Nitric acid Chemical Properties
- Melting point:
- -42 °C
- Boiling point:
- 120.5 °C(lit.)
- 1.41 g/mL at 20 °C
- vapor density
- 1 (vs air)
- vapor pressure
- 8 mm Hg ( 20 °C)
- Flash point:
- storage temp.
- Miscible with water.
- -1.3(at 25℃)
- Liquid, Double Sub-Boiling Quartz Distillation
- colorless to deep yellow
- Specific Gravity
- d 20/4 1.4826
- Suffocating fumes detectable at <5.0 ppm
- <1 (H2O, 20℃)
- Water Solubility
- >100 g/100 mL (20 ºC)
- Exposure limits
- TLV-TWA 2 ppm (5 mg/m3) (ACGIH, MSHA, OSHA, and NIOSH); STEL 4 ppm (～10 mg/m3) (ACGIH).
- CAS DataBase Reference
- 7697-37-2(CAS DataBase Reference)
- NIST Chemistry Reference
- Nitric acid(7697-37-2)
- EPA Substance Registry System
- Nitric acid (7697-37-2)
- Hazard Codes
- Risk Statements
- Safety Statements
- UN 3264 8/PG 3
- WGK Germany
- HS Code
- 2808 00 00
- Hazardous Substances Data
- 7697-37-2(Hazardous Substances Data)
- LC50 inhal (rat)
2500 ppm (1 h)
2 ppm (5 mg/m3)
2 ppm (5.2 mg/m3)
4 ppm (10 mg/m3)
Nitric acid Usage And Synthesis
Nitric acid (HNO3) is an important industrial acid used to alter or produce many products such as fertilizers and explosives. It reacts with ammonia to produce ammonium nitrate, an important commercial chemical.
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%.
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.
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.
Colorless liquid; highly corrosive; refractive index 1.397 at 16.5°C; density 1.503 g/L; freezes at –42°C; boils at 83°C; completely miscible with water; forms a constant boiling azeotrope with water at 68.8 wt% nitric acid; the azeotrope has density 1.41 g/mL and boils at 121°C.
Nitric acid was known to alchemists in ancient times. Cavendish in 1784 synthesized the acid by applying an electric spark to humid air. Earlier in 1776, Lavoisier determined that the acid contained oxygen. In 1798, Milner prepared nitric acid from ammonia along with nitrogen oxides by oxidation of ammonia vapor over red-hot manganese dioxide. In 1816, Gay-Lussac and Berthollet established its composition.
Nitric acid is one of the most important industrial chemicals in the world. Its largest use is in the fertilizer industry for producing various nitrate fertilizers. Such fertilizers include ammonium-, sodium-, potassium-, and calcium nitrates. Other major applications of nitric acid are in making nitrates and nitrooganics for use in explosives, gunpowder, and fireworks. Ammonium nitrate, nitroglycerine, nitrocellulose, and trinitrotoluenes are examples of such explosives, while barium and strontium nitrates are used in fireworks. NITRIC ACID 635Another major application is in producing cyclohexanone, a raw material for adipic acid and caprolactam to produce nylon.
Nitric acid is a common laboratory reagent. It also is one of the most used oxidizing agents, applied in several organic and inorganic syntheses. Some synthetic applications of nitric acid include the production of diazo dyes, varnishes, lacquers, plastics, polyurethanes, and detergents. Other applications are in metal etching, ore extractions, pickling of stainless steel, rocket propellant, for processing nuclear fuel, as a solvent in aqua regia, for sample digestion in metal analysis by AA or ICP, and in preparing analytical standards.
Concentrated nitric acid used in commerce is not 100% pure nitric acid. It is the constant boiling mixture containing 68% pure acid.
Nitric acid is an important starting material for the production of fertilizers and chemicals. Diluted nitric acid is used for dissolving and etching metals Product Data Sheet
Nitric acid is an important material for the production of explosives. Concentrated nitric acid, usually mixed with sulfuric acid (mixed acid), is used for nitrating organic compounds. Product Data Sheet
The main use of nitric acid is for the production of fertilizer, with approximately threefourthsof nitric acid production being used for this purpose. Ammonium nitrate is the preferred nitrogen fertilizer owing to itsease in production, economics, and high nitrogen content, which is 35%. Nitric acid can alsobe used for the acidulation of phosphate rock to produce nitrogen-phosphorus fertilizers.Nitric acid is a strong oxidizer, which makes it useful in explosives and as a rocketpropellant.
