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People have explored the chemistry of silver compounds for centuries, often chasing their lustrous properties and unique effects. Silver acetate came into focus during the late 1800s, when chemists started pushing deeper into organometallics and simple metal salts. The compound stood out compared to silver nitrate because of its lower reactivity and useful solubility in water and organic solvents. Laboratories in Europe drove most of the early research, digging into its structure and exploring its use in photography, analytical chemistry, and medicine. Early findings sparked curiosity about its antibacterial action, leading to periodic surges of interest. Later, in the twentieth century, as researchers got their hands on more advanced tools, they mapped out silver acetate’s crystal lattice, identifying how its acetate groups arranged themselves around each silver ion. The story of silver acetate reflects the greater curiosity that surrounded silver’s role in chemistry and health, especially as regulations and scientific scrutiny increased over time.
Silver acetate, best recognized by its formula AgC₂H₃O₂, stands as a white crystalline powder or solid with a faintly bitter taste. Unlike its more common cousin, silver nitrate, silver acetate offers a more gentle chemical touch and a shorter shelf life when exposed to light or moisture. Commercially, most labs use it bottled tightly to cut down exposure, keeping its quality intact. In my work, opening a bottle usually releases a faint whiff reminiscent of vinegar, which is no surprise given the acetate ion at play. Since silver acetate dissolves in both water and certain organic solvents, it proves useful in transition-metal catalysis and laboratory synthesis. In electronics and fine specialty applications, its easy conversion into other silver salts or complexes makes it handy as a starting material. There’s never been a large-scale market, mostly because its price and sensitivity narrow its uses to a few technical fields.
At room temperature, silver acetate takes on a needle-like crystalline form, and spills of fine powder easily float down to surfaces—a small reminder of how dust control matters around sensitive electronics. On the color spectrum, fresh material looks stark white, but it darkens quickly in sunlight, shedding a pale brownish cast as silver particles begin to form. Solubility charts show about 1.04g dissolves in 100g water at 20°C, and more dissolves as temperature goes up. Silver acetate handles like an ionic salt but includes the quirks you’d expect from silver: photosensitivity, a tendency to react with halides, and mild oxidizing power. I’ve seen it react quickly with sulfides and phosphates, yielding brown or black precipitates—a familiar sign of silver’s behavior. Temperature, humidity, and trace contaminants shift stability over days or weeks, which means small errors in handling can impact lab outcomes. Its melting point, roughly at 220°C (with decomposition), kinda puts practical limits on direct heating for most applications.
In any lab or industry setting, good labeling on silver acetate is not about bureaucracy but about safety. Labels usually mention purity, batch number, and a reminder about light sensitivity. Products with over 99% purity suit most modern chemistry labs, with trace metallic or organic impurities kept tightly in check. Some suppliers include warnings about temperature conditions and the need to keep containers dry and sealed. In my experience, a simple amber glass bottle with a tight plastic lid works best, stowing the powder away from sunlight and humidity. Silver acetate does attract stricter storage and transport attention because its silver content pushes it into regulated chemical lists, especially in regions with tight controls on toxic silver discharge.
Making silver acetate comes down to a double displacement approach—dissolving silver nitrate in water, then trickling in a stoichiometric amount of sodium or potassium acetate. Immediately, a white precipitate falls out, which collects easily by filtration. Rinsing and drying under low light yields a fairly pure sample, though full-scale industrial production goes a bit further with controlled crystallization and quality checks for residual nitrate or acetate ions. Given the expense of silver and the risk of contamination, recovery and recycling of silver-rich filtrates are always part of the process. At home, the process looks simple on paper, but precision in measurement and cleanliness makes a difference, as traces of impurities can change its color or reactivity. Avoiding exposure to strong light during work-up matters: even standard fluorescent lights can trigger slow decomposition if you dawdle with wet solid on the bench.
Silver acetate’s reactivity opens doors in organic and inorganic chemistry. Professionals often turn to it to introduce the silver ion into more complex molecules or to mediate oxidative coupling. Carboxylation reactions or the replacement of halide ions with acetate in organohalides gets a significant boost from silver acetate’s activity. Heating or photolysis triggers the decomposition of acetate groups, making it possible to deposit metallic silver onto surfaces—a touchstone in the preparation of special mirrors and electroconductive layers. In my lab projects, swapping silver ions from acetate into organosilver intermediates led to creative routes in fine chemical synthesis, especially for pharmaceuticals or small-molecule biological probes. The product does not always behave kindly—excess reagent and trace acid can drop metallic silver or silver oxide out early, stressing the importance of keeping solutions neutral and well-balanced.
