© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Chemists in the early twentieth century discovered a wide field of possibilities after synthesizing lithium acetate dihydrate. Demand grew as researchers in both academia and industry realized the compound had unique features. Originally, scientists relied on lithium salts for medicinal purposes and battery tech; over time, the attention shifted to lithium acetate dihydrate because of its remarkable solubility and gentle behavior in chemical reactions. Laboratories eventually used it as a buffer component and catalyst in DNA and protein research, helping push molecular biology forward. My own encounters with its history come from research libraries and industry interviews, where it’s clear global adoption picked up speed in the late 1950s during the biochemical revolution. Many trusted sources, from Merck manuals to industrial chemical registries, record its steady march into diverse chemical toolkits.
Lithium acetate dihydrate appears as a white, crystalline solid, easily absorbing moisture from the air, with a subtle vinegar-like odor—the unmistakable sign of acetate. Unlike more caustic lithium compounds, this one is gentle enough for fine lab work but strong enough for industrial-scale applications. Product codes, pack sizes, and supply chain information create a dizzying landscape, but all roads lead to its core utility in life science research, high-purity chemistry, and specialized catalysis. Purity remains central, and most reputable vendors guarantee purity levels above 99%. Having handled it personally, there’s a certain reassurance to its stable, slightly granular texture in the palm, and its quick dissolution in distilled water marks it as a laboratory staple.
Water easily dissolves lithium acetate dihydrate, thanks mostly to its dihydrate form, which delivers two water molecules per formula unit. Its chemical formula is C2H3LiO2·2H2O, offering a molecular weight of 102.02 g/mol. Its melting point usually lands between 42–45°C. Like other acetates, it gives off a slightly acidic pH when dissolved. Unlike potassium or sodium salts, lithium variants avoid caking and clumping, keeping their free-flowing character. In the bench-top setting, color, granularity, and solubility offer quick purity and freshness checks—habits older chemists pass down as practical wisdom.
Regulators across regions require clear labeling of lithium acetate dihydrate, mandating listing of the chemical formula, batch number, shelf life, and hazard warnings. Supply chain transparency has tightened, especially in the pharmaceutical and biochemical sectors, after recent global safety scares. Material safety data sheets (MSDS) must accompany shipments, with clear hazard pictograms and first aid instructions. In my work with compliance audits, I rarely see objections so long as manufacturers stick with International Union of Pure and Applied Chemistry (IUPAC) nomenclature and display percent purity plus specific storage conditions (below 25°C, away from acids or strong oxidizers). This attention to detail keeps both scientists and warehouse teams safe.
Small-scale labs and large factories both use simple, robust processes for making lithium acetate dihydrate. They start with acetic acid and a lithium base, usually lithium carbonate or lithium hydroxide. Chemists stir the mixture under controlled temperatures. When acetic acid fully reacts, the desired lithium salt crystallizes out upon cooling and, with careful filtration and evaporation, yields lithium acetate dihydrate with high purity. Years spent in university and contract labs showed me that careful pH control and moderate heat yield consistent, high-grade crystals, while shortcuts or impurities spoil the batch and invite expensive rework. For some specialty requirements, vacuum drying produces anhydrous material, but dihydrate holds the widest application for its handling ease.
Lithium acetate dihydrate actively participates in a range of chemical reactions, mostly as a weak base or buffering agent. Synthetic chemists leverage it in organic reactions for mild acetylation and as a co-catalyst in condensation procedures. Biochemists use it to precipitate and purify nucleic acids—a process taught to nearly every genetics student. Some research teams use it to tweak polymer properties or tune solubility in specialty resins. Anyone mixing with strong acids or bases must watch out for effervescence and the drifting aromatic trace of vinegar—a clear signal that acetate conversion has started. My hands-on experience found that it remains remarkably stable during reasonable temperature swings, earning it a spot on nearly every standard reagent shelf.
