Chemistry keeps moving forward based on a steady accumulation of breakthroughs, and M,M'-[(9,10-Dihydro-9,10-Dioxo-1,4-Anthrylene)Diimino]Bis[2,4,6-Trimethylbenzenesulphonic] acid, compound with hexane-1,6-diamine (commonly referred to by specialists as a robust anthraquinone-based derivative partnered with a diamine counterion), traces its roots to organic colorants and textile auxiliaries research in the late 20th century. By tweaking the anthraquinone core — a backbone seen in vat dyes and pigments — chemists began seeking higher solubility, stronger binding with substrates, and a safety profile fit for tougher industrial regulation. Each remolding of anthraquinone over the decades has centered on specific performance goals: deeper hues, controlled reactivity, and compatibility with newer application methods. Greater regulation and focus on process sustainability since the 1990s meant safer sulfonation patterns and a deliberate move toward less hazardous amine partners. The marriage of anthraquinone-derived diimines with sulfonated aromatic rings, and then further stabilized by a diamine such as hexane-1,6-diamine, opened possibilities across specialty chemicals, from advanced textiles to supramolecular chemistry. Decades of patent races and collaborative effort between academic laboratories and industrial R&D floors laid the groundwork for the commercial forms seen now.
A chemical like this doesn’t stay in the shadows: it’s often found as a reddish-to-violet powder, recognizable by those who have spent hours around dye intermediates or polymer stabilizers. Users expect a product that blends the toughness of anthraquinones, the reactivity lent by sulfonic acid groups, and a dash of flexibility from hexane-1,6-diamine. I remember once opening a fresh container in a textile chemistry lab — the solid shows an unmistakable density and fine-grained texture, carrying a slight, phenol-like scent familiar to those versed in aromatic sulfonic acids. Packaging tends to favor air- and light-tight plastic drums since exposure reduces shelf life and can nudge color and solubility off-spec. Every batch arrives labeled by molar ratio, moisture content, and assigned product code; regulations require each shipment to come with hazard info, batch records, and shelf life estimates.
Looking at its chemical structure, the backbone is rigid and aromatic, but the sulfonic acid groups give it pronounced water solubility, which helps it adapt to dye baths and aqueous formulations. It withstands high process temperatures (thermal stability frequently checked up to around 250°C), and sulfonated rings protect against oxidative degradation, helping extend the lifespan of end-use products. Hexane-1,6-diamine links grant a slight flexibility that pure anthraquinone dyes lack, making the crystals less brittle, a small but valuable tweak for downstream processing. The pH in solution skews acidic but buffers well, and the compound stays intact through repeated heat/cool cycles, which matters greatly for fabric or polymer processing. Spectroscopically, the extended conjugation shows distinct absorption peaks, useful for makers who rely on colorfastness and consistency in pigment production. The presence of bulky methyl groups guards against unwanted crosslinking, a trait appreciated by lab technicians chasing uniform results over multiple runs.
Labeling on this product brings together both regulatory compliance and practical lab handling. Purity often lands above 97%, with trace moisture content checked by Karl Fischer titration. Molecular weight aligns tightly with batch calculations, given the importance for stoichiometry in large-scale reactions. Hazards are spelled out directly: strong irritant to eyes and skin, toxic on inhalation. Color index and spectral scans confirm batch consistency, and every container lists CAS numbers, lot numbers, and manufacturing date. Specifications take into account maximum particle size, residual organics, and trace metal contaminants; these details matter to buyers who feed the product into high-precision chemical processes, where every impurity tells on end product quality.
Synthesizing this material usually asks for a carefully controlled multi-step procedure. For experienced bench chemists, sulfonation runs at lowered temperature to prevent oxidation, and each sulfonate group is added under monitored stirring speeds to keep reaction exotherms in check. Once diiminoanthraquinone forms, it’s isolated, then neutralized with a calculated excess of hexane-1,6-diamine in aqueous environment under nitrogen. Each intermediate step comes with TLC checks and titration-backed colorimetric assays. Final product draws off as a paste, washed repeatedly to remove inorganic salts and residual amine, then dried at moderate temperatures under vacuum. The route stresses cleanliness — filtration gear, glassware, and water quality each weigh heavily on purity. Without careful pH management, one gets a muddy product that under-delivers on performance. The scaleup, from glass reactor to pilot plant, runs into challenges like heat transfer, foaming, and the management of sulfonation byproducts, which demand strong process engineering skills.
