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Ammonium formate started making waves in laboratories soon after chemists managed to synthesize it from formic acid and ammonia. Back in the late 1800s, researchers in both Europe and North America spent plenty of hours trying to wrangle organic acids and their salts into more workable chemical tools for emerging scientists. The drive mainly came from efforts to improve catalysts and reduce metals in safer, cleaner ways compared to harsh mineral acids. Academic papers from the middle of the twentieth century point to ammonium formate gaining steady ground in reduction experiments and chromatography. I found that, by the time the 1970s rolled around, big chemical companies began listing it in catalogs as purification processes shaped up and demand in industrial labs increased. Throughout all that time, compositional standards tightened and the chemical earned a solid reputation for both reliability and utility on the bench.
Ammonium formate goes by C-H5-N-O2 in chemical shorthand and looks much like a white crystalline powder, though sometimes it comes off with a slightly tacky feel in humid environments. In stores that serve local labs and on global chemical dealer catalogs, you’ll find it in sealed plastic or glass containers, usually labeled to warn about its tendency to absorb moisture and give off a faint scent, like vinegar mixed with ammonia. Some variants get granularized for better handling or come as aqueous solutions, mostly for chromatography and biochemistry work. I’ve seen it stabilize mobile phases in HPLC and step into reduction reactions where classic hydrides prove too reactive or just unsafe.
Ammonium formate settles at a melting point around 116–120°C and dissolves freely in water and lower alcohols without fuss. Its density sits at about 1.27 g/cm³. The material decomposes at higher temperatures, giving off formamide, ammonia, carbon dioxide, and a whiff of formic acid. Dry ammonium formate keeps best at room temperature in sealed containers, protected from humidity which can kick off caking and slow degradation. One notable point: left exposed, the powder can clump, though it’s not nearly as hygroscopic as straight ammonium salts. Hydrolysis, if left unchecked in water, will tip a solution more acidic as ammonium and formate ions shift their equilibrium. Reactivity is mild under ambient conditions but jumps in the presence of strong acids, oxidizing agents, or heavy metals.
Manufacturers mark technical grades by purity, moisture percentage, and traces of metallic impurities—iron, copper, and sodium show up as key markers. Typical lab grades offer at least 97% purity with moisture content under 0.5%, though higher-research grades go above 99%. Labels show molecular formula and weight (63.06 g/mol), storage instructions, batch numbers, and hazard notations following GHS standards. Packaging ranges from 100-gram bottles to multi-kilogram drums, always with clear expiry dates. In larger outfits, barcode tracking pumps up traceability from warehouse to workbench, as regulatory regimes demand clean records for every reagent used in regulated environments.
Simple chemistry creates ammonium formate on an industrial scale. Mix formic acid (often derived from the carbonylation of methanol or direct synthesis from carbon monoxide and water) with high-purity aqueous ammonia, keep the temperature under close watch, and concentrate the liquor to drive off water while crystallizing the salt. Some labs coax the reaction gently at low temperatures, aiming for small, even crystals, while larger operations turn to continuous evaporators. The mother liquor, once drained, yields crude salt; subsequent recrystallization clears contaminant ions, which can otherwise interfere with analytical work. For extra-high-purity requirements, strictly deionized water and vacuum drying step in, trimming down residual mineral content.
In labs where reductive reactions matter, ammonium formate proves its worth by decomposing in the presence of palladium catalysts, yielding hydrogen in situ—key for hydrogenation and deprotection steps in complex molecule building. The salt reduces nitro and keto compounds under mild conditions and sits at the core of catalytic transfer hydrogenation. In biochemistry, it buffers mobile phases for protein and nucleic acid separations. Modifications sometimes involve swapping in D2O or isotopically labeled formic acid to create tracers for analytical experiments. On the flip side, it can react with strong acids to liberate pure formic acid or serve as a precursor in stepwise synthesis pathways, chipping away to formamide or higher-order amides when cooked up in the right conditions. Once, I saw a team use it to free up costlier hydrogenation catalysts by regenerating them in situ, saving cash and device downtime.
