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People started paying attention to pimelic acid in the mid-19th century, thanks to the classic organic chemists unraveling dicarboxylic acids. Pimelic acid isn’t flashy like citric acid or oxalic acid, but as part of the straight-chain dicarboxylic acids, it pulled its weight in foundational work. Over time, researchers kept circling back to it for synthesis routes and as a model for chain-length effects in biochemical pathways. In my early days working in a university lab, we’d joke that pimelic acid never made headlines, but we couldn’t get through a semester’s research rotation without running into its derivatives or using it to test a catalyst’s range. Its quiet durability says something about chemistry: the real utility often outlasts the trends.
In solid form, pimelic acid feels grainy, sometimes a little sticky in humid air. It melts somewhere just shy of 130°C, right between its shorter and longer cousins. It dissolves in hot water pretty well and blends into ethanol or acetone after a bit of stirring. Its chemical formula looks neat on paper: C7H12O4. The structure, with its two carboxylic acid groups tethered by a five-carbon chain, makes it more flexible than the lower dicarboxylic acids and slightly heavy but approachable for chemical transformations. In the storeroom, you recognize its faintly sour, fatty scent if you’ve spent enough years opening the same brown bottles. Where a chemist sees two reactive ends aching for coupling, the practical side sees a building block that doesn’t argue with the rest of the synthesis.
Most people working with pimelic acid focus on purity over fancy labeling. Reliable sources report it between 98% and 99% pure. Labels warn about irritant properties, so wearing gloves and goggles is the kind of baseline care without which you don’t get far in a wet chemistry job. Documentation covers melting point, molecular weight, water-solubility, and sometimes even details like residue on ignition for those making salts or polymers. Still, what matters most is consistency—a bottle from today needs to match the stuff used ten years ago, or else you waste days on troubleshooting reactions.
Early chemists prepared pimelic acid through oxidation of cyclic ketones or alkanes, sometimes by nitration routes involving adipic or suberic acid. In my grad school years, the lab stuck mostly to oxidizing cycloheptanone or heptane using methods developed before WWII, upgraded with modern oxidizing agents to cut out the mess and keep yields consistent. Today’s processes have become greener, swapping out harsh chromates and permanganates for more selective oxidants when possible. Biotechnological approaches edge in as well, with engineered bacteria breaking down amino acids or odd-long-chain hydrocarbons, but large-scale work still leans on reliable old oxidative chemistry. Getting a clean, crystalline crop still takes patience, time, and the occasional curse at stubborn filtration if you rush the cooling phase.
What keeps pimelic acid circulating through chemical research isn’t just its own structure; it’s what others can coax out of it. Those carboxy groups spawn esters, amides, and salts with ease, making it a backbone in flavor chemistry, polymer design, and even medical research. One of my colleagues once chronicled weeks spent tweaking dialkyl pimelate synthesis just to get plasticizers for an aerospace application. With decent solubility and willingness to react, pimelic acid doesn’t make chemists fight for its attention. You see hydrogenation, halogenation, and simple reductions all work out without major fuss, and the intermediates feed into bigger molecules with minimal purification drama.
Ask a few chemists about pimelic acid, and names like heptanedioic acid, 1,5-pentanedicarboxylic acid, or just plain “pimelate” come up. Catalogs, patents, and journal articles still juggle these synonyms. For anyone ordering, citing, or cross-checking hazards, the alternate names lead to confusion if you’re not careful. In my experience, having a mental crosswalk between names saves days of searching for the right safety data sheet or tracking down obscure literature, especially since suppliers sometimes hedge between nomenclature depending on the language of origin or decade the label came from.
There’s nothing especially sinister about pimelic acid, but taking shortcuts in handling powders tends to backfire. Inhaled dust triggers throat irritation and sometimes headaches—something I learned after a hurried spill cleanup. Contact with concentrated solutions stings, and lingering powder on gloves can burn unnoticed skin patches. The rule in our lab stays clear: keep it off your skin, cap containers immediately, and don’t get lazy with ventilation. Agencies like OSHA and the European Chemicals Agency lay out guidelines more as preventive reminders than red tape. Simple protective kit, reasonable ventilation, and avoiding food in the acid-handling zone covers most bases. Waste needs separate neutralization, but most of it doesn’t class as hazardous unless you let it pile up in stray corners.