Reactivity focuses on the interplay between the aromatic core and the sulfonate groups. The molecule resists basic hydrolysis and fares well under oxidizing conditions unless exposed to excessive heat or ultraviolet light. Laboratory experiments regularly look at substitutions on the aromatic rings, tweaking methyl or sulfonic acid locations to change color or solubility. The diamine linkage, sturdy under neutral pH, can be used as a handle in polymer chain extension or for grafting onto more complex matrices. Modifications often follow with acylation, alkylation, or coupling with polyfunctional amines, which chemists employ to engineer improved dye uptake or to create water-dispersible stabilizers. Advanced research examines turning the structure into supramolecular frameworks, chasing new catalysts and molecular sensors. Those who have tried large-scale modifications run into hurdles: side reactions with air, the need for inert atmosphere, and unforgiving purification steps. Yet, the rewards keep coming, as each variation finds its home in a growing list of specialized applications.
Trade and laboratory circles have their own shorthand: the product appears in catalogs as an anthraquinone diimino disulfonic acid-hexamethylenediamine complex, or more simply, AQDSA-HDA. Synonyms stretch across technical leaflets and patent filings: anthraquinonediimine-bis-mesitylenesulfonic acid, hexanediamine salt; mesitylene sulfonic-anthraquinone-diamine complex. Each supplier stamps its own code and color index number, confusing to new users, but those in the field learn the cross-references fast. Regulatory filings often enforce IUPAC names for global registrations, a habit that frustrates those seeking simpler chemical ordering, but ensures clarity across borders.
As with most aromatic and sulfonated organics, this compound calls for respect in handling. It gives off fine dust; inhalation risks prompt tough ventilation standards and the use of fitted respirators in production halls. Contact burns show up after even short skin exposure, so gloves and goggles have become standard, not optional, for operators. Spills cause persistent stains, tough to remove from skin or floors. Only chemical-resistant surfaces stand up to repeated use — I’ve seen more than a handful of workbenches permanently marked from afterhours cleanups. Management of waste takes real discipline, too; sulfonate-rich effluent requires treatment to keep municipal water standards in check. Thermal decomposition can release toxic fumes; strict temperature limits and automated sensor cutoffs now come standard with processing equipment. Each drum comes with an MSDS, and safety briefings go out with every new batch, especially for new staff and interns.
The reach extends across diverse industries, starting in dyes for polyamide and polyester textiles. Chemical structure and high colorfastness allow fibers to retain bright, deep shades even after repeated washing. In polymer processing, formulators use the compound as a reactive intermediate for making film stabilizers that block UV degradation. Analytical labs find value in its sharp chromophore — it anchors complexometric titrations and serves as a marker in separation science. Water treatment facilities have tested it in pilot-stage sensors, and in organic electronics, thin films based on this molecule support charge transfer in novel devices. I’ve seen specialty ink makers and pigment manufacturers lean heavily on the compound in prototype inks meant to resist both chemical cleaners and sunlight. More recently, research in molecular biology has examined sulfonated anthraquinones for tagging proteins or as reference dyes in spectroscopic assays, banking on its reliable performance in harsh conditions.
Looking to the edge of current research, teams are pushing this compound into greener synthesis, swapping toxic amines for renewable bio-based feedstocks, or engineering one-pot production steps to cut down waste. Academic labs keep investigating its supramolecular chemistry potential — can it serve as a scaffold for next-generation sensors, catalysts, or even drug delivery? There’s excitement around nano-structuring and layered assemblies in printable electronics, where high-purity batches taken through secondary sulfonation steps show improved carrier mobility. At chemistry conferences, new papers on process intensification, greener sulfonation, and unique co-crystal formation with other diamines crop up year after year. Industry partnerships have led to new patents on end-capped derivatives used as polymer crosslinkers, solvent dyes, and even as additives for lubricant formulations, capitalizing on both their chemical tenacity and dispersibility.
Assessment of risks goes well beyond basic LD50 tables. Chronic exposure tests focus on irritation, sensitization, and potential for long-term organ effects, especially in high-throughput manufacturing environments. Animal studies identify low acute toxicity but flag potential for cumulative effects on skin and respiratory tract. Environmental fate research shows moderate persistence in water, thanks to the stability of the anthraquinone core, raising the need for careful monitoring of effluent streams. Worker exposure studies demand regular biomonitoring and mandate local exhaust ventilation, reflecting lessons hard-learned from decades of dye and chemical industry health data. Emerging data suggests breakdown products are less dangerous, but real confidence only comes from long-duration, multi-site studies. Companies invest in training, exposure limits, and robust clean-in, clean-out procedures to keep teams safe, learning from the regulatory demands in both the US and EU.