Across catalogs and regulatory documents, ammonium formate goes by several names: Ammonium methanoate, Formic acid ammonium salt, and the EINECS number 208-692-3. CAS registry tags it with the number 540-69-2. Regulatory listings often tuck it under organic salt categories, while trade journals and technical studies flip between the IUPAC and common names, depending on context. Science journals like to keep to the shortest label, often sticking to "ammonium formate" unless they drift into reactivity studies, where its methanoate moniker pops up to ease communication.
Working with ammonium formate doesn’t stir up the same level of concern as stronger acids or bases, but it demands respect. Direct contact causes mild skin and eye irritation, especially in concentrated solutions. Inhalation of dust or vapor can irritate mucous membranes, so gloves, goggles, and dust masks serve as solid precautionary steps. Labs that grind or weigh it in large batches keep local exhaust or HEPA-filtered hoods running. Storage guidelines stress cool, dry locations far from strong acids and oxidizers; spills clean up quickly with water and absorbent pads. Disposal routes in most countries allow moderate dilution and flushing with water, though big users funnel waste to professional treatment to avoid boosting waterway nitrogen loads. Safety data sheets cover reactivity, first aid, and fire-fighting techniques, emphasizing that the chemical, while not highly flammable, decomposes if overheated, releasing hazardous fumes including ammonia and oxides of nitrogen—agents best avoided by good practice and regular ventilation checks. Here, regulatory training and up-to-date handling certifications for lab staff become a non-negotiable foundation for smooth day-to-day work.
Ammonium formate rides high in analytical chemistry, forming a core component of mobile phases in LC/MS and HPLC, where it fine-tunes pH and shapes peak separation for biologically relevant molecules. It also steps into catalysis, particularly in transfer hydrogenation, where it brings milder reduction steps to complex organic substrates without calling in explosive or unstable reagents. In pharmaceuticals, the compound helps create key intermediates for active drugs, while textile and leather processors use smaller amounts as a pH buffer and mild reducing agent. Environmental labs appreciate its role in breaking down nitrogen oxides and trapping atmospheric nitrogen for gas analysis. Because it doesn’t build up persistent residues, industries tend to favor it where trace-level detection really matters—think pesticide testing or food safety compliance. Teaching labs keep it on hand for redox demonstration experiments, showcasing both its reactivity and relative safety to new students.
In the last decade, the pace of study on ammonium formate sped up, especially as instrument makers and green chemists hunted down safer and more sustainable chemical tools. Analytical chemists dug deep into its buffering capacity under high-pressure liquid chromatography, optimizing protocols for both reproducibility and sensitivity. Patent literature tracks a steady drumbeat of new catalyst systems that use ammonium formate to generate hydrogen or manipulate selective reductions. Researchers in protein science and metabolomics keep improving sample preparation by precisely adjusting salt concentration and minimizing suppression in mass spectrometry. Multinational consortia, including big pharma groups, run comparative studies of ammonium formate versus phosphate buffers where regulatory clean-room processes rule. I’ve followed a few projects harnessing its rapid breakdown under mild heating to drive low-energy hydrogen production, nudging industry toward more circular chemistries.
Toxicologists rate ammonium formate as having moderate acute toxicity. Ingestion triggers nausea and gastric distress, and high-level exposure delivers headaches and shortness of breath. Chronic effects remain rare at occupational exposure levels, though animal studies highlight that large doses disrupt acid–base balance and impact kidney function. Routine safety reviews pin the LD50 (oral, rat) at roughly 1580 mg/kg; this reference guides most hazard communication. Environmental impact surveys conclude that small amounts degrade quickly in water and soil, and regulatory reports label it as non-persistent and low-risk for accumulation. Even so, waste management best practices aim to limit large discharges, particularly where sensitive aquatic environments lie downstream. Emergency protocols urge prompt medical evaluation for accidental ingestion or inhalation, following established toxicological pathways used for ammonia and low-molar weight organic acids.
The road ahead for ammonium formate carries promise as chemical manufacturing leans into lower-impact, resource-efficient synthesis. With hydrogen technologies gathering speed and regulatory bodies demanding greener processes, its use in catalytic hydrogenation and fuel cell research should only climb. Portable reduction systems, especially in on-the-go chemical investigation tools for environmental monitoring, stand to gain from its ease of handling and effective chemical footprint. More instrument makers now turn to ammonium formate for solvent optimization, designing columns and detection systems tuned around its chemical properties. Advances in biotechnology and drug design will continue to call for predictable, stable reagents that marry efficiency with manageability—qualities this compound delivers. I see industry-facing R&D teams working up custom modifiers to push the buffering capacity further or exploit derivatizations for trace detection. With regulations tightening around chemical emissions and waste, ammonium formate’s clean decomposition and low residue factor keep it in the running for new production and analytical innovations. If past experience guides, its quiet utility now could soon translate to headline roles in safer, smarter chemistry.
