Long before modern laboratories looked so high-tech, chemists searched for ways to separate mirror-image molecules. That search led Emil Fischer and his team, back in the late 19th century, to start using derivatives of tartaric acid as standard setters for chiral resolution. Among the variants, (2R,3R)-(-)-dibenzoyl-L-tartaric acid started gaining recognition thanks to its clear ability to split racemic bases into their enantiomers. This molecule, in many ways, connects the dusty notebooks of early stereochemistry with the chiral columns used in today’s pharma plants. As understanding of stereochemistry improved, scientists started demanding purer forms of chiral compounds. Decades of refinement and smarter organic chemistry pushed dibenzoyl-L-tartaric acid from a niche reagent to a go-to option for separating the right-handed from their left-handed molecular twins. What began as an academic curiosity now serves as a backbone for the manufacturing of single-enantiomer drugs and fine chemicals on commercial scales.
(2R,3R)-(-)-Dibenzoyl-L-tartaric acid anhydrous shows up as a crystalline powder, unmistakably white or faintly off-white, carrying a molecular formula of C18H14O8. In practical terms, it means this compound does more than sit in catalogs, waiting for a place as a chiral selector in separations and analysis. Production lines, both small and large, stock up on it to resolve various basic compounds into enantiomerically pure forms. In the context of modern pharmaceutical synthesis, synthetics and chemical suppliers rely on its predictable purity and chiral specificity as essential checks in their workflows. The story of this compound’s presence in labs and production settings isn’t just about chemistry; it’s about reliability as the stakes for purity get higher with every passing year.
This acid doesn’t surprise with wild physical antics—its melting point usually floats around 190–194°C, and it shows limited solubility in water, though it dissolves well in organic solvents like ethanol, methanol, and ethyl acetate. These properties make it convenient to handle in common organic synthesis steps. As a dicarboxylic acid, it carries two carboxylic acid groups, which can engage in classic acid-base and esterification chemistry, and two benzoyl esters. The presence of these groups brings a reliable chemical grip for forming salts and co-crystals. The anhydrous form removes the unpredictability of water content, something that can trip up a separation or yield calculation. Sometimes, those tiny differences mean the difference between clean separation and a frustrating gummy mess.
Many chemical suppliers grade (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous by enantiomeric excess, chemical purity, ash content, and moisture percentage. High-performance liquid chromatography (HPLC) and specific optical rotation serve as standard identifiers; users expect to see specific [α]D values in the range of –110° to –114° in methanol, confirming identity and chirality. Typical bottle labeling lists purity (usually >98%), batch number, CAS number 32634-66-5, storage guidelines (usually cool and dry), and warnings on contact, inhalation, and appropriate PPE. Experienced chemists tend to check both paperwork and product before scaling up, since minor impurities can carry over to a final drug substance.
Lab and commercial production routes often start from natural L-tartaric acid. A reaction with benzoyl chloride, often under basic aqueous or anhydrous conditions, attaches benzoyl groups to both free hydroxyls. Workers monitor the reaction for careful pH control and temperature, since runaway conditions lead to sticky by-products or unreacted tartaric acid. The work-up includes filtration, washing, and sometimes recrystallization from hot ethanol or methanol. These basic steps have stood up to scale-up, but many factories automate key stages with process controls and in-line sensors, squeezing out unexpected loss or contamination. Even today, a skilled eye and a sharp nose help spot the batch gone off track.
In synthetic chemistry, (2R,3R)-(-)-dibenzoyl-L-tartaric acid’s most appreciated trick comes from its ability to form stable salts with chiral bases. It reacts well with alkaloids and amines, turning racemic mixes into separable diastereomeric salts. These can be split, leaving the desired enantiomer ready for further transformation. Once the chiral salt work is done, acidification brings back the resolved base. Some researchers tweak the parent tartaric acid with different acyl groups, but the dibenzoyl version still holds its ground as a workhorse. Chemical reduction, basic hydrolysis, or gentle heating can sometimes return useful derivatives for other synthetic needs.
