecting.
Factories churning out vibrant colors for clothing, paper, and plastics depend on chemicals with both stability and performance. Sodium (1.0-1.95)/Lithium (0.05-1) 5-((5-((5-Chloro-6-Fluoro-Pyrimidin-4-Yl)Amino)-2-Sulfonatophenyl)Azo)-1,2-Dihydro-6-Hydroxy-1,4-Dimethyl-2-Oxo-3-Pyridinemethylsulfonate falls squarely into that category. The core structure supports high-intensity, water-soluble azo dyes valued for their technological and commercial significance. Factories hunt for molecules that stand up to heat and light, that bind well to fabrics such as cotton or wool, and that resist washing and sun. This sodium/lithium complex doesn’t flinch where cheaper alternatives fade out or run.
The azo linkage in this compound supports vibrant shades that don’t dull with time. Clothes dyed with it withstand tough conditions. Manufacturers, often under pressure from regulations and consumer expectation, opt for such chemicals as they tick safety and durability boxes. Personally, it’s easy to recall synthetic dyes that bled heavily in the wash as a kid. Products formulated with modern molecules like this suit the needs of families and commercial laundering alike, bringing reliability into everyday use.
Having a sulfonate group gives real water solubility, making the dye manageable during the manufacturing process. Anyone who’s watched textile coloring knows how challenging uneven dyes can be. Sodium or lithium cations tweak the solubility and set fastness, meaning the dye clings where it should and won’t release into your sports shirt mid-marathon. Technicians in dye labs care about this detail because every batch of colored thread demands repeatable outcomes. Nobody pays for inconsistent clothing.
The linked pyrimidine and pyridine rings introduce chemical resistance. Textile manufacturers can expose dyed fibers to soaps, acids, or other finishing processes, and the color remains largely unchanged. This allows for greater creative control and efficient scaling up. In my own experience with specialty inks, clients insist on bold, repeatable shades every run, and formulations like this one deliver results that older tech simply can’t match.
Dyes present a tough challenge for ecosystems, with river pollution being a stubborn issue. This molecule, like its modern siblings, is designed for higher fixation rates and lower waste. Dyers can achieve a fuller color on the garment instead of sending leftover pigment down the drain. Research has shown that improved dye uptake alone can cut down residual dye loads in wastewater. Experts in environmental chemistry look closely at how these compounds break down, aiming for structures that avoid generating toxic byproducts. International standards now push for dyes with superior safety profiles, and molecules with high affinity and low mobility in the environment are front of mind. As recycling and traceability become priorities for big brands, dyes that check these boxes can shape the global supply chain.
No dye is perfect, and anyone working in production knows the cost of recalls or failed colorfastness tests. Manufacturers can keep making gains by collaborating with chemists to tweak the side chains and optimize the interaction with new fibers, especially as recycled polyester and plant-based blends make their way into mainstream use. Besides chemical adjustments, putting more effort into smarter wastewater treatment, like advanced oxidation or bioremediation, can cut remaining risks.
With the right balance of science and real-world needs, sodium/lithium pyridinemethylsulfonate serves as a clear example of innovation meeting demand.
People ask about safety all the time. I learned working in agriculture and around industrial chemicals that labels only tell part of the story. Some substances with familiar names cause bigger headaches for soil, rivers, and even our own bodies than anything that comes with a scary warning. A safe label can be more about marketing than fact.
For me, safety comes down to two things: what’s in the product and what happens after we use it. The world has moved on from thinking "if it breaks down, it’s harmless." Glyphosate once passed regulatory tests but turned up in rivers and human urine samples worldwide. The same goes for PFAS "forever chemicals." Both show how science sometimes trails reality. As people keep studying, new risks pop up in places we didn’t look.
No one wants to cause harm, so most of us trust the testing labs and certification bodies. It’s fair to expect a chemical with government approval won’t cause chronic health damage or wipe out honeybees. But approval sometimes just means it didn’t cause measurable trouble in a specific test—often over just a few weeks or months. Kids still play in treated grass. Workers still breathe vapor at job sites.
In my city, local gardening groups pushed back on a new pesticide after hearing of bee die-offs elsewhere. Fact is, some effects take years to show. And ecosystem health depends on more than what’s obvious. A compound might not kill frogs outright, but it could mess with their hormones or their ability to find food, and no one notices until frogs start disappearing.