The first time I realized pimelic acid’s reach, it surprised me. What began as a reagent in polymer labs soon made its way into food flavoring chemistry, due to its moderate, acidic profile that helps craft esters for fruity notes. Pharmaceuticals folks work it into synthetic pathways for antibiotics and precursors to active compounds and even to anchor complex molecules used in diagnostics. Early research into nylon variants still banks on pimelic acid and its derivatives, although petroleum-sourced adipic and sebacic acids tend to crowd it out at scale. There’s a new twist: bioplastics and renewable-based polyamides open the door for mid-chain dicarboxylic acids as linking units.
Academic and industrial labs treat pimelic acid as a teaching tool for chain-elongation, reactivity, and energetic studies. In recent years, bioengineers spend long nights pushing metabolic pathways in E. coli and yeast to ramp up biosynthesis, betting on lower energy, less hazardous feedstocks. Materials scientists keep probing its role in novel copolymers or biodegradable plastics, particularly as design requirements get more stringent and environmental regulations step up. In my own project years ago, we built metal-organic frameworks using pimelate linkers, tracking how subtle changes in the spacer’s length and flexibility shaped gas sorption. Finding those functional sweet spots takes both luck and knowing which experiments to chase after failure. It’s never glamorous, but the persistence pays off in odd but useful discoveries.
Long-term, pimelic acid’s hazard profile doesn’t alarm regulators or research safety committees. Studies on rats and aquatic models point out only mild acute toxicity at very high doses, with reversible local irritation more common than lasting systemic harm. Despite that, repeated pours down the sink or careless handling in tight spaces can aggravate asthmatics or sensitive folks. My advice comes from experience—take everyday irritant safeguards seriously, prevent waste from spreading, and respect accumulations in confined workspaces. More granular research focuses on downstream breakdown products, ensuring ecological impacts get flagged before large-scale synthetic routes hit industrial phase. Following regulatory disclosures and new hazard assessments remains worth the time.
The push for sustainable chemicals puts new attention on “forgotten” intermediates. Pimelic acid, with its tractable synthesis from biological sources and tunable properties, fits the emerging narrative of green chemistry. Technical advances—like new microbial cell factories or catalysts that skip over the harshest reagents—create openings for increased production without the waste of legacy approaches. Next-gen polymers, alternative fuels, pharmaceutical tailoring, and new diagnostic agents all keep pimelic acid on the map, despite louder competition. The molecule never carries the prestige of household names, but as people in research know, dependable compounds form the backbone of real progress. Pimelic acid will keep showing up in lab notebooks and product pipelines as long as the world’s appetite for innovation and practicality continues to grow.
Pimelic acid sounds like something tucked away in a chemistry textbook, but it actually plays a bigger role than most people realize. Every time I dive into how these acids get used, I’m struck by how many products around us depend on chemicals most of us could barely spell. Pimelic acid is one of them. So, what’s it for, and why should we care?
Pimelic acid isn’t a household name, but nylon certainly is. Making nylon relies on a family of chemicals called dicarboxylic acids, and pimelic acid lines up right in the middle of that family. Chemists use it as a building block to create nylon 7, which lands in fibers, toothbrushes, industrial parts, and plenty of those everyday things we hardly notice. People tend to talk about recycling plastics; fewer folks ever wonder where the original ingredients come from. If manufacturing runs short of key building blocks like pimelic acid, all this production slows or stops. Supply chains ripple when someone can’t secure a simple ingredient.
Whenever I research medications, I’m reminded that a lot of the science traces back to surprisingly basic chemicals. Pimelic acid serves as a starting material for producing some drugs. Take antibiotics and some anticonvulsants—these depend on a web of reactions that often begin with small core molecules. Pimelic acid’s unique structure makes it handy for transformations most other acids can’t provide. For people needing those medicines, it’s more than just a step in the process—access hinges on steady supplies of every ingredient in the chain.
In research, pimelic acid occasionally shows up in stories about metabolism and enzyme work. Scientists can use it as a probe or a reference point to figure out how certain organisms process fats and proteins. If you study rare inherited diseases, odd bits of dicarboxylic acids like pimelic keep popping up in discussions. They turn into clues for understanding metabolic errors in human bodies. Not every discovery makes front-page news, but each piece adds something to what doctors and researchers eventually use in health care conversations.
