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Fransisco is currently looking up this subject and i suggest he stops cause he needs more food from cosco....GO BUY STUFF IN BULK YOU ASIAN CHINK!

Colorless when pure, older samples tend to acquire a stronger yellow cast due to the accumulation of oxides of nitrogen. If the solution contains more than 86% nitric acid, it is referred to as fuming nitric acid. Fuming nitric acid is characterized as white fuming nitric acid and red fuming nitric acid, depending on the amount of nitrogen dioxide present. At concentrations above 95%, it tends to develop a slight yellow colour due to its tendency to adsorb water from the atmosphere.

Properties

Pure anhydrous nitric acid (100%) is a colorless liquid with a density of 1.522 g/cm³ which solidifies at −42 °C to form white crystals and boils at 83 °C. When boiling in light, even at room temperature, there is a partial decomposition with the formation of nitrogen dioxide following the reaction:

4 HNO₃ → 2 H₂O + 4 NO₂ + O₂ (72°C)

which means that anhydrous nitric acid should be stored below 0 °C to avoid decomposition. The nitrogen dioxide (NO₂) remains dissolved in the nitric acid coloring it yellow, or red at higher temperatures. While the pure acid tends to give off white fumes when exposed to air, acid with dissolved nitrogen dioxide gives off reddish-brown vapours, leading to the common name "red fuming acid" or "fuming nitric acid". Fuming nitric acid is also referred to as 16-molar nitric acid –– as the most concentrated form of nitric acid at Standard Temperature and Pressure (STP).

Nitric acid is miscible with water and distillation gives an azeotrope with a concentration of 68% HNO₃ and a boiling temperature of 120.5 °C at 1 atm, which is the ordinary concentrated nitric acid of commerce. Two solid hydrates are known; the monohydrate (HNO₃·H₂O) and the trihydrate (HNO₃·3H₂O). It is isoelectronic with the bicarbonate ion.

Nitrogen oxides (NO_x) are soluble in nitric acid and this property influences more or less all the physical characteristics depending on the concentration of the oxides. These mainly include the vapor pressure above the liquid and the boiling temperature, as well as the color mentioned above.

Nitric acid is subject to thermal or light decomposition with increasing concentration and this may give rise to some non-negligible variations in the vapour pressure above the liquid because the nitrogen oxides produced dissolve partly or completely in the acid.

Acidic properties

Being a typical acid, nitric acid reacts with alkalis, basic oxides, and carbonates to form salts, such as ammonium nitrate. Due to its oxidizing nature, nitric acid generally does not donate its proton (that is, it does not liberate hydrogen) on reaction with metals and the resulting salts are usually in the higher oxidized states. For this reason, heavy corrosion can be expected and should be guarded against by the appropriate use of corrosion resistant metals or alloys.

Nitric acid has an acid dissociation constant (pK_a) of −1.4: in aqueous solution, it almost completely (93% at 0.1 mol/L) ionizes into the nitrate ion NO⁻
₃ and a hydrated proton, known as a hydronium ion, H
₃O⁺
.

HNO
₃ + H
₂O ⇌ H
₃O⁺
+ NO⁻
₃

Oxidizing properties

Reactions with metals

Being a powerful oxidizing agent, nitric acid reacts violently with many organic materials and the reactions may be explosive. Depending on the acid concentration, temperature and the reducing agent involved, the end products can be variable. Reaction takes place with all metals except a few of the precious metal series and certain alloys. This characteristic has made it a common agent to be used in acid tests. As a general rule, oxidizing reactions occur primarily with the concentrated acid, favouring the formation of nitrogen dioxide (NO₂).

Cu + 4 H⁺ + 2 NO₃⁻ → Cu²⁺ + 2 NO₂ + 2 H₂O

The acidic properties tend to dominate with dilute acid, coupled with the preferential formation of nitric oxide (NO). However, when the reaction is carried out in the presence of atmospheric oxygen, the nitric oxide rapidly reacts to form brown nitrogen dioxide.

