In the long tale of organosulfur chemistry, Piperazine-1-dithiocarboxylic acid showed up as researchers kept pushing the limits of piperazine and sulfur compound modification. Chemists in the mid-20th century started fiddling with dithiocarboxylic functionality, hoping to tap into new ligand and pharmaceutical properties. Looking back, you see a pattern: as soon as a backbone like piperazine turned up in biologically active molecules, folks started wondering what would happen if they introduced sulfur donors. The answer, often, was new biological activities and chelating agents for metals. The origins of this acid came about in the search for compounds that would interact in selective ways with transition metals or block certain enzymes. Now, you find a decent number of patents, especially from medicinal chemists and coordination chemistry circles, from an era when researchers wanted compounds tailor-made for binding and reactivity.
Piperazine-1-dithiocarboxylic acid belongs to the group of dithiocarbamates, sitting on the molecular fence between simple dithiocarbamic acids and functionalized cyclic amines. Each molecule carries the piperazine ring with a dithiocarboxylic acid group at one nitrogen. With that structure, it manages to cross the boundary between organosulfur chemistry and pharmacology, attracting research in both. Laboratories, particularly those working on metal extraction, catalysis, pesticide development, or enzyme inhibition, have given the acid a steady demand over the years.
This compound tends to appear as a slightly yellowish crystalline powder. It dissolves in polar solvents such as water, ethanol, and dimethyl sulfoxide. The presence of both secondary amine and dithiocarboxylic acid functional groups gives it flexibility in coordination chemistry and a distinct sulfur odor. The acid detaches protons easily under alkaline conditions, making it a good ligand for metal ions. Sensitivity to air, due to potential oxidation of the dithiocarboxyl group, remains a practical challenge that makes storage and handling in the lab a bit tricky. Thermal stability hovers around the typical range for organic acids with sulfur content, generally decomposing rather than melting cleanly.
Specification sheets coming from industrial producers usually list purity at 98% or higher. Heavy metal content, moisture level, and melting range help labs gauge suitability for research or synthesis. Product labeling includes molecular formula (C5H10N2S2), molecular weight, storage conditions (cool, dry, air-tight containers), and sometimes hazard statements relating to potential toxicity or skin sensitivity. The better suppliers also include a certificate of analysis and batch traceability as part of good laboratory and manufacturing practice standards, contributing to data reliability.
Synthesizing Piperazine-1-dithiocarboxylic acid isn’t overly complicated. Most protocols start with piperazine, reacting it with carbon disulfide in the presence of a base such as sodium hydroxide. This produces the sodium salt, which then gets acidified—typically with a mineral acid—yielding the free dithiocarboxylic acid. Purification often relies on recrystallization from ethanol or water to remove side products. While the procedure doesn’t demand exotic reagents, care must be taken due to the toxicity and volatility of intermediates like carbon disulfide.
Chemists value Piperazine-1-dithiocarboxylic acid for its versatility. The dithiocarboxylate group reacts readily with transition metal ions, forming stable complexes used in metal extraction and catalysis. Alkylation, acylation, and salt formation with various cations also deliver a range of derivatives that extend its use. The sulfur atoms play a key role, binding strongly to soft metals like mercury, copper, or silver. In biochemistry labs, modifications allow the compound to serve as an enzyme inhibitor or as a functional group on larger polymer scaffolds. Researchers often tweak the piperazine ring or the acid functionality to fine-tune solubility or target binding.
Several alternate names crop up in literature and suppliers’ catalogs, reflecting slightly different chemical perspectives or salt forms. Synonyms include Piperazine dithiocarbamic acid, 1-Piperazinecarbodithioic acid, and rarely, 1,4-Diazacyclohexane-dithiocarboxylic acid. The sodium or ammonium salts surface as separate commercial offerings, used where solubility in water and ease of reaction with metal ions outpace the free acid’s performance. Careful identification by CAS number remains the most foolproof way to avoid confusion.
Handling Piperazine-1-dithiocarboxylic acid requires real attention to safety. Inhalation or skin contact with dithiocarboxylic acids, especially those derived from carbon disulfide, can irritate or cause allergic reactions. Use of gloves, protective eyewear, good ventilation, and chemical fume hoods represents standard practice. Spill management focuses on containing the material, cleaning up with inert absorbents, and disposing through chemical waste channels rather than drains. Lab workers get briefed on symptoms such as skin rash or respiratory discomfort tied to dithiocarbamate exposure. Material safety data sheets lay out response plans for accidental exposure or fire, which generally involves dry chemical or foam extinguishers, since water may spread contamination.