Walk into any chemistry lab and you’ll likely spot a white crystalline powder tucked alongside bottles of acids and solvents. Ammonium formate doesn’t carry the flash of gold or the bite of strong acids, but it does a hefty job. The main action happens behind the scenes in the world of chemical synthesis and analysis—a world that quietly powers medicine, clean water, and modern materials.
Ammonium formate shows up a lot in the work of people like me, who’ve spent late nights troubleshooting machines or getting chemicals to work together right. It shines as a buffer in high-performance liquid chromatography (HPLC). In simpler terms, HPLC lets scientists separate and identify what’s in everything from blood samples to groundwater. These days, labs want methods that not only separate things well but also avoid nasty residues in sensitive instruments. Ammonium formate dissolves in water or methanol and doesn’t leave behind sticky leftovers. This simple property means fewer broken machines, faster results, and happier lab workers.
Drug companies lean on ammonium formate for making pure products. For example, it plays a key role as a hydrogen source for gentle reduction reactions, especially through a process known as catalytic transfer hydrogenation. Instead of dealing with dangerous gases under high pressure, chemists can use ammonium formate with a palladium catalyst to safely turn nitro groups into amines—a common step in making medicine. It takes out some of the risk and makes life easier for anyone handling it. That shift toward safer chemistry has real meaning for the safety of those workers and for the cost of producing the pills people take every day.
Beyond drug development, ammonium formate has a place among folks testing soil and water. Many government agencies and private labs use HPLC with buffers including ammonium formate to track pollutants like pesticides or pharmaceutical residues. People trust those results when setting limits for tap water and keeping agriculture honest. Getting clear and accurate readings depends on these buffers while making sure leftover chemicals don’t add to waste streams.
I remember pushing cost projections for small research projects: sodium buffers were cheap, but didn’t always work well with organic blends. Ammonium formate landed in the sweet spot. It’s affordable and available through standard suppliers. Its safety profile outshines alternatives like formic acid alone, which can be tough on skin and equipment. Rather than rely only on strong acids or more expensive blends, switching to this compound means safer storage and less corrosion on pricey lab hardware.
People need to remember that even mild-sounding chemicals demand good handling. Storing ammonium formate properly, avoiding mixing it with strong oxidizers, and planning disposal routes keep staff and communities safe. Lots of labs want greener processes, so they’ve started recapturing and recycling spent buffer solutions. College labs and businesses have both seen success by collecting and treating ammonium formate waste, instead of washing it straight down the drain.
Ammonium formate remains a quiet workhorse for science and industry. Its role in safer lab work, cleaner reactions, and more accurate measurements often goes unnoticed—yet without it, many breakthroughs wouldn’t make it past the starting line. As people push for more sustainable labs, finding smarter ways to use and recycle ammonium formate will matter even more. The small choices in the chemicals we lean on can change how we make discoveries and protect our world.
Anyone working in labs or chemical production will meet ammonium formate sooner or later. Plenty of folks turn to it for its role in making pharmaceuticals, improving chromatography, or working up hydrogen in certain reactions. More than once, I’ve measured out this white, crystalline powder for experiments. People ask: Is it actually safe?
It helps to look at safety from real-life experience, not just technical data sheets. Breathing in ammonium formate dust can irritate the respiratory tract. Its powder forms can bother the skin or eyes if you end up with a pinch where it doesn’t belong. Let’s not underestimate what irritation can mean: missed days, lost focus, or bigger mistakes if discomfort prompts someone to rush.
The chemical can release formic acid and ammonia — both irritants — especially if it gets hot or mixed with acids or bases. Dumping it down a sink or storing near strong acids sounds convenient, but you never know when a bit of careless mixing will create fumes. Proper labeling and storage keep people safe. I’ve seen new staff miss this step and wind up with headaches or worse after mixing chemicals in a hurry.
