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CAS NUMBER: 7697-37-2
EC NUMBER: 231-714-2
MOLECULAR FORMULA: HNO3
MOLECULAR WEIGHT: 63.01
Nitric acid (HNO3) is a highly corrosive mineral acid.
Nitric acid is usually utilized for abstracting transition metal catalyst from single-walled carbon nanotubes (SWNTs) in order to purify them.
The effect of nitric acid on the oxidation of multiwalled carbon nanotubes (MWCNTs) has been investigated by sample weight, Raman spectrum, solubility, morphology and alignment examinations.
Nitric acid (HNO3), also known as aqua fortis (Latin for "strong water") and spirit of niter, is a highly corrosive mineral acid.
The pure compound is colorless, but older samples tend to acquire a yellow cast due to decomposition into oxides of nitrogen and water.
Most commercially available nitric acid has a concentration of 68% in water.
When the solution contains more than 86% HNO3, it is referred to as fuming nitric acid.
Depending on the amount of nitrogen dioxide present, fuming nitric acid is further characterized as red fuming nitric acid at concentrations above 86%, or white fuming nitric acid at concentrations above 95%.
Nitric acid is the primary reagent used for nitration the addition of a nitro group, typically to an organic molecule.
While some resulting nitro compounds are shock- and thermally-sensitive explosives, a few are stable enough to be used in munitions and demolition, while others are still more stable and used as pigments in inks and dyes.
Nitric acid is also commonly used as a strong oxidizing agent.
Nitric acid, red fuming appears as a pale yellow to reddish brown liquid generating red-brown fumes and having a suffocating odor.
Very toxic by inhalation.
Corrosive to metals or tissue.
Prolonged exposure to low concentrations or short term exposure to high concentrations may result in adverse health effects.
Rate of onset: Immediate Persistence: Hours days Odor threshold: ~1 ppm Source/use/other hazard: Used in many industries; Very corrosive to skin/mucous membranes as well as metals & other materials.
Nitric acid is a nitrogen oxoacid of formula HNO3 in which the nitrogen atom is bonded to a hydroxy group and by equivalent bonds to the remaining two oxygen atoms.
Nitric acid has a role as a protic solvent and a reagent.
Nitric acid is a conjugate acid of a nitrate.
Nitric acid (HNO3). A colorless liquid that is used in the manufacture of inorganic and organic nitrates and nitro compounds for fertilizers, dye intermediates, explosives, and many different organic chemicals.
Continued exposure to vapor may cause chronic bronchitis; chemical pneumonitis may occur.
Nitric acid, (HNO3), colourless, fuming, and highly corrosive liquid (freezing point −42 °C [−44 °F], boiling point 83 °C [181 °F]) that is a common laboratory reagent and an important industrial chemical for the manufacture of fertilizers and explosives.
Nitric acid is toxic and can cause severe burns.
The preparation and use of nitric acid were known to the early alchemists.
A common laboratory process used for many years, ascribed to a German chemist, Johann Rudolf Glauber (1648), consisted of heating potassium nitrate with concentrated sulfuric acid.
In 1776 Antoine-Laurent Lavoisier showed that it contained oxygen, and in 1816 Joseph-Louis Gay-Lussac and Claude-Louis Berthollet established its chemical composition.
The principal method of manufacture of nitric acid is the catalytic oxidation of ammonia.
In the method developed by the German chemist Wilhelm Ostwald in 1901, ammonia gas is successively oxidized to nitric oxide and nitrogen dioxide by air or oxygen in the presence of a platinum gauze catalyst.
The nitrogen dioxide is absorbed in water to form nitric acid.
The resulting acid-in-water solution (about 50–70 percent by weight acid) can be dehydrated by distillation with sulfuric acid.
Nitric acid (HNO₃) is a colorless liquid with yellow or red fumes with an acrid odor.
Exposure to nitric acid can cause irritation to the eyes, skin, and mucous membrane; it can also cause delayed pulmonary edema, pneumonitis, bronchitis, and dental erosion.
Nitric acid is highly corrosive. Workers may be harmed from exposure to nitric acid.
The level of exposure depends upon the dose, duration, and work being done.
Nitric acid has the molecular formula HNO3 and is also known as aqua fortis.
Nitric acid is a highly corrosive acid, mainly used as a precursor to a variety of nitrogen compounds, especially fertilizers.
Nitric acid can also be used as an oxidant and cleaning agent.
Nitric acid is used in a wide variety of chemical processes where cleaning, oxidising or etching is required, including making synthetic fibres, dying, electrical circuit board making, electroplating, explosives, laboratory chemicals, metal cleaning and etching, semiconductors, pharmaceutical manufacture.
