© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
The early stories of chromium chemistry tell of curiosity-driven discoveries. In the late 18th century, French chemist Louis-Nicolas Vauquelin isolated chromium from Siberian red lead. By the 19th century, advances in industrial chemistry paved the way to refined chromium(III) salts, including nitrate forms. Scientists found that the trivalent chromium ion produced vivid colored compounds, which inspired new research in pigments and tanning. As chemical understanding deepened, production methods evolved beyond basic precipitation and crystallization. Today’s Chromium (III) Nitrate Nonahydrate crystallizes from decades of refinement, made far purer and more reliable by better purification and quality controls demanded by manufacturers.
This bright, violet-to-deep purplish crystalline solid has attracted chemists, industrial designers, and researchers for its stability and solubility. Its IUPAC name is Chromium(III) nitrate nonahydrate, with the formula Cr(NO3)3·9H2O, and it captures attention on lab shelves with its intense hue and relatively high density. Availability spans lab-grade reagents, industrial supplies for glass production, and tailored research samples. Purchasing can range from grams for small syntheses to bulk orders for industrial application, often supplied with strict labeling on packaging for traceability. Producers stamp lot numbers, purity levels (sometimes 98% or higher), and handling instructions on every bottle or drum.
This salt shows a melting point around 60 °C, at which point it decomposes, releasing water and potentially nitrogen oxides. Highly soluble in water and ethanol, it produces striking purple solutions. The molecule holds nine water molecules of crystallization, accounting for the ‘nonahydrate’ suffix. Its crystalline structure allows for orderly stacking, but the hydrated form means it handles atmospheric moisture readily, leading to clumping if left open to air—something every chemist has witnessed when a forgotten jar cakes overnight. The nitrate ions contribute to its role as an oxidizer in specific scenarios, though not nearly as fierce as sodium nitrate or potassium nitrate.
Quality control agencies scrutinize purity, moisture content, and heavy-metal contamination. Commercial bottles often bear warnings about oxidizing hazards and corrosion. Manufacturers report minimum assay values, with reputable suppliers offering Certificates of Analysis. Those details matter for anyone in R&D or analytics, since impurities complicate results. Regulations in Europe, the U.S., and Asia set expectations: clear labeling for chemical hazard pictograms, UN number (UN2720), batch numbers, hazard statements regarding skin and eye irritation, and reminders about proper PPE during handling. For those of us who have ordered cases of this salt, a skim through the data sheet is not optional.
Preparation often means slow dissolution of chromium(III) oxide or chromium(III) hydroxide in cold dilute nitric acid. The trick is an even, controlled addition to reduce side reactions or the formation of insoluble hydroxy-nitrates. Industrial-scale methods start with ore-based chromium sources, upgrade them to pure oxide, and then rinse them through acidification tanks, often in stainless steel reactors. The process ends with chilling the solution and evaporating just enough water to coax out the vivid, glassy crystals, which are quickly filtered and stored away from air. To those with a DIY streak: lab preparation demands careful temperature and acid control, as chromium can pop out of solution fast, forming toothy crystals before you plan for it.
Chromium (III) Nitrate Nonahydrate reacts eagerly in the presence of ligands, forming a host of coordination complexes prized in inorganic chemistry research. Mix it with ammonia or ethylenediamine, and watch as the color shifts, marking the creation of chromium-amine complexes. Reduction reactions can convert the trivalent ion down to the more reactive chromium(II) species, while heating—whether deliberate or not—drives off hydration water and releases nitrogen oxides. Its nitrate group opens routes for nitrate-for-chloride exchange via reactions with hydrochloric acid, swapping out one anion for another, and allowing customization for downstream syntheses. In the presence of strong bases, chromium hydroxide may precipitate, sometimes complicating uses in less-controlled environments if pH drifts.
Over the years, the reagent has picked up several aliases in catalogs and textbooks alike. Common synonyms include Chromium trinitrate, Chromium nitrate nonahydrate, and chromic nitrate. Some catalogs dust off old Latin nomenclature—Chromii nitras nonahydras—but the key identifiers remain its CAS number (7789-02-8) and its chemical formula. Major suppliers might brand bottles as “Certified Reagent Grade” or “ACS Reagent” if the material fits certain purity criteria. That difference matters for academic labs publishing research or manufacturing labs tracing precursors for compliance.