Piperazine-1-dithiocarboxylic acid finds its strongest uptake in research focused on metal chelation and catalysis. Environmental chemists take interest in it as a complexing agent for heavy metal extraction from wastewaters, given the affinity of the sulfur groups. The pharmaceutical crowd has explored derivatives for potential antifungal, antibacterial, and antiparasitic uses, since sulfur-bearing moieties often disrupt enzymes crucial for pathogen survival. Polymer chemists use the acid as a building block for functionalized resins that scavenger metal ions. It also shows up in analytical chemistry, where complex formation with metals assists in detection or separation processes. These varied applications make it a sort of utility player in the chemical toolbox.
For years, teams working in both academic and industrial settings have looked for ways to expand what Piperazine-1-dithiocarboxylic acid can do. I’ve seen researchers mix it into new catalytic systems aiming for green chemistry credentials, reducing reliance on expensive metals by forming robust complexes with first-row transition elements. Others have grafted it onto solid supports, pushing into flow chemistry where recovery and reuse of catalyst-laden resins become cost savers. Collaborative work between biochemists and material chemists has led to more stable bioactive conjugates, riding on the backbone of the dithiocarboxyl group. The research network revolves around the acid’s adaptability and the ability to tune derivatives for the job at hand—whether isolating heavy metals in contaminated soils or delivering a new scaffold for drug candidates.
Every time a new dithiocarboxylic acid crop up, questions on toxicity follow. Studies with Piperazine-1-dithiocarboxylic acid raise flags on both acute and chronic exposure. Dithiocarbamates as a group can produce liver and kidney stress in high doses; metabolic breakdown sometimes yields carbon disulfide, a known neurotoxin. Animal studies give variable results, but doses above laboratory exposure limits trigger toxic symptoms pretty fast. At the same time, the acid shows promise in targeted therapies that depend on its metal-binding or enzyme-blocking ability. Toxicology labs keep hammering away at the question: can this molecule deliver therapeutic benefit without risky side effects, or can we make a derivative that passes muster in longer-term safety testing?
Looking ahead, the future for Piperazine-1-dithiocarboxylic acid spins out in several directions. The green chemistry movement has spotlighted compounds that can selectively bind and recover toxic metals, with research platforms ready to test new dithiocarbamate systems in real-world remediation. Advanced drug design trends, especially in neglected diseases, often revisit sulfur chemistry searching for candidates that evade resistance and operate via new mechanisms. Collaborative groups—combining expertise in computational chemistry, toxicology, and process development—keep this acid in the running for innovative applications. At the same time, regulatory scrutiny on dithiocarbamates will keep stirring the pot, demanding ever-better safety and environmental data. The challenge, as always, sits in drawing out maximum utility without crossing lines set by health and sustainability concerns. In my own lab experience, simple tweaks to the piperazine or sulfur groups can mean the difference between a promising candidate and a nonstarter, which keeps the story of Piperazine-1-dithiocarboxylic acid moving into new chapters.
Staring at a name like Piperazine-1-Dithiocarboxylic Acid, the mind hitches a ride straight to the depths of a chemistry textbook. Truth is, this isn’t some mysterious compound locked away in a forgotten science lab. Over the past decade, I’ve seen it pop up in corners of manufacturing and even bits of pharmaceutical research. The world around us runs on chemicals like this, and understanding their impact bridges the gap between technical talk and daily life.
Industries don’t hang onto a chemical unless it gets the job done. Piperazine-1-Dithiocarboxylic Acid steps into the game as a chelating agent. That underlines its talent for grabbing and holding metal ions—think of it like the hands on a strong grip. Metal ions in water, factories or mines create trouble, leading to scaling, corrosion, or lower yields in industrial processes. This compound's ability to lock up those metal ions means cleaner water, smoother chemical reactions, and more efficient metal recovery in places like copper or gold mining. Every time a mining operation expects higher recovery of precious metals with lower contamination, this chemical finds its way onto the scene.
Pharmaceutical labs take a different angle. Researchers explore the structure of this acid for building new molecules. They probe whether its sulfur-rich backbone can help craft fresh antibiotics or cancer drugs—since many medicines gain power from the weird shapes and reactivities of sulfur-based groups. The toolbox for drug development keeps growing, and each addition like this increases the odds of finding something life-changing.
A chemical doesn't earn attention only as a problem-solver. Any formula powerful enough to wrangle metal ions draws questions about what happens if it hits the environment in the wrong way. Trace residues from mining or industrial drainage could slip downstream. Local communities have the right to know what's in their air and water, especially since sulfur compounds wreak havoc with aquatic life or add stink to water sources if mismanaged. Scientists still study long-term effects, but the principle stays simple: handle chemicals with respect and good oversight.