Across catalogs, you’ll often see (2R,3R)-(-)-dibenzoyl-L-tartaric acid offered as “(–)-DBTA,” “Dibenzoyl Tartrate,” or just “L-DBTA.” In European and Asian markets, the naming sometimes shifts toward “(2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous,” emphasizing water-free form for those planning precise reactions. Laboratories logged years of paperwork using older synonyms, but the CAS number simplifies tracking and sourcing globally. This web of names comes up during purchasing or regulatory review, showing just how global the market for this compound has become.
Workers in synthesis and separation labs learn early on that (2R,3R)-(-)-dibenzoyl-L-tartaric acid doesn’t pose outsized risks compared to many organic acids, but that doesn’t mean it deserves casual handling. The acid can irritate eyes, skin, and the lungs if inhaled or spilled, putting standard gloves, goggles, and fume hoods into daily routines. Spills, though rare outside heavy industrial use, ask for careful cleanup—shoveling solids into designated waste, making sure no dust floats. Staff receive OSHA or EU-style training, covering emergency washes and the expected steps in case of accidental splashes or exposures. Safety data sheets list no acute systemic toxicity at common exposure levels, but experienced professionals keep first aid and proper signage in reach anyway.
Pharmaceutical plants and contract research labs rely on this acid to physically pull apart enantiomers for drug synthesis. Common targets include β-blockers, chiral alkaloids, some amines used in anesthetics or antidepressants, and intermediates for agrochemicals. In academic settings, it’s a teaching aid for undergraduates learning about resolution—the basic benchwork with DBTA connects to advanced research in asymmetric catalysis and molecular recognition. Analytical chemists in forensics sometimes use chiral derivatives of DBTA to check for impurities in controlled substances. Beyond the lab, the biggest impact comes in making medications safer and more effective by delivering the active stereoisomer without the risks of its mirror twin.
R&D teams at chemical and pharmaceutical companies keep DBTA on their list for ongoing studies in green chemistry and resolution technology. Streamlining the reaction, reducing solvent use, and scaling up with improved environmental profiles draw continued attention. In tandem, analytical groups study alternative chiral resolving agents, but DBTA remains a standard benchmark—any new process needs to beat its yield, purity, and cost profile. Developments in solid-phase resolution, automated crystallization, or in-situ chiral sensing all reference DBTA in the supporting literature. Research on hybrid materials—where organic molecules like DBTA get grafted onto silica or polymer beads—aims to speed up industrial-scale separations with less waste and lower manual labor.
Published animal studies point to low acute oral and dermal toxicity for (2R,3R)-(-)-dibenzoyl-L-tartaric acid. Long-term exposure data remain limited, but predictive modeling hasn’t shown strong evidence for carcinogenicity or chronic organ effects. Most incidents involve reversible irritation rather than systemic harm; emergency protocols focus on removing the compound quickly from exposed skin or eyes. Although regulatory agencies don’t classify it as particularly hazardous, experienced chemists share a steady respect for potential workplace issues, especially with accidental mixing, poor ventilation, or cross-contamination in multi-use facilities. Routine monitoring and clear safety signage keep incidents rare and minor.
Chiral resolution isn’t fading—if anything, it’s becoming more crucial as synthetic drugs and specialty chemicals favor single-enantiomer forms for safety, efficacy, and regulatory compliance. Advances in continuous-flow chemistry, automation, and greener solvents could shift some old batch processes to more efficient ones. As drug developers push for more sustainable production, DBTA’s relatively benign profile and proven track record help it stay in the picture, even as new materials and technologies emerge. Startups and established players alike keep one eye on replacements, but for now, (2R,3R)-(-)-dibenzoyl-L-tartaric acid still gathers demand as a trusted, straightforward resolution tool, bridging the classic with the cutting edge.
(2R,3R)-(-)-Dibenzoyl-L-tartaric acid anhydrous isn’t something folks pick up at the corner store, yet it quietly powers the pharmaceutical world from behind the scenes. The main reason? Its knack for separating mirror-image molecules, or enantiomers, in drug development and production. My time working with research labs has shown me that getting the right enantiomer isn’t a small achievement—human bodies react to each mirror-image form differently, sometimes with life-or-death consequences. Thalidomide, for example, forced everyone to realize just how crucial chiral purity is in medicines. This acid serves as a chiral resolving agent, helping scientists isolate or produce single-enantiomer compounds with the accuracy modern medicine demands.