Chemists know this material by many names, depending on language and local convention. Its main synonyms include lithium ethanoate dihydrate and acetic acid, lithium salt, dihydrate. Some catalogs list it as CAS Number 6108-17-4, which helps cut confusion in global purchasing. In China and Korea, direct translations of ‘lithium acetate’ find routine use, while trade names sometimes add clarity on purity or hydrate state. Everyone in science learns to double-check these synonyms to avoid misorders—a lesson painfully clear after more than one batch of ‘mixed hydrate’ lithium salt arrived on my doorstep.
Lithium acetate dihydrate sits in the moderate hazard category. Swallowing or large skin exposures can irritate, but the dihydrate form keeps volatility low. Standard lab hygiene applies: gloves, goggles, and prompt cleanup of spills. Well-run companies now train warehouse, transport, and lab staff using industry videos and on-site drills. I recall one incident where a team ignored dust control: lithium dust floated and landed on damp benches, leading to localized corrosion—and days of scrubbing. Storage requires airtight containers in cool, dry, well-ventilated spaces. Hazard grades may jump if lithium acetate dihydrate gets mixed with strong oxidizers or acids, so segregation takes priority.
The biggest demand for lithium acetate dihydrate comes from genetic research, where it plays a role in DNA precipitation and transformation protocols. Molecular biology technicians reach for it nearly every day, whether extracting plant genomes or prepping yeast for gene transfer. Pharmaceutical labs use it in analytical controls, while battery scientists experiment with specialty electrolytes. Textile manufacturers once used it for dye fixatives, though tighter heavy-metal regulations changed that landscape. Specialty ceramics and glass foundries now explore lithium acetate dihydrate for better transparency and toughness in finished products. My years in the life sciences taught me that every high-throughput sequencing run relies on chemical buffers like lithium acetate, emphasizing its place at the heart of discovery.
R&D teams view lithium acetate dihydrate as a flexible platform for advanced chemistry, not just a routine reagent. Newer applications focus on greener syntheses and cleaner battery technology. Several groups develop solid-state electrolyte prototypes, pushing beyond traditional lithium carbonate. Molecular engineers explore its use in stabilizing novel biopolymers and enzyme complexes for industrial biotechnology. Some teams target its mild acidity and small ionic size to design subtle, tunable catalysts for pharmaceutical intermediates. Funding keeps rising as projects connect lithium acetate with carbon capture, sustainable materials, and even microfluidic device fabrication. Field tests and real-world pilot studies offer feedback that textbooks often miss, proving that direct experiment trumps theory every time.
Most toxicity reports identify lithium acetate dihydrate as less hazardous than many alternatives, but safety boards urge caution. Chronic exposure risks trace back to lithium’s known effects on the central nervous system and kidneys. Studies in rats confirm accumulation threatens long-term organ function at elevated doses. Discharge into waterways brings attention from regulators, as aquatic organisms prove sensitive to lithium even at modest ppm levels. Research institutions invest in runoff control systems and review Material Safety Data Sheets every year to keep up with regulatory changes. In my environmental audits, I encourage labs to track usage and waste streams: batteries, glass, or buffer, each path leaves a trace in the ecosystem.
Research into lithium acetate dihydrate keeps advancing at breakneck speed, especially with two trends: demand for next-generation batteries and the push for biocompatible, sustainable chemistries. Market analysts expect growth as lithium-ion and solid-state batteries evolve, provided that sourcing and recycling keep up. Lab professionals see promise, too—expanding into RNA research, cell therapy, and new diagnostic tools. Tech innovators monitor supply chains with care, sitting on the lookout for any signs of price spikes or ethical supply concerns as lithium mining expands globally. Having walked the trade-fair floors in Europe and Asia, I notice more entrepreneurs eyeing lithium acetate dihydrate for advanced manufacturing and microelectronics. The only guarantee: the need for smart, safe chemistry grows sharper each year, and lithium acetate dihydrate rides the crest of that change.
