© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Ammonium Iron(II) Sulfate Hexahydrate—some folks call it Mohr’s Salt—is a classic in chemistry labs. The substance stands out among the hydrated iron salts thanks to its soft green crystals. Run your finger across a sample and it feels cool and slightly slippery. Chemists and students both have memories of prepping solutions with this salt, the gentle green getting everywhere if you’re not careful. Its chemical formula, (NH4)2Fe(SO4)2·6H2O, marks it as a double salt, binding iron, ammonium, sulfate and water together. It’s remarkable—not just for its structure, but for the way it balances these components into a reliable, predictable compound.
Crystals of this substance win no contests for glamour, but they’re a staple for good reason. Under the microscope, they appear pale green and slightly vitreous. The density lands around 1.86 g/cm³, which any seasoned chemist can spot as heavier than your everyday salts like sodium chloride but still manageable by hand. Unlike many iron compounds, this salt comes as flakes, powder, solid chunks, or neat little crystals—each form tailored to a lab’s practical workflow. Drop pieces of the crystal in water and watch them dissolve with no fuss, producing a clear, pale-green solution that signals purity. The strong hydration, courtesy of the six water molecules, keeps the salt stable even when left out on the benchtop, a real help to anyone tired of chemicals turning to mush in humid air.
Any chemistry teacher will tell you, this salt finds its way into countless experiments. It serves as a reliable source of ferrous ions for redox titrations or colorimetric analysis. Those who have used it in lab routines know the calm it brings—less risk of oxidation compared to plain old iron(II) sulfate, fewer headaches about storage. In my own time working with titrations, this salt offered consistent results thanks to its chemical structure. The mixture of ammonium and sulfate ions helps tamp down oxidation, giving the iron a chance to do its job as Fe2+ rather than flipping to Fe3+ before you’re ready.
Specifications matter, whether you’re running research or teaching the basics. Based on its chemistry, this salt carries a molar mass of about 392.14 g/mol. Material like this doesn’t come in a “liquid” state, at least not on a shelf. You see it as crystals, powder, or maybe as a fine granular solid. Mix it with water and you get a solution, but the substance itself is distinctly solid. Its HS Code, a detail important for trade, often reads as 2833.29 based on international freight rules for similar salts. These codes keep everything above-board, which helps importers, exporters and safety inspectors track where chemical materials move across borders.
Working with any chemical raises the question: how hazardous is it? Ammonium Iron(II) Sulfate Hexahydrate deserves respect but not fear. It isn’t wildly reactive, nor does it carry the acute toxicity of some more notorious iron salts. But it can still pose risks. Skin and eye contact should be avoided. Inhalation of dust from powders can bother the throat and lungs. Iron compounds, in general, can be harmful if swallowed in significant amounts—the iron content can overwhelm the body’s ability to process it, leading to iron poisoning. From personal habit, gloves and a dust mask become routine when handling fine powders. One other point—keep this compound away from oxidizers. That’s a rule from both a teacher’s playbook and experience. The ammonium can release ammonia, and the iron can react unpleasantly if mixed with strong acids or bases. Rinse the spilled crystals up right away, and always store in a dry spot, far from kids or food, since curiosity and chemistry don’t mix safely at home.
Behind the scenes, the manufacturing of Ammonium Iron(II) Sulfate Hexahydrate taps into the wider story of chemical production. The raw materials mostly include sulfuric acid, ammonium sulfate, and iron(II) sulfate. Each one comes from major industrial processes. Mining and refining give us iron(II) sulfate, while sulfuric acid production stands as one of the world’s largest chemical industries. From this simple trio, manufacturers grow large crystals through carefully controlled crystallization, often monitored for purity and composition at every step. I’ve watched this process in medium-scale labs and it’s striking how fast precision gives way to practical troubleshooting—pH, concentration, temperature—all matter in getting the crystals just right and avoiding waste.
Products like Ammonium Iron(II) Sulfate Hexahydrate aren’t headliners in the media, but they quietly enable advances in science, education and industry. Their reliable behavior supports critical measurements, synthesis, and even environmental monitoring. Still, the conversation around hazard labeling and storage deserves more attention: old protocols can let things slip through the cracks, leading to near-misses—something I’ve seen in shared storage rooms. Adding better training and regular safety audits would solve plenty of these issues. More collaboration between chemical producers, transporters, and users can cut down on misunderstandings about the real and perceived risks.
We use Ammonium Iron(II) Sulfate Hexahydrate because it works, plain and simple. It earns its place due to clear, predictable behavior and ease of use. Its presence reminds us that the backbone of progress isn’t always glamorous—it’s in these quiet workhorses of the lab, handled with care, passed from generation to generation. Keeping an eye on practice, safety, and the details that often go unnoticed stands as the real key to making sure resources like this support progress without unintended cost.