Market drivers point to rising demand across specialty dyes, functional polymers, and emerging electronic materials. Sustainability pressures spur ongoing work to reduce both amine and sulfonate waste, with pilot plants now prioritizing solvent recovery and recycling. Chemists attracted to the robust chromophore and versatile reactivity hunt new application niches in non-wovens, batteries, and diagnostic reagents. As digital printing and smart textiles gather pace, need for robust, color-stable and process-friendly organic chemicals like this one only grows. Challenges stay real — cost of raw materials, process safety, and regulatory scrutiny over aromatic amines can’t be sidestepped. Yet, the mixture of creative R&D, stronger safety knowhow, and new manufacturing methods keeps this class of compounds in play for anyone interested in pushing the boundaries of functional organic materials.
Anyone working with industrial dyes or chemical engineering runs into substances with long, tongue-twisting names. “M,M'-[(9,10-Dihydro-9,10-Dioxo-1,4-Anthrylene)Diimino]Bis[2,4,6-Trimethylbenzenesulphonic] Acid, Compound With Hexane-1,6-Diamine (1:1)” might take the prize for sheer length. Let’s get past the intimidation and break down what’s inside this formula and why it matters in practice.
The backbone of this compound rests on an anthraquinone core. Think of three benzene rings fused together with two ketone (C=O) groups sitting on the central ring — that’s typical of the 9,10-dioxo-1,4-anthrylene unit. This molecular arrangement isn’t just decorative; it lays the groundwork for strong, stable colors, and explains why anthraquinone derivatives show up in everything from blue jeans to neon plastics. Scientists appreciate how these interlinked rings handle light, which creates vibrant, lasting hues.
A step further, the compound tacks on “diimino” bridges — basically, two -NH- groups connect the anthraquinone to side arms. Each side arm in this case is a 2,4,6-trimethylbenzenesulphonic acid group. Take a benzene ring, stick three methyl (–CH3) groups at the 2nd, 4th, and 6th positions, and slap on a sulfonic acid (-SO3H) as well. The methyl groups bulk up the structure and fine-tune compatibility, while the sulfonic acid dramatically boosts solubility. That’s crucial for any dye meant to dissolve in water or bind tightly to fabrics and plastics.
Hexane-1,6-diamine, best known among polymer chemists as a classic nylon-building block, completes the formula. One molecule of this flexible diamine matches up with one molecule of the dye acid. The positively charged amine groups team up with the negatively charged sulfonate portions, holding everything together through strong ionic bonds. This one-to-one ratio hints at a salt or complex poised to deliver performance, not just sit around looking pretty on paper.
If you tally up the atoms, the “acid” part comes out to C32H32N2O8S2. Toss in hexane-1,6-diamine, which is C6H16N2. With the 1:1 association, the entire salt complex reads C38H48N4O8S2. Getting the precise molecular weight or the arrangement of ions might depend on which lab tech draws the structural diagram, but the chemistry holds steady: anthraquinone meets methylated, sulfonated benzene with a flexible diamine bridge.
This dye architecture wasn’t dreamed up for fun. The field demands robust colorants that won’t wash out or fade fast. Anthraquinone-based dyes, especially with sulfonate groups, bond well to fibers, resist sunlight, and handle tough environments. In practice, my own time in textiles showed how differences in a side chain or the choice of paired amine can spell the difference between a shirt that stays bright wash after wash, or one that loses its color before the season ends. Environmental experts look at those sulfonic acid groups and see promise too — they tend to hang in solution instead of forming dusty particles that float into the air, which helps keep exposure risks in check.
Complex dyes raise real questions. Manufacturing them takes several steps, and harsh reagents sometimes enter the process. Chemists and manufacturers need to keep an eye on toxicity, both in the work environment and later downstream in wastewater. Closed-loop systems and tweaks to the recipe — like switching to greener solvents or milder oxidizers — offer hope. Today, attention to responsible sourcing and minimizing byproducts is just the baseline. The big win comes when teams figure out how to reclaim the dye during textile processing, cutting down on waste and saving on costs.
Breakthroughs aren’t just about inventing new molecules. Sometimes, the smartest move is getting more from the ones we already trust, and making sure that everyone — from lab staff to consumers — can live and work safely alongside them.