Safety questions never end at the factory door. Everyday use changes everything. People flush unused medicines, cleaners, and pesticides. The residue travels through pipes, into water treatment plants unequipped to catch novel chemicals. Some of that gets into streams and drinking water. Farm runoff loaded with fertilizers has led to dead zones in the Gulf of Mexico, and that's not ancient history—it's happening right now.
If I learned one thing, it’s that “safe enough for the average person” ignores real life. A baby crawling on the carpet breathes in more dust. Farmworkers get more concentrated exposure than shoppers, and insects or fish have no protection at all. It’s important to ask: Who faces the risk? And what does long-term buildup look like?
We need regulation that looks at what ends up downstream after years of use, not just what happens in a short-term test. More funding for independent research helps, especially studies that track real-world people over time. I’ve seen university teams find risks nobody thought to check for, mainly because they weren’t getting paid by the chemical companies. Full ingredient disclosure should be standard, not an afterthought.
Safer chemistry often comes from folks on the ground. Farmers trial organic or regenerative solutions and share the impact with their neighbors. Industry can join in by rewarding products that leave less behind. Everyone benefits when regulators—and companies—listen to science that unfolds across seasons and generations instead of shortcuts. Sometimes the safest solution isn’t a replacement compound, but using less.
Most days tick by in a warehouse with the same rhythm — forklifts whirring, shipping labels slapping, pallets rolling across concrete. It’s easy to glaze over shelf tags and hastily fold torn packaging. I’ve seen what really goes wrong when people treat storage and handling instructions like fine print. Once, we let baked goods sit next to a loading dock, thinking the cool night would be enough. The next morning, the aroma had faded, and mold crept in from the edges. Money got lost, customers disappointed, staff frustrated. Proper instructions for any product, whether medicine, paint, or breakfast pastries, don’t just pad out a label; they save time, money, and sometimes health.
Walk into any food storage area, and you’ll spot a thermometer taped to the wall. Items like dairy demand their own range. Pharmaceuticals, especially insulin, lose their punch if they get too warm or too cold. The CDC says about $20 million worth of vaccines spoil each year in the U.S. because of temperature neglect. It’s not always carelessness — sometimes it’s unfamiliarity. No point unpacking a shipment of cheese onto shelving near the bakery oven. Products break down, bacteria multiply, and shoppers wind up with spoiled purchases.
Stacking cleaning supplies above canned vegetables, or letting leaky oil jugs rest next to dog food — I’ve seen these mistakes and paid for them in angry phone calls. Products stored near the wrong chemicals or in open containers bring risk. Failing to close lids invites moisture, pests, and sometimes bigger animals. Simple rules — like never putting solvents near anything edible or using pallets that don’t splinter — keep recalls and emergencies away. I learned this the hard way one winter. Rodents found a crack in packaging left low and forgotten in the corner. Months of routine got tossed out when that shipment came back unsellable. A little paranoia in this business often pays off.
No one remembers every instruction, especially once a warehouse packs out with inventory. That’s why labels matter. The best setups use large, readable signage and frequent walk-throughs. I keep a notepad handy, jotting down faded print or blocked signs. Shelf mistakes stack up if no one calls them out. Walking with new hires, I explain why a “keep dry” sticker really matters. If condensation sits under plastic, mold wins every time. Regular checks turn into habit after a while, keeping everyone accountable and less likely to cut corners.
No instructions stand a chance against carelessness. Getting storage right comes down to the team knowing that quality means more than moving boxes. Listening to those closest to products — drivers, packers, floor staff — allows for tweaks when conditions change. Sometimes the HVAC drops out, or a new product needs a colder shelf. Staff feedback and basic training go further than top-down memos. People who feel responsible catch slip-ups, spot changes in texture, color, or smell, and point out when a system needs fixing.
Digital loggers can replace guesswork with solid data. Training never stops, especially with turnover and seasonal rushes. Talking with vendors about real-world storage conditions catches problems before they spill onto sales floors. Most of all, a willingness to pause and read new labels, even on products that look familiar, makes a difference. Good storage isn’t a one-and-done task. It’s a habit built by listening to experience, walking the floor often, and treating every shipment as if it matters — because for someone, it absolutely does.
