Nitric Acid Information - Guidelines on the Proper Way of Using Nitric Acid [manufacturingdata] Question by Thorbjorn: How does one manufacture nitric acid? It is the key chemical for smokeless powders. Best answer for How does one manufacture nitric acid?:
Answer by casey54
buy two nitrics and soak them in water.
Answer by artman59
Much of the nitric acid produced in the world is manufactured via a high-temperature catalytic oxidation of ammonia. This process consists of three main steps: ammonia oxidation, nitric oxide oxidation, and absorption. This process can be performed at one or multiple pressures.
Answer by pa28_180flyer
I dont know why you would want to, unless you were trying to make ammonium nitrate. A mixture composed of a 1:9 ratio of ammonia and air is oxidized at a temperature near 1400 °F (760 °C) in a catalytic converter according to the reaction: 4 NH3 + 5O2 --> 4 NO + 6H2O The most common catalyst is composed of about 90% platinum and 10% rhodium (by weight). The catalyst is formed into wire gauze and inserted into the converter. The exothermic reaction proceeds to a nitric oxide yield of about 93-98%. The nitric oxide is cooled (and water condensed) to a temperature of 100 °F (37.8 °C) or less at a pressure up to 115 psia (7.8 bara). The nitric oxide reacts (noncatalytically) with oxygen to form nitrogen dioxide and nitrogen tetroxide via the reaction: 2 NO + O2 --> 2 NO2 + N2O4 This reaction is very dependent on both temperature and pressure. Low temperatures and high pressures favor the production of nitrogen dioxide (preferred) over nitrogen tetroxide. After being cooled, the nitrogen dioxide/nitrogen tetroxide mixture enters an absorption column. The gaseous mixture is introduced at the bottom of the column while liquid dinitrogen tetroxide and deionized water enter at the top. Liquids flow countercurrent to the gases in the system while the oxidation takes place between the trays and absorption takes place on the trays (usually bubble cap trays). The reaction in the absorption column proceeds by: 3 NO2 + H2O --> 2 HNO3 + NO A second air stream entering the column further oxidizes the NO and removes the NO2 from the product acid. Acid concentrations leaving the absorption tower are typically between 55-65% by weight.
Answer by alooo...
The manufacture of nitric acid is a three-stage process. The first stage is the oxidation of ammonia and it uses a platinum/rhodium catalyst. world annual production approximately 60 million tonnes gas mixture 10% ammonia + 90% air pressure 4 to 10 atmospheres temperature 975 - 1225 K catalyst gauze of 90% platinum 10% rhodium conversion 96% The three main stages in the manufacture of nitric acid a) ammonia oxidation 4NH3 + 5O2 -> 4NO + 6H2O DH = - 900 kJmol-1 b) nitric oxide oxidation 2NO + O2 ->2NO2 DH = - 115 kJmol-1 2NO2 -> N2O4 DH = - 58 kJmol-1 c) dinitrogen tetroxide absorption 3N2O4 + 2H2O -> 4HNO3 + 2NO DH = - 103 kJmol-1
Answer by poortycoon_4
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. Nitric 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. The 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. The 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. White 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)
Answer by terror_2287
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. Nitric 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. The 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. The 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. White 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).
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manufacturing nitric acid]
On June 5, 2012, the Company provided an assessment of the damages and its plan to resume production at the El Dorado Facility. As planned, we restarted regular nitric acid and ammonium nitrate production, on a partial basis in June, and we are on ... LSB Industries, Inc. Reports Progress on El Dorado, Arkansas and Pryor ...
With a chemical formula of NH03, nitric acid is one of those substances used in laboratory processes, and while it has various valuable uses, it has a potential to be dangerous if not used properly. Colorless or light yellow, the substance is highly corrosive and it is a strong oxidizing agent. Concentrated nitric acid is not compatible with many substances, which include metallic bases, strong bases, hydrogen sulfide, carbides, turpentine, and combustible organics.
Considering the above-mentioned properties of the substance, its proper handling and use must be taken into account. One of the immediate things that must be done when storing the chemical product is to appropriately label its container. Labeling of the substance will help avoid accidental ingestion or swallowing of the substance. You should know that ingestion of the chemical product can cause burns to the mouth as well as to the throat, esophagus, and stomach.
Moreover, there are cases that it can lead to death.
It must also be stocked in a storage area that is cool, dry, and has good ventilation. Make sure that it is not exposed to direct sunlight and the aforementioned incompatible materials. Remember to add the acid slowly to water and in small amounts when diluting. It is a no-no to add water to the acid, for it can result to uncontrolled boiling and splashing.
The substance is indeed a strong acid and its contact with your skin and eyes can cause burns and may result to permanent damage to the eyes. Thus, it is strongly advised to wear safety glasses when handling the chemical product. If you are handling nitric acid which has a concentration of up to 70%, consider using gloves, especially those that are either made of neoprene, butyl rubber, or polyethylene.
There are things that you can immediately do when accidents take place, though. When someone ingests the substance, do not commit the mistake of inducing vomiting. What should be done instead is to give the victim with plenty of water. You can also give the victim milk, if it is available. If skin contact takes place, immediately flush the affected skin with a good amount of water for at least 15 minutes. You can also do the same to the affected eye if the substance comes into contact with your eye or eyes. In case of inhalation of the vapor of the substance, go to a spot where there is fresh air.
Yes, accidents with regard to the use of the substance can happen, but its value in the society should not be disregarded. One of its main uses is being a component in the preparation and manufacture of fertilizers such as ammonium nitrate. It also proves useful in the jewelry industry as when the substance is combined with hydrochloric acid, aqua regia is formed; aqua regia is able to dissolve precious metals just like platinum and gold.
Nitric acid is also a component in making explosives, which include trinitrotoluene or T.N.T and nitroglycerine. It is also used in the production of fungicides, perfumes, dyes, and several drugs, etching designs on brass, bronze ware, and copper, and in reprocessing spent nuclear fuels.
As in almost anything in life, accidents can be prevented by being informed, being careful and by following directions. Handling and using a potentially dangerous substance such as nitric acid entails responsibility. Being ignorant is not an excuse. Ask questions when in doubt. Read labels and instructions carefully. Remember that there are many things at stake when the substance is not used properly, and these include not only your health but also the health of the people around you.
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