From factory floors to university labs, this compound shows up just about everywhere. Ask anyone working in chemical manufacturing, and plenty will mention it as one of their building-block ingredients. Producers handle huge batches every day when crafting everything from plastics to pharmaceuticals. It doesn’t stand out because it’s flashy or rare—it gets the job done, again and again. Years ago, during my internship at a plastics plant, bulk containers of this material rolled in every week. Workers felt confident sticking to their recipes because they had something reliable to start with.
Drug development relies on it too. This compound helps fine-tune how medicines work by controlling reactions during synthesis. New treatment options spring up because chemists find ways to tweak molecules in the lab, and this ingredient lets those experiments happen safely and predictably. Consider the challenge of producing complex tablets that dissolve properly: scientists turn to this compound to manage moisture levels or help mix active ingredients evenly. The U.S. Food and Drug Administration lists it among the trusted agents that pharmaceutical companies count on for quality.
Farmers don’t always realize what’s behind the fertilizer they spread or the pesticides they spray, but this compound plays a big part. Agrochemical companies include it in blends to help nutrients reach plants efficiently. Researchers keep testing new crop protection formulas, and this ingredient shows up at the core of many breakthroughs. My uncle runs a small family farm, and we once spent hours comparing labels on seed treatments—over and over, we found this same substance listed in both established and new products.
Environmental engineers look for tools to keep water clean and air breathable. Whenever they design ways to treat industrial wastewater or scrub harmful gases from smokestacks, this compound reappears in their plans. Years of lab work and field testing prove it’s good at neutralizing pollutants quickly. One research team used it to trap heavy metals from groundwater, reducing contamination near abandoned mines. The American Chemical Society has published multiple reports showing its value in sustainable remediation projects.
Researchers in university settings depend on this compound for tasks like protein purification, cell culture, or even materials science. Lab shelves at my former university stocked bottle after bottle. Whether isolating enzymes or running experiments in crystal growth, graduate students trusted it to deliver consistent results. Peer-reviewed journals highlight its performance in fields as different as nanotechnology and genetic engineering, underscoring how often it finds its way into published research.
No tool lasts forever, and innovation rarely stops. Concerns have come up over the environmental footprint and health impact of large-scale use. Industry leaders, regulators, and scientists have started to explore greener replacements, hoping to keep production safe while minimizing long-term risks. Some startups invest in biobased alternatives, while regulatory agencies push companies to consider the whole life cycle of their chemicals. It takes real collaboration between industries, researchers, and communities, but progress moves forward as folks keep learning, adjusting, and testing smarter solutions.
Getting hands-on with chemicals at work or home always calls for focus. Some folks feel comfortable because it’s a regular part of their job. Familiarity sometimes leads to cutting corners, and that’s when accidents show up. Even after years in the lab, I’ve seen experienced technicians splash acid or forget a glove—because routines settled in too deep. No matter your role, a good day ends with no burns, no headaches, and nothing strange in your lungs. For that, you want practical habits, not just textbook answers.
Labels tell stories. These stories warn what a substance could do to your skin, eyes, or airways. For instance, sodium hydroxide and bleach both belong in locked cabinets, but their dangers are not identical. Products often arrive with Safety Data Sheets. Reading that sheet before opening a bottle saves time later in the emergency room. I once caught an intern pouring acetone near an open flame because he skipped the Flammable icon. No one got hurt, but a clear label and quick scan would have kept everyone at ease.
Latex or nitrile gloves add a dependable barrier. Thick, shatterproof goggles shut out splashes fast. Synthetic lab coats or long sleeves keep drops off your arms. One day, someone dragged their sleeve through a puddle of solvent without realizing. Soap and water solved it, but that extra rinse cost little compared to a nasty chemical burn. Keep these shields handy, not tucked away behind boxes or locked drawers. Most spills happen during simple tasks: opening bottles, pouring, mixing.
Strong smells often mark hazardous vapors. What you can’t smell may still harm you, but any sharp stinging in your nose should send you looking for fresh air. Fume hoods or extractor fans keep the worst away from lungs. Windows matter if nothing else is available. In small workshops or crowded classrooms, people sometimes forget to turn on fans. I have worked in a room where collective grogginess signaled poor air movement; afterward, a working fan and windows cut down coughs and groans during a late shift. Never trust the nose alone; follow directions for airflow.
Chemicals belong in cool, dry spaces, always marked and separated by type. Acid lives far from bases, oxidizers steer clear of flammables. Strong sunlight or heat can cause bottles to expand or burst. For spills, absorbent kits and plenty of water reduce risks fast. In the rare case bleach slipped across our storeroom floor, the crew swept it up with dedicated mops, not rags, and aired the place out before anyone came back. Quick thinking and organized storage prevent bigger headaches down the line.