3 Cu + 8 HNO₃ → 3 Cu(NO₃)₂ + 2 NO + 4 H₂O

2 NO + O₂ → 2 NO₂

Since nitric acid is an oxidizing agent, hydrogen (H₂) is rarely formed. Only magnesium (Mg), Manganese (Mn) and calcium (Ca) react with cold, dilute nitric acid to give hydrogen:

Mg (s) + 2 HNO₃ (aq) → Mg(NO₃)₂ (aq) + H₂ (g)

Passivation

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. Typical passivation concentrations range from 18% to 22% by weight.

Reactions with non-metals

Reaction with non-metallic elements, with the exceptions of nitrogen, oxygen, noble gases, silicon and halogens, usually oxidizes them to their highest oxidation states as acids with the formation of nitrogen dioxide for concentrated acid and nitric oxide for dilute acid.

C + 4 HNO₃ → CO₂ + 4 NO₂ + 2 H₂O

or

3 C + 4 HNO₃ → 3 CO₂ + 4 NO + 2 H₂O

Xanthoproteic test

Nitric acid reacts with proteins to form yellow nitrated products. This reaction is known as the xanthoproteic reaction. This test is carried out by adding concentrated nitric acid to the substance being tested, and then heating the mixture. If proteins are present that contains amino acids with aromatic rings, the mixture turns yellow. Upon adding a strong base such as liquid ammonia, the color turns orange. These color changes are caused by nitrated aromatic rings in the protein.^[1]^[2] Xanthoproteins are formed when the acid contacts epithelial cells and are a certain giveaway of inadequate safety precautions when handling nitric acid.

Grades

The concentrated nitric acid of commerce consists of the maximum boiling azeotrope of nitric acid and water. Technical grades are normally 68% HNO₃, (approx 15 molar), while reagent grades are specified at 70% HNO₃. The density of concentrated nitric acid is 1.42 g/ml. An older density scale is occasionally seen, with concentrated nitric acid specified as 42° Baumé.

White fuming nitric acid, also called 100% nitric acid or WFNA, is very close to anhydrous nitric acid. One specification for white fuming nitric acid is that it has a maximum of 2% water and a maximum of 0.5% dissolved NO₂. Anhydrous nitric acid has a density of 1.513 g/ml. (Approx. conc. 24 molar).

A commercial grade of fuming nitric acid, referred to in the trade as "strong nitric acid" contains 90% HNO₃ and has a density of 1.50 g/ml. This grade is much used in the explosives industry. It is not as volatile nor as corrosive as the anhydrous acid. (Approx. Conc. 21.4 molar).

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. Because of the dissolved nitrogen dioxide, the density of red fuming nitric acid is lower at 1.490 g/ml.

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).

Industrial production

Nitric acid is made by reacting nitrogen dioxide (NO₂) with water.

3 NO₂ + H₂O → 2 HNO₃ + NO

Normally, the nitric oxide produced by the reaction is reoxidized by the oxygen in air to produce additional nitrogen dioxide.

Dilute nitric acid may be concentrated by distillation up to 68% acid, which is a maximum boiling azeotrope containing 32% water. In the laboratory, further concentration involves distillation with either sulfuric acid or magnesium nitrate which act as dehydrating agents. Such distillations must be done with all-glass apparatus at reduced pressure, to prevent decomposition of the acid. Industrially, strong nitric acid is produced by dissolving additional nitrogen dioxide in 68% nitric acid in an absorption tower.^[3] Dissolved nitrogen oxides are either stripped in the case of white fuming nitric acid, or remain in solution to form red fuming nitric acid. More recently, electrochemical means have been developed to produce anhydrous acid from concentrated nitric acid feedstock.^[4]

Commercial grade nitric acid solutions are usually between 52% and 68% nitric acid. Production of nitric acid is via the Ostwald process, named after German chemist Wilhelm Ostwald. In this process, anhydrous ammonia is oxidized to nitric oxide, which is then reacted with oxygen in air to form nitrogen dioxide. This is subsequently absorbed in water to form nitric acid and nitric oxide. The nitric oxide is cycled back for reoxidation. By using ammonia derived from the Haber process, the final product can be produced from nitrogen, hydrogen, and oxygen which are derived from air and natural gas as the sole feedstocks.^[5]