Health workers in chemical plants know safety rules for a reason. Piperazine derivatives, in high doses, can lead to skin irritation or longer-lasting issues if inhaled. From personal protective gear to well-ventilated workspaces, the safety playbook sticks close at hand. Nobody saves money or time by skimping on health safeguards.
Piperazine-1-Dithiocarboxylic Acid isn’t about hype or science fiction; it belongs to the everyday grind of manufacturing, water treatment, and medical innovation. This compound keeps water clearer, helps maximize resource extraction, and might shape tomorrow’s medicines. The next time you hear about cleaner mining operations or new drug discoveries, remember that advances often hide behind strange, tongue-twisting chemical names. Real progress involves treating these tools with caution, advocating for strong environmental laws, and making sure research marches on in open and responsible ways. Wise stewardship serves both industry and community, so responsible use sets the foundation for trust and sustainable growth.
Piperazine-1-dithiocarboxylic acid carries the chemical formula C5H10N2S2. At first glance, it just looks like a collection of symbols. Break it down and you see five carbon atoms, ten hydrogen atoms, two nitrogen atoms, and two sulfur atoms. Chemistry isn’t just about naming compounds; it’s about understanding how pieces fit together in ways that expand options in science, medicine, and industry.
Plant chemists know the frustration of chasing the right compound and ending up with a dud because of a missed atom or a misread structure. Piperazine-1-dithiocarboxylic acid contains a six-membered piperazine ring, giving it some sturdy skeleton. Replace some typical atoms with sulfur, and suddenly it can grab onto metals, which makes it interesting for a range of uses—from chelation processes in labs to specialty formulations.
There’s more than just theory at play. Skip a sulfur and you miss out on the properties that made dithiocarboxylic acid a go-to for certain applications. Adding sulfur into the backbone can help in complex formation, and that often plays a role in chemical synthesis, extraction of heavy metals, or even in early stages of pharmaceutical development. Sloppy formulas cost real money and time, which many research teams can’t spare.
In day-to-day work, accuracy matters. Using Piperazine-1-dithiocarboxylic acid with a confirmed structure unlocks reliable results for people working with transition metals or in fine-tuned organic synthesis. Chemists have used these types of molecules for years in processes like flotation agents for mining. There’s also curiosity about how sulfur atoms, when precisely placed, make a difference in medicinal chemistry—not just for theoreticians but for anyone working to develop new treatments.
Companies focusing on wastewater treatment appreciate compounds that bind tightly to toxic metals. The two sulfur atoms in Piperazine-1-dithiocarboxylic acid act like magnets for heavy metal ions, offering effective cleanup of contaminated sites. This is not some pie-in-the-sky benefit; those properties save lives and help cities clean their water.
Getting the chemical structures right brings benefits, but there’s more work to do. Mislabeling or poor documentation still happens in supply chains, and that invites serious risk. Transparent sourcing, open databases, and strict labeling help keep everything accurate.
Academic settings should put extra emphasis on structural chemistry, focusing not just on memorizing formulas but teaching the importance of each bond, ring, and atom. Investing in updated analytical tools such as NMR and mass spectrometry produces quicker and more reliable identification, saving research teams from making costly mistakes down the road.
Knowing that Piperazine-1-dithiocarboxylic acid has the formula C5H10N2S2 helps more than just a classroom pop quiz score. That knowledge carries into safer labs, cleaner water, and better-targeted research. Each atom counts. In my own work, double-checking the formula has prevented more than one headache, and made sure experiments didn’t blow up—literally or financially.
In everyday work, chemical safety feels like a headache until something goes wrong. A lot of folks recall moments in labs or warehouses where a rushed job or ignorance led to a sticky, hazardous mess. Piperazine-1-dithiocarboxylic acid isn’t a household name, but its storage deserves just as much attention as any classic lab staple, especially since improper storage can spark health concerns or ruin expensive supplies.
This compound stands out for its reactivity. It doesn’t catch fire easily, but moisture can break it down, and sunlight speeds up those reactions. Most lab workers remember the warning labels and odd smells of sulfur compounds that end up leaking from poor containers. Keeping this substance dry and away from light stops it from releasing toxic gases or forming irritating dust that can become a problem for anyone nearby.
Glass jars with tight-sealing lids work better than plastic since some plastics allow air or vapor to slip through, giving moisture a path inside. Storing it in glass, away from direct sunlight and humidity, keeps it from degrading. Every chemist I know shares stories about powder clumping or turning yellow when someone stored it in a humid closet. Even experienced researchers reach for silica gel packs and desiccators for a reason—they know a little humidity can wreck purity, cost the lab cash, and possibly release something harmful.
