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There’s a rich history behind 2,6-pyridinedicarboxylic acid, a compound often found in the stories of both fundamental chemistry and applied research. My first experience with it came during a graduate lab project focused on coordination chemistry, where we needed organic ligands able to stabilize metal ions in complex reactions. This acid, with its stable pyridine ring and carboxylic groups, turned out to be a regular feature in published syntheses as far back as the early 20th century. Early chemists valued it for these qualities, and its derivatives have surfaced again and again, from dye manufacture to complexometric titrations. What marked its progress through history wasn’t flashy innovation but a steady record of versatility and reliability in organic and inorganic laboratories.
The appeal of 2,6-pyridinedicarboxylic acid comes straight from its basic structure. Fundamental and clear-cut, this molecule sports a pyridine core—a nitrogen-containing aromatic ring—decorated with two carboxylic acid groups at the 2 and 6 positions. This setup delivers unique binding opportunities for metals and forms the backbone for many specialized ligands. The product sits solid, often offered as a crystalline powder that holds up to standard bench handling. Over the years, I’ve seen research groups and industry teams alike find utility in its acidic strength, aromatic stability, and the ease with which its core structure morphs into derivatives. Whether making a novel catalyst or a pharmaceutical intermediate, this acid is a foundation-builder, not just a reagent.
At the bench, you’ll find 2,6-pyridinedicarboxylic acid a white to off-white crystalline substance—dense, grainy, sometimes clumpy depending on storage. It dissolves modestly in water and with effort in polar organic solvents. The melting point hangs high, reflecting its aromatic system and the two stiff carboxyl groups. Chemically, it holds up well to moderate heat and can participate in both acid-base and redox chemistry. One striking feature is its ability to chelate metal ions, drawing on both the pyridine nitrogen and the adjacent carboxylates; this quality makes it a tool for building metal complexes with specific, task-oriented architectures. There’s not much flashiness here, just stable, predictable performance—exactly what you want in a core organic molecule.
A bottle of 2,6-pyridinedicarboxylic acid should arrive with clarity about its purity, typically measured in the high nineties or above for research use. Labels tell you its molecular weight and the best storage conditions—usually a cool, dry shelf away from sunlight and moisture. Lab-grade suppliers provide details on lot testing so that researchers can replicate results and maintain quality control. As a hands-on chemist, I value clear technical specifications because they reduce the troubleshooting time that often plagues synthetic work when reagents don’t perform as expected.
Industrial and academic labs prepare 2,6-pyridinedicarboxylic acid using various synthetic routes, but most often through oxidation of 2,6-lutidine or related precursors. I’ve run oxidation reactions in similar contexts, and they tend to be straightforward in concept but sometimes fiddly in execution—yields swing based on the quality of the starting material and the precision of the reaction conditions. In some set-ups, manganese dioxide serves as an efficient oxidizer, helping pull hydrogens and encouraging the formation of those hallmark carboxyl groups. Purification can be a beast, requiring repeated recrystallization to knock out side-products and deliver that satisfying, crisp crystalline finish.
Once you have pure 2,6-pyridinedicarboxylic acid in hand, a world of possibilities opens up for chemical transformation. Its carboxyl groups serve as launchpads for amide formation, esterification, or transformations into acid chlorides. In my own synthetic work, I’ve found the molecule eager to play the role of ligand; metal salts grab onto the available nitrogen and carboxyl oxygens, forming robust complexes used in catalysis, analytical chemistry, or new materials research. Its aromatic core tolerates mild substituents at other positions, making it adaptable for unique molecular designs. There’s a reason synthetic chemists return to this acid—it’s flexible but reliable, allowing exploration without constant surprises.
In journals and catalogs, you’ll see 2,6-pyridinedicarboxylic acid under a handful of names. Dipicolinic acid is the one that first stuck with me from undergraduate textbooks. Other labels include quinolinic acid (confusingly, although that more strictly refers to a positional isomer) and pyridine-2,6-dicarboxylic acid. Trade catalogs tend to go with CAS numbers or plain IUPAC nomenclature, avoiding brand names. Consistent naming really matters to avoid misidentification, especially when reaching for this compound across different disciplines or countries.