Nitric acid is used in the manufacture of fertilisers and other organic chemicals, in the printing industry for photoengraving, in jewellery manufacturing, and for wet chemical etching.
Nitric acid is a colorless, corrosive liquid that is the most common nitrogen acid.
Nitric acid 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.
Nitric acid is named because of the fumes emitted by acid when it combines with moist air.
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%.
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.
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.
USES OF NITRIC ACID:
The main industrial use of nitric acid is for the production of fertilizers.
Nitric acid is neutralized with ammonia to give ammonium nitrate.
This application consumes 75–80% of the 26 million tonnes produced annually (1987).
The other main applications are for the production of explosives, nylon precursors, and specialty organic compounds.
Nitric acid is one of the most common types of acid used in acid attacks.
Nitric acid is used in many industries.
Nitric acid’s used in the manufacture of fertilizers, dyes, and explosives.
Nitric acid is also used in the polymer industry.
Nitric Acid is used in many industrial applications for its oxidizing or acidic qualities, including:
Nitric acid is an important starting material for the production of fertilizers and chemicals.
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.
This heavy, clear or slightly yellowish fluid is very poisonous and causes severe burns on contact with the skin.
Nitric acid 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.
Nitric acid 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.
The main use of nitric acid is for the production of fertilizer, with approximately threefourthsof nitric acid production being used for this purpose.
Nitric acid 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.
Nitric acid 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.
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.
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.
Nitric acid is also madefrom ammonia by catalytic oxidation, or fromthe nitric oxide produced from air.
-The production of nitrogen products intended mainly for fertilization – read more about crop nutrition
-Adipic acid-intermediate of nylon 6,6 chemistry, used in the production of artificial fibers, nylon yarns and plastic parts for automobiles
-Polyurethanes (MDI and TDI): insulation, foams, paints and coatings
APPLICATION OF NITRIC ACID:
Nitric acid was used to increase the number of acid sites by altering the surface of activated carbon.
Nitric acid may be used:
-In combination with acetic anhydride and zeolite catalysts for the preparation of p-nitrotoluene with high regioselectivity.
-In the pretreatment of rice straw for enhanced production of xylose.
-To minimize the extent of cation ordering in LiNi0.5Mn1.5O4, a transition metal-substituted spinel material, by surface treatment.
PROPERTIES OF NITRIC ACID:
-Quality Level: 200
-grade: ACS reagent
-vapor pressure: 8 mmHg ( 20 °C)
-assay: 68.0-70.0% (ACS specification) 70%
-form: liquid
-ign. residue: ≤5 ppm
-color: APHA: ≤10
-PH: < 1.0
-boiling point: 120.5 °C (lit.)
-density: 1.413 g/mL at 20 °C (lit.)
PHYSCIAL AND CHEMICAL PROPERTIES OF NITRIC ACID:
Commercially available nitric acid is an azeotrope with water at a concentration of 68% HNO3.
Nitric acid has a boiling temperature of 120.5 °C at 1 atm.
Nitric acid is known as "concentrated nitric acid".
Pure concentrated nitric acid is a colourless liquid at room temperature.
Two solid hydrates are known: the monohydrate (HNO3·H2O or [H3O]NO3) and the trihydrate (HNO3·3H2O).
An older density scale is occasionally seen, with concentrated nitric acid specified as 42° Baumé.
Nitric acid is a transparent, colourless or yellowish, corrosive liquid with an acrid or pungent odour.
Nitric acid is a strong,fire-hazardous oxidant.
Nitric acid 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.
Nitric acid is a reddish fuming liquid. Fumes in moist air. Often used in an aqueous solution.
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.
PRODUCTION OF NITRIC ACID:
Nitric Acid is a clear, yellow liquid with a strong odor.
To produce it, we start with ammonia, which is also produced in our own plants.
Nitric acid is oxidized on platinum webs, producing nitrous gases such as NO2.
These gases are then absorbed in water.
From this, we get weak Nitric Acid (W-NA) which is up to 68% (azeotrope).
Through a rectification process we increase the concertation up to 99% concentrated Nitric Acid (C-NA).
Since our weak Nitric Acid is produced from gases ammonia and air.
Nitric acid is very pure and does not contain heavy metals.
STORAGE OF NITRIC ACID:
No metal or light-weight metal containers.
Tightly closed.
Do not store near flammable materials. locked or just
Store Nitric acid in places where qualified or authorized persons can access it.
SYNONYM:
Hydrogen nitrate
Aqua fortis
Azotic acid
Salpetersaeure
nitrooxidanyl
RFNA
Acide nitrique
Red fuming nitric acid
HNO3
UNII-411VRN1TV4
Nitric acid [NF]
HONO2
MFCD00011349
CHEMBL1352
411VRN1TV4
CHEBI:48107