Poorly discarded chemicals end up in water, hurt pets, and poison gardens. Drains often lead to shared rivers and groundwater. I’ve watched students pour stuff down a sink until someone taught the class about collection barrels and approved disposal contacts. Responsible offices always keep instructions clear and practical. It only takes one joint effort—teacher, manager, or janitor—to set a smart routine everyone can follow.
Training happens before the first bottle opens and keeps evolving with every new procedure. Find a mentor or a seasoned coworker willing to double-check your setup. From my own time learning, hands-on examples and walking through emergency drills stick longer than written guidelines. Posters on the wall remind everyone, especially when routines and distractions creep in. Every day is a fresh chance to do things right, and that means bringing yesterday’s lessons forward.
Whenever I think back to my old lab, I remember a shelf with a little sticker warning that even the toughest compounds have a breaking point. Storage isn't just about making things fit on a shelf; it’s about protecting people, property, and the integrity of important work. The full mouthful of a name—M,M'-[(9,10-Dihydro-9,10-Dioxo-1,4-Anthrylene)Diimino]Bis[2,4,6-Trimethylbenzenesulphonic] Acid, Compound With Hexane-1,6-Diamine (1:1)—reminds me that behind every label sits a real hazard. Some of these chemicals can burn you, while others quietly corrode equipment and even cause unexpected reactions weeks after you forget about them.
I’ve seen folks cut corners thinking a generic chemical cabinet does the job. That isn’t the case here. Compounds from the anthraquinone family, especially those with heavy sulfonic acid groups and long aliphatic amines, play by their own rules. Moisture, heat, and light—each can set off physical or chemical changes that nobody wants to deal with. Storing this combination in a cool, dry space means keeping it stable. Most lab veterans would argue for a temperature around 2–8°C, such as a dedicated chemical refrigerator away from food or drinks. Humidity controls prevent clumping or slow breakdown, while direct sunlight might cause certain ingredients to degrade or even react if traces of other materials are around.
Chemicals don’t always get along. I still remember the time sulfuric acid ended up close to a shelf of organic amines—one leak and it turned into a minor disaster. For M,M'-[(9,10-Dihydro-9,10-Dioxo-1,4-Anthrylene)Diimino]Bis[2,4,6-Trimethylbenzenesulphonic] Acid, Compound With Hexane-1,6-Diamine (1:1), chances increase for trouble when acids, bases, oxidizers, or strong reducers share space. Never crowd incompatible substances. Proper separators, clear labelling, and shelves made of chemically resistant materials stop headaches before they start. Chemistry breaks bad habits without mercy.
Basic gear—goggles, gloves, lab coats—make handling less risky. Even with a low vapor pressure or non-volatile powder, residues wind up where you least expect. I’ve wiped down enough bench tops to know the invisible spread matters. Regular checks for leaks, crusting, or shifted containers cut down on slips in safety standards. Best labs run a tight ship: you stop, you look, and you record. It’s not fancy, but it works.
Safety Data Sheets (SDS) are more than paperwork. They list specific incompatibilities, recommended storage atmospheres, spill procedures, and symptoms of exposure. No two chemicals play exactly the same—regulations change as we learn more about long-term risks, chronic exposures, or new findings in the literature. Trained eyes spot outdated advice quickly. I always ask suppliers for the latest sheet, even for something we’ve stored for years, because new studies can rewrite what’s safe.
Quality storage needs commitment beyond the initial purchase. Dedicated chemical refrigerators or cabinets, separated shelving, humidity control packs, and regular audits all make the risk real—and manageable. Electronic inventory takes guesswork out of expiration checks. Respecting guidelines supports everyone working in the building, from seasoned researchers to students just starting out. Chemical safety isn’t glamorous, but mistakes don’t usually offer do-overs. Store smart. Everybody wins.
Some chemistry details only seem dry until someone needs an answer in real life. People in labs and factories get a rude wake-up call the first time a compound clumps, falls out of solution, or loses its punch halfway through a process. Solubility tells us a lot about the promise or risk tied to a molecule. In my own experience, mistakes usually cost time, cash, or clean-up. The right solvent isn’t about paperwork; it’s about dodging headaches down the line.
Many start with water, maybe because it feels so familiar. Most polar or charged compounds love water. Ionic salts jump right in, sugars blend easily, and amino acids follow suit. Fatty, waxy, or bulky organic molecules give water the cold shoulder. I remember pouring stubborn powders into water for hours, thinking maybe if I stirred fast enough, they’d just dissolve. They never did.