Anyone who’s spent enough time in a laboratory recognizes the importance of working safely, especially around powders like this with acidic properties. 2,6-Pyridinedicarboxylic acid has a low-to-moderate hazard profile; it can cause environmental harm with careless disposal and mild irritation on skin or eyes. Good practice demands gloves, eye protection, and careful weighing in a fume hood if dust clouds threaten. As green chemistry principles creep further into teaching and research, the focus shifts to minimizing waste and exposure wherever possible. Safety data sheets urge precautions not just for personal health but for environmental responsibility, and these standards should guide every bench procedure involving this compound.
Much of the real-world value of 2,6-pyridinedicarboxylic acid lies in how laboratories and industries harness its coordination properties. Microbiologists know it as a significant signaling molecule within spore-forming bacteria, especially Bacillus species. The acid’s ability to bind metals like Ca(II) makes bacterial spores resistant to heat and desiccation, a natural marvel that’s inspired research into sterilization and food safety. In my own research, I’ve seen the compound serve as a scaffold in pharmaceuticals and as a chelating agent for environmental testing. Materials scientists, in turn, use complexes of this acid to design metal-organic frameworks (MOFs), which promise breakthroughs in gas storage and selective catalysis. Across fields, its reputation as a dependable ligand and building block continues to grow.
Innovation often rides on the back of reliable building blocks. 2,6-Pyridinedicarboxylic acid features heavily in the hunt for new catalysts, specialty polymers, and medical diagnostics. Research journals document a steady march of derivatives, with scientists tweaking side groups or adding functionality to improve binding, reactivity, and selectivity. I’ve read reports of researchers developing selective sensors for transition metals based on this acid’s affinity, providing cheaper, faster analysis for polluted water or industrial feedstocks. The push into green chemistry brings new focus to modifications that limit toxicity, increase biodegradability, or streamline recycling of metal complexes.
No review of an industrial or laboratory chemical is really complete without an eye toward toxicity and environmental impact. Studies on 2,6-pyridinedicarboxylic acid have generally found low acute toxicity, but chronic exposure or mishandling remains a concern—especially given the compound’s environmental persistence. As a molecule that often finds itself in soil or water systems, its fate and effects on non-target species demand continued vigilance. Regulatory agencies in some regions ask for transparency regarding handling and waste disposal, and research teams are expected to examine effects at both organismal and ecological levels. Newer analytical techniques allow ever-lower detection thresholds and better biomonitoring, building confidence in claims of safety but also raising the bar for responsible use.
Looking ahead, 2,6-pyridinedicarboxylic acid doesn’t show signs of fading into chemical obscurity. Its established utility in spore biology, catalysis, and coordination chemistry will only expand as researchers discover new applications in energy storage, environmental remediation, and next-generation sensors. Academic initiatives keep turning up unexpected uses—from antimicrobial agents to gene regulation frameworks—by leveraging the molecule’s versatile skeleton. Continued R&D will likely focus on more environmentally friendly synthesis and recycling strategies, helping push this stalwart compound further into the era of sustainable chemistry. With a growing community of scientists and engineers dedicated to better, safer, and more effective materials, this acid will keep earning its place on chemical shelves around the world.
2,6-Pyridinedicarboxylic acid stands out in the world of specialty chemicals for a reason. Those who spend any time in laboratories come across this molecule often, especially in synthesis work. With its structure based on a pyridine ring carrying two carboxylic groups, it manages to pop up across research, industry, and environmental applications. I’ve seen firsthand how just a small bottle of this powder can lay the foundation for larger processes in drug development and advanced materials science.