Prior to the introduction of the Haber process for the production of ammonia in 1923, nitric acid was produced using the Birkeland–Eyde process, also known as the arc process. This process is based upon the oxidation of atmospheric nitrogen by atmospheric oxygen to nitric oxide at very high temperatures. An electric arc was used to provide the high temperatures, and yields of up to 4% nitric oxide were obtained. The nitric oxide was cooled and oxidized by the remaining atmospheric oxygen to nitrogen dioxide, and this was subsequently absorbed in dilute nitric acid. The process was very energy intensive and was rapidly displaced by the Ostwald process once cheap ammonia became available.

Laboratory synthesis

In laboratory, nitric acid can be made from copper(II) nitrate or by reacting approximately equal masses of a nitrate salt with 96% sulfuric acid (H₂SO₄), and distilling this mixture at nitric acid's boiling point of 83 °C until only a white crystalline mass, a metal sulfate, remains in the reaction vessel. The red fuming nitric acid obtained may be converted to the white nitric acid.

H
₂SO
₄ + NO⁻
₃ → HSO⁻
₄ (s) + HNO
₃ (g)

The dissolved NO_x are readily removed using reduced pressure at room temperature (10-30 min at 200 mmHg or 27 kPa) to give white fuming nitric acid. This procedure can also be performed under reduced pressure and temperature in one step in order to produce less nitrogen dioxide gas.^{[citation needed]}

Uses

The main use of nitric acid is for the production of fertilizers, other important uses include the production of explosives, etching and dissolution of metals especially as a component of aqua regia for the purification and extraction of gold, and in chemical synthesis.

Elemental Analysis

In elemental analysis by ICP-MS, ICP-AES, GFAA, and Flame AA, dilute nitric acid (0.5 to 5.0 %) is used as a matrix compound for determining metal traces in solutions.^[6] Ultrapure trace metal grade acid is required for such determination, because small amounts of metal ions could affect the result of the analysis.

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 FAA. Typically these digestions use a 50% solution of the purchased HNO
₃ mixed with Type 1 DI Water.^[7]

Woodworking

In a low concentration (approximately 10%), nitric acid is often used to artificially age pine and maple. The color produced is a grey-gold very much like very old wax or oil finished wood (wood finishing).^[8]

Other uses

IWFNA^{[clarification needed]} may be used as the oxidizer in liquid fuel rockets.^[9] IRFNA^{[clarification needed]} was one of 3 liquid fuel components for the BOMARC missile.^[10]

A solution of nitric acid and alcohol, Nital, is used for etching of metals to reveal the microstructure.

Commercially available aqueous blends of 5-30% nitric acid and 15-40% 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).

Alone, it is useful in metallurgy and refining as it reacts with most metals, and in organic syntheses.

A mixture of concentrated nitric and sulfuric acids causes the nitration of aromatic compounds, such as benzene. Examination of the infrared spectrum of the acid mixture using a corrosive resistant diamond cell shows Infrared peaks close to that expected for carbon dioxide. The species responsible for the peaks is the nitronium ion, NO⁺
₂, which like CO
₂, is a linear molecule. The nitronium ion is the species responsible for nitration: being positive, it is attacked by electron-rich benzene rings. This is described more fully in organic chemistry books.

Safety

Nitric acid is a powerful oxidizing agent, and the reactions of nitric acid with compounds such as cyanides, carbides, and metallic powders can be explosive. Reactions of nitric acid with many organic compounds, such as turpentine, are violent and hypergolic (i.e., self-igniting). Due to its properties it is stored away from bases and organics.

