7697-37-2

Nitric acid is a colorless to yellow or red liquid sometimes fuming reddish brown vapors with a suffocating odor. NITRATING ACID, MIXTURE, (WITH > 50% NITRIC ACID)(7697-37-2) is soluble in water with release of heat. NITRATING ACID, MIXTURE, (WITH > 50% NITRIC ACID)(7697-37-2) is corrosive to metals or tissue. NITRATING ACID, MIXTURE, (WITH > 50% NITRIC ACID)(7697-37-2) will accelerate the burning of combustible materials and NITRATING ACID, MIXTURE, (WITH > 50% NITRIC ACID)(7697-37-2) may even cause ignition upon contact with combustible material. NITRATING ACID, MIXTURE, (WITH > 50% NITRIC ACID)(7697-37-2) is fully soluble in water and may react violently upon contact with water with the evolution of heat, fumes and spattering. Prolonged exposure to low concentrations or short term exposure to high concentrations may result in adverse health effects. Density 10.4 lb/gal.

Nitric acid; ignites upon contact with alcohols, amines, ammonia, beryllium alkyls, boranes, dicyanogen, hydrazines, hydrocarbons, hydrogen, nitroalkanes, powdered metals, silanes, or thiols [Bretherick 1979. p.174]. The reaction of finely divided antimony and nitric acid can be violent [Pascal 10:504. 1931-34]. Bromine pentafluoride reacts violently with strong nitric acid and strong sulfuric acid [Mellor 2, Supp. 1:172. 1956]. Experiments show that mixtures of over 50% nitric acid by weight in acetic anhydride may act as detonating explosives [BCISC 42:2. 1971]. An etching agent of equal portions of acetone, nitric acid, and 75% acetic acid exploded 4 hours after NITRATING ACID, MIXTURE, (WITH > 50% NITRIC ACID) was prepared and placed in a closed bottle. This is similar to a formulation for the preparation of tetranitromethane a sensitive explosive [Chem. Eng. News 38: 56. 1960]. Phosphine is violently decomposed by concentrated nitric acid, and flame is produced. Warm fuming nitric acid, dropped in a container of phosphine gas produces an explosion [Edin. Roy. Soc. 13:88. 1835]. An explosion occurs when nitric acid is brought into contact with phosphorus trichloride [Comp. Rend. 28:86]. The reaction of sodium azide and strong nitric acid is energetic [Mellor 8, Supp 2:315. 1967]. Reacts violently with water with the production of heat, fumes, and spattering.

Fumes in air. Fully soluble in water with release of heat. Reacts violently with water with the production of heat, fumes, and spattering.

Nitric acid is the second most important industrial acid and its production represents the sixth largest chemical industry in the United States. Nitric acid is used in chemicals, explosives, fertilizers, steel pickling; metal cleaning. The largest use of nitric acid is in the production of fertilizers. Almost 15% of the production goes into the manufacture of explosives, with the remaining 10% distributed among a variety of uses, such as etching, bright-dipping; electroplating, photoengraving, production of rocket fuel; and pesticide manufacture.

Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Vapors may accumulate in confined areas (basement, tanks, hopper/tank cars etc.). Substance will react with water (some violently), releasing corrosive and/or toxic gases and runoff. Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated or if contaminated with water.

If this chemical gets into the eyes, remove any contact lenses at once and irrigate immediately for at least 15 minutes, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts the skin, remove contaminated clothing and wash immediately with soap and water. Seek medical attention immediately. If this chemical has been inhaled, remove from exposure, begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR if heart action has stopped. Transfer promptly to a medical facility. When this chemical has been swallowed, get medical attention. If victim is conscious, administer water, or milk. Do not induce vomiting. Medical observation is recommended for 24 48 hours after breathing overexposure, as pulmonary edema may be delayed. As first aid for pneumonitis or pulmonary edema, a doctor or authorized paramedic may consider administering a drug or other inhalation therapy.