This acid finds its way into coordination chemistry because it forms stable complexes with metals. Chemists use these complexes to study catalytic reactions and mimic natural enzymes, which improve our understanding of biological processes. While working in a lab focused on metal-organic frameworks, I relied on this compound to create crystalline materials with uniquely tailored properties for gas storage and sensing. It’s gratifying to see projects move from a beaker in the corner to experiments that address big questions about clean energy or climate monitoring.
2,6-Pyridinedicarboxylic acid also acts as a building block in pharmaceutical synthesis. During my postdoc, several drug candidates came together as a series of connected rings, and this acid showed up in a few key steps. Its functionality streamlines the design and tweaking of molecules that might become the next generation of antibiotics or therapeutic agents. This doesn't just happen behind closed doors in pharma labs—it makes a real impact on public health.
Sometimes this acid plays a quieter role as an analytical reagent. Water testing labs use it to determine the presence of certain metal ions. Its chemical grip helps catch trace metals in samples pulled from rivers and lakes, making it a small, unseen player in keeping drinking water safer. I remember assisting an environmental science class, and this single step in a detection kit helped students make sense of their complex local water samples.
Research groups tracking soil health also turn to 2,6-pyridinedicarboxylic acid. It interacts with minerals and organic matter, giving scientists insights into nutrient cycles and contamination. These small-but-powerful uses ripple out, supporting larger efforts in sustainable agriculture and pollution management.
Ensuring safe use and proper disposal has come up often in my own lab work. Like many organic acids, this compound can cause irritation and environmental harm if handled carelessly. Training students and staff to respect its hazards is a shared responsibility. We keep things straightforward: fume hoods, gloves, and clear instructions on labeling and storage.
On a bigger scale, chemical suppliers who provide this acid face tight regulations on purity and shipping. I have seen certification paperwork that tracks every gram from factory to end user, meeting both safety and environmental expectations. These steps aren’t just bureaucratic red tape—they matter to the people relying on the results. Trace impurities can distort research results or lead to false readings in environmental monitoring. Reliable sources and a commitment to transparency keep everything moving in the right direction.
2,6-Pyridinedicarboxylic acid remains a backbone for a lot of promising work, especially in green chemistry and public health. With smart handling, clear transparency between stakeholders, and respect for the risks involved, this simple molecule continues to support innovation across fields. Its impact stretches further than we often see at first glance—out of the lab, into the environment, and into the products and data we count on every day.
Science classrooms often toss around complex names, and "2,6-Pyridinedicarboxylic acid" sounds like one of them. Underneath, it's a chemical with a straightforward structure and real-world importance. The core idea—two carboxylic acid groups sitting at the 2 and 6 positions of a pyridine ring—speaks to the chemistry behind products we use and technologies that shape healthcare and industry.
2,6-Pyridinedicarboxylic acid, also called dipicolinic acid, has six atoms — five carbons and one nitrogen — forming a ring, known as a pyridine ring. Two -COOH groups sit directly across from each other, at the second and sixth positions. Chemists love this shape for its symmetry and predictable behavior during reactions. In practical terms, this structure means it latches tightly onto certain metals, helping bind, stabilize, or remove them—jobs that pop up everywhere from environmental laboratories to pharmaceutical factories.
Working as an engineer, I've bumped into this acid's usefulness often. In the realm of biotechnology, 2,6-Pyridinedicarboxylic acid forms a major chunk of bacterial spores. The natural world treats it as a shield, withstanding heat and UV radiation. That ties into medical sterilization, because the stubborn presence of these spores keeps us paying attention to the chemistry of disinfection. Hospitals and research labs rely on the molecule’s unique properties to develop stronger, safer sterilization strategies.
Chemists reach for this molecule during the separation of rare earth elements. Its structure grabs onto tricky ions that ordinary acids would miss. The precision and strength of this binding, drawn from the spacing of the carboxylic acids and the nitrogen in the ring, proves valuable in recycling metals or cleaning up contaminants in water. It's not just theory — published research in journals like Journal of Inorganic Chemistry backs up these claims, documenting the molecule’s stubborn grip on metallic ions and its role in advanced purification techniques.