The science backs up real-world stories. The European Chemicals Agency lists ammonium formate as an irritant but doesn’t push it onto the list of substances that cause cancer, birth defects, or major chronic health issues when handled in small quantities with protection. Wearing gloves, goggles, and a lab coat stops the most common problems. A good fume hood, or even just a window nearby, makes it much safer to weigh and mix the material without a cloud of fine dust.
I’ve handled bigger spills too. The reassuring part? With rubber gloves and enough ventilation, cleaning up a mess turns into more of an inconvenience than anything dangerous. It’s easy to forget the basics: don’t eat at your bench, keep hands away from the face, and wash up before leaving. Not glamorous advice, but it works.
Avoiding trouble means treating ammonium formate with respect. Training goes much further than any printed label. I’ve worked with students who felt silly reviewing basic chemical handling, only to realize later that skipping it brings risk not just for themselves, but for everyone nearby. Feedback from folks in the room is gold—more eyes spot forgotten labels or a spill on the sleeve. In team settings, reminders come naturally and everyone stays alert.
Regulations might seem strict, but these are built from hard-won lessons over time. The Occupational Safety and Health Administration recommends limits on exposure due to irritation risk. That comes straight from the experience of people who didn’t always have personal protective gear or clearly marked ventilation. Good management supplies up-to-date safety data sheets, keeps gear handy, and encourages questions.
A safer environment means more than a checklist. Encouraging a culture where staff look out for hazards, share near-miss stories, and actually use the safety tools provided gets results. Switching to pre-measured forms or safer alternatives makes sense in many operations, especially where less-experienced handlers work. Some producers now supply ammonium formate in tablets or sealed containers to limit dust and accidents. There’s evidence this reduces injuries and keeps everyone focused on their main task rather than damage control.
Every compound gets its start from the world of chemistry where patterns and formulas don’t just help scientists — they give direction to countless industries. Ammonium formate comes together from two everyday pieces: ammonium and formate. This compound’s formula, NH4HCOO, keeps coming up in labs, pharmaceutical workshops, and classrooms.
Years ago in college, my first real hands-on encounter with this salt stood out. Someone showed me the white powder, explained how just one ammonium ion (NH4+) and one formate ion (HCOO-) collided to create it, and suddenly, all those textbook equations snapped into focus. No long equation — just a clean fusion bringing together nitrogen, hydrogen, carbon, and oxygen.
The chemical formula spells out these connections. It doesn’t just tell you what’s inside. It gives a map: four hydrogens and a nitrogen tie up with a carbon, two more oxygens, and another hydrogen. It matters in labs because this balance shapes whether a reaction succeeds or falls flat.
Large-scale labs and backyard tinkerers both run into ammonium formate. It finds its way into food science, pharmaceuticals, and even gas chromatography. Its decomposition at low temperatures means it offers a clean source of hydrogen. For those working with sensitive reactions where impurities cloud results, this feature stands out.
I watched a friend struggle for weeks with a reaction meant to create a delicate organic compound. After swapping in ammonium formate as a gentle hydrogen donor, yields improved. The difference? Less residue, clearer results, and less time troubleshooting.
You don’t always need complex machinery to make ammonium formate. Reacting ammonia with formic acid gets you there, plain and simple. This accessibility matters if you’re in a small research lab or a classroom where budgets stretch thin.
Safety remains a key issue. Ammonia’s vapors and formic acid’s corrosive nature mean basic protective gear is non-negotiable. At the university, I learned to check for spills and proper ventilation before even opening a bottle. These habits stick and translate to safer, more reliable research.
A formula as short as NH4HCOO holds weight because small mistakes with numbers or letters mean botched experiments and wasted money. This isn’t just a chemistry quiz answer — it touches anything that depends on precise formulations, like medication purity or energy storage tech.
Science keeps pushing forward because details, even in one-line formulas, never slip past the careful hands of researchers and workers. No matter the application, clarity in those formulas signals trust. It also stops costly accidents and product recalls before they ever start.
Getting comfortable with the chemical formula of ammonium formate lets anyone — student, technician, or seasoned scientist — handle both the practical and safety sides of chemistry. Schools and workplaces can push for regular training, clear labeling, and routine safety checks. Even a short refresher session on reading and writing formulas helps. Tools like apps and checklists keep identification sharp and cut down on expensive mistakes.