Chiral resolution sounds technical, but the real-world impact cuts clear. In pharmaceutical labs, a racemic mixture—a jumble of both left- and right-handed versions of a molecule—hits a wall. Not every process or human enzyme treats these forms the same way. (2R,3R)-(-)-Dibenzoyl-L-tartaric acid interacts specifically with one enantiomer, forming a salt or complex that sets the two apart. It’s a physical separation, usually a crystallization step, that lets chemists pull one form out of the mess. This is how factories churn out safer single-enantiomer drugs for illnesses ranging from heart disease to depression, replacing old practices that risked unpredictable outcomes.
The FDA increasingly steers drug makers toward chirally pure compounds. A drug's safety profile often rides on the difference between enantiomers. If the wrong one slips through, effectiveness drops or dangerous side effects show up. It’s not rare to see this acid working behind the scenes in the creation of beta-blockers, anti-inflammatories, and antidepressants. The move away from racemic drugs isn’t just a compliance move; it’s about reducing patient risk and giving doctors better tools.
Producing enantiomerically pure substances costs more than simple chemical syntheses did years ago. The processes involve careful controls, high purity standards, and specialized reagents. Cutting corners could mean legal headaches, product recalls, and, worst of all, harm to patients. Chemists favor using (2R,3R)-(-)-dibenzoyl-L-tartaric acid since it provides fairly high yields and reliability, cutting losses where cost pressures already run high. In my experience with chemical suppliers, demand for this acid isn’t likely to taper off unless truly disruptive technologies arrive.
One challenge facing smaller labs and start-ups is sourcing high-purity resolving agents at reasonable prices. Large pharmaceutical companies buy in bulk, but independent researchers sometimes struggle. Better supply chain management and investment in domestic production could help fill this gap. Speeding up the regulatory review of suppliers also plays a part. Transparency around sourcing and purity saves headaches later and helps drive up trust in generics and new therapies alike.
As treatments get more personal and regulations tighten, demand for higher purity and enantiomer-selective drugs will keep climbing. (2R,3R)-(-)-Dibenzoyl-L-tartaric acid anhydrous stands to keep its spot in the chemist’s toolkit—in labs that prize quality, patient safety, and compliance. Keeping it affordable and widely available benefits not just pharmaceutical companies but every patient relying on these medicines for a healthier, safer life.
Chemistry has become a cornerstone of modern life, yet people outside the lab don't often talk about what actually counts as "pure" when scientists use a compound. The question about the purity of (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous walks that line—this compound gets used by people who care about small differences in shape and charge, which matter hugely for research and manufacturing. Chiral reagents show their worth where it really matters: in separating mirror-image molecules that can act completely differently in the human body or on a production line.
(2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous tends to land on chemists’ benches with purity levels advertised at 98% or greater. Major chemical suppliers like Sigma-Aldrich and Alfa Aesar list this figure right on their websites and certificates of analysis. Researchers keep their eyes on that percentage, but they also look for another number: chiral purity, which means having almost entirely the right form of the molecule without its mirror image sneaking in. That value usually clocks in above 99% for serious scientific use.
From experience, separating compounds by hand is no party—one tiny contaminant can send results off in the wrong direction. In pharmaceuticals, for example, missing the mark on chiral purity once led to unforeseen side effects with drugs where one mirror image healed and the other harmed. For scientists, a percentage point off in reagent quality means failed research, wasted resources, and a big headache hunting for what went wrong. That's not theory; any bench chemist has stories about ruined data because someone underestimated a compound’s actual purity.
Getting that 98% number isn't about luck. Producers filter batches with care, using crystallization and chromatography to pull out the wrong forms and leftover solvents. Buyers use NMR, HPLC, and TLC tests to double-check, since paperwork alone doesn't always tell the full story. Modern labs run purity tests on every new batch that arrives, which protects them against mix-ups, degradation, or errors made during transport.
Purity stays at risk during storage and shipping—moisture or exposure to light can erode quality, especially for compounds like this that hold water cautiously at bay. Keeping chemicals anhydrous means tight seals and dry environments, often with desiccants alongside. Labs with high standards maintain logs of lot numbers and retest after any sign of trouble.
People have begun to push for even better transparency: sharing analytical data directly online, opting into independent third-party certifications, and demanding prompt recalls when suppliers detect problems downstream. Teaching new researchers to recognize signs of impurity and understand data sheets gets stressed in every decent lab, because relying on supplier claims alone invites error.