Chemists don’t always stick to one name. You’ll see it called acetic acid silver salt, silver ethanate, or even just AgOAc. On order forms and inventory sheets, the formula AgC₂H₃O₂ sometimes stands alone. Older texts use ‘argentum aceticum,’ linking back to classical Latin, though modern practitioners stick to the plain English. Barcode systems and chemical registries prefer simplicity: one number, one clear name. That clarity helps avoid confusion, considering that silver forms a whole parade of other salts—chloride, carbonate, oxide, and nitrate among them—that behave quite differently and pack distinct risks.
Handling silver acetate safely always comes down to respecting its irritant and toxic potential. Silver ions have a way of binding to proteins in skin, hair, and mucous membranes, making gloves and eyewear a non-negotiable part of the process. Small spills can leave stubborn brown or grey stains—barely dangerous, but a persistent visual reminder to wash promptly using soap and lots of water. Inhalation is a low risk since dust doesn’t fly easily under careful transfer, but grinding or careless scooping creates airborne powder. Large-scale facilities rely on controlled dosing, extraction hoods, and spill trays. Disposal brings its own twists: silver falls under strict hazardous waste laws, so nobody washes it down the drain unless they want serious trouble with regulators. Over weeks of heavy use, staff exposed to silver acetate need regular health checks for argyria—a permanent blue-grey skin discoloration caused by chronic silver accumulation. In my own experience, even basic respect for handling procedures keeps problems at bay, provided everyone follows instructions and treats the material with focus rather than fear.
Silver acetate never became a household staple, but its reach cuts across several high-value technical fields. Synthetic chemists draw on it to create organosilver intermediates, a crucial step in fine chemical and pharmaceutical synthesis. Some research groups use it to promote difficult coupling reactions or as a mild oxidant where more aggressive agents risk damaging sensitive molecules. In electronics, deposition of thin silver films for conductive coatings, special mirrors, or optoelectronics rests on silver acetate’s ability to deposit metal under mild conditions. Medical researchers once eyed it for bactericidal dressings and surface treatments; though newer antibiotics took over, the potential for topical disinfectants still gets attention in certain veterinary and burn-care applications. Outside the mainstream, a few analytical techniques pull silver acetate in for precipitation reactions, separating and detecting halogens or organic functional groups in complex samples.
Interest in silver acetate as an R&D platform tracks the broader trends in sustainable chemistry and material science. Green chemistry advocates look to it as a milder route for silver ion delivery, reducing the risks tied to more aggressive silver salts like nitrate. Multinuclear catalysis themes keep appearing at conferences, where silver acetate acts as a ligand donor or partner to transition metals, giving rise to new classes of catalytic cycles. Nanotechnology labs call on its decomposition pathways to shape silver nanoparticles with stricter control over size and dispersity than pure metal salts allow. Around the world, universities and private labs explore its use as an antibacterial or antifungal agent for coatings, sensors, and water purification. My own reading and lab time confirms a steady push to make silver acetate processing less wasteful, focusing on closed-loop recovery, green solvents, and low-waste synthesis. Environmental impact and cost remain top-of-mind, given silver’s notorious price swings and the sluggish pace of recycling for precious metals.
Toxicology studies on silver acetate show a complicated picture. Silver ions have real power to disrupt enzymes and cellular membranes, accounting for its bactericidal punch. At the same time, repeated exposure can cause cumulative silver buildup in tissues, a persistent risk for workers and the environment. Data from animal models show moderate toxicity via ingestion, with most of the acute effect tied to the silver rather than the acetate ion. In water and soil, silver compounds threaten aquatic life, even at low concentrations. Most modern safety reviews stress minimizing direct skin contact and advocating for closed systems where possible. I’ve sat through enough lab safety briefings to learn that spills, though rare, must get prompt attention and strict logging. Regulators around the globe watch silver discharge closely, driving many labs toward safer disposal and recovery methods. Less is known about the subtle effects from trace airborne silver, so newer studies look at dust exposure, surface contamination, and long-term inhalation risk.