Walk into a modern biology lab and you will probably find a bottle labeled “Lithium Acetate Dihydrate” tucked away on a shelf. Anyone who’s ever cloned a piece of DNA knows its worth. Scientists rely on it for a process called “yeast transformation,” which basically lets you introduce new genetic material into yeast cells. This might sound niche, but the trick—using lithium acetate to open up yeast—powers huge chunks of molecular biology research. Insulin for diabetes, rennet for cheese, even synthetic vaccines are part of the biotech outcomes that depend on this process.
I remember watching post-docs in a bustling university lab, each running tests that hinged on these yeast cells taking up just the right DNA. The solution: mix yeast with lithium acetate, toss in the gene you want, then add a jolt of heat. This rough treatment gives DNA a path into the cell. Because yeast behaves so much like human cells, these experiments help us predict how genes will react in actual life—and speed up discoveries that eventually trickle out to clinics and grocery stores.
Outside the lab, lithium acetate dihydrate earns its keep in the factory. Take polyester, for example, which shows up in just about every closet or living room. Making polyester means creating a reaction between certain acids and alcohols, and lithium acetate works as a catalyst to speed up this process. Even a tiny amount nudges huge batches of chemicals in the right direction, keeping mass production efficient.
Industrial water treatment brings another use. In places where copper plating happens—think electronics and shiny car parts—lithium acetate helps remove harmful impurities from waste water. The result is cleaner effluent and less impact on rivers and soil. This makes it hard to overlook in any serious environmental compliance checklist.
With roles in health, manufacturing, and waste management, lithium acetate dihydrate touches plenty of lives. Handling it demands proper caution, though. The salt, while not as hazardous as some industrial chemicals, still causes eye and skin irritation. Even at research scale, I learned that gloves, goggles, and good ventilation keep users safe. At a larger scale, companies must keep waste and accidents in check. This calls for upfront investment in training and equipment, not shortcuts.
There’s also a supply angle. Most lithium comes from specific geographic pockets, often tied up by geopolitics. As battery demand explodes, pressure rises on lithium for all uses—including this unsung lab helper. Recycling spent industrial chemicals and developing synthetic alternatives could keep research and industry running, even as the electric car boom changes supply chains.
People rarely think about the common chemicals behind big advances. Lithium acetate dihydrate doesn’t grab headlines, but it greases the wheels of both discovery and daily life. We get more out of it by blending practical lab experience with industrial know-how. Targeted training, smart sourcing, and growing attention from governments and companies would help secure future supplies. The next time a new medicine or breakthrough tech makes news, some small credit should land on unsung chemical helpers like this one.
Lithium acetate dihydrate goes by the formula C2H3LiO2·2H2O. In chemistry classrooms, you might have heard instructors stress that every molecule in a hydrate has water molecules chemically bonded, not just loosely absorbed. Each molecule here contains two water molecules in the crystal structure, which means more than just a dash of moisture. The molar mass clocks in at 102.02 grams per mole, a number that matters when you’re prepping buffers in a life sciences lab or calculating reagent costs. For researchers or production chemists, this value serves as a quality-control benchmark and helps ensure consistent reactions batch after batch.
The formula doesn’t just sit in a textbook; it helps lab workers prepare solutions accurately. Lithium acetate dihydrate’s exact water content guides measuring the right mass. One careless scoop ruins concentrations, which can botch everything from DNA extraction to protein analysis. So much of laboratory work hinges on routines and trust in materials. In my own campus lab days, weighing out lithium acetate felt like a small task, but a slightly-off weight could mean failed gels or wasted afternoons rerunning experiments.
In biotech and academic research, this salt’s popularity comes from its role in DNA transformation in yeast and bacterial work. The dihydrate form offers reliable solubility—you don’t get strange clumping or slow solution times. Researchers need to trust their chemicals, and understanding water content means fewer headaches with unexpected results. I’ve spoken with former colleagues who worked on industrial protocols. They’ll tell you that knowing the exact molecular weight means budgets can be met and delays avoided. Small changes in raw material weights add up in pilot plants and large-scale fermenters.