Nitric acid is used for nitrating numerous other compounds to produce nitrates. Nitricacid is used to produce adipic acid (C6H4O10), which is used in the production of nylon (seeNylon).
Additional uses of nitric acid are for oxidation, nitration, and as a catalyst in numerousreactions. Salts of nitric acid are collectively called nitrates, which are soluble in water. Nitricacid is used in the production of many items such as dyes, pharmaceuticals, and syntheticfabrics.It is also used in a variety of processes including print making.
Nitric acid is used extensively in the metal industries. Nitric acid is used to pickle steel and brass surfaces in metal processing.
This heavy, clear or slightly yellowish fluid is very poisonous and causes severe burns on contact with the skin. It was made by the distillation of an alkali-metal nitrate combined with sulfuric acid. The combination of nitric and sulfuric acids was used to convert plain cotton to cellulose nitrate. Nitric acid was used in the wet plate process as an additive to ferrous sulfate developers to promote a whiter image color for ambrotypes and ferrotypes. It was also added to lower the pH of the silver bath for collodion plates. Adding acid to the silver bath made collodion plates less sensitive to light, which had the beneficial effect of reducing the occurrence non-image fog.
Nitric acid is one of the most widely usedindustrial chemicals. It is employed in the production of fertilizers, explosives, dyes, synthetic fibers, and many inorganic and organicnitrates; and as a common laboratory reagent..
fuming corrosive liquid that is a strong
acid. Nitric acid can be made in a laboratory
by the distillation of a mixture of an
alkali metal nitrate and concentrated sulfuric
acid. Commercially it is prepared by the
catalytic oxidation of ammonia and is supplied
as concentrated nitric acid, which
contains 68% of the acid and is often colored
yellow by dissolved oxides of nitrogen.
Nitric acid is a strong oxidizing agent.
Most metals are converted to their nitrates
with the evolution of oxides of nitrogen
(the composition of the mixture of the oxides
depends on the temperature and on the
concentration of the nitric acid used).
Some non-metals (e.g. sulfur and phosphorus phosphorus) react to produce oxyacids. Organic substances (e.g. sawdust and ethanol) react violently, but the more stable aromatic compounds, such as benzene and toluene, can be converted to nitro compounds in controllable reactions.
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 can be prepared by several methods, but the primary method is by the oxidationof ammonia using the Ostwald method, which was named for Wilhelm Ostwald(1853–1932). The Ostwald method enabled the Germans to produce explosives in World War I after their nitrate supplies were cut off. The first step in nitric acid production involves theoxidation of ammonia at a temperature of approximately 900°C to produce nitric oxide, NO,and water: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g).This process is carried out in the presence ofa 90% platinum/10% rhodium catalyst in the form of wire gauze. The nitric oxide producedis further oxidized noncatalytically at a low temperature (less than 50°C) to form nitrogendioxide and its dimer nitrogen tetroxide, N2O4: 2NO(g) + O2 → 2NO2(g) N2O4(g).Thefinal step involves absorbing the nitrogen dioxide-dimer in water to produce nitric acid:3NO2(g) + 2H2O(l) → 2HNO3(aq) + NO(g).
Nitric acid may be produced by several methods. In the laboratory, it is prepared by distilling a solution of potassium nitrate in concentrated sulfuric acid containing equal amounts (by weight) of each.
KNO3 + H2SO4 → KHSO4 + HNO3
Nitric acid decomposes to nitrogen dioxide. Therefore, the temperature must be kept as low as possible. During this preparation, nitric acid condenses as a fuming liquid. The pure acid may be obtained when it is collected at –42°C, its freezing point. When nitric acid is collected by condensation at room temperature, it may decompose partially to nitrogen pentaoxide, N2O5, which fumes in moist air. Early commercial processes were based on reaction of Chile saltpeter (NaNO3) with sulfuric acid. Concentrated nitric acid was obtained by distilling the reaction mixture.
Nitric acid also may be obtained by rapid passage of air through an electric 636 NITRIC ACIDarc. The method is based on Cavendish’s first preparation of nitric acid. In this method, nitrogen and oxygen first combine to form nitric oxide. The gaseous product mixture usually containing about 2% nitric oxide is combined with excess oxygen to form nitrogen dioxide and nitrogen pentoxide. Dissolution of these gases in water forms nitric acid. The process, however, is expensive and unsuitable for commercial application.
