Commonly used as a laboratory reagent, nitric acid is used in the manufacture of explosives including nitroglycerin, trinitrotoluene (TNT) and cyclotrimethylenetrinitramine (RDX), as well as fertilizers such as ammonium nitrate. Contaminated clothing is removed immediately and the underlying skin washed thoroughly. : 63.01 NFPA#: 3-0-2 1.0 mol/L, Concentration: 10% v/v Ethanol Composition: Methyl Alcohol 82.49%, Nitric Acid 12.26%, Water 5.25% Boiling Point: Approximately 64C Density: 0.9 Melting Point: Color: Colorless to light yellow liquid Physical State: Liquid Flash Point: 16C pH Range: Solubility Information:, Thomas Scientific 2022 All Rights Reserved. On a laboratory scale, such distillation must be done in all glass apparatus at reduced pressure, to prevent decomposition of the acid. ], Skin: Prevent skin contact Eyes: Prevent eye contact Wash skin: When contaminated Remove: When wet or contaminated Change: No recommendation Provide: Eyewash (pH, NIOSH REL : TWA 2 ppm (5 mg/m 3 ) ST 4 ppm (10 mg/m 3 ) OSHA PEL ? As a general rule, oxidizing reactions occur primarily with the concentrated acid, favoring the formation of nitrogen dioxide (NO2). Nitration of organic compounds with nitric acid is the primary method of synthesis of many common explosives, such as nitroglycerin and trinitrotoluene (TNT). If proteins that contain amino acids with aromatic rings are present, the mixture turns yellow.
In laboratory, nitric acid can be made from Copper(II) nitrate or by reacting approximately equal masses of potassium nitrate (KNO3) with 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. ISO 14104 is one of the standards detailing this well known procedure. Production from one deposit was 800 tons per year.[38][39]. HNO3 F.W.
Find out how LUMITOS supports you with online marketing. [12][13] Xanthoproteic acid is formed when the acid contacts epithelial cells. Being a strong oxidizing agent, nitric acid can react violently with many compounds. Dilute nitric acid behaves as a typical acid in its reaction with most metals. In a low concentration (approximately 10%), nitric acid is often used to artificially age pine and maple. Further concentration to 98% can be achieved by dehydration with concentrated H2SO4. Due to its oxidizing nature, nitric acid does not (with some exceptions) liberate hydrogen on reaction with metals and the resulting salts are usually in the higher oxidized state. One formulation of RFNA specifies a minimum of 17% NO2, another specifies 13% NO2. [25], Commercially available aqueous blends of 530% nitric acid and 1540% phosphoric acid are commonly used for cleaning food and dairy equipment primarily to remove precipitated calcium and magnesium compounds (either deposited from the process stream or resulting from the use of hard water during production and cleaning). One specification for white fuming nitric acid is that it has a maximum of 2% water and a maximum of 0.5% dissolved NO2. Normally, the nitric oxide produced by the reaction is reoxidized by the oxygen in air to produce additional nitrogen dioxide. Some precious metals, such as pure gold and platinum-group metals do not react with nitric acid, though pure gold does react with aqua regia, a mixture of concentrated nitric acid and hydrochloric acid. The standard first-aid treatment for acid spills on the skin is, as for other corrosive agents, irrigation with large quantities of water. Fresh water was pumped into the top through another earthenware pipe to replace the fluid removed. Depending on the acid concentration, temperature and the reducing agent involved, the end products can be variable. [Note: Often used in an aqueous solution. In the laboratory, further concentration involves distillation with either sulfuric acid or magnesium nitrate, which serve as dehydrating agents. [30] It was also described by works attributed to Albert the Great and Ramon Lull, who prepared it by distilling a mixture containing niter and green vitriol and called it "eau forte" (aqua fortis). Nitric oxide is then reacted with oxygen in air to form nitrogen dioxide. This procedure can also be performed under reduced pressure and temperature in one step in order to produce less nitrogen dioxide gas. [17], The main industrial use of nitric acid is for the production of fertilizers. White fuming nitric acid, also called 100% nitric acid or WFNA, is very close to the anhydrous nitric acid product.
Such distillations must be done with all-glass apparatus at reduced pressure, to prevent decomposition of the acid. An older density scale is occasionally seen, with concentrated nitric acid specified as 42Baum.[6].
Reaction then takes place with all metals except the precious metal series and certain alloys. (Oil), Very soluble in water and ether.