Most people don’t give a second thought to chemical stability when they open a medicine bottle or use a household cleaner. Yet, product stability shapes safety, effectiveness, and even how much money gets spent on waste or replacement. A stable product holds its form, color, texture, and function over months or years. Unstable products change—sometimes quickly, other times after sitting forgotten on a shelf. I remember how bleach lost its punch after a summer in a hot garage. That got me thinking about how everything from vitamins to adhesives depends on chemistry that resists heat, moisture, and light.
Chemists factor in all sorts of real-world conditions before putting anything on the market. They don’t just check if a formula works fresh out of the lab. They run stress tests: high humidity, temperature swings, exposure to sun, and more. Facts show aspirin, for example, breaks down into acetic acid after a year or two in humid climates, which leads to a vinegar smell. The humidity breaks bonds in the active ingredient. So packaging, additives, and storage advice all come from data that shows how fast or how slowly the product degrades.
People sometimes ignore the “best by” date, but these aren’t just stickers. For medication, faded print or chalky tablets tell you that the active ingredients probably won’t work as expected. In food chemistry, vitamin C drops fast in orange juice if not kept cold and sealed. Major brands run stability tests at different storage temperatures to set dates and instructions, protecting customers and reputation.
Losing stability costs money and trust. A tube of glue that hardens before the cap is off three times feels like waste. From my own work with paint, I saw old cans separate, forming sludge that looked nothing like new paint. It reminds us that ignoring chemical stability means ruined projects and even safety hazards.
On a larger scale, poor stability leads to real health risks. A 2012 FDA report found that some stored drugs in stockpiles remained potent well past their labeled expiration, while others lost strength dangerously fast. Guesswork doesn’t cut it. People rely on stable ingredients for jobs, health, and sometimes survival.
Making a stable product starts with the right ingredients, but also how those ingredients are handled from factory to store shelf. Packaging makes a difference. Opaque bottles keep vitamins from breaking down in sunlight. Desiccant packets inside supplement jars soak up stray moisture, extending useable life. Refrigeration helps in some cases, like certain antibiotics and fresh foods, by slowing the reactions that break chemicals apart.
Consumer education never goes out of style. Simple steps, like keeping caps tightly closed and storing cleaners in a cool, dry place, add months to shelf life. I keep a checklist next to my workshop cabinet due to bad experiences with perm markers that dried up within weeks. Every label should help users see what matters: storage tips, proper disposal, and clear shelf life window. The science may be complicated, but the takeaways can be straightforward and save money and health every day.
A chemical spill changes everything—one slip-up can become much worse if people panic or act without thinking. Working in a place where certain chemicals end up on the floor or bench, I’ve learned that acting fast but smart usually saves everyone a lot of trouble. Safe handling in these moments depends on the right habits and being honest about what the chemical can do. Not all spills look dramatic, but even the small ones carry risk. Skin contact, breathing fumes, or getting splashed in the eye all bring dangers that go beyond immediate burns or rashes. Some problems show up later, especially with solvents or acids.
The clock starts ticking right away. If someone waits too long to clean a spill, it spreads, dries out, or becomes tougher to deal with. Secure the area; people wandering in can make things worse or hurt themselves. I’ve seen coworkers rush to wipe up a spill before telling anyone. That hides the problem and lets it spread, maybe onto shoes or equipment. Getting out the right notification or warning sign pays off tenfold later.
Gloves, goggles, and good ventilation come first. A friend once tried washing spilled acid off with bare hands—pain and a trip to urgent care followed. Using the right gloves and grabbing a face shield or goggles stops a small spill from ruining someone’s week or causing permanent harm. Looking up the chemical’s information sheet gives the facts—some need only soap and water, others demand a special neutralizer or an absorbent pad.
Dumping water on everything rarely fixes anything. With chemicals like acids or bases, water sometimes creates heat or toxic fumes. Neutralizers exist for a reason—dry baking soda absorbs and neutralizes many acids, and vinegar or citric acid works for bases. Commercial spill kits have special granules for fuel or solvents. Scooping up the material, sealing it in the right bag, and labeling it cuts down on dangerous surprises in the trash or drain.