Long term, better automation and analytic tech—like cloud-connected instruments that update purity in real time—promise to cut down on uncertainty and let chemists catch problems before they cost time or reputations. For now, anyone using (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous needs to respect numbers on a label, but also learn to trust and verify. That habit keeps the science solid, the products reliable, and everyone’s results a little closer to the truth.
Chemicals like (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous call for a different kind of respect than what we give everyday items. This compound doesn’t tolerate sloppy handling and careless storage. Anyone working with it should recognize the risks and take storage seriously—something I learned firsthand in the lab. Early in my career, I underestimated moisture’s sneaky power. Even low humidity can damage the purity of moisture-sensitive substances. That kind of mistake is costly and embarrassing.
The biggest threat to (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous is water. Even a tiny amount can start a reaction, change its structure, or leave you with an impure compound. I always store this chemical in a tightly sealed container, using glass over plastic to stop any air or water vapor from sneaking in. A desiccator with a strong drying agent, like silica gel, offers another layer of protection. That small effort means all the difference between a good experiment and a wasted batch.
Heat causes subtle changes too. My lab stores this compound in a dedicated fridge or at room temperature—never close to hot equipment, radiators, or windows. Direct sunlight isn’t just a myth: it speeds up chemical decomposition and sometimes leaves ugly streaks of yellow or brown in what should be a pure, white powder.
Sloppy labeling gets people in trouble. Every container should plainly say the full chemical name, concentration, date received, and the name of whoever opened it. Mistaking one tartaric acid salt for another leads to ruined syntheses and possible safety risks.
I learned to keep strong acids, strong bases, peroxides, and oxidizers off shelves where this material is stored. Sometimes, one bad spill sets off an accident nobody wanted. Even a broken container raises problems, so I use storage bins or secondary containment. No cutting corners on personal protection, either. Lab coats and gloves never go out of style.
Old reagents often pose higher risks. Each year, I go through all chemical stores. Anything past its expiration date goes to waste storage, following our safety manager’s instructions. This simple check frees up shelf space and cuts down on dangerous errors.
Our lab switched from paper logbooks to a digital system a few years ago. Now, we scan the barcode on each reagent every time it’s moved. This setup makes it much easier to track where the (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous lives, who last used it, and whether supplies need a refill. Auditors and safety inspectors notice when records are complete and consistent.
Store each container away from sources of water—including those humidifiers and overly enthusiastic custodians who mop floors late at night. Make a habit of checking container seals after every use. Stash all chemicals off the floor and below shoulder height to avoid drops and spills. Any time a new coworker joins, give them a full walk-through of the chemical store—better safe than sorry.
No fancy equipment required—just common sense and good habits. In my experience, treating chemicals with care saves money, time, and sometimes your skin.
Every chemist who’s prepared a chiral resolution or tried to separate enantiomers knows how much headache solubility questions can bring. We all want something that will dissolve easily, react consistently, and keep the workflow moving. Go into a synthesis or purification without knowing your compound’s solubility, and plenty of time gets wasted chasing precipitation, emulsions, or sticky residues. That’s especially true for (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous, a favorite in academic and industrial labs for resolving bases and amines.
Anyone who has weighed out this stuff knows it looks like a white powder, more at home with crystals than with salt. L-tartaric acid, by comparison, dissolves easily in water because of all those hydrophilic hydroxyl and carboxyl groups. Once you swap out some hydrogens for big benzoyl groups, things change quickly. The compound keeps its backbone but now picks up bulky, less polar groups that tilt the scales toward organic solvents.
Try dissolving (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous in pure water, and you’ll mostly end up watching it float or settle to the bottom. Sure, a trace might go into solution, but practical use calls for higher concentrations than that. Real solubility pops up in organic solvents—methanol, ethanol, acetonitrile, acetone, or ethyl acetate. The molecule’s benzoyl groups interact smoothly with these organics. In my experience, the best results come from alcohols or moderately polar solvents. Avoid going straight to hexane or diethyl ether, which just leaves you with undissolved powder and disappointment.
I’ve tried to push this compound into water by heating or adding a base. Usually, adding base forms the salt and improves water solubility a bit, but not enough to match the ease of using organic solvents. This means that for salt formation or preparative chromatography, organic-based systems usually save the day.