The very binding power that makes 2,6-Pyridinedicarboxylic acid useful can also cause headaches. In wastewater, it may cling to metals that should remain, stripping the ecosystem of vital nutrients. This challenge nudges researchers to engineer “smart” resins and filters — technologies aimed at controlling where and how the acid works, building selectivity into cleanup processes. Manufacturers turn to real-time monitoring tools, using spectroscopic analysis and automation to track where and how these acids pop up along the process chain. Tight regulation makes sense when considering both worker safety and downstream water purity.
Sustainable chemistry needs building blocks like this to balance industrial power with environmental care. Emerging fields, from green electronics to advanced catalysis, see the value in reliable, reusable chelators. Academic teams in Europe and Asia have demonstrated that modifications to the pyridine ring can lead to new medicine candidates and longer-lasting materials. There’s an ongoing drive to fine-tune both the raw structure and the manufacturing methods, aiming for simpler waste streams and greener synthesis paths built around this molecule.
2,6-Pyridinedicarboxylic acid isn’t just a mouthful; it's a trusted tool in science and engineering. Its distinctive structure opens doors from sterilization to metal recovery. Practical challenges spur even smarter designs, and the constant drive for safer, greener solutions puts this molecule in the limelight of scientific progress.
People tend to get uneasy around the word acid, especially if it’s a chemical name straight from a lab supply catalog. 2,6-Pyridinedicarboxylic acid sounds just like something you wouldn’t want on your skin or near your food. Still, I’ve handled plenty of lab chemicals in my time, and not every compound with a scary-sounding name deserves a spot on the hazardous shelf.
This compound shows up mostly in research, medicine development, and chemistry classrooms. Universities and labs use it for some reactions or as an ingredient to create other molecules. A lot of paperwork and caution tends to paint every chemical as dangerous, but diving into the facts about 2,6-pyridinedicarboxylic acid helps clear the air.
Sifting through safety sheets and regulatory lists, 2,6-pyridinedicarboxylic acid doesn’t set off alarms like strong acids or solvents do. The chemical does not fall under lists for acute toxicity or carcinogens flagged by the Occupational Safety and Health Administration (OSHA), European Chemicals Agency (ECHA), or International Agency for Research on Cancer (IARC). From my experience, that’s the first thing most safety officers check. It also means the long-term risks have been probed by experts before it ever reached a classroom shelf or research bench.
Looking at material safety data, this acid may cause mild skin or eye irritation if handled carelessly. Breathing in the dust irritates nose and throat, much like flour or other dry powders can. Nobody wants a cloud of anything in their lungs. On a scale of real risk, it fits closer to table salt — don’t eat it, don’t rub it in your eyes, keep it in sealed containers the same way you’d treat pretty much anything you use in a lab. It’s not corrosive and doesn’t release toxic fumes when you mix it with water or air. Poison control databases and wildlife impact logs show nothing out of ordinary, so there’s little to worry about spills or runoff causing a rush for hazmat suits.
A chemical doesn’t need a skull-and-crossbones label to be treated with respect. I’ve seen cases where people skipped basic safety steps and ended up with rashes, coughs, or cleanup headaches because of basic accidents. Gloves and goggles take care of most of these problems. Labeling containers, good air flow, and not letting food near the workspace are standard advice for any lab, and they work just as well here.
Manufacturers and transporters follow regulations to keep things safe during storage and shipping. That keeps big spills from becoming a problem for the environment or neighborhoods. Sites like PubChem or European Chemicals Agency let anyone check the safety and regulations in plain language. As someone who’s taught chemistry to newcomers, I always encourage people to look at the most updated sheets and ask if anything looks unclear.
