what are the uses,dangers and other characteristics of ammonium nitrate?
151276
agricultural - as fertilizer\n\nIt also is able to be used as an explosive when combined with an oxidizer or accelerant. Timothy Mcvey used this in his bomb that destroyed the federal building in Oklahoma City. It is or was used in blasting for construction purposes as well. Its sale in quantity is now monitored due to its potential abuse, so I hope you're a farmer.
823469
All nitrates are soluble.  You would need to consult a table of solubilities to see what other ions you could use to precipitate out the cations.\n\nEx:  If you had silver nitrate in a solution you could add something with a halide ion such as sodium chloride.  The silver ion would precipitate out with the chloride ion.  If no ppt forms with the sodium chloride you know it was not silver ions.\n\nThen look for other ions that you could test for.
1033934
Nitric acid is made by mixing nitrogen dioxide (NO2) with water. Creating a very pure nitric acid usually involves distillation with sulfuric acid, as nitric acid forms an azeotrope with water with a composition of 68% nitric acid and 32% water. Commercial grade nitric acid solutions are usually between 52% and 68% nitric acid. Commercial production of nitric acid is via the Ostwald process after Wilhelm Ostwald.\n\nNitric acid can be made from Copper(II) nitrate or by reacting 200 g of potassium nitrate (KNO3) in 106 ml of 96% sulfuric acid (H2SO4), and distilling this mixture at nitric acid's boiling point of 83 °C until only a white crystalline mass, potassium hydrogen sulfate (KHSO4), remains in the reaction vessel. The obtained red fuming nitric acid may be converted to the white nitric acid. Note that in a laboratory setting, it is necessary to use all-glass equipment, ideally a one-piece retort, because nitric acid attacks cork and rubber, and leaks can be extremely dangerous.\n\nThe dissolved NOx are readily removed using reduced pressure at room temperature (10-30 min at 200 mmHg or 27 kPa). Obtained white fuming nitric acid has density 1.51 g/cm³. This procedure can also be performed under reduced pressure and temperature in one step in order to produce less nitrogen dioxide gas.\n\nThe acid can also be synthesized by oxidizing ammonia, but the product is diluted by the water also formed as part of the reaction. However, this synthesization method is important in producing ammonium nitrate from ammonia derived from the Haber process, because the final product can be produced from nitrogen, hydrogen, and oxygen as the sole feedstocks.\n\nWhite fuming nitric acid, also called 100% nitric acid or WFNA, is very close to the anhydrous nitric acid product. One specification for white fuming nitric acid is that it has a maximum of 2 % water and a maximum of 0.5 % dissolved NO2. Red fuming nitric acid, or RFNA, contains substantial quantities of dissolved nitrogen dioxide (NO2) leaving the solution with a reddish-brown color. One formulation of RFNA specifies a minimum of 17% NO2, another specifies 13% NO2. In either event, an inhibited fuming nitric acid (either IWFNA, or IRFNA) can be made by the addition of 0.6 to 0.7% hydrogen fluoride, HF. This fluoride is added for corrosion resistance in metal tanks (the fluoride creates a metal fluoride layer that protects the metal)
700039
nitrogen - Liquid nitrogen is used for cooling experiments\noxygen - Always used in breathing and burning fuel. Given in hospitals, used as rocket fuel. \ncarbon dioxide - Used in carbonated drinks, fire extinguishers, and dry ice.\nargon - used as an inert gas to prevent reactions and preserve things.\nhelium - Used in balloons and helium-neon lasers.\nneon - Used in neon signs and helium-neon lasers.\nmethane - Is natural gas, used for heating & generating electricity.
755657
You might be able to find it at a pharmacy. A chemical supply shop, or an older style apothecary or chemist type shop might have it. Searching for its chemical name (potassium nitrate) might also help.\nAside from these, the only other source I know  of  is the underside of a dung heap.
929088
Explain the reaction of Potassium Nitrate mixed with Amonia Sulfite,with a pinch of Magnesium powder,and a foot of Magnesium Ribbon,and last but not least Benzyl Chloride. It is very important you use Benzyl Chloride.
76820
I agree with the previous answer; magnesium nitrate is probably more soluble, at 125 g/100 mL water versus magnesium chloride's 54.2 g/100 mL.  Nitrate's ionic bond (not "bound") is weaker probably because of its higher electron density pulling away from that bond.  \n\nSolubility rules tell us that all nitrates are soluble, but silver, mercury, and lead chlorides are insoluble.
947511
no there isn't but it will last about 1-2 hours. ammonium nitrate and water it the reaction.
335271
Acute methemoglobinemia caused in adults by ingestion of potassium nitrate
943386
Here are two ways to get the same answer of -1.\n\nThe nitrogen in nitrate has a formal charge of +5, and the total charges on the bound oxygens is -6 (3@-2 each), so the net charge for nitrate is -1.\n\nDon't rely on the model of ammonia, NH3, with three bonds and a lone pair.  The nitrogen in nitrate has been oxidized to the extent that all five valence electrons are involved in making 5 bonds to the three oxygen atoms.  Since each oxygen is capable of two bonds, the result is that there is on average one extra charge for the NO3 "radical", or -1 net.\n\nHope this helps.
596845
Nitriogen dioxide is toxic by inhalation. Symptoms of poisoning (lung edema) tend to appear several hours after one has inhaled a low but potentially fatal dose. Also, low concentrations (4 ppm) will anesthesize the nose, thus creating a potential for overexposure.\n\nLong-term exposure to NO2 at concentrations above 40–100 µg/m³ causes adverse health effects [2]. The most important source of NO2 are internal combustion engines, which emit nitrogen oxides near people.
497768
Ammonium hydroxide.  Bleach.  Sports drinks like Gatorade (they have electrolytes).