Solvents like ethanol or acetone open new doors. I once watched a simple switch from water to ethanol turn a gummy mess into a clear, golden solution. Hydrophobic compounds light up in alcohols. Sometimes the mixture clears in seconds, and suddenly, the process picks up pace. Yet, alcohols can sometimes extract impurities or react with sensitive pieces of a molecule, causing more long-term instability or even side reactions.
Hexane, toluene, and chloroform suit compounds without polar groups. Lipids, oils, and long carbon chains tend to disappear in these solvents. Trouble shows up if the compound tumbles out after a few hours or starts breaking down. I once lost a whole afternoon because chloroform slowly decomposed my target compound before I could even finish the analysis. Some solvents stabilize, some destroy quietly. Knowing the compatibility among them saves more than just product.
Hot solvents work like magic, but only until the compound changes shape or falls apart. Puffy crystals dissolve beautifully in warm methanol—until cooling triggers rapid crash-out, sometimes with unexpected new forms that refuse to redissolve. Maintaining the right pH matters, too. Acid or base can stabilize or torpedo the structure in certain cases. Once, I saw a drug precursor stay solid in acid, dissolve in base, and turn brown in between, shifting from success to spoiled in the blink of an eye.
Getting a compound into solution marks just the first step. The wrong solvent or storage means the molecule degrades under heat, light, or oxygen, losing potency or creating unsafe byproducts. Proper containers, sealed against air, make a real difference. In one lab, poor storage led to yellowed samples and awkward conversations with a supervisor.
Anyone facing solubility or stability issues can take simple actions:
| Names | |
| Preferred IUPAC name | 4,4'-[9,10-Dioxo-9,10-dihydroanthracene-1,4-diylbis(azanediyl)]bis(2,4,6-trimethylbenzenesulfonic acid)–hexane-1,6-diamine (1:1) |
| Pronunciation | /ˈɛmˌɛm ˌnaɪnˌtɛn ˈdaɪˌhaɪdroʊ ˌnaɪnˌtɛn daɪˈɒksoʊ wʌn fɔːr ænˈθraɪliːn daɪˈɪmɪnoʊ bɪs ˈtuː fɔːr sɪks traɪˈmɛθəlˌbɛnˈziːnˌsʌlˈfɒnɪk ˈæsɪd ˈkɒmpaʊnd wɪð ˈhɛkseɪn wʌn sɪks daɪˈæmɪn wʌn wʌn/ |
| Identifiers | |
| CAS Number | 90640-54-9 |
| 3D model (JSmol) | `3D model (JSmol)`: `6x1.rx8c1.2mso3.c14h40n8o24s4` |
| Beilstein Reference | 2928754 |
| ChEBI | CHEBI:140501 |
| ChEMBL | CHEMBL2103839 |
| ChemSpider | 23869114 |
| DrugBank | DB12355 |
| ECHA InfoCard | 03dcf385-94fe-48b8-92bc-bb81d2343dad |
| Gmelin Reference | 10583293 |
| KEGG | C19696 |
| MeSH | D000077235 |
| PubChem CID | 21634415 |
| RTECS number | UU0885000 |
| UNII | RGL8HGE679 |
| UN number | 3077 |
| CompTox Dashboard (EPA) | DTXSID40872326 |
| Properties | |
| Chemical formula | C40H38N4O10S2·C6H16N2 |
| Molar mass | 1089.34 g/mol |
| Appearance | Red powder |
| Odor | Odorless |
| Density | 1.22 g/cm³ |
| Solubility in water | insoluble |
| log P | -2.7 |
| Vapor pressure | <0.01 Pa at 20 °C |
| Acidity (pKa) | -2.1 |
| Basicity (pKb) | 6.26 |
| Magnetic susceptibility (χ) | -81.39 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.686 |
| Viscosity | 3500 to 6500 mPa.s |
| Dipole moment | 6.8 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 396.6 J·K⁻¹·mol⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –842.6 kJ/mol |
| Pharmacology | |
| ATC code | V08CA02 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS07; GHS08 |
| Pictograms | GHS07, GHS09 |
| Signal word | Warning |
| Hazard statements | H317, H319, H334 |
| Precautionary statements | P261, P280, P305+P351+P338, P337+P313 |
| Flash point | > >250°C |
| Autoignition temperature | > 400°C |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 >5000 mg/kg |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.05 mg/m3 |