Looking ahead, silver acetate’s future seems to rest on innovation in both science and industry. The ongoing push for greener chemical processes keeps silver acetate relevant, especially when paired with recyclable solvents and integrated waste capture. New tools in nanoscale synthesis and additive manufacturing call for silver compounds that enable delicate metal deposition. Biomedical engineering keeps the door open for silver’s reemergence in wound care, implant coatings, and antimicrobial surfaces—it’s a field where resistance to conventional antibiotics pushes researchers to revisit old metals. In electronics and optoelectronics, ever-thinner, purer silver layers find uses ranging from flexible circuits to solar cell contacts. The key will be cost: efficiently recovering and reusing silver from spent processes, rather than relying on continuous mining, defines success. Drawing from what I’ve seen in the lab, the future of silver acetate won’t be in blockbuster applications, but rather in its subtle, powerful support of high-precision, low-footprint chemical processes that demand just a touch of silver’s special chemistry.
Silver acetate doesn’t grab headlines like antibiotics or semiconductors, though it quietly plays a role in both the laboratory and a few odd corners of daily life. In chemistry labs, it helps turn raw materials into something more useful, which brings me back to summers in college, hunched over a fume hood, turning glass vials of cloudy liquids into crystalline products. The role of silver acetate in organic chemistry lies in the way it lets scientists add or swap functional groups on carbon chains—think upgrading raw gas into useful fuel. These processes build new compounds, many of which come up in drug development and advanced materials research.
Much of today’s conversation around antimicrobials centers on drug resistance and the overuse of antibiotics. Silver compounds, acetate included, make an interesting counterpoint. The silver ion has a way of scrambling bacteria’s ability to function. Hospitals once coated medical devices in silver-based substances to reduce infections, and some still do. Silver acetate itself showed up in specialty coatings for things like wound dressings or medical equipment, serving as a silent guardian against infection. For those who've worked with silver compounds, the power to stop bacteria in their tracks looks impressive, even though over-reliance on silver won't solve every problem. Still, it adds another line of defense, especially on surfaces that need to stay clean.
Silver acetate pops up in history books about public health, too. After researchers noticed this compound’s bitter taste, it wound up in stop-smoking aids during the 1970s and 80s. People sprayed the acetate solution on cigarettes, hoping the resulting taste would break the habit. It wasn’t a magic fix, but studies showed some smokers managed to quit. I remember sorting through old pharmacy records for a research project and seeing the stiff price tags and lengthy warning labels. There’s a reminder here about the lengths people will travel for a healthier life, and how chemistry, for better or worse, finds its way into human behavior.
Beyond medicine and behavior change, silver acetate keeps its foot in several industrial doors. It reacts with halides—fluorides, chlorides, bromides—to help manufacturers purify chemicals or clean up unwanted byproducts. In my time visiting chemical plants, silver salts always held a reputation for effectiveness and cost. They’re not cheap, so plants usually reserve them for processes where nothing else works as well. Silver acetate sometimes helps in making catalysts for specialty reactions that manufacturers can't substitute easily, which speaks to its unique value in advanced chemical work.
Handling silver acetate brings its own education. Anyone who’s spent time in a proper lab learns fast about safety: the compound stains skin black and toxic fumes demand full protective gear. That risk teaches respect for materials, a lesson as old as science itself. Waste from silver processes can pollute water, if not handled correctly. Facility managers install silver recovery systems, and researchers look for ways to reuse what they can. Silver remains both resource and responsibility.
The story of silver acetate shows how a single chemical can punch far above its weight—from fighting bacteria to nudging people toward healthier choices. Its risks remind us that progress in chemistry always involves thinking through the tradeoffs, one reaction at a time.
Silver acetate, with the chemical formula AgC2H3O2 (sometimes shown as AgCH3COO), rarely grabs headlines outside specialist circles. Yet this simple white salt can tell you a lot about the tricky balance between chemistry in the lab and out in the real world. Silver acetate isn’t just some dusty compound gathering cobwebs on a shelf; it shows up in experiments, medicine, and helps shape discussions around safety and environmental concerns.