Note that in a laboratory setting, it is necessary to use all-glass equipment, ideally a one-piece retort, because anhydrous nitric acid attacks cork, rubber, and skin, and leaks can be extremely dangerous. Anhydrous nitric acid is a colorless mobile liquid with a density of 1.512g/cm3 that solidifies at 42C (44F) to form white crystals[clarification needed]. 57.97%, Nitric Acid 42.03% Boiling Point: Approximately 100C Density: 1.26 Melting Point: Approximately 0C Color: Colorless to light yellow liquid Physical State: Liquid pH Range: Solubility Information: Miscible Shelf Life: 24 Months Storage: Ambient DOT: UN2031, NITRIC ACID,, Chemical name: Nitric acid Material form: Liquid Density (g/cm3): 1.42 Molecular weight: 63.01 Molecular formula: HNO3 Chemical purity: =65% (T) UN Number: UN 2031, 65% w/w Composition: Nitric Acid 65.25%, Water 34.75% Boiling Point: 120.5C Density: 1.45 Color: Colorless to light yellow liquid Physical State: Liquid pH Range: Solubility Information: Miscible Shelf Life: 24 Months Storage: Ambient DOT: UN2031, NITRIC ACID, 8, P.G. In the laboratory, nitric acid can be made by thermal decomposition of copper(II) nitrate, producing nitrogen dioxide and oxygen gases, which are then passed through water to give nitric acid. [15], Dilute nitric acid may be concentrated by distillation up to 68% acid, which is a maximum boiling azeotrope. Reaction with non-metallic elements, with the exception of silicon and halogens, usually oxidizes them to their highest oxidation states as acids with the formation of nitrogen dioxide for concentrated acid and nitrogen oxide for dilute acid. [19] IRFNA (inhibited red fuming nitric acid) was one of three liquid fuel components for the BOMARC missile.[20]. This grade is often used in the explosives industry. Another early production method was invented by French engineer Albert Nodon around 1913. This method of production is still in use today. Nitric acid is subject to thermal or light decomposition and for this reason it was often stored in brown glass bottles: This reaction may give rise to some non-negligible variations in the vapor pressure above the liquid because the nitrogen oxides produced dissolve partly or completely in the acid. CopyCopied, InChI=1S/HNO3/c2-1(3)4/h(H,2,3,4)
Production of nitric acid is via the Ostwald process, named after German chemist Wilhelm Ostwald. 1997-2022 LUMITOS AG, All rights reserved, https://www.chemeurope.com/en/encyclopedia/Nitric_acid.html, Your browser is not current. For the Gulf Shores television station, see, He goes on to point out that "nitrous air" is the reverse, or "nitric acid deprived of air and water. A nonvolatile residue of the metal hydrogen sulfate remains in the distillation vessel. With these non-active or less electropositive metals the products depend on temperature and the acid concentration. As a general rule of course, oxidizing reactions occur primarily with the concentrated acid, favouring the formation of nitrogen dioxide (NO2). This is subsequently absorbed in water to form nitric acid and nitric oxide. While the pure acid tends to give off white fumes when exposed to air, acid with dissolved nitrogen dioxide gives off reddish-brown vapors, leading to the common names "red fuming nitric acid" and "white fuming nitric acid". Nitric acid is one of the most common types of acid used in acid attacks. Depending on the acid concentration, temperature and the reducing agent involved, the end products can be variable. To use all the functions on Chemie.DE please activate JavaScript. Being a typical acid, nitric acid reacts with alkalis, basic oxides, and carbonates to form salts, including ammonium nitrate. The industrial production of nitric acid from atmospheric air began in 1905 with the BirkelandEyde process, also known as the arc process. One use for IWFNA is as an oxidizer in liquid fuel rockets. Being a powerful oxidizing agent, nitric acid reacts violently with many organic materials and the reactions may be explosive. Note:Results reported at time of bottling in glass. Commercial production of nitric acid is via the Ostwald process after Wilhelm Ostwald. The pKa value rises to 1 at a temperature of 250C.[9]. Cast iron cathodes were sunk into the peat surrounding it. Typically these digestions use a 50% solution of the purchased HNO3 mixed with Type 1 DI Water. Metals that are passivated by concentrated nitric acid are iron, cobalt, chromium, nickel, and aluminium.[10]. The resulting nitrates are converted to various complexes that can be reacted and extracted selectively in order to separate the metals from each other. One specification for white fuming nitric acid is that it has a maximum of 2% water and a maximum of 0.5% dissolved NO2. ", Muraoka, Hisashi (1995) "Silicon wafer cleaning fluid with HNO, National Institute for Occupational Safety and Health, "The crystal structures of the low-temperature and high-pressure polymorphs of nitric acid", "Freeze mob to highlight the issue of acid attacks", "On Some Chemical Agencies of Electricity", "The Production of Nitrates by the Direct Electrolysis of Peat Deposits", National Pollutant Inventory Nitric Acid Fact Sheet, Faceted Application of Subject Terminology, https://en.wikipedia.org/w/index.php?title=Nitric_acid&oldid=1097868786, Wikipedia articles needing page number citations from April 2019, Wikipedia articles incorporating a citation from the 1911 Encyclopaedia Britannica with Wikisource reference, Short description is different from Wikidata, Wikipedia indefinitely semi-protected pages, Chemical articles with multiple compound IDs, Multiple chemicals in an infobox that need indexing, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Wikipedia articles needing clarification from May 2020, Articles with unsourced statements from September 2011, Creative Commons Attribution-ShareAlike License 3.0, 83C (181F; 356K) 68% solution boils at 121C (250F; 394K), This page was last edited on 13 July 2022, at 01:57. Typical passivation concentrations range from 20% to 50% by volume (see ASTM A967-05). Concentrated nitric acid oxidizes I2, P4, and S8 into HIO3, H3PO4, and H2SO4, respectively. Nitric acid reacts with proteins to form yellow nitrated products. CopyCopied, GRYLNZFGIOXLOG-UHFFFAOYSA-N
However, the powerful oxidizing properties of nitric acid are thermodynamic in nature, but sometimes its oxidation reactions are rather kinetically non-favored. : TWA 2 ppm (5 mg/m 3 ). "[33][a] In 1785 Henry Cavendish determined its precise composition and showed that it could be synthesized by passing a stream of electric sparks through moist air.