Handling this compound raises safety flags mostly because of its oxidizing power and mild toxicity. Skin, eyes, and lungs require protection; contact leads to irritation and, at higher concentrations, tissue damage. Laboratories should lean on fume hoods and splash goggles for open handling. Industrial settings install ventilation, automated weighing, and proper waste streams to reduce risk. Chromium(III) itself is less toxic than its hexavalent sibling, but that distinction slips away if dust or solution splashes aren’t contained. Regulators limit exposure based on time-weighted averages, so handling protocols focus on minimizing contact through engineered controls and solid training. I’ve worked in glass facilities where a dedicated hazard log tracked every nitrate shipment—don’t underestimate audit compliance in this area.
Glass coloring stands out as a prominent use, creating deep green and blue hues. Ceramics benefit from its role as a glaze component, bringing both color and catalytic properties. Analytical chemistry labs use chromium(III) nitrate as a standard oxidizing agent and as a source of trivalent chromium for reactions requiring well-defined purity. In organic synthesis, the compound catalyzes oxidation or enables creation of special chromium complexes for research. Textile industries have harnessed it for mordanting and dye-fixing, though eco-regulations now restrict some uses due to downstream impacts. Students and professional chemists alike revisit its reactions for classic undergraduate experiments or to seed crystal gardens as visual demonstrations of coordination chemistry.
R&D teams turn to Chromium (III) Nitrate Nonahydrate for catalyst development, materials discovery, and thin-film deposition. I’ve seen teams combine it with other metal nitrates to develop mixed-oxide catalysts, hunting for greener options in emissions control. Surface science labs use its compounds as precursors for electrodeposition or sol-gel films, hoping to coax better corrosion resistance or new electronic properties. Environmental researchers keep an eye on trivalent chromium’s behavior in soil and water—tracking how nitrate ligands shift mobility and uptake by plants or microbes. Each year, publications describe new complexes and nano-materials that draw upon this compound as a reliable source of chromium in a form that dissolves easily and links into larger molecular structures without fuss.
Science has measured chromium(III) as less toxic than chromium(VI), but research digs deeper. Inhalation studies on dust and solution exposure have shown that chronic handling without protection can still cause respiratory and dermal issues. Recent research targets the long-term fate of trivalent chromium in the environment, as nitrate partners can leach through soil, and under specific conditions, bacteria might oxidize chromium(III) back to chrome(VI), introducing regulatory headaches. Animal studies indicate low acute toxicity for oral intake, but long-term accumulation could mess with kidney and liver function. Workers handling this compound regularly deserve robust air and wipe-down monitoring.
Trends in specialty glass manufacturing and catalytic research keep demand steady for this classic compound. As researchers sidestep chromium(VI) for health reasons, the focus lands on trivalent sources like Chromium (III) Nitrate Nonahydrate, aiming to unlock new chemistries that run cleaner and safer. Laboratory automation has begun to trace purity and performance in real time—a huge leap for consistent outcomes. Regulatory authorities push for reductions in environmental release, so process design in factories tilts toward closed-loop recycling or complete conversion. Education leans into this salt’s chemistry for teaching coordination, precipitation, and redox reactions, ensuring each new generation of students gets hands-on with something both visually striking and conceptually rich. The story of this compound keeps threading through modern labs and workshops—a reminder that classic chemicals rarely fade from relevance, even as science grows more precise.
Chromium(III) nitrate nonahydrate sounds like something you need a lab coat just to pronounce, but it shows up in more practical corners of the world than most folks imagine. I’ve spent time in both classrooms and industry shops—seeing the different faces this stuff wears. Out in the real world, it isn’t just a jar on a chemist’s shelf. It gets right into processes that turn raw materials into finished products we use daily.