Heat speeds up breakdown. Suppliers and lab texts agree: 15 to 25°C, away from radiators or hot pipes, stops the substance from going weird or dangerous. Refrigerators help for long-term storage, but only if containers stay labeled and sealed. Darkness adds another layer of protection, since sunlight nudges chemical reactions forward. Workers who’ve seen a once-white chemical turn brown overnight pay close attention to that advice.
Ignoring labels leads to mistakes with any chemical, but labeling Piperazine-1-dithiocarboxylic acid with both its full name and hazards provides vital backup. In a busy environment, clear writing keeps people safe by stopping accidental mix-ups. Almost every unsafe lab incident involves an unlabeled container—once you see the aftermath, you never skip the marker again.
Anyone handling or restocking chemicals should put on gloves and work in a ventilated spot. Accidental skin contact or inhalation can trigger real health issues. One close call in a crowded storeroom—when dust wafted into the air—taught me to move gently with containers, avoid spills, and shut lids quickly. Safety gear always feels like an inconvenience until it saves your skin.
Safety authorities, like OSHA, regularly update advice as new hazards or incidents pop up, so it pays to check resources now and then. Sharing real stories among colleagues and updating protocols together reduces mistakes. Most problems come from rushing or skipping steps everyone assumes are “just for beginners.” Taking a little extra care with Piperazine-1-dithiocarboxylic acid means avoiding bigger headaches down the road, for both people and budgets.
I’ve worked with enough chemicals over the years to know shortcuts bring real risks. Piperazine-1-dithiocarboxylic acid, used in specialized chemical syntheses, brings hazards that shouldn’t be ignored. When you open a bottle of this stuff, gloves and good sense ought to be your first line of defense. I always start by looking up the material safety data sheet (MSDS) for the official details on exposure limits, hazards, and suggested handling techniques. Knowing the specifics changes how you handle it day-to-day.
Chemical-resistant gloves, well-fitted goggles, a simple lab coat—these make a difference. Enthusiasm won’t keep you safe if your skin or eyes get splashed. Some acids eat through fabric and skin before you can blink. That’s why I never work alone with hazardous compounds. If something goes wrong, someone nearby can step in with a safety shower, help flush out your eyes, or call for help. Never trust a quick splash to rinse off all traces. Once, I thought a minor spill on my gloves was no big deal—my gloves weren’t rated for chemical acids, and I paid for it with a mild burn. Lesson learned. Latex just doesn’t cut it for everything; only nitrile or neoprene gloves provide real defense here.
One sniff of a strong sulphurous odor taught me solid ventilation keeps you alert and healthy. Fume hoods pull vapors away from your face. I once skipped this step for a “quick reaction,” convinced nothing dangerous would happen. My mistake left me coughing and light-headed for half an hour. These kinds of acids produce fumes that mess with your lungs and eyes. Good labs always keep a working hood and test the airflow regularly.
No one likes cleaning up after a long day, but sweeping up powder, wiping spills, and properly labeling containers beats a frantic emergency call. I jot down everything I’ve used, and double-check storage—dry, labeled, away from heat and sunlight. These acids can break down and release toxic gases if left in the wrong spot or exposed to moisture. I’ve seen old chemical storage with crusted lids and faded labels—a recipe for confusion and accidents. Building good habits—checking weights, locking lids, and logging dates—keeps labs safe and organized.
Experience only gets you so far if your coworkers haven’t received proper training. I remember an incident where someone misread a label, creating a reaction we weren’t prepared for. We paused all work, went over our labeling protocol, and brought in a safety officer to retrain the team. Investing time to teach new hires how to handle chemicals, where to find eye washers and showers, and how to spot risky situations gives everyone a sense of control. You see fewer mistakes with confident, well-informed workers.
No shortcut or rushed process saves enough time to risk health. Handling piperazine-1-dithiocarboxylic acid safely means staying humble—reading protocols, using equipment effectively, watching your coworkers’ backs, and keeping the workspace neat and labeled. That attitude, more than any one gadget or extra rule, keeps people from harm. It’s about community and self-respect in a place where complacency can hurt anybody.
People working in chemical research or manufacturing quickly learn that purity grades aren’t just technical footnotes. The fine print matters, especially with compounds like piperazine-1-dithiocarboxylic acid. Few buyers pick up a chemical blind—they want to know if trace impurities could throw off an experiment, raise contamination risk, or cause downstream headaches. Piperazine-1-dithiocarboxylic acid turns up in pharmaceuticals, pesticides, and even rubber additives, so it crosses paths with tough regulations and a range of technical demands.