I care about what goes into products I buy and what ends up in soil and water. Pimelic acid production pulls from petrochemicals, and the industry leaves a footprint. Each chemical factory handles waste and emissions a bit differently. Regulatory agencies keep eyes on that. Right now, more companies try developing biological processes—using microbes to make acids like pimelic out of plant sugars instead of oil. Switching to renewable sources and cleaner methods matters. Shortcuts don’t last, so working on cleaner production lines makes sense for business and for community health. The more we see industry push for renewable starting materials, the better it will be for every person living downstream or downwind.
Pimelic acid feels like a chemical name most people have never thought about. It crops up in biochemistry, tucked in with molecules that help run the show in our cells. This seven-carbon dicarboxylic acid helps set up building blocks for life in plants and bacteria. Still, the question matters: should humans worry if this compound lands in supplements, personal care, or food?
It's normal to feel a touch cautious about acids in general. Most folks don’t want to put their skin or health at risk from something that sounds straight out of a lab. Pimelic acid appears in trace amounts in nature, including a few food plants. Most people won’t come across large doses at the grocery store, pharmacy, or even in cleaning products. Production mainly stays confined to specialized industrial use or as a chemical intermediate—think research, not mass market shelves.
No solid data points to pimelic acid as a danger to human health in amounts encountered through diet or environment. Animal testing gives us part of the picture. Research published in PubChem and confirmed through the European Chemicals Agency reports very low acute toxicity in rodents. No evidence hints at the compound being mutagenic or carcinogenic. Testing hasn’t shown disruption in reproductive functions or allergy reactions on contact. The Environmental Protection Agency doesn't list pimelic acid in priority risk groups.
Regulatory bodies in the United States, Europe, and Asia keep a tight watch on chemicals slated for use near people. If a company tries to add pimelic acid to food or cosmetics, they need proper safety data to back things up. Regulators want to know about breakdown processes in the body, long-term effects, and environmental consequences before clearing any new use. This oversight has kept accidents low with acids and similar chemicals for decades.
Even with a good safety record in lab environments, the risk never drops to zero. Accidental spills or improper handling can irritate skin, eyes, or airways. Lab workers need gloves, ventilation, and information to keep exposures in check. It’s the same story for most acids and strong bases. I’ve learned by working in a research lab—attention, practice, and safe storage keep people protected.
As new uses for pimelic acid come to market, companies could publish test results and independent safety reviews online for anyone to read. Giving the public clear, honest updates on what these chemicals do, and where they end up, breeds trust. Modern technology gives every company a shot at traceable, transparent supply chains—people want to know where substances come from, and what risk or benefit comes with each ingredient.
Molecules like pimelic acid enable important work behind the scenes, building blocks for pharmaceuticals or specialty plastics. Most people have little to fear as long as scientists and regulators understand the risks and enforce clear guidelines. Responsible innovation and public access to research offer better protection than silence or secrecy ever could. Open science, communication, and respect for established limits can answer health questions before they become public worries.
Most chemistry classrooms don’t dwell on pimelic acid, but this seven-carbon dicarboxylic acid holds its own story. Its chemical structure, HOOC-(CH2)5-COOH, spells out two carboxyl groups stationed on opposite ends of a five-carbon chain. What makes this chain different isn’t some headline-grabbing property, but the simple fact that the arrangement builds a bridge between the world of short-chain acids and complex molecules.
While the formula doesn’t impress right away, its backbone opens doors in organic synthesis labs. Chemists see in pimelic acid a starting point that comes with both bite and length. The seven-carbon chain delivers flexibility; its carboxyl edges create reaction hotspots. This means pimelic acid can serve as a scaffold molecule in ring-closure steps, creating new compounds that might build towards pharmaceuticals, flavors, or specialty materials.
If you picture it visually, there’s a stretch of five carbon atoms between two carboxylic acid groups, each group able to react with other molecules. The carboxyl clusters act like magnets in water, giving pimelic acid decent solubility and fueling its involvement in biochemistry.
People often overlook minor players in chemistry, but there’s a reason pimelic acid matters. Human metabolism brushes against pimelic acid’s path. In fact, the body’s effort to break down some amino acids brings it close to pimelic acid’s territory, especially in the synthesis of lysine. Mistakes in these pathways can hint at metabolic diseases, so understanding the molecular setup of pimelic acid helps researchers spot problem points.
Synthetic chemists also keep a stash nearby for building block work. Ring systems in drugs and plastics sometimes demand a chain of just this length — too long or too short and the reaction slams shut or stalls out. Pimelic acid steps in, reacts at both ends, and builds out new shapes that rigid molecules can’t handle. The hands-on difference speaks for itself in any well-lit synthesis bench.