One of the big spots this compound turns up is in making chromium-based chemicals. Think of it as a key ingredient in many synthetic routes—kind of a shortcut for chemists to get the exact form of chromium they need. For instance, the pigment industry sees heavy use for chromium(III) compounds because they give rich green tones. Those deep colors in glassware or ceramics often start with just this kind of raw material. It’s a building block, not just a bystander.
People love their metal goods shiny and tough. Chromium(III) nitrate shows up here, too, especially in electroplating and surface treatment. Factories use it as a precursor in processes that finish off metal parts—from auto trim to tools—giving them strength and a sleek, corrosion-resistant shell. Spending time in a small tool workshop, I’ve seen best results come from pre-treatments that involve chromium solutions. The stuff doesn't just help the finish look good. It keeps it that way after countless uses.
Chemical reactions need helpers, and chromium(III) nitrate stands out as a starting point for catalysts. In some cases, researchers make complex catalysts for organic synthesis directly from this compound. These catalysts help pharmaceutical and agrochemical companies run reactions cleaner and at lower energy costs. Better catalysts mean greener production with less waste, which everyone can get behind—especially since tighter environmental rules have pressured companies to rethink their processes.
Over my years running lab classes, I noticed how instructors keep chromium(III) nitrate on their shelves as a staple for teaching basics like transition metal chemistry. It’s easy for students to handle and gives bold color changes in reactions, making abstract lessons stick much better. Safe classroom use for experiments like qualitative ion tests or simple coordination reactions helps new generations of scientists learn with their hands, not just their heads.
Of course, nothing about industrial or laboratory chemicals is simple these days. Chromium compounds, including this one, come with a safety list. Proper storage stops leaks and dust, gloves and eyewear block skin and eye contact, and keeping it away from foods is a no-brainer. On the environmental side, nonahydrate forms are much less hazardous than the chromium(VI) compounds once common in industry. Still, disposing of any chromium waste means following clear rules—nobody gets a free pass to dump leftovers down the drain. Smarter handling keeps everyone healthier and the environment cleaner.
Chromium(III) nitrate nonahydrate might hide behind a technical-sounding name, but it holds value in the worlds of making, teaching, and innovating. As industries push for safer and greener methods, more research digs into substitutes and recycling, so this compound’s role won’t stay fixed forever. Still, it remains a practical, reliable piece of the puzzle for now—one worth understanding beyond the science and safety sheets.
Chromium (III) nitrate nonahydrate looks like a complicated name, but in a lab, it’s a familiar staple. Its formula, Cr(NO3)3·9H2O, spells out one chromium ion tied to three nitrate ions, all wrapped up with nine water molecules. Students and scientists rely on this chemical for tests, experiments, and making other chromium compounds. This hydration level makes things easier, providing a predictable starting point for calculations—no need to wonder how much water might sneak in from the air.
Many metalworking pros will tell you, this nitrate finds use in chrome plating and as a reagent for analytical chemistry. You might see it dissolved in a beaker, turning the solution a bright purple shade. That color, along with its makeup, proves useful for detecting or separating other elements. Chromium (III) compounds matter in pigments and catalysts as well. As an undergraduate, my first reaction with a transition metal salt involved weighing out this vivid purple crystal, making sure none clung stubbornly to the sides of the spatula. That experience taught me attention to detail—a quality you can’t skim over where chemicals are concerned.
Anyone working with chromium compounds learns quickly about safety. Hexavalent chromium, which shows up in some industrial wastes, can threaten health and the environment. Chromium (III), like in this nitrate, is far less toxic but still deserves respect. Gloves and goggles don’t just sit on the shelf for decoration. Because the formula Cr(NO3)3·9H2O clearly tells us what we’re handling, spills and disposal decisions get easier. Government guidelines treat this and other chemicals seriously, reflecting real-world risks instead of downplaying them.
Platers, chemists, and even artists lean on reliable chemicals. Knowing exactly what’s in your jar means fewer failed experiments and safer workplaces. In specialty glassmaking and corrosion protection, consistency helps avoid expensive mistakes. But keeping detailed records goes beyond compliance—mistakes with numbers or labels quickly cost time and money. I’ve seen entire batches of lab samples scrapped over minor discrepancies; the formula avoids those headaches by standardizing what’s expected.