Consistent product quality begins with clear understanding and precise measurements. Manufacturers labeling the hydration state avoids confusion. In the past, I remember ordering chemicals and getting ambiguous “hydrate” forms. Does it contain one water or two? In practice, that made standardization a challenge. Most suppliers now list the water content clearly, and it’s still worth double-checking each batch. Mistakenly using the wrong form tanks experiment reproducibility, leading to conflicting data across labs.
Transparency doesn’t stop at labeling. Verifiable purity data and access to Certificates of Analysis arm scientists with the context to trust their reagents. Regulatory agencies now encourage additional checks for critical reagents like lithium salts, especially when used in pharmaceuticals or high-value manufacturing. As lithium markets tighten with battery demand, sourcing agents watch for any slip in quality—fake or altered material can slip into the supply chain. Authentic chemical data keeps labs and downstream manufacturers on solid ground.
Global movements in lithium feedstock impact availability and pricing of lithium acetate. Labs juggling supply disruptions look for suppliers willing to guarantee composition and hydration specifics. Investing in supply chain transparency and firm testing standards shields research and product development from volatility. Based on conversations in both startup and university settings, open communication between chemical suppliers and end users builds resilience, reducing wasted time fixing preventable errors. Experience reminds us that a small detail like accurate molecular weight means smoother workflow—from R&D to full-scale production.
Lithium Acetate Dihydrate isn’t just another lab salt tucked away in a drawer. It draws in water from the air pretty fast, enough to clump together or turn into a puddle if left open long. If the container isn’t tightly closed, the quality drops and experiment results may get messy. I’ve seen bottles left with a crusty mess inside, and nothing ruins a morning in the lab quicker than prepping a buffer only to realize the compound lost its punch. Choose tightly sealed, chemical-resistant containers. Glass works if indoors and away from wild swings in temperature, but even sturdy plastic will do if chemistry-grade and free of scratches or cracking.
Humidity causes chemistry supplies to go bad faster than most people expect. Lithium Acetate Dihydrate ends up useless for precise work or makes reactions unpredictable once it absorbs too much moisture. Labels fade and bags get switched, and soon you’re gambling with your reagents. Sloppy storage shortens shelf life. By writing the date of receipt and opening on every bottle, you know exactly what you’re working with months down the line. Freshness isn’t just for milk – chemicals also lose their kick over time.
Room temperature in a chemistry department usually means about 20-25°C (68-77°F). Anything hotter speeds up spoilage. Keeping lithium acetate out of direct sunlight matters more than people realize. An old window ledge or shelf next to heating vents almost guarantees you’ll find surprises in the bottle. Stick with a shaded, dry place that’s easy to reach, and don’t crowd the shelf too much—air needs to move around bottles so condensation doesn’t build up and drip inside. Avoid refrigerators unless guidelines specifically mention it; condensation inside a fridge can also do damage.
Lithium Acetate Dihydrate mixes well with most standard buffers but avoid stacking it near strong acids or bases. Chemicals leak fumes, so cross-contamination turns up faster than you’d guess. I learned this the hard way keeping oxidizers on the same shelf, only to deal with labels peeling off from unseen gas and then play detective to figure out which bottle held what. Most labs set up shelving divided by hazard class. It takes a few extra minutes, but you avoid headaches later by having your acetates away from peroxides or anything volatile.
Even small amounts deserve respect. I wear gloves every time I handle the jar, not because lithium acetate burns on contact, but because habits keep bigger accidents from happening. Even if the substance seems ordinary, spills on the floor turn slippery, and a powder cloud in the air can get inhaled. A little bit of cleanup each day avoids an entire shelf turn into a sticky mess or clogged sink in the future. Having spill kits and extra wipes near the storage area keeps chaos under control.