Production volume has never matched that of its shorter cousins like succinic or adipic acid, but pimelic acid’s niche use still spurs talk on cost and sustainability. Today, most production leans on petrochemical sources. Researchers want to push that toward greener options, eyeing biosynthetic routes in modified bacteria. I remember seeing pilot experiments where E. coli, coaxed by genetic tweaks, started churning out seven-carbon dicarboxylic acids from simple sugars. Scaling up proved tricky, with yields swinging up and down, but the promise was real.
From a regulatory standpoint, the simple structure offers clarity. It’s not flagged as highly toxic, but its relatives in the dicarboxylic acid family have been studied for environmental buildup. Efforts in green chemistry revolve around keeping waste streams clean — using catalysts that cut out solvents, squeezing more product from fewer steps, or making sure unused acid loops back into production.
Pimelic acid’s skeleton might look mundane at first, but its utility shows up across chemistry and life sciences. While you won’t find headlines or major industrial fortunes riding on it, the seven-carbon chain continues to offer a hand in experiments, product development, and understanding human metabolism a little better. Chemistry often works this way — small pieces, quietly supporting big changes.
Anyone who’s worked in a chemical storeroom knows the difference between a tidy shelf and a potential hazard. Pimelic acid has a role in various research and industrial fields. Experience teaches the value of respecting chemical properties, and this applies to seemingly simple organic acids as much as it does to more dangerous reagents. A careless approach to storage risks mess, wasted investment, and potential harm.
Pimelic acid comes as a white crystalline solid, not terribly volatile or explosive. Even so, it deserves respect. Heat or moisture can influence many organic acids, leading to slow changes that reduce purity over time. Impurities in stored chemicals can put research work or quality control at risk. Excess humidity tends to cause clumping or partial dissolution, sometimes even chemical breakdown. I’ve seen containers ruined just because someone left a cap loose after use.
Pimelic acid doesn’t have a strong odor, so accidental spills aren’t obvious until the mess has spread. Like many carboxylic acids, it’s stable under normal lab conditions, but that stability drops if it picks up contaminants or absorbs water from the air. This matters for anyone hoping a bottle will last through several projects.
Room temperature storage works for pimelic acid, provided fluctuations are avoided. Direct sunlight raises the temperature in storage cabinets, and light can accelerate degradation for some compounds, even ones that seem stable at first glance. Avoid sunny windows, radiators, or other heat sources. A cool, shaded storeroom or a designated cabinet away from light saves a lot of headaches. It’s not about freezing the sample, just giving it a consistent, moderate environment.
This kind of acid absorbs moisture easily. Keep containers tightly sealed, preferably using screw caps with a good liner. Every time the jar opens, it has another shot at grabbing water molecules out of the air. A silica gel packet inside a secondary container cuts down on moisture drifting in. Watch out for old stoppers or cracked lids—these turn a stable product into a frustrating mess.
Don’t mix tools between bottles. Cross-contamination, even at low levels, introduces new variables and ends up costing time chasing mysterious results. Clean scoops and spatulas help keep research reliable and prevent headaches down the line. Mark containers clearly with dates of opening, and rotate stock regularly—old supplies turn suspect well before visible changes show up.
Proper protective gear goes without saying, even for low-toxicity solids. Gloves protect not just fingers but also avoid introducing oils into the container that could foul future uses. Powder spill cleanup works best using a damp cloth (with gloves on) instead of sweeping. Accidental spills turn hazardous when left to spread. Good ventilation reduces dust, making the workspace safer for daily use.
Storing chemicals like pimelic acid gets overlooked, especially when the substance doesn’t look menacing on the shelf. Solid storage practices protect investments, ensure reliable results, and keep everyone in the lab safer. A little attention paid to moisture, heat, and clean handling reduces problems before they start. This kind of care reflects pride in the work and respect for the science—both are well worth the effort.
Pimelic acid plays a role in organic chemistry labs and specialty manufacturing. If you ended up searching for where to buy it, odds are you already have a project—maybe research, or perhaps something more technical—waiting on this single compound. From my own time working with university labs, the trickiest part is never just picking a source. It’s figuring out how tight your sourcing and documentation needs to be, especially for anything beyond a classroom experiment.
University stockrooms and science supply stores often serve as the go-to, provided you have credentials. If your goal is professional-grade research, don’t bother with third-party auction sites or general retailers. Companies like Sigma-Aldrich, Alfa Aesar, and Fisher Scientific keep consistent listings and clear safety documentation. These are major players, and they’ve been around for years. Their online catalogs list pimelic acid by the gram, and usually offer several packaging sizes.