Schools and businesses can help by teaching not just what the formula is, but why it matters. Clear labels, up-to-date storage rules, and well-trained staff make for smoother, safer operations. As automation and digital inventories become more common, accuracy grows even more important. A single misplaced digit in the formula—mixing up the number of waters, for example—can throw off everything from cost calculations to safety data sheets.
Promoting safe, smart chemistry doesn’t end with one compound. Efforts to track usage, innovate safer alternatives, and recycle still matter, especially where scale grows. Good science starts with correct information; chromium (III) nitrate nonahydrate’s formula reflects that precision. In my own experience, small details like this set the stage for breakthroughs or mistakes.
Chromium (III) nitrate nonahydrate isn’t just another salt tossed in the back of a supply closet. Anyone who’s spent time in a lab knows it stains hands pink, triggers headaches if the lid’s left off, and chews through sensitive metals over time. Because it's often used in chemical syntheses and dye production, this compound shows up in university labs, research centers, and plating shops. Having handled countless jars in my own work, there’s no question: storing it right means keeping people and projects safe.
This chemical absorbs water from the air, so leaving a jar open long enough turns it into a sludgy cake. Worse, it reacts with metals and releases harmful fumes with heat. The safety data sheets spell out the risk, but the reality hits when someone spills it or forgets a container in a humid room. I’ve seen label ink run, glass jar lids fuse, and crust develop around the rim. Cleanup’s not simple, and mistakes linger for days. If you’re anywhere near it, you’ll want to know what not to do.
Keep it in tightly sealed glass containers. This isn’t negotiable. Plastic sometimes cracks or lets small amounts of moisture inside, and metal almost always reacts. Those old amber glass jars with fitted lids come out ahead every time. I’ve found that even minor lapses lead to clumped solid that takes chiseling to remove.
Store containers in a cool, dry, and well-ventilated area. Humidity spells disaster, so skip basements or overstuffed cabinets near sinks. I’ve seen well-meaning teams lose half a sample stash in a single weekend just because jars were left next to a steamy dishwasher. Shelving above shoulder height, away from sunlight and heat, cuts down on accidents and keeps labels readable. Some labs use desiccator cabinets or even small dehumidifiers close to chemicals like this one; those efforts pay off.
Clear, legible labeling is more than a bureaucratic hoop to jump through. There was a near-mixup in an old shared lab when nitrate salts all got relabeled with the same marker. Good labeling includes the chemical name, date received or opened, and hazard warnings. A quick check on labels at the start of every shift lowers confusion during audits or emergencies.
Organizing chemical storage doesn’t just mean following a checklist. It’s a sign of respect for colleagues, students, and custodial staff. I once spent months in a building where people got careless, and the number of fatigue headaches and skin irritations climbed. Responsible handling extends to sharing information and walking new lab members through the process. A seasoned mentor would point out why you never pile nitrate containers next to acids or organic solvents. They’d demonstrate spill containment kits, point out emergency showers, and stress glove checks.
OSHA, the CDC, and international agencies echo this same advice on chemical hygiene. Their guidelines stem from decades of accidents and near misses—a few extra minutes spent securing a jar today could save an entire lab from disruption tomorrow. Experience can feel like an inconvenience, but stories of ruined experiments and minor ER visits turn that lesson into common sense.
Keeping a lab inventory up to date and reviewing storage protocols with fresh eyes each semester catches issues before they grow. Encouraging a culture where anyone can point out a risky setup, without fear of blame, helps. Chemistry happens because people respect their materials and each other. In my own routine, stopping to double-check lids and throw out damaged containers never felt wasted. Every secure shelf and accurate label helps turn a risky compound into just another safe, reliable part of science.
Chromium (III) Nitrate Nonahydrate turns up in classrooms, research labs, and a handful of industries. The pale purple crystals come with a batch of curiosity and concern. Safety sheets and chemical labels can spook anyone, but the daily realities of working with this stuff are more layered. In my time studying and working in industrial chemistry, I’ve seen how assumptions around “hazardous” chemicals can get twisted. It pays to stop, check reputable studies, and ask the awkward questions.