UN2031 Nitric acid other than red fuming, with .70% nitric acid or Nitric acid other than red fuming, with at least 65%, but not ＞70% nitric acid, Hazard Class: 8; Labels: 8-Corrosive material, 5.1-Oxidizer. UN2032 Nitric acid, red fuming, Hazard Class: 8; Labels: 8-Corrosive material, 5.1-Oxidizer, 6.1-Poisonous material. Inhalation, Hazard Zone B. UN2031 Nitric acid other than red fuming, with ＞20% and ＜65% nitric acid or Nitric acid other than red fuming, with not ＞20% nitric acid, Hazard Class: 8; Labels: 8-Corrosive material.

A strong oxidizer and strong acid. Reacts violently with combustible and reducing agents; carbides, hydrogen sulfide, turpentine, charcoal, alcohol, powdered metals; strong bases. Heat causes decomposition producing nitrogen oxides. Attacks some plastics. Corrosive to metals.

Nitric acid is a colorless, corrosive liquid that is the most common nitrogen acid. It has been used for hundreds of years. Nitric acid is a mineral acid that was called spirit of nitre and aqua fortis, which means strong water.

Fuming nitric acid is named because of the fumes emitted by acid when it combines with moist air. Fuming nitric acid is highly concentrated and is labeled either red fuming nitric acid or white fuming nitric acid. Red fuming nitric acid, as the name implies, emits a reddishbrown fume on exposure to air. The color comes from nitrogen dioxide, which is liberated on exposure to air. The nitric acid concentration of red fuming nitric acid is approximately 85% or greater, with a substantial amount of dissolved nitrogen dioxide. White fuming nitric acid is highly concentrated anhydrous nitric acid with concentrations of 98–99%; the remaining 1–2% is water and nitrogen dioxide. Most commercial grade nitric acid has a concentration of between 50% and 70%.

Nitric acid is a colorless to light brown fuming liquid with an acrid, suffocating odor. Fuming nitric acid is a reddish fuming liquid. Fumes in moist air. Often used in an aqueous solution. Fuming nitric acid is concentrated nitric acid that contains dissolved nitrogen dioxide. Nitric acid is a solution of nitrogen dioxide, NO2, in water and so-called fuming nitric acid contains an excess of NO2 and is yellow to brownish-red in color.

Nitricacid,HN03, is a strong,fire-hazardous oxidant. It is a colorless or yellowish liquid that is miscible with water and boils at 86℃ (187 ℉). Nitric acid, also known as aqua fortis, is used for chemical synthesis, explosives, and fertilizer manufacture, and in metallurgy, etching, engraving, and ore flotation.

Soda ash-slaked lime is added to form the neutral solution of nitrate of sodium and calcium. This solution can be discharged after dilution with water. Also, nitric acid can be recovered and reused in some cases as with acrylic fiber spin solutions. Consult with environmental regulatory agencies for guidance on acceptable disposal practices. Generators of waste containing this contaminant (≥100 kg/mo) must conform with EPA regulations governing storage, transportation, treatment, and waste disposal.

nitric acid: A colourless corrosivepoisonous liquid, HNO3; r.d. 1.50;m.p. –42°C; b.p. 83°C. Nitric acid maybe prepared in the laboratory by thedistillation of a mixture of an alkalimetalnitrate and concentratedsulphuric acid. The industrial productionis by the oxidation of ammoniato nitrogen monoxide, theoxidation of this to nitrogen dioxide,and the reaction of nitrogen dioxidewith water to form nitric acid and nitrogenmonoxide (which is recycled).The first reaction (NH₃ to NO) iscatalysed by platinum or platinum/rhodium in the form of fine wiregauze. The oxidation of NO and theabsorption of NO₂ to form the productare noncatalytic and proceedwith high yields but both reactionsare second-order and slow. Increasesin pressure reduce the selectivity ofthe reaction and therefore ratherlarge gas absorption towers are required.In practice the absorbing acidis refrigerated to around 2°C and acommercial ‘concentrated nitric acid’at about 67% is produced.Nitric acid is a strong acid (highlydissociated in aqueous solution) anddilute solutions behave much likeother mineral acids. Concentrated niniobium tric acid is a strong oxidizing agent.
Most metals dissolve to form nitratesbut with the evolution of nitrogenoxides. Concentrated nitric acid alsoreacts with several nonmetals to givethe oxo acid or oxide. Nitric acid isgenerally stored in dark brown bottlesbecause of the photolytic decompositionto dinitrogen tetroxide. Seealso nitration.