No one’s above learning the basics, especially in settings where one wrong figure can ripple through to the final result. The chemical formula NH4HCOO might seem small, but in my experience, getting it right opens doors while sloppy habits slam them shut.
Ammonium formate shows up in many labs and industrial spaces, mostly for chemical synthesis and analytical chemistry. It looks innocent enough: a white, crystalline solid, easy to underestimate. Under the wrong conditions, it can decompose, releasing gases and posing health and safety issues. Getting storage wrong risks costly clean-ups, ruined experiments, and serious hazards for anyone nearby.
Let’s get practical. Any chemical with reactivity concerns deserves respect. Ammonium formate, with its tendency to break down above room temperature, benefits from a cool, dry place. Talking from experience, a storeroom sitting above 25°C can turn this solid into a problem. Stick to below 25°C, shade away from windows or direct sunlight, never near heaters nor vents blowing warm air.
Humidity doesn’t mix well with ammonium formate either. I have seen containers clump up and even leak after a humid morning left the lab air dense with moisture. The container should seal tightly—plastic or glass works, but always with a good screw cap. Broken seals turn a shelf-stable powder into a sticky mess or worse, a source of contamination.
Mixing ammonium formate with the wrong neighbor spells trouble. Strong acids, alkalis, oxidizers, and nitrites all bring out its reactive side, which means those aren’t storage buddies. Shelving matters. Anyone who’s spent time in a shared lab knows shelving mistakes lead to more than just confusion—unexpected reactions can wreck not only the chemicals, but the storage environment itself. Flammable solvents and oxidizers should always stay a few shelves away.
You find chemicals tucked away in every possible spot in some older research spaces. Poor labeling turns storage into a guessing game. Every bottle or jar should show the chemical name, concentration or purity if needed, date received, and hazard warnings. Re-labeling takes five minutes, but saves hours of trouble. Follow the Globally Harmonized System (GHS) for hazard communication. Sharp, legible markers and ready-to-read hazard codes make sure anyone can act fast during emergencies.
Any spill or leak from improper storage demands quick response. Having easy access to spill kits, gloves, safety goggles, and a fume hood saves the day. Never cut corners with protective gear. I once saw someone skip gloves because “it’s just ammonium formate” and weeks later, we dealt with an allergic rash and ruined samples. Treat every handling, including transfers between containers, with the expectation of an unexpected reaction or slip.
Routine audits for storage work. You spot leaks, rust, broken lids, or expired stock before they bite. Training matters even more. There are always new faces in university labs and research centers. Peer-to-peer teaching about safe handling, proper sealing, and shelf organization drives down risk better than any memo or safety poster ever could.
Modern labs use digital inventory tools for tracking, QR code tagging, and automatic expiry reminders. It doesn’t take high-tech to boost safety—simple spreadsheets or logbooks with check-in and check-out records go a long way. Companies can support this by distributing chemicals in tamper-proof, air-tight packaging and providing detailed safety data sheets with each batch.
Safe storage starts with clear routines and low tolerance for shortcuts. Sometimes, great science hinges on where and how a bottle sits on a shelf.
Ammonium formate, widely present in labs and across industry, changes things fast with its simple chemical makeup. Plenty of people see this compound as mild, but it brings a few real risks to the table. After working around it, one lesson stands out: chemicals with the label “mild” still find ways to cause problems when ignored or handled without preparation.
Let’s get straight to what most people care about: health. Breathing in ammonium formate dust doesn’t sound dangerous. Still, I’ve helped clean up lab spaces where people developed a nagging cough and irritated eyes. It often starts as a tickle in your throat or watery eyes, but over time, those small symptoms stack up. We’re not talking about instant emergencies, but chronic exposure likely creates more serious, lasting effects like respiratory trouble or skin reactions. Direct contact feels like a mild sting; repeated exposure can dry out skin or trigger larger rashes.
Accidental spills, especially in closed rooms lacking ventilation, really crank up the risk. The smell, sharp and chemical, catches you by surprise. Ammonium formate can break down, especially when heated, releasing formic acid and ammonia gas. Each byproduct marks a new set of risks, with ammonia able to cause severe eye or lung irritation in unprotected people.