Plenty of folks have a gut reaction to the word “chromium.” Bad press follows the hexavalent kind—Chromium (VI). Erin Brockovich showed the world why that's worth fearing. The world of chromium compounds isn’t black and white, though. Chromium (III) Nitrate Nonahydrate contains the trivalent form. Chemically, it’s much less toxic to humans. Our bodies actually need trace amounts of chromium (III) for things like glucose processing. Toxicity emerges from dosage, exposure route, and chronic contact.
Inhalation, direct skin contact, or swallowing any lab-grade chemical should raise red flags. Chromium (III) Nitrate Nonahydrate causes skin and eye irritation, mostly because it’s acidic and the nitrate part can burn. Get it on your hands or inhale dust, and irritation follows. Swallow a large amount, and there’s risk of nausea or vomiting. Extended exposure, week after week, lacks strong evidence for cancer or organ damage—unlike hexavalent chromium.
Lab mice don’t love eating tons of the stuff, but the amounts causing sickness in studies sit way above what an average person could touch. The United States Environmental Protection Agency and the CDC both agree: chromium (III) compounds don’t push the same panic buttons as the hexavalent kind. Toxicologists see mild to moderate problems, with proper handling limiting any serious risk. Spills get cleaned with gloves and goggles because the nitrate increases fire risk when mixed with organic stuff.
My peers in wastewater management point to another angle. Dumping chromium nitrate into rivers or landfills adds nitrate pollution, which throws aquatic life out of balance. Chromium doesn’t vanish—it cycles. The trivalent form binds to soils, rarely running off, but the nitrate ions can set off algal blooms in lakes if nobody pays attention.
Caution pays off more than panic. Gloves, goggles, lab coats—these aren’t overkill, they’re bare minimum. Good training means no accidental mixing with fuels or acids. Students learn fast after they see a small spill fizz or smoke. Supervisors will keep inventories tight, order small amounts, and monitor students who are new to these handling rules. Industry veterans install fume hoods, even for low-to-moderate hazard compounds, to keep air clear.
Waste disposal hits most of the risk. My advice: Stick with approved chemical disposal channels. Don’t pour leftovers down the drain. Don’t treat environmental guidelines as red tape. That stuff matters—at work and at home.
Every chemical comes with a story, but facts and experience clear up the confusion. Chromium (III) Nitrate Nonahydrate deserves attention and respect. The “hazardous” label fits only in the right setting, under the right conditions. Genuine risks fade when people follow practices tested across generations of scientists and engineers. Doing the basics well matters more than horror stories or scare headlines.
Chromium (III) nitrate nonahydrate isn’t the sort of chemical that pops up in daily conversation, but it plays a quiet role behind the scenes in plenty of science labs and industries. The published solubility value in water stands right around 75 grams per 100 milliliters at 20°C. That’s a lot. This isn’t a compound that stubbornly sits at the bottom of the beaker. Mix it with water, and it vanishes fast, leaving a deep violet solution. Plenty of students get their first serious taste of “water-loving” compounds with this one.
Most folks might shrug at a solubility stat. I used to, before teaching chemistry labs and watching what actually happens when things dissolve—and when they don’t. If you try to dissolve too much of a less soluble salt like barium sulfate, you get a cloudy mess. Chromic nitrate, though, floods the solution with chromium ions. It’s convenient, sure, saving time and glassware headaches.
For anyone working in metal plating, textile dyeing, or the synthesis of catalysts, getting a full dose of chromium (III) ions into the solution is absolutely important. Less soluble alternatives often force you to adjust temperatures, play with agitation, or hunt for solvents better left on the shelf. Here, the numbers matter because they make the work possible, not just easier.
Plenty of substances with high water solubility keep both regulators and environmental engineers awake at night. With chromium (III) nitrate, the stakes are fairly high. It dissolves into drinking water sources in contaminated sites. In small lab-scale spills, problems tend to stay small. In industry, trace runoff hits surface water and spreads fast.