Concentrated nitric acid dyes human skin yellow due to a reaction with the keratin. These yellow stains turn orange when neutralized.^[11]

Nitric acid in culture

Nitric acid is featured in two Charlie Chan films from the 1930s, as well as in Confessions of a Dangerous Mind (2002), starring George Clooney.^[12] Artist Allela Cornell committed suicide in 1946 by drinking nitric acid.^[13] Nitric acid is also featured on the "Pern" books by Anne McCaffrey, where it is known as "agenothree" because of linguistic drift.^[14]^[15]

References

^ Sherman, Henry Clapp (2007). Methods of Organic Analysis. READ BOOKS. p. 315. ISBN 1408628023.
^ Knowles, Frank (2007). A Practical Course in Agricultural Chemistry. READ BOOKS. p. 76. ISBN 1406745839.
^ Urbanski, Tadeusz (1965). Chemistry and technology of explosives. Oxford: Pergamon Press. pp. 85–86. ISBN 978-0-08-010239-9. {{cite book}}: |access-date= requires |url= (help)
^ US 6200456
^ Considine Douglas M., ed. (1974). Chemical and process technology encyclopedia. New York: McGraw-Hill. pp. 769–72. ISBN 978-0-07-012423-3. {{cite book}}: |access-date= requires |url= (help)
^ Franson, Mary A. H., Clesceri Lenore S., Greenberg Arnold E., Eaton Andrew D., ed. (1998). Standard methods for the examination of water and wastewater (20th ed.). American Public Health Association, American Water Works Association, Water Environment Federation. ISBN 978-0-87553-235-6. {{cite book}}: |access-date= requires |url= (help)CS1 maint: multiple names: editors list (link)
^ EPA Method 200.8
^ Jewitt, Jeff (1997). Hand-applied finishes (illustrated ed.). Taunton Press. ISBN 978-1-56158-154-2. Retrieved 2009-05-28.
^ Clark, John D. Ignition!. ISBN 0-8135-0725-1.
^ "BOMARC Summary". BILLONY.COM. Retrieved 2009-05-28.
^ Paul, May (2007). "Nitric Acid". Retrieved 2009-05-28. {{cite web}}: Unknown parameter |month= ignored (help)
^ Nitric Acid at the Internet Movie Database
^ Wilson, A. Beautiful Shadow: A Life of Patricia Highsmith. Bloomsbury, London. 2004.
^ McCaffrey, Anne (1979). Dragonquest. ISBN 978-0345335081.
^ McCaffrey, Anne (1981). The White Dragon. ISBN 978-0345275677.

External links

[1] Sherman, Henry Clapp (2007). Methods of Organic Analysis. READ BOOKS. p. 315. ISBN 1408628023.

[2] Knowles, Frank (2007). A Practical Course in Agricultural Chemistry. READ BOOKS. p. 76. ISBN 1406745839.

[3] Urbanski, Tadeusz (1965). Chemistry and technology of explosives. Oxford: Pergamon Press. pp. 85–86. ISBN 978-0-08-010239-9. {{cite book}}: |access-date= requires |url= (help)

[4] US 6200456

[5] Considine Douglas M., ed. (1974). Chemical and process technology encyclopedia. New York: McGraw-Hill. pp. 769–72. ISBN 978-0-07-012423-3. {{cite book}}: |access-date= requires |url= (help)

[6] Franson, Mary A. H., Clesceri Lenore S., Greenberg Arnold E., Eaton Andrew D., ed. (1998). Standard methods for the examination of water and wastewater (20th ed.). American Public Health Association, American Water Works Association, Water Environment Federation. ISBN 978-0-87553-235-6. {{cite book}}: |access-date= requires |url= (help)CS1 maint: multiple names: editors list (link)

[7] EPA Method 200.8

[8] Jewitt, Jeff (1997). Hand-applied finishes (illustrated ed.). Taunton Press. ISBN 978-1-56158-154-2. Retrieved 2009-05-28.

[9] Clark, John D. Ignition!. ISBN 0-8135-0725-1.

[10] "BOMARC Summary". BILLONY.COM. Retrieved 2009-05-28.