2,6-Pyridinedicarboxylic acid isn’t the sort of compound you’ll see on nightly news warnings. Used the way manufacturers and scientists intend, it’s about as safe as most cleaning products or garden chemicals. The risks show up with carelessness or in huge volumes, but common-sense habits make all the difference. Clear labels, reliable storage, gloves, and routine checks give peace of mind for users and bystanders alike. Being cautious with any unfamiliar chemical is wise. I tell students — knowledge, not panic, keeps everyone safe.
This compound shows up in labs and production facilities where folks are synthesizing specialty chemicals, electronics, or even targeting innovative treatments in pharmaceuticals. It doesn’t grab headlines like more notorious acids, but overlooking its care can spell trouble for the materials, the gear, and the people nearby.
From my days in the lab, I’ve learned that chemical storage can’t be treated as an afterthought. Left unchecked, even stable powders can degrade or spark issues impossible to ignore. A little moisture creeps in, and you get caking or slow decomposition. Once, in a cluttered storeroom, we lost an entire batch after a careless cap let in humidity. The hassle of cleanup and inventory loss still stings. Lessons like these drive home the point: chemical stewardship starts with the shelf where you park your container.
What works best for this acid is a dry, cool spot far from direct sun and heat sources. It doesn’t like big swings in temperature. Anyone who’s worked in an old warehouse knows how erratic thermostats can torpedo your best intentions. Digital monitoring isn’t a luxury—it’s a smart insurance policy.
Sealable glass or plastic vessels do the job, provided they’re clean and tight enough to keep air and water out. I’ve seen corrosion start on lids left half-screwed. Always label the vessels with hazard info and the date received—simple but often skipped steps.
Some folks dump containers together on a single shelf, thinking it saves time. In reality, crowding invites cross-contamination or accidental mixing. Set clear boundaries: acids go with acids, but make sure nothing reactive sits nearby. Stay away from metal shelving that could start tiny reactions if a spill happens. That’s a rule hammered home by safety officers everywhere.
Another misstep: skipping personal protection. Handling powdered acids without gloves or a mask can expose skin and lungs—problems that add up. Goggles and simple nitrile gloves make a world of difference and should wait by the shelf, not in a drawer across the room.
Regular checks keep surprises at bay. Mark the calendar and actually open the containers; look for clumps, color changes, or odd odors. Dispose of the questionable stuff according to hazardous waste rules—most local governments have clear guidelines for lab chemicals.
Folks in smaller outfits sometimes cut corners with makeshift shelving or old food jars. That might seem thrifty, but it’s penny wise, pound foolish; the repair bill for corroded surfaces usually outweighs the price of certified vessels. I’ve seen supervisors called in for audits after a cracked jar triggered an alarm. No one wants to tangle with emergency services over a preventable mishap.
Chemicals like 2,6-Pyridinedicarboxylic acid won’t cause chaos if treated with foresight. Keep containers sealed, climate steady, and storage separate from reactive neighbors. Quick cleanups, clear labeling, and consistent checks make for an atmosphere where problems rarely crop up. It takes less time and money than disaster recovery ever will. Smart practices pay off, for safety and for science itself.
Some folks treat molecular weight as just a number in textbooks. Truth is, it shows up in real lab work and product formulation. If you've ever poured out a white, crystalline powder labeled 2,6-Pyridinedicarboxylic Acid, you've probably glanced at its molecular weight. The number for this compound sits at 167.12 g/mol. Getting that weight right matters for far more than labels or calculations: every mole, every titration, and every recipe in your process depends on it.
Chemists know this molecule by a few names, like dipicolinic acid or DPA. Its main claim to fame? It's a key marker for bacterial spores, especially those from Bacillus and Clostridium, which play roles in both soil health and biodefense. Detection kits and biosafety researchers rely on this molecular weight to prep culture media, measure concentrations, or analyze residues in environmental samples. Inaccuracy at this stage throws off entire experiments. Nobody wants to redo overnight growth curves over a calculation slip.