Most sources say that chromium (III) is less toxic than chromium (VI)—and that’s true. Still, elevated chromium levels can stress aquatic life and linger in sediments. I’ve seen teams struggle with wastewater treatment, fighting to keep heavy metal levels below ever-tightening state and federal goals. Solubility here isn’t just about dissolving powders for lab experiments. It warps into a water treatment headache or an environmental debate at city councils.
Good chemistry teachers hammer home the rule: “Dilution is not the solution to pollution.” That stuck with me. As easy as it is to get chromium (III) nitrate into water, pulling it back out takes engineering muscle—precipitation reactions, ion exchange, and constant monitoring of discharge. Regulatory bodies like the EPA set strict discharge limits, so industry and wastewater operators need to lean on science and practical routine.
Personal experience—and plenty of EPA incident reports—make clear that simple tools work best. Precipitate the chromium out with a base like sodium hydroxide. Filter, then analyze. Don’t just let it swirl down the drain. If more sites approached heavy metal runoff with this focus, it would go a long way toward easing public fears about chemical manufacturing.
For the chemical user, solubility is a blessing and a challenge. Fast-dissolving salts like chromium (III) nitrate cut down on processing time, while also demanding extra care for the environment. Whenever handling any water-soluble metal compound, it makes sense to think beyond the lab glassware and consider the next stop for those ions.
| Names | |
| Preferred IUPAC name | chromium(3+) nitrate nonahydrate |
| Other names |
Chromium trinitrate nonahydrate Chromic nitrate nonahydrate Chromium(III) nitrate 9-hydrate Nitric acid, chromium(3+) salt, nonahydrate |
| Pronunciation | /ˈkroʊmiəm θri naɪˈtreɪt ˌnəʊnaɪˈhaɪdreɪt/ |
| Identifiers | |
| CAS Number | 7789-02-8 |
| Beilstein Reference | 3613774 |
| ChEBI | CHEBI:78053 |
| ChEMBL | CHEMBL1201594 |
| ChemSpider | 21169618 |
| DrugBank | DB14545 |
| ECHA InfoCard | ECHA InfoCard: 03e53eaf-5f0e-4136-8dac-8450396b05ba |
| EC Number | 231-861-7 |
| Gmelin Reference | 77819 |
| KEGG | C14847 |
| MeSH | D014003 |
| PubChem CID | 24574 |
| RTECS number | GB6300000 |
| UNII | 9G2L3HSQ2V |
| UN number | UN2720 |
| Properties | |
| Chemical formula | Cr(NO3)3·9H2O |
| Molar mass | 400.15 g/mol |
| Appearance | Dark purple to reddish crystals |
| Odor | Odorless |
| Density | 1.85 g/cm³ |
| Solubility in water | Very soluble in water |
| log P | -4.0 |
| Vapor pressure | <0.1 mm Hg (25 °C) |
| Acidity (pKa) | -3. |
| Basicity (pKb) | -6.6 |
| Magnetic susceptibility (χ) | +1460.0e-6 cm³/mol |
| Refractive index (nD) | 1.548 |
| Viscosity | Viscous liquid |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 231 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -604.0 kJ/mol |
| Pharmacology | |
| ATC code | A12CC04 |
| Hazards | |
| Main hazards | Oxidizer, harmful if swallowed, causes serious eye irritation |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05,GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | Causes serious eye irritation. |
| Precautionary statements | P261, P264, P273, P280, P301+P312, P302+P352, P305+P351+P338, P312, P332+P313, P337+P313, P362+P364 |
| NFPA 704 (fire diamond) | 2-0-2-OX |
| Lethal dose or concentration | LD₅₀ Oral - Rat - 325 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 > 5,000 mg/kg |
| NIOSH | NOEC1001000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Chromium (III) compounds: 0.5 mg/m³ (as Cr) |
| REL (Recommended) | REL: 0.5 mg/m³ |
| Related compounds | |
| Related compounds |
Chromium(III) acetate Chromium(III) chloride Chromium(III) fluoride Chromium(III) iodide Chromium(III) oxide Chromium(III) sulfate Chromium(III) potassium sulfate |