Nitric acid is a corrosive substance causingyellow burns on the skin. It corrodes the bodytissues by converting the complex proteinsto a yellow substance called xanthoproteicacid (Meyer 1989). Ingestion of acid canproduce burning and corrosion of the mouthand stomach. A dose of 5–10 mL can befatal to humans.
Chronic exposure to the vapor and mist ofnitric acid may produce bronchitis and chemical pneumonitis (Fairhall 1957). It emitsNO2, a highly toxic gas formed by its decomposition in the presence of light. Nitric acidis less corrosive than sulfuric acid. Its vaporand mist may erode teeth..

Explosibility Not a combustible substance, but a strong oxidizer. Contact with easily oxidizible materials including many organic substances may result in fires or explosions.

Nitric acid (HNO) is a mineral acid which combines with metals or alkalis to form nitrates. It can be made synthetically by passing ammonia and air over a metallic catalyst.
Nitric acid is used in the manufacture of ammonium nitrate for explosives and fertilizers. Two other types of nitric acid - red fuming nitric acid and white fuming nitric acid are known. White fuming nitric acid contains more than 97.5 % nitric acid, less than 2 % water and less than 0.5% oxides of nitrogen. Red fuming nitric acid contains more than 86% nitric acid, 6 to 15% oxides of nitrogen and less than 5 % water. It is used as a rocket fuel and nitrating agent. Important production process for the manufacture of nitric acid are elaborated in the entry Nitric acid production processes.
Nitric acid production processes₂
About 75% of nitric acid produced in the world is used for producing fertilizers (and about 15% for explosives). The remaining acid is used in making synthetic fibers, dyes and plastic.
Nitric acid can be produced by (a) acidulation of natural sodium nitrate with sulphuric acid, (b) direct synthesis from nitrogen and oxygen, and (c) oxidation of ammonia.
Nitric acid is a strong acid and a powerful oxidizing agent. Concentrated nitric acid on distillation at atmospheric pressure starts boiling at 78.2℃ but decomposes eventually to give 68% nitric acid with a boiling point of 120.5℃. The standard limit of chlorine is less than 5 ppmw and that of nitrous acid (HNO₂) less than 5 ppmw. Anhydrous nitric acid does not exist in liquid form.
Anhydrous ammonia and a platinum catalyst are required for the manufacture of nitric acid. The oxides of nitrogen that are used in the production of nitric acid are nitrous oxide (N₂O), nitric oxide (NO), nitrogen dioxide (NO₂) and dinitrogen tetroxide (N₂O₄). A mixture of nitrogen oxides, usually NO and NO₂, is commonly referred to as NO_x.
The production of weak nitric acid consists of the following three steps: (a) catalytic ammonia oxidation to nitric oxide, (b) oxidation of nitric oxide to nitrogen I dioxide, and (c)acidic absorption of nitrogen dioxide in water.
The absorber performance is improved by high pressure and low temperature, and a high oxygen content in the gas phase. However, in the ammonia converter, the oxidation of ammonia is favored by low pressure.
Methods of production: Many processes for producing nitric acid are now available. They differ not in fundamental principals, but primarily in design details of the plant, operating conditions for the plant size, cost considerations relating to raw materials, energy and installation.
The production of nitric acid by the oxidation of ammonia goes through the following steps or units: (a) ammonia preparation-vaporization, superheating and filtration of anhydrous ammonia, (b) process air preparation involving preheating, filtration and compression, (c) catalytic ammonia oxidation, (d) cooling of the reaction products with various media such as process air, boiler water, tail gas, etc., (e) oxidation of nitric oxide to higher oxides, (f) nitrogen oxides absorption in water to form nitric acid, (g) acid bleaching by additional air or other means, (h) tail gas treatment to reduce air pollution and to improve overall efficiency of the plant, (i) recovery of energy from the heated and compressed process gases, and (i) recovery of catalyst platinum.
The anhydrous ammonia and the process air used must be free both from the oil content and catalyst poisons to avoid fouling of the vaporizer and catalyst screens. The ratio of ammonia to air and the flow rate of each component must be carefully controlled to ensure maximum conversion efficiency, explosion prevention and plant output maximization.
The normal catalyst used in the process is a platinumrhodium gauze or mesh. It not only promotes reaction but also meets the other operating criteria such as those to counter the severe corrosive and oxidation atmosphere, etc. The usual rhodium percentage in the catalyst is in the range of 4 to 10%. To achieve higher efficiencies and smaller platinum losses, knitted gauzes are used. Chrome-nickel alloy grids are used to support the fine screens.
Platinum catalysts can be poisoned by such elements as As, Bi, P, Pb, S, Si and Sn. These elements lead to the formation of inactive compounds in the wires and thus decrease the catalytic activity. In some instances contamination with traces of Cr, Ni or Fe temporarily reduces the conversion efficiency which can often be restored by treatment with hydrochloric acid.