Currently, nitric acid is manufactured exclusively by catalytic oxidation of ammonia. Platinum or platinum-rhodium is an effective catalyst of this oxidation (Ostwald process). Three basic steps in such ammonia oxidation process are: (1) oxidation of ammonia to form nitric oxide:
4NH3 + 5O2 → 4NO + 6H2O
The above reaction is rapid and shifts almost fully to the product side. (2) oxidation of nitric oxide to form nitrogen dioxide:
2NO + O2 → 2NO2
The above reaction also is rapid and goes almost to completion below 150°C. (3) dissolution of nitrogen dioxide in water:
3NO2 + H2O → 2HNO3 + NO
This reaction is moderately exothermic, releasing 32.4 kcal/mol.
Several mechanisms have been proposed for absorption of nitrogen dioxide in water. Nitrogen dioxide readily dimerizes to tetroxide, N2O4, at low temperatures and increasing pressure.
2NO2 ↔ N2O4 ?Hrxn = –13.7 kcal/mol
Absorption of tetroxide in water also could form nitric acid and nitric oxide:
3N2O4 + 2H2O → 4HNO3 + 2NO
Several modifications in plant design and process conditions for ammonia oxidation processes have taken place in recent years. These variations are more or less based on operating pressures and temperatures, reduction of NOx emission and other environmental regulations, and the desired plant production capacity.
Nitric acid obtained in standard ammonia oxidation is usually 50 to 70% by weight aqueous solution. Pure nitric acid of 98-99% may be obtained either by extractive distillation or by direct strong nitric (DSN) processes. In the distillation method, concentrated nitric acid of 50-70% is distilled with 93% sulfuric acid in a steam-heated tower. Sulfuric acid acts as a dehydrating agent. The distilled nitric acid vapor is condensed to pure nitric acid, while sulfuric acid absorbing water from 50-70% nitric acid loses its strength to about 70% and collects at the bottom. The 70% sulfuric acid is concentrated back to 93% NITRIC ACID 637for reuse by removal of water in a sulfuric acid concentrator.
In the DSN process, nitrogen tetroxide, N2O4 obtained from ammonia oxidation is absorbed by concentrated nitric acid in the presence of air or oxygen to yield pure nitric acid. Alternatively, N2O4 may be separated from the product gases of the ammonia oxidation process by refrigeration and then is treated with dilute nitric acid in air or oxygen.
Nitric acid is a colorless to yellow or red liquid sometimes fuming reddish brown vapors with a suffocating odor. Nitric acid is soluble in water with release of heat. Nitric acid is corrosive to metals or tissue. Nitric acid will accelerate the burning of combustible materials and Nitric acid may even cause ignition upon contact with combustible material. Nitric acid 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.
Air & Water Reactions
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; 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 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.
Because it is a strong oxidizing agent, nitric acid may undergo violent reactions with powerful reducing agents. Many nitration reactions of organics yield explosive products. Pure nitric acid is highly corrosive to skin causing severe injury. Concentrated acid (68.8 wt %) is moderately corrosive to skin. The acid may decompose under heating or photochemically, liberating toxic nitrogen dioxide gas.
Concentrated nitric acid and its vapors are highly corrosive to the eyes, skin, and
mucous membranes. Dilute solutions cause mild skin irritation and hardening of the
epidermis. Contact with concentrated nitric acid stains the skin yellow and produces
deep painful burns. Eye contact can cause severe burns and permanent damage.
Inhalation of high concentrations can lead to severe respiratory irritation and delayed
effects, including pulmonary edema, which may be fatal. Ingestion of nitric acid may
result in burning and corrosion of the mouth, throat, and stomach. An oral dose of 10
mL can be fatal in humans.
Tests in animals demonstrate no carcinogenic or developmental toxicity for nitric acid. Tests for mutagenic activity or for reproductive hazards have not been performed.
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..
Not a combustible substance, but a strong oxidizer. Contact with easily oxidizible materials including many organic substances may result in fires or explosions.
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.
Flammability and Explosibility
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
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 NOx.
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.
Poison by inhalation. A corrosive irritant to skin, eyes, and mucous membranes. A very dangerous fire hazard and very powerful oxidizing agent. Can react explosively with many reducing agents. Wdl react with water or steam to produce heat and toxic, corrosive, and flammable vapors.When heated to decomposition it emits hghly toxic fumes of NOx. See also NITRIC ACID.
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.
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.
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.
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.]
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.
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.