Every spill or waste stream carries ammonium formate into watersheds and soil. Water samples tell the story better than any regulatory pamphlet: aquatic life takes a hit even at low concentrations. Dead zones form downstream when runoff happens, not because of just one big spill, but ongoing leaks and small mistakes. Nitrification in local water rises, kicking off a cycle of excess algae and dead fish. Rural communities with private wells worry over groundwater quality—not from large disasters but daily routine discharge from production or research sites.
Ammonium formate also has a part in atmospheric issues. As it breaks down, it releases ammonia, which links to particulate matter in the air and contributes to smog, especially near factories. We have to remember that what escapes indoors can eventually leak outside, affecting neighborhoods far beyond the industrial fence.
Some might glance at ammonium formate and think it’s too tame to pose a fire risk. That’s not so. Get it hot enough—say, left near a heat source or mixed by accident with strong acids—and it reacts fast. Major incidents start because someone skipped over the small print on a label and mixed incompatible chemicals, causing heat, gas pressure, and sometimes fire. Even inside the safety of a research lab, familiar smells turn dangerous without solid planning. Anyone dealing with ammonium-containing compounds learns the lesson quickly: safe storage and chemical compatibility aren’t just paperwork.
Controlling risks takes real vigilance. Good ventilation does more than clear the air—it’s fundamental for safety. After years in both busy labs and production sites, I’ve seen how a culture of double-checking storage conditions and using gloves, goggles, and proper containers makes a difference. Regular training and taking minor symptoms seriously helps avoid bigger surprises down the line. Waste management needs as much thought as use: neutralization, containment, and disposal plans separate careless workplaces from the careful ones.
Community right-to-know measures matter, as do regular audits and honest communication. Companies and labs who admit mistakes and share best practices boost safety for everyone inside and outside the facility. Lessons learned rarely come from an instruction manual—they grow from direct experience, concern, and follow-through.
| Names | |
| Preferred IUPAC name | azanium methanoate |
| Other names |
Formic acid, ammonium salt Ammonium methanoate |
| Pronunciation | /əˈmoʊniəm ˈfɔːr.meɪt/ |
| Identifiers | |
| CAS Number | 540-69-2 |
| Beilstein Reference | 3539460 |
| ChEBI | CHEBI:62948 |
| ChEMBL | CHEMBL1233516 |
| ChemSpider | 57904 |
| DrugBank | DB11377 |
| ECHA InfoCard | ECHA InfoCard: 100.028.800 |
| EC Number | 223-320-4 |
| Gmelin Reference | 7788 |
| KEGG | C01059 |
| MeSH | D000648 |
| PubChem CID | 2723781 |
| RTECS number | BXX1845000 |
| UNII | 9JPO19507Z |
| UN number | UN2073 |
| CompTox Dashboard (EPA) | DTXSID4020293 |
| Properties | |
| Chemical formula | NH4HCO2 |
| Molar mass | 63.06 g/mol |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 1.28 g/cm³ |
| Solubility in water | very soluble |
| log P | “-3.37” |
| Acidity (pKa) | pKa1 = 3.75 (formic acid), pKa2 = 9.25 (ammonium ion) |
| Basicity (pKb) | 8.81 |
| Magnetic susceptibility (χ) | -48.0×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.413 |
| Viscosity | 1.9 mPa·s (at 25 °C) |
| Dipole moment | 2.58 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 130.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -567.5 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -567.3 kJ/mol |
| Pharmacology | |
| ATC code | V04CX01 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin and eye irritation, may cause respiratory irritation. |
| GHS labelling | GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H319: Causes serious eye irritation. |
| Precautionary statements | P264, P270, P273, P280, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 1-0-0 |
| Autoignition temperature | > 520 °C (968 °F; 793 K) |
| Lethal dose or concentration | LD50 (oral, rat): 2760 mg/kg |
| LD50 (median dose) | LD50 (median dose) of Ammonium Formate: Oral, rat: 2760 mg/kg |
| NIOSH | Not Listed |
| PEL (Permissible) | PEL (Permissible) for Ammonium Formate: Not established |
| REL (Recommended) | 2–8°C |
| Related compounds | |
| Related compounds |
Sodium formate Potassium formate Ammonium acetate Ammonium benzoate |