Also called aqua fortis and azotic acid, nitricacid is a colorless to reddish fuming liquid ofthe composition HNO₃, having a wide varietyof uses for pickling metals, etching, and in themanufacture of nitrocellulose, plastics, dyestuffs,and explosives. It has a specific gravityof 1.502 (95% acid) and a boiling point of 86°C,and is soluble in water. Its fumes have a suffocatingaction, and it is highly corrosive andcaustic. Fuming nitric acid is any water solutioncontaining more than 86% acid and having aspecific gravity above 1.480. Nitric acid is madeby the action of sulfuric acid on sodium nitrateand condensation of the fumes. It is also madefrom ammonia by catalytic oxidation, or fromthe nitric oxide produced from air.

Nitric acid is used in the manufacture of ammonium nitrate fertilizer and explosives, in steel etching, and in reprocessing spent nuclear fuel. There are two types of fuming nitric acid. White fuming nitric acid is concentrated with 97.5% nitric acid and less than 2% water. It is a colorless to pale-yellow liquid that fumes strongly. It is decomposed by heat and exposure to light and becomes red in color from nitrogen dioxide. Red fuming nitric acid contains more than 85% nitric acid, 6%–15% nitrogen dioxide, and 5% water. The four-digit UN identification number for red fuming nitric acid is 2032. The NFPA 704 designation is health 4, flammability 0, and reactivity 1. The prefix “oxy” appears in the white section of the diamond. Red fuming nitric acid is considered an oxidizer. Both white and red fuming acids are toxic by inhalation, strong corrosives, and dangerous fire risks that may explode upon contact with reducing agents. They are used in the production of nitro compounds, rocket fuels, and as laboratory reagents.

Nitric acid was not mutagenic in limited studies.4 There is no information regarding the carcinogenic properties of nitric acid, but an association between incidences of laryngeal cancer and exposure to acid mists has been indicated.4

Splash goggles and rubber gloves should be worn when handling this acid, and containers of nitric acid should be stored in a well ventilated location separated from organic substances and other combustible materials.

The acid is obtained colourless (approx. 92%) by direct distillation of fuming HNO3 under reduced pressure at 40-50o with an air leak at the head of the fractionating column. Store it in a desiccator kept in a refrigerator. Nitrite-free HNO3 can be obtained by vacuum distillation from urea. [Ward et al. Inorg Synth III 13 1950, Kaplan & Schechter Inorg Synth IV 53 1953.]