55366
The term nitrogen oxide is imprecise and can be used to refer to any of these oxides (oxygen compounds) of nitrogen, or to a mixture of them:\n\nNitric oxide (NO), nitrogen(II) oxide \nNitrogen dioxide (NO2) \nDinitrogen oxide (N2O) (Nitrous oxide) \nDinitrogen trioxide (N2O3) \nDinitrogen tetroxide (N2O4) \nDinitrogen pentoxide (N2O5) \nA mixture is often formed in chemical reactions that produce nitrogen oxides, with the proportions depending on the specific reaction and the conditions it is performed in. This is one reason why home production of N2O is undesirable; the other two stable oxides - which are extremely toxic - are liable to be produced.\n\nNote that the last 3 listed above are unstable.
858428
Nothing chemically should happen, outside of creating something that really smells.  Ammonia vapors can be hazardous, as can moth balls, whether they are napthalene based or p-Dichlorobenzene based, so try not to spend too much time sniffing them.  They will not create an explosive, although mothballs are flammable.
843520
When taking nitric oxide donors, organic nitrites and nitrates, such as glyceryl trinitrate, sodium nitroprusside, amyl nitrite ("poppers")\n \nIn men for whom sexual intercourse is inadvisable due to cardiovascular risk factors\n \nSevere hepatic impairment (decreased liver function)\n \nSevere impairment in renal function \n\nHypotension (low blood pressure) \n\nRecent stroke or heart attack \n\nHereditary degenerative retinal disorders (including genetic disorders of retinal phosphodiesterases)
785715
I believe that that is aluminum nitrate, more commonly written as Al(NO3)3.  It's used in deodorant.
373034
(m)\n\nSynonyms: Nitric acid, zinc salt solution; Zinc Nitrate Solution \nCAS No.: 7779-88-6 (Anhydrous) \nMolecular Weight: Not applicable to mixtures. \nChemical Formula: Zn(NO3)2 \nProduct Codes: 4346 \n\nEmergency Overview \n-------------------------- \nDANGER! STRONG OXIDIZER. CONTACT WITH OTHER MATERIAL MAY CAUSE FIRE. HARMFUL IF SWALLOWED OR INHALED. CAUSES IRRITATION TO SKIN, EYES AND RESPIRATORY TRACT\n\n\nPotential Health Effects \n---------------------------------- \n\nInhalation: \nCauses irritation to the respiratory tract. Symptoms may include coughing, shortness of breath. Methemoglobinemia may occur. \nIngestion: \nCauses irritation of the gastrointestinal tract. If appreciable amounts are ingested, abdominal pain, cramps and nausea may result together with faintness and bluish lips and skin (methemoglobinemia). \nSkin Contact: \nCauses irritation to skin. Symptoms include redness, itching, and pain. \nEye Contact: \nIrritant. Causes redness, tears and pain, possibly blurred vision. \nChronic Exposure: \nZinc salts are eliminated fairly promptly, making chronic effects less than acute. \nAggravation of Pre-existing Conditions: \nNo information found. \n\nFirst Aid Measures\nInhalation: \nRemove to fresh air. If not breathing, give artificial respiration. If breathing is difficult, give oxygen. Get medical attention. \nIngestion: \nIf swallowed, DO NOT INDUCE VOMITING. Give large quantities of water. Never give anything by mouth to an unconscious person. Get medical attention immediately. \nSkin Contact: \nWipe off excess material from skin then immediately flush skin with plenty of water for at least 15 minutes. Remove contaminated clothing and shoes. Get medical attention. Wash clothing before reuse. Thoroughly clean shoes before reuse. \nEye Contact: \nImmediately flush eyes with plenty of water for at least 15 minutes, lifting lower and upper eyelids occasionally. Get medical attention immediately. \n\nFire Fighting Measures\nFire: \nNot combustible, but substance is a strong oxidizer and its heat of reaction with reducing agents or combustibles may cause ignition. Increases flammability of any combustible substance in contact with it. \nExplosion: \nNot considered to be an explosion hazard. \nFire Extinguishing Media: \nWater or water spray in early stages of fire. Foam or dry chemical may also be used. \nSpecial Information: \nIn the event of a fire, wear full protective clothing and NIOSH-approved self-contained breathing apparatus with full facepiece operated in the pressure demand or other positive pressure mode. \n\n\nHandling and Storage\nKeep in a tightly closed container, stored in a cool, dry, ventilated area. Protect against physical damage and moisture. Isolate from any source of heat or ignition. Avoid storage on wood floors. Separate from incompatibles, combustibles, organic or other readily oxidizable materials. Containers of this material may be hazardous when empty since they retain product residues (vapors, liquid); observe all warnings and precautions listed for the product. \n\nPhysical and Chemical Properties\nAppearance: \nColorless to yellowish liquid. \nOdor: \nSlight nitric acid odor. \nSolubility: \nSoluble in water. \nSpecific Gravity: \nNo information found. \npH: \nNo information found. \n% Volatiles by volume @ 21C (70F): \n0 \nBoiling Point: \nNo information found. \nMelting Point: \nNo information found. \nVapor Density (Air=1): \nNo information found. \nVapor Pressure (mm Hg): \nNo information found. \nEvaporation Rate (BuAc=1): \nNo information found. \n\nStability: \nStable under ordinary conditions of use and storage. \nHazardous Decomposition Products: \nOxides of nitrogen and toxic metal fumes may form when heated to decomposition. \nHazardous Polymerization: \nWill not occur. \nIncompatibilities: \nMetal powders, cyanides, sodium hypophosphite, stannous chloride, phosphorus, thiocyanates, carbon, metallic sulfides, sulfur, organic materials. Substance is capable of reac