Every chemist or production manager I’ve spoken with echoes a similar truth: not all piperazine-1-dithiocarboxylic acid shares the same purity. Sourcing decisions often revolve around these nitty-gritty numbers—a product quoted at 97% might seem close enough to one at 99.5%, but those fractional differences hide real risks. At 97% purity, minor contaminants left over from synthesis or handling can spoil a batch or skew toxicity studies. Hit 99% or higher and you’re likely paying more, but the peace of mind counts, especially in medicinal chemistry or sensitive electronics.
Labs doing routine reactions sometimes accept mid-range grades to save on costs, since a trace of impurity may not ruin every outcome. For pharmaceuticals, any foreign material can get flagged during quality checks. Regulatory agencies, including the FDA or EMA, have no patience for unknowns. Upgrading to pharmaceutical or analytical grade adds expense but cuts the odds of project delays from non-compliance.
In my own experience, finding the right grade often means cross-referencing catalog numbers and spec sheets from suppliers such as Sigma-Aldrich, Alfa Aesar, or TCI. Each one lists purity, moisture content, and allowable levels for certain trace metals. The highest costs track with narrow impurity tolerances and verified COAs (Certificates of Analysis) accompanying each batch. Some vendors let customers request custom purification or batch testing—helpful for those rare projects where the generic lot isn’t clean enough.
Industry reports and academic journals back up what I’ve seen: piperazine-1-dithiocarboxylic acid rarely lands in just “one size fits all.” The flexibility serves real needs. Agrochemical firms don’t always sweat the same impurity limits as drug companies do. Trying to shortcut here can wind up costing a lot more down the line if rework or recalls come into play.
It pays to call out purity requirements up front, especially for scale-ups or high-stakes synthesis. Trusted suppliers keep detailed records and often answer direct questions about their purification protocols. While smaller suppliers offer discounted options, due diligence makes a difference: an overlooked impurity at the research stage can scale up to a bigger—and more expensive—problem during production.
Users checking for more than just the percent number on the bottle—asking about batch traceability, impurity profile, and documented test methods—build a safety net that protects projects and end-users. One of the smartest habits I’ve seen is double-checking from batch to batch, rather than making assumptions based on catalog claims. When the difference between success and a setback comes down to less than one percent, it pays to get picky.
| Names | |
| Preferred IUPAC name | 1,4-Diazinane-1-carbodithioic acid |
| Other names |
Piperazine-1-carbodithioic acid 1-Piperazinedithiocarbothioic acid 1,4-Diazacyclohexane-1-dithiocarbothioic acid |
| Pronunciation | /paɪˌpɛrəˌziːn wʌn daɪˌθaɪəʊkɑːrˈbɒksɪk ˈæsɪd/ |
| Identifiers | |
| CAS Number | 10102-23-5 |
| Beilstein Reference | 120873 |
| ChEBI | CHEBI:38842 |
| ChEMBL | CHEMBL2184731 |
| ChemSpider | 21578044 |
| DrugBank | DB07970 |
| ECHA InfoCard | 18ab0c6d-7f7d-4dfa-a263-d73e96a1d4da |
| EC Number | EC 205-685-2 |
| Gmelin Reference | 73182 |
| KEGG | C06124 |
| MeSH | D010903 |
| PubChem CID | 123137 |
| RTECS number | UG9100000 |
| UNII | S3X6XA766J |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | DTXSID20167 |
| Properties | |
| Chemical formula | C4H10N2S2 |
| Molar mass | 209.3 g/mol |
| Appearance | White to off-white solid |
| Odor | unpleasant |
| Density | 1.31 g/cm³ |
| Solubility in water | Slightly soluble |
| log P | 0.18 |
| Vapor pressure | 1.50E-7 mmHg at 25°C |
| Acidity (pKa) | pKa ≈ 6.1 |
| Basicity (pKb) | 3.30 |
| Magnetic susceptibility (χ) | -44 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.649 |
| Viscosity | 40 cP |
| Dipole moment | 4.61 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 222.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -450.7 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | D08AF07 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin irritation, causes serious eye irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P261, P264, P270, P271, P272, P273, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P363, P332+P313, P337+P313, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Flash point | 100°C |
| Lethal dose or concentration | LD50 oral rat 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): **470 mg/kg (oral, rat)** |
| NIOSH | SU 2975000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | REL (Recommended Exposure Limit) for Piperazine-1-Dithiocarboxylic Acid: "0.5 mg/m3 (as total dust), 8-hour TWA |
| Related compounds | |
| Related compounds |
Dithiocarbamic acid Piperazine 1,4-Piperazinedicarboxylic acid Piperazine-1-carboxylic acid Dithiocarbonic acid |