Search through chemical data sheets, and the trend remains the same. Tokyo Chemical Industry, Sigma-Aldrich, and Alfa Aesar all point to low or negligible water solubility for this compound. Researchers looking to carry out asymmetric synthesis or chiral resolutions usually pick alcohols for initial dissolution. Publications report ethanol or methanol as the solvent of choice. Some use THF or acetonitrile because these give consistent solubilizing power without breaking down the tartaric acid derivative.
Regulatory and safety documentation also highlight handling this compound as an organic-solvent soluble material. Prudence in the lab means checking for purity through recrystallization—something that almost always involves an alcohol or an ester to encourage slow, orderly crystal growth.
Working with this compound is less about brute force and more about choosing solvents wisely. If you want to prepare a solution for enantiomer separation, go straight to ethanol or methanol, check solubility limits, and adjust volumes carefully. Filtration after incomplete dissolution leads to inconsistent results—so save time by mixing thoroughly to let the powder soak in and dissolve.
Anyone handling waste or cleanup will notice the low water solubility right away. Clean beakers need a rinse with ethanol or acetone before heading to aqueous washing. Teams mixing up large batches in industry settings will echo these habits—no one likes clogs in the line or loss of resolution yield due to poor dissolution.
Learning by doing counts for more than most theory. In the case of (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous, picking the right solvent not only saves time but keeps results reliable. Pay attention to solvent selection, and the entire downstream process runs smoother—greater purity, faster reactions, and less stress over solubility surprises.
Most people outside laboratory circles rarely hear about a CAS number. Chemists know these numbers as keys to sort through a complex web of molecules, mixtures, and commercial chemical products. A single compound might carry three or more names, some impossible to pronounce, but a CAS number stays the same around the world.
This compound pops up in chiral chemistry and separates enantiomers in pharmaceutical manufacturing. The full CAS number for (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous is 32634-66-5. Whether sourcing this compound for a research project or quality control, searching by CAS number helps you skip past confusion brought by synonyms.
I’ve seen chemical catalogs littered with misspellings and language mismatches. Researchers working with chiral acids for resolution steps often complain that product quality varies when suppliers rely on incomplete or outdated nomenclature. The CAS number brings order to this chaos. Scientists and quality control staff flock to these seven- to ten-digit sequences—which always lead to the right chemical, no matter the country or the lab.
Buying or handling chemicals always involves a level of risk. Mistaking one tartaric acid derivative for another can set back a production batch, affect enantiomeric purity, or trigger regulatory headaches. Recently, I heard from a colleague at a mid-sized pharmaceutical company: confusion between a hydrated salt and the anhydrous version, because a shipment only carried a chemical name, spelled trouble for both analysis and final product quality. A simple CAS search might have avoided hours of troubleshooting and paperwork.
Safety data, regulatory filings, transport, and customs documentation rely on unambiguous identification. Many chemical accidents in factories started with someone pulling a similar-sounding compound from a shelf. The number 32634-66-5 acts like a barcode for all people handling (2R,3R)-(-)-dibenzoyl-L-tartaric acid anhydrous, from bench chemists to shipping managers.
Sourcing managers lean on CAS numbers to screen out substandard ingredients and flag counterfeits. Lab technicians typing “32634-66-5” into inventory databases can quickly match batch reports or material certifications, cutting down on time wasted hunting through vendor lists. In a market where counterfeit or mislabeled chemicals show up far too often, CAS numbers shrink errors and build trust between suppliers and buyers.
Manufacturers and labs face constant pressure to improve traceability. Simple tools like good labeling and electronic databases reduce error, but mistakes still slip into the system. Switching to CAS-based tracking and documenting every transition, from warehouse to waste management, tackles misidentification at its root. Training scientists and technicians to double-check against these identifiers every time they work with a new batch stops most avoidable mistakes before they grow out of hand.
The world’s chemical inventory stains the pages of journals, catalogs, and customs forms with hard-to-read names and varying levels of precision. Ask for 32634-66-5, and no matter who’s listening, the same molecule shows up, free from translation slips or old habits. Relying on the CAS number means more reliability, better safety, and smoother workflows—things every chemical user should demand.
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