There’s a point where learning the basics, like the formula AgC2H3O2, starts to matter in daily practice. Silver acetate acts as a starting material for countless reactions, especially in organic synthesis. Its components—silver, carbon, hydrogen, and oxygen—each play a unique part in how the compound behaves. The silver atom lends the compound antimicrobial strength, making it attractive for medical purposes since the late 19th century. Chemists rely on its easy decomposition to metallic silver, using it to coat glassware or as a mild oxidizing agent when tougher chemicals would cause chaos.
It doesn’t take a doctorate to appreciate the value of knowing what goes into a material. I remember working on a project in college where the formula saved my skin; one calculation went off the rails until I checked the stoichiometry directly using AgC2H3O2. Chemistry may seem dry, but one wrong step in grams-to-moles math can wreck a day’s work. For industry, too, the formula is not just an ID tag. It helps techs avoid mistakes in mixing, storing, and disposing of chemicals. Wastewater treatment plants have found silver compounds in the outflow, making the chemical’s makeup a hot topic for downstream testing and environmental controls.
Silver acetate is less famous than its cousin silver nitrate, but it doesn’t escape scrutiny. The compound’s mild antimicrobial powers have led to its presence in old remedies, though ingestion brings risks: too much silver in the body can trigger a permanent gray tinge to skin—a condition known as argyria. Governments regulate silver content in products for good reason. In fact, the Environmental Protection Agency (EPA) lists silver on its drinking water contaminant candidate list.
Responsible use starts with understanding chemical identities. Handling procedures don’t just grow out of thin air; they’re built around formulas and the properties implied by them. Labs that work with silver acetate need specific cleanup strategies because of the way it breaks down and how silver ions move through the environment.
We can’t ignore waste. As research and medicine evolve, silver acetate use will likely rise. Smarter recycling—like methods to recover silver from used labware or repurpose silver ions from industrial runoff—can cut waste and costs. On top of that, more accurate testing methods help reduce the chance of accidental pollution.
The chemistry packed into AgC2H3O2 shapes a lot of what happens in science labs, factories, and even our regulatory agencies. At its core, grasping a chemical formula goes beyond memorization. It fuels progress, advances safety, and opens up new solutions.
People who spend time in a lab or in advanced chemistry classes see silver acetate on the bench now and then. It looks like a simple white powder, almost unimposing. For those who have worked with similar chemicals before, it might seem low-risk. Its uses crop up in fields from organic synthesis to photography. Most aren't working with buckets of it, but a careless attitude can get the best of anyone.
Trusting a substance just because it’s not a household name can mislead. Silver acetate earned its spot in safety manuals for good reason. Coughing, burning sensations, and even damage to mucous membranes have shown up in people who inhaled dust from the compound. Touching it, even without a cut or burn, might still cause skin irritation for those with sensitive skin.
A bigger problem lurks with silver ions. Studies show silver can accumulate in the body, particularly in skin and eyes. Chronic exposure—rare for casual users but possible for researchers—can set off a silver staining reaction called argyria. Skin, gums, or eyes take on a bluish tint, and, though painless, it’s permanent.
In the past, I watched a colleague handle silver salts without gloves, then unconsciously rub his eyes. He ended the day with redness and swelling that stuck around for days. Warnings don’t come just from dusty textbooks.
It’s tempting to brush off gloves for “just one quick experiment.” That’s a risk not worth taking. The powder can be unforgiving if it gets into cuts, eyes, or on food. Even tiny bits can cause big headaches later, especially since silver sticks around in the body.
Accidents aren’t rare. NIOSH and OSHA flag silver acetate as hazardous, recommending good ventilation and gloves. It has a low solubility in water, but that doesn’t mean it won't travel through the body or environment. Silver compounds have made their way into rivers and soils, harming fish and invertebrates. This is one reason for strict disposal requirements for silver solutions or contaminated materials.
Common sense works well. Gloves, goggles, and a fume hood prevent problems before they start. Washing hands after use keeps stray dust from leaving the lab. Treat any spill with caution—a spill kit and proper cleaning supplies save time, money, and trouble down the line. Lab training may seem tedious, yet those drills make sure that, in a real mess-up, no one freezes or forgets protocol.