The calculation isn’t magic. You lay out the atoms: C7H5NO4. That adds up like this: 7 carbons, 5 hydrogens, 1 nitrogen, 4 oxygens. Multiply the atomic weights:
Total: 84.07 + 5.05 + 14.01 + 64.00 = 167.13 g/mol (You’ll notice minor rounding in references, but it’s right in line with 167.12 g/mol you’ll see in databases like PubChem.)
Molecular weight isn’t just something you memorize for exams. I once prepared a buffer stock with the wrong calculation. It threw off the pH, made the whole student group question their glassware, and tanks precious research hours. In pharmaceutical prep, even a 0.5 g/mol miscount means dosing errors or failed quality control. If you work at a scale, that mistake multiplies fast, causing wasted materials and regulatory headaches.
Anyone can Google a number, but not all sources offer the same trust. Peer-reviewed chemical suppliers and government platforms like PubChem and Sigma-Aldrich keep their numbers straight, reviewing submissions and flagging errors. The chemistry community tends to call out mistakes quickly. Those with years at the bench and up-to-date regulatory training can usually spot an off-number just by looking at the chemical formula. Experience makes a difference.
Mistakes in calculations sneak in during late-night lab sessions or batch prepping under pressure. I keep laminated periodic tables around, use reliable digital calculators, and double-check with coworkers before any large-scale weighing. Building these habits saves time, money, and reputation—all things you can’t afford to lose in research or production environments.
So while the molecular weight of 2,6-Pyridinedicarboxylic Acid might sound like just a technical detail, those digits ripple across science and industry. Whether measuring bacterial spores or mixing new materials, accuracy here keeps the rest of the process on track.
| Names | |
| Preferred IUPAC name | Pyridine-2,6-dicarboxylic acid |
| Other names |
Dipicolinic acid Pyridine-2,6-dicarboxylic acid 2,6-Dicarboxypyridine DPA |
| Pronunciation | /ˌpɪr.ɪˈdiːn.daɪ.kɑːkˈsɪl.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 499-83-2 |
| Beilstein Reference | **136470** |
| ChEBI | CHEBI:28643 |
| ChEMBL | CHEMBL1077 |
| ChemSpider | ChemSpider ID: 10241 |
| DrugBank | DB04218 |
| ECHA InfoCard | ECHA InfoCard: 100.003.226 |
| EC Number | EC 246-129-2 |
| Gmelin Reference | 7779 |
| KEGG | C00347 |
| MeSH | D002932 |
| PubChem CID | 86 |
| RTECS number | UY9625000 |
| UNII | 00TWH8A5CM |
| UN number | UN2811 |
| Properties | |
| Chemical formula | C7H5NO4 |
| Molar mass | 167.12 g/mol |
| Appearance | White to off-white powder |
| Odor | Odorless |
| Density | 1.511 g/cm³ |
| Solubility in water | Slightly soluble |
| log P | -0.6 |
| Vapor pressure | 1.85E-7 mmHg at 25°C |
| Acidity (pKa) | 2.36, 4.43 |
| Basicity (pKb) | pKb = 10.11 |
| Magnetic susceptibility (χ) | -37.6e-6 cm³/mol |
| Refractive index (nD) | 1.640 |
| Dipole moment | 2.69 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 179.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -979.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1322.0 kJ/mol |
| Pharmacology | |
| ATC code | V03CX06 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. |
| GHS labelling | GHS07, GHS05 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H319: Causes serious eye irritation. |
| Precautionary statements | P261, P264, P270, P271, P272, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 2,1,1,0 |
| Flash point | > 265 °C |
| Autoignition temperature | 550 °C |
| Lethal dose or concentration | LD50 oral rat 2400 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 > 2000 mg/kg |
| NIOSH | SN2980000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.3 mg/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Quinolinic acid Dipicolinic acid Picolinic acid 2,3-Pyridinedicarboxylic acid 2,4-Pyridinedicarboxylic acid 2,5-Pyridinedicarboxylic acid 3,5-Pyridinedicarboxylic acid |