These salts can be used to purify gold and other metals beyond 99.9% purity by processes of recrystallization and selective precipitation. The formation of this protective layer is called passivation. A mixture of nitric and sulfuric acids introduces a nitro substituent onto various aromatic compounds by electrophilic aromatic substitution. Concentrated nitric acid stains human skin yellow due to its reaction with the keratin. This test is carried out by adding concentrated nitric acid to the substance being tested, and then heating the mixture. [35][36] The nitric oxide was cooled and oxidized by the remaining atmospheric oxygen to nitrogen dioxide, and this was subsequently absorbed in water in a series of packed column or plate column absorption towers to produce dilute nitric acid. Commercial-grade fuming nitric acid contains 98% HNO3 and has a density of 1.50g/cm3. The presence of small amounts of nitrous acid (HNO2) greatly increases the rate of reaction. Concentration: 1% v/v Composition: Water 98.95%, Nitric Acid 1.05% Boiling Point: 100C Density: 1.01 Melting Point: 0.0C Color: Colorless liquid Physical State: Liquid pH Range: 0.8 Solubility Information: Miscible Shelf Life: 24 Months Storage: Ambient DOT: NOT REGULATED. Other Notes: The article number 07102-4X2.5L will be discontinued. Reaction of HNO3 with various original and synthetic mineral dust/mineral oxide surfaces was studied in a, Concentration: 18% w/w in Methanol Composition: Methyl Alcohol 82%, Nitric Acid 12.60%, Water 5.40% Boiling Point: Approximately 64C Density: 0.9 Melting Point: Color: Colorless to light yellow liquid Physical State: Liquid Flash Point: 16C pH Range: Solubility Information:, State: Liquid pH Range: <1 Solubility Information: Miscible Synonyms: Aqua fortis, Spirit of niter, Eau forte, Hydrogen nitrate, Acidum nitricum Shelf Life: 37 Months Storage: Ambient Packaging Type: Clear, Glass Container DOT: UN2031, NITRIC ACID, 8, P.G.II, Molecular Formula: HCl Molecular Weight: 36.46 Linear Structural Formula: HCl MDL Number: MFCD00011324 Purity: 36.5-38% Density: 1.2 g/mL at 25 C (lit.) Reaction takes place with all metals except the noble metals series and certain alloys. Nitric acid can act as a base with respect to an acid such as sulfuric acid: The nitronium ion, NO+2, is the active reagent in aromatic nitration reactions. Further concentration involves distillation with sulfuric acid which acts as a dehydrating agent.
About 20% of the produced oxides of nitrogen remained unreacted so the final towers contained an alkali solution to neutralize the rest. Obtained white fuming nitric acid has density 1.51 g/cm. This reaction is known as the xanthoproteic reaction. It is also typically used in the digestion process of turbid water samples, sludge samples, solid samples as well as other types of unique samples which require elemental analysis via ICP-MS, ICP-OES, ICP-AES, GFAA and flame atomic absorption spectroscopy. [8], The dissolved NOx is readily removed using reduced pressure at room temperature (1030minutes at 200mmHg or 27kPa) to give white fuming nitric acid. Nitric acid is a corrosive acid and a powerful oxidizing agent.
Only magnesium (Mg) and calcium (Ca) react with cold, dilute nitric acid to give hydrogen: Although chromium (Cr), iron (Fe) and aluminium (Al) readily dissolve in dilute nitric acid, the concentrated acid forms a metal oxide layer that protects the metal from further oxidation, which is called passivation. In elemental analysis by ICP-MS, ICP-AES, GFAA, and Flame AA, dilute nitric acid (0.55.0%) is used as a matrix compound for determining metal traces in solutions.
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