Proper labeling and storage let everyone know what they’re dealing with. Don’t store silver acetate near materials that easily burn; this compound can make a fire risk worse by providing oxygen. Even at the end of an experiment, attention pays off. Collect waste promptly and label it for hazardous disposal.
Even a career in chemistry or a related job doesn’t guarantee immunity to lapses in judgment. I learned a valuable lesson: treat every unfamiliar white powder as if it might cause trouble. There’s comfort knowing that good habits become second nature. Silver acetate deserves the same respect as more notorious chemicals. Treat it right, and it’ll never become a headline for the wrong reasons.
Every time I’ve pulled silver acetate from the supply shelf, the guidelines have echoed in my head. From a chemist’s point of view, safety isn’t about showy storage cabinets and expensive signs—it’s about keeping things simple, sharp, and straightforward. Silver acetate brings its own set of quirks. It’s less notorious than silver nitrate, but it reacts to light, heat, and some common materials like a moody cat reacts to a new house guest.
Direct sunlight surprises more chemicals than you’d think. Silver acetate gets feisty under strong light, sometimes turning darker, sometimes breaking down, always making things messier. So I keep mine in an amber glass bottle, or hidden deep in a shelf where daylight never visits. This trick cuts down on breakdown and keeps reordering at bay. Lab supplies cost enough already without wasting material to careless storage.
Moisture sneaks into lids and fiddles with crystal structures. Silver acetate holds up okay in dry conditions, but humidity brings in clumping, dilution, and, worst of all, slow-forming acids that could pit your glassware. I tuck bottles away in a desiccator jar filled with silica gel packets—easier and cheaper than battling ruined reagents. Even in a closet, a sealed plastic tub with a pack of silica can work wonders. Letting chemicals get damp out of laziness isn’t a shortcut, it’s an expensive mistake.
Leaving bottles near a heating vent or refrigerator exhaust goes beyond comfort—heat makes silver acetate degrade, sometimes releasing faint vinegar smells that linger longer than today’s to-do list. Keep it at room temperature, away from direct heat sources, and you will thank yourself later. A cool, steady spot wins over any dramatic science fiction cooling idea. The material wants a boring life on your shelf.
The best chemists I know never toss everything on a shelf like a jumble sale. I keep my silver acetate well away from strong acids, ammonia, and easily oxidized materials. No one wants weird stains or new mystery compounds forming in a dark corner. Once, a coworker’s casual storage turned into a sticky, dark puddle that took half a day to clean up. A little labeling and thought before putting a bottle down can save hours, and possibly keep your department out of the news for all the wrong reasons.
It’s easy to take gloves and goggles for granted, but silver salts stain skin and can be more irritating than a thousand paper cuts. I’ve learned to check labels, use basic equipment, and keep my chemical workspace clear. I wash up right after handling, too. The stains and the irritation aren’t worth a rushed morning.
Obvious labels matter. New hires, old-timers, and visitors layer into a lab’s daily routine, and clear writing saves mistakes. “Silver acetate—keep dry, dark, room temp” scrawled in clear marker, not faded into chemical hieroglyphs, solves more issues than a dozen supplement policies.
All these steps come from past lessons, minor mishaps, and a lot of listening to folks smarter than me. Keeping silver acetate safe isn’t about ticking boxes. It’s about respecting chemicals, protecting investments, and making sure you don’t spend next Friday fighting with a smelly cleanup.
Silver acetate stands out right away for its color. Most chemicals in a college lab look dull or simply white, but this compound strikes with a pale yellow shade. Holding the powder, you will notice a texture almost like fine flour. It doesn’t clump the way sugar does, making it easy to scoop or weigh out for experiments. Its weak vinegar-like smell makes it memorable if you’ve ever handled it during a chemistry course, although the scent drifts away quickly.
Drop a bit of silver acetate in water and you’ll see it doesn’t dissolve right away. Unlike table salt or sugar, this faint yellow powder resists mixing in. It’s only slightly soluble (about 1 gram dissolves in 100 milliliters at room temperature). Sometimes, the persistent cloud in the beaker can confuse new chemistry students who expect chemicals to vanish into the liquid. This low solubility plays a role in real-world uses, especially for those working with silver recovery or antimicrobial materials.