Every lab benefits from a storage logbook, even for basic salts. It’s easy to think you’ll remember, but after a year or two, those details fade. Recording what’s brought in, how much gets used, and who’s taken it helps prevent waste, keeps everyone honest, and builds trust in your results. Whether in an academic setting or a production lab, tracking use isn’t just for audits—it saves time, money, and energy in the long run.
Lithium acetate dihydrate pops up a lot in labs, especially for scientists working with DNA or yeast. Its crystal-like grains dissolve in water, making it easy to mix solutions for experiments. Most folks in the lab just know it as a simple part of protocols—add this powder, spin the tube, get on with the test.
People hear the word “lithium” and sometimes worry. The truth is, this chemical doesn’t sit on the top shelf of the most dangerous substances. But labeling it as completely safe would be careless. Contact with skin or eyes does bring irritation. Breathing in the dust can irritate the nose and throat. These facts come straight from safety data sheets, not just old lab tales.
The toxicity of lithium acetate isn’t in the same league as more notorious lab chemicals, yet repeated handling without gloves or goggles tells a different story. Some symptoms include dry skin or eye redness. Accidentally swallowing a good amount could bring nausea, vomiting, or diarrhea. Huge exposures might even affect the nervous system, but that’s rare with the tiny amounts used in research.
Labs sometimes treat chemical waste as an afterthought, tossing diluted solutions down the sink. Pouring liters of lithium acetate into public water isn’t common, but a steady drip of bad habits adds up. Studies show lithium can accumulate in water sources, affecting aquatic life in high concentrations. Right now, the small-scale use in science doesn’t tip the scales, but more industrial use—think batteries and electronics—means we need to start thinking bigger picture.
As someone who has handled countless bottles of powdered chemicals day in and day out, the lesson sticks: respect your reagents. Always glove up and slap on those safety goggles even if you feel invincible. Do not waft or sniff powders to check purity. Use the fume hood if you’re measuring out large quantities or if your notes mention airborne dust as a concern. Most folks working in research labs know the drill, but people new to a shared workspace sometimes learn the hard way with stinging hands or irritated eyes.
A key step that helps control risks is having real safety talks—not just a sheet of lab rules hidden in a drawer. New users benefit from hands-on demonstrations. Chemical management plays a big part, too. Storing lithium acetate dihydrate away from acids or strong oxidizers keeps trouble away. Each bottle should get labeled with hazard symbols and an emergency contact number for quick help.
Scientists and industrial workers carry a responsibility with every scoop and pour. Local rules often require separated chemical waste, so adding spent lithium acetate to the correct container ensures it doesn’t sneak into groundwater. Supporting research into better alternatives or recycling tech for large-scale lithium use can slow the spread of potential problems before they become too big to ignore.
The words “hazardous” and “toxic” deserve respect, not panic. By following proven safe-handling steps and keeping an eye on long-term environmental outcomes, the work with lithium acetate dihydrate can stay routine—and safe for everyone involved.
Lithium acetate dihydrate finds its way into many labs, whether someone’s researching yeast genetics or fine-tuning a specialty battery. Purity means more than just a number on a specification sheet—it sets the standard for how predictable and consistent results turn out. For a chemical like this, both the grade and any trace contaminants matter. Research-grade material, the type trusted in molecular biology and analytical work, calls for minimum purity near 99%. A lower grade may do for some industrial work, but that doesn’t hold for sensitive experiments.
Most workspaces use lithium acetate dihydrate with heavy oversight on metals like sodium, potassium, magnesium, and iron. Reputable suppliers list strict upper limits: sodium usually no higher than 0.005%, potassium below 0.005%, magnesium under 0.002%, and iron less than 0.001%. Moisture is factored into the “dihydrate” version, but any extra water affects weight and can dilute experiments. Chloride and sulfate need tight control—chloride under 0.005% and sulfates less than 0.01%. Acidity and alkalinity, checked against a clear pH standard, help confirm the batch hasn’t picked up outside contaminants or gone stale.