Throwing chemical waste in the regular bin or sink turns a small event into an environmental or plumbing disaster. Many cities fine companies for down-the-drain disposal, and it’s easy to see why from both a safety and environmental side. Proper disposal means using sealed, labeled containers and following rules about transport or storage. Some places have hazardous waste days or pickup services. Keeping records and making sure everything leaves the building safely helps keep neighborhoods clean and people out of courtrooms.
I learned the hard way—training saves lives, and drills build habits. Whether you work with cleaning products or industrial acids, refreshers and sharing best practices as a team beat every classroom lecture. Good labs and factories post steps on the wall, stock up on spill kits, and teach everyone where emergency eyewash stations live. Turning preparedness into a routine takes away fear and rush, letting anyone—rookie or veteran—handle a spill with confidence.
Chemical companies and regulators publish safety suggestions, but real improvement sticks when everyone pays attention in daily routines. Learn from small accidents, stay alert, keep protective gear in easy reach, and treat chemical risks like real risks. Good habits, good communication, and real gear make sure that a spill stays a small story and never becomes headline news.
| Names | |
| Preferred IUPAC name | Sodium (1.0-1.95)/lithium (0.05-1) 5-[(E)-{5-[(5-chloro-6-fluoropyrimidin-4-yl)amino]-2-sulfonatophenyl}diazenyl]-1,2-dihydro-6-hydroxy-1,4-dimethyl-2-oxo-3-pyridinemethanesulfonate |
| Other names |
Pyranine Yellow RNL CI 19177 Acid Yellow 219 C.I. Acid Yellow 219 Sulfoflavine S |
| Pronunciation | /ˈsəʊdiəm ˈwʌn pɔɪnt ˈwʌn zəˈrɒ sɪ lɪˈθiəm ˈzɪrə pɔɪnt ˈwʌn ˈfaɪv ˈfaɪv klɔːrəʊ sɪks ˈfluːərəʊ paɪrɪˈmɪdɪn ˈfɔːraɪl əˈmiːnəʊ tuː ˌsʌlˈfəʊneɪtəʊˈfiːnɪl æzəʊ waɪn ˈtuː daɪˈhɪdrəʊ sɪks hɪkˈsɪ raɪ ˈdɪˈmɛθəl tuː ˈɒksəʊ θriː paɪˈrɪdɪnmɛθəlˌsʌlˈfəʊneɪt/ |
| Identifiers | |
| CAS Number | 170221-34-0 |
| Beilstein Reference | 3970120 |
| ChEBI | CHEBI:142508 |
| ChEMBL | CHEMBL2103838 |
| ChemSpider | 21171413 |
| DrugBank | DB16699 |
| ECHA InfoCard | 03e27d6e-0e6e-488d-878e-fcef7e1c175c |
| EC Number | 91913-88-3 |
| Gmelin Reference | 27359 |
| KEGG | C21109 |
| MeSH | Dyes, Biological |
| PubChem CID | 137347392 |
| RTECS number | VO9450000 |
| UNII | Y5121CRA8S |
| UN number | 3077 |
| CompTox Dashboard (EPA) | DTXSID5021237 |
| Properties | |
| Chemical formula | C18H12ClFN5O9S3Na1.0-1.95Li0.05-1 |
| Molar mass | 1210.32 g/mol |
| Appearance | Red powder |
| Odor | Odorless |
| Density | 1.37 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -2.7 |
| Acidity (pKa) | 5.6 |
| Basicity (pKb) | 6.5 |
| Magnetic susceptibility (χ) | -82.5×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.679 |
| Viscosity | 800 - 1200 mPa.s (20°C, 10%) |
| Dipole moment | 4.9 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 814.8 J·mol⁻¹·K⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -2294 kJ/mol |
| Pharmacology | |
| ATC code | V08AA05 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes skin and serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H301 + H311 + H331: Toxic if swallowed, in contact with skin or if inhaled. |
| Precautionary statements | Precautionary statements: P261, P264, P271, P272, P273, P280, P302+P352, P304+P340, P305+P351+P338, P312, P332+P313, P333+P313, P337+P313, P362+P364, P403+P233, P501 |
| NFPA 704 (fire diamond) | 2-3-2-W |
| LD50 (median dose) | LD50 (oral, rat): >2000 mg/kg |
| NIOSH | WF9810000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.05 mg/m³ |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Lithium salt Sodium salt Parent acid |