[11] Paul, May (2007). "Nitric Acid". Retrieved 2009-05-28. {{cite web}}: Unknown parameter |month= ignored (help)

[12] Nitric Acid at the Internet Movie Database

[13] Wilson, A. Beautiful Shadow: A Life of Patricia Highsmith. Bloomsbury, London. 2004.

[14] McCaffrey, Anne (1979). Dragonquest. ISBN 978-0345335081.

[15] McCaffrey, Anne (1981). The White Dragon. ISBN 978-0345275677.

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@@ Line 1: / Line 1: @@
+Fransisco is currently looking up this subject and i suggest he stops cause he needs more food from cosco....GO BUY STUFF IN BULK YOU ASIAN CHINK!
-{{chembox
-| Watchedfields = changed
-| verifiedrevid = 269313403
-| Name = Nitric acid
-| ImageFile = Nitric acid resonance median.png
-| ImageSize = 150px
-| ImageFile1 = Nitric-acid-resonance-A.png
-| ImageSize1 = 270px
-| ImageFileL2 = Nitric-acid-2D-dimensions.png
-| ImageSizeL2 = 150px
-| ImageFileR2 = Nitric-acid-3D-balls-B.png
-| ImageSizeR2 = 150px
-| IUPACName = Nitric acid
-|   OtherNames = Aqua fortis<br/>Spirit of nitre<br/>Salpetre acid<br/>Hydrogen Nitrate<br/>Azotic acid
-| Section1 = {{Chembox Identifiers
-|   CASNo = 7697-37-2
-|    CASNo_Ref = {{cascite}}
-|   ChEBI = 48107
-|   ChemSpiderID = 919
-|   RTECS = QU5775000
-|   UNNumber = 2031
-|   EINECS = 231-714-2
- }}
-| Section2 = {{Chembox Properties
-|   Formula = HNO<sub>3</sub>
-|   MolarMass = 63.012 g/mol
-|   Appearance = Clear, colorless liquid
-|   Density = 1.5129 g/cm<sup>3</sup>
-|   Solubility = completely miscible
-|   MeltingPtC = -42
-|   BoilingPtC = 83
-|   Boiling_notes  = bp of pure acid. 68% solution boils at 120.5&nbsp;°C
-|   pKa = -1.4
-|   Viscosity =
-|   RefractIndex = 1.397 (16.5 °C)
-|   Dipole = 2.17 ± 0.02 [[Debye|D]]
-  }}
-| Section7 = {{Chembox Hazards
-|   ExternalMSDS = [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc01/icsc0183.htm ICSC 0183]
-|   EUIndex = 007-004-00-1
-|   EUClass = Oxidant ('''O''')<br/>Corrosive ('''C''')
-|   RPhrases = {{R8}}, {{R35}}
-|   SPhrases = {{S1/2}}, {{S23}}, {{S26}}, {{S36}}, {{S45}}
-|   NFPA-H = 4
-|   NFPA-R = 0
-|   NFPA-F = 0
-|   NFPA-O = OX
-|   FlashPt = Non-flammable
-  }}
-| Section8 = {{Chembox Related
-|   OtherAnions = [[Nitrous acid]]
-|   OtherCations = [[Sodium nitrate]]<br/>[[Potassium nitrate]]<br/>[[Ammonium nitrate]]
-|   OtherCpds = [[Dinitrogen pentoxide]]
-  }}
-}}
-'''Nitric acid''' ([[Hydrogen|H]][[nitrate|NO<sub>3</sub>]]), also known as '''''[[aqua fortis]]''''' and '''spirit of nitre''', is a highly [[corrosion|corrosive]] and [[toxic]] [[strong acid]].
 Colorless when pure, older samples tend to acquire a stronger yellow cast due to the accumulation of [[nitrogen oxide|oxides of nitrogen]]. If the solution contains more than 86% nitric acid, it is referred to as '''fuming nitric acid'''. Fuming nitric acid is characterized as [[white fuming nitric acid]] and [[red fuming nitric acid]], depending on the amount of [[nitrogen dioxide]] present. At concentrations above 95%, it tends to develop a slight yellow colour due to its tendency to adsorb water from the atmosphere.