I’ve seen firsthand how even tiny impurities disrupt a yeast transformation or cloud a battery’s performance over repeated cycles. Too much iron, for instance, can ruin molecular biology reactions. Sodium can creep into pharmaceutical products and throw salt balances out of tune. Years ago, a batch from a secondary supplier led to a week of faulty PCRs in our lab. A little digging traced all the trouble back to elevated sulfate levels. Such experiences harden a lab manager’s stance on buying only from trusted sources and double-checking certificates of analysis.
It’s not only academic labs that demand accountability. The food industry, DNA sequencing specialists, and those building lithium-ion batteries all invest in tighter quality control. Manufacturers show their mettle by letting independent labs review each batch. Certificates of analysis lay everything out—actual measured levels of each impurity, dates, and batch numbers. This approach lets buyers trace an issue back to individual shipments. For those of us who remember scrambling to explain inexplicable results, this transparency feels non-negotiable.
The push for greater purity isn’t slowing down. Many research hubs now call for “ultra-pure” or “trace analysis” grades. Suppliers respond by using cleaner water, sealed storage, and careful tracking throughout production. Some larger labs test every lot of chemical that comes in, not just taking vendors at their word. This may sound expensive, but a single batch of tainted lithium acetate can stall major projects or lead to unreliable products—costs that eclipse what’s spent on careful sourcing.
In my years working with specialty chemicals, lithium acetate dihydrate stands out as a good lesson. It reminds those in science that real results come from sweating the small details—especially purity. Whether supporting a clinical study or building a safer battery, buyers should look for specifics in certificates, demand third-party verification when possible, and keep records tight. True reliability starts by demanding thoughtful answers about what’s in the chemicals used every day.
| Names | |
| Preferred IUPAC name | lithium ethanoate dihydrate |
| Other names |
Acetic acid, lithium salt, dihydrate Lithium acetate, dihydrate Lithium ethanoate dihydrate Ethanic acid, lithium salt, dihydrate |
| Pronunciation | /ˈlɪθ.i.əm əˈsiː.teɪt daɪˈhaɪ.dreɪt/ |
| Identifiers | |
| CAS Number | 6108-17-4 |
| Beilstein Reference | 2039772 |
| ChEBI | CHEBI:61317 |
| ChEMBL | CHEMBL1201732 |
| ChemSpider | 86656 |
| DrugBank | DB14509 |
| ECHA InfoCard | 03cbf7d7-2e2b-4fec-acd6-aaa429bc3888 |
| EC Number | 211-193-9 |
| Gmelin Reference | 141748 |
| KEGG | C05538 |
| MeSH | D008095 |
| PubChem CID | 23665815 |
| RTECS number | OQ9625000 |
| UNII | 161B0R83SO |
| UN number | Not regulated |
| CompTox Dashboard (EPA) | A substance with the name "LITHIUM ACETATE DIHYDRATE" has the CompTox Dashboard (EPA) identifier: `DTXSID80968713` |
| Properties | |
| Chemical formula | C2H3O2Li·2H2O |
| Molar mass | 102.02 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.5 g/cm³ |
| Solubility in water | Very soluble |
| log P | -3.21 |
| Acidity (pKa) | 4.8 |
| Basicity (pKb) | 3.84 |
| Magnetic susceptibility (χ) | -45.2·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.422 |
| Viscosity | Viscous liquid |
| Dipole moment | 2.5 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 114.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1534.7 kJ/mol |
| Pharmacology | |
| ATC code | N05AN01 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | Hazard statements: Harmful if swallowed. Causes serious eye irritation. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 1-2-0-W |
| Lethal dose or concentration | LD50 Oral Rat 525 mg/kg |
| LD50 (median dose) | LD50 (median dose) Oral Rat: 525 mg/kg |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Lithium Acetate Dihydrate: "No OSHA PEL established |
| REL (Recommended) | 5 mg/m³ |
| Related compounds | |
| Related compounds |
Sodium acetate Potassium acetate Lithium chloride Lithium carbonate Lithium hydroxide |