On-campus, restrictions tend to follow strict guidelines, especially since chemical diversion and improper handling can land both buyers and suppliers in trouble. Most reputable distributors request a business or academic account, sometimes with additional paperwork depending on local laws. Anyone with experience in chemical purchasing knows: institutional buying isn’t about grabbing the lowest price, it’s about traceability, certificates of analysis, and batch numbers.
If your experience stops at high school chemistry, step lightly. Pimelic acid itself isn’t the most hazardous compound, but purchasing and shipping any specialty chemical means compliance with transport and handling regulations. Companies ship under international guidelines—like those set by OSHA or the UN—and will not turn a blind eye to missing credentials. Year after year, there are reports of seized shipments due to incomplete data or missing permits.
From a safety standpoint, even a simple dicarboxylic acid requires gloves, goggles, good ventilation, and responsible storage. I learned early—after an accidental spill involving a far less benign compound—that it only takes one overlooked item to disrupt an entire lab’s workflow. The experts I learned from always kept meticulous records, because mistakes were easier to patch up with clear documentation. That kind of discipline makes a difference, especially in regulated environments.
Import bans, counterfeit chemicals, and mislabeled packages have popped up for a reason. Pimelic acid sourced from an unknown party online might come cut with contaminants, or not be pimelic acid at all. There are a few hard rules that have come out of years of trial and error: Buy direct from established suppliers, use only verified business credentials during purchase, and always demand documentation for provenance and purity. No shortcut pays off in the long term, especially if publishing results or passing regulatory audits matters.
Reliable supply means investing time in paperwork, background checks, and sometimes waiting for approvals. Quick orders through consumer platforms usually skip these steps, but problems crop up down the road. Every veteran in the field I’ve met agrees: expertise and trust grow from slow, methodical efforts—never from gambling on cheap shortcuts.
Buying pimelic acid isn’t just a shopping run. It’s a small part of a larger network of safety, legitimacy, and scientific integrity. So, start with what you know—your reason for purchase, who can supply it, and whether your lab or institution can back you up with the necessary credentials. With patience and the right approach, you’ll find a supplier that meets both safety and quality standards, ensuring your work moves forward without a hitch.
| Names | |
| Preferred IUPAC name | heptanedioic acid |
| Other names |
Heptanedioic acid 1,5-Pentanedicarboxylic acid Enanthic acid dicarboxylic |
| Pronunciation | /paɪˈmɛl.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 111-16-0 |
| Beilstein Reference | 1206743 |
| ChEBI | CHEBI:30780 |
| ChEMBL | CHEMBL1403 |
| ChemSpider | 12011 |
| DrugBank | DB03766 |
| ECHA InfoCard | 03d8ed98-4426-40ae-9168-7cfb1ba4e8d2 |
| EC Number | 206-794-5 |
| Gmelin Reference | 8345 |
| KEGG | C00966 |
| MeSH | D010865 |
| PubChem CID | 8675 |
| RTECS number | RW0440000 |
| UNII | 88X26109FA |
| UN number | UN1871 |
| CompTox Dashboard (EPA) | DTXSID4036265 |
| Properties | |
| Chemical formula | C7H12O4 |
| Molar mass | 146.14 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.46 g/cm³ |
| Solubility in water | Slightly soluble in water |
| log P | 0.23 |
| Vapor pressure | 1.16E-6 mmHg at 25°C |
| Acidity (pKa) | 4.41 |
| Basicity (pKb) | 4.98 |
| Magnetic susceptibility (χ) | χ = -58.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.433 |
| Viscosity | 2.30 mPa·s (at 100°C) |
| Dipole moment | 3.72 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 231.5 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -941.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3586.1 kJ/mol |
| Pharmacology | |
| ATC code | A16AB11 |
| Hazards | |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H315: Causes skin irritation. H319: Causes serious eye irritation. |
| Precautionary statements | P264, P270, P280, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 2-1-0 |
| Flash point | 214 °C |
| Autoignition temperature | 440 °C |
| Lethal dose or concentration | LD50 oral rat 3050 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat oral 6,680 mg/kg |
| NIOSH | KWQ70750 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 200-400 mg/day |
| Related compounds | |
| Related compounds |
Glutaric acid Adipic acid Suberic acid Azelaic acid |