The melting point of silver acetate sits around 220 degrees Celsius. If you try to heat it higher, it breaks down before it boils. Heating past its melting point releases acetic acid vapors and dark, metallic silver starts to collect. This decomposition means it’s rarely melted or boiled in industrial setups. Handling silver acetate at high temperatures calls for care and proper ventilation because those fumes irritate the nose and lungs.
If you look at it under a microscope or grow a large enough sample, silver acetate forms crystals—flat, needle-like shapes. Its structure follows a monoclinic arrangement, which means the atoms pack in a specific inclined way rather than the perfect cubes seen in some salts. This explains why the powder has a soft glimmer instead of a glassy shine. The density clocks in at about 3.26 grams per cubic centimeter, noticeably heavier than water or many organic solids. Pour some on a scale and the numbers climb faster than you’d expect from a pile of powder the same size as baking soda.
Store silver acetate in a sunny spot, and the yellow starts to deepen. Over time, it turns darker due to a slow reaction with light. Silver ions in the powder shift into tiny bits of metallic silver—almost like those old black-and-white photos developing. That’s why most scientists keep it in colored bottles or dark drawers. Air itself doesn’t bother it much, but both high humidity and direct sunlight shorten its shelf life.
Getting silver acetate on your hands won’t burn, but it stains skin a greyish color that’s slow to wash out. Lab students usually remember to keep gloves on just from experience. If you pour leftovers down the drain, you aren’t just wasting silver—the runoff harms aquatic life. Many labs now collect waste and send it to recycling, using the leftover silver for new processes or products.
Physical properties guide how people use and store silver acetate. That pale yellow powder, held together in a simple glass bottle, brings together key lessons from many branches of science: safe handling, environmental care, and the small ways matter surprises us under a microscope or in the palm of your hand.
| Names | |
| Preferred IUPAC name | Silver ethanolate |
| Other names |
Acetic acid silver salt Silver ethanoate |
| Pronunciation | /ˈsɪl.vər əˈsiː.teɪt/ |
| Identifiers | |
| CAS Number | 563-63-3 |
| Beilstein Reference | 1901876 |
| ChEBI | CHEBI:85258 |
| ChEMBL | CHEMBL1223403 |
| ChemSpider | 13152 |
| DrugBank | DB01323 |
| ECHA InfoCard | 100.012.700 |
| EC Number | 206-112-6 |
| Gmelin Reference | 754 |
| KEGG | C13921 |
| MeSH | D000690 |
| PubChem CID | 8995 |
| RTECS number | AJ4300000 |
| UNII | 4Z5B6RUH9O |
| UN number | UN2811 |
| Properties | |
| Chemical formula | AgC2H3O2 |
| Molar mass | 166.91 g/mol |
| Appearance | White to grayish powder |
| Odor | Odorless |
| Density | 1.74 g/cm³ |
| Solubility in water | 1.02 g/100 mL (20 °C) |
| log P | -0.41 |
| Vapor pressure | <0.01 mmHg (25°C) |
| Acidity (pKa) | Acidity (pKa): 4.76 |
| Basicity (pKb) | pKb = 9.23 |
| Magnetic susceptibility (χ) | -26.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.52 |
| Dipole moment | 2.17 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | S⦵298 = 143.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -208.0 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -318.5 kJ/mol |
| Pharmacology | |
| ATC code | S01AX11 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes severe skin burns and eye damage, may cause respiratory irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS07,GHS09 |
| Signal word | Danger |
| Hazard statements | H302: Harmful if swallowed. |
| Precautionary statements | P210, P261, P264, P270, P271, P301+P312, P304+P340, P305+P351+P338, P312, P330, P337+P313, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 2-3-2 |
| Explosive limits | Non-explosive |
| Lethal dose or concentration | LD₅₀ (oral, rat): 36 mg/kg |
| LD50 (median dose) | LD50 (median dose): 36 mg/kg (oral, rat) |
| NIOSH | SR 1400 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) of Silver Acetate: "0.01 mg/m³ (as Ag) |
| REL (Recommended) | 50 mg/L |
| IDLH (Immediate danger) | IDLH: 10 mg/m³ |
| Related compounds | |
| Related compounds |
Silver nitrate Silver carbonate Silver chloride Acetic acid Potassium acetate Sodium acetate |
