Nitric acid formula HNO3 is a strong acid. Spirit of Nera and Aqua Fortis are also names commonly associated with it. Pure and uncoloured, it gets a yellowish cast as it ages. Nitrogen oxides and water are formed when nitric acid decomposes. A highly toxic and corrosive substance. Severe burns are caused by it. Nitrate salts are formed when it reacts with hydroxides, metals, and oxides. HNO3 chemical name is Nitric acid or Chemical formula of nitric acid is HNO3. Oxidizing agents like HNO3 are used in many industrial processes. Catalytic oxidation of ammonia can be used to manufacture it. Chemicals containing this compound are often used in laboratories and are important in industrial processes such as manufacturing explosives and fertilizers. Nitric acid has a PH of roughly 3.01.
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3 oxygen atoms are present in each molecule with 1 nitrogen atom and 1 hydrogen atom in each molecule. A double bond exists between both oxygen and nitrogen atoms in HNO3. In addition to being singly bonded to the nitrogen atom, another oxygen atom is also singly bonded to a hydrogen atom. Oxygen atoms with a charge of -1 are single bonded to nitrogen atoms, forming the last oxygen atom of the nitric acid molecule. A molecule's nitrogen atom has a charge of +1 since it participates in four covalent bonds (with three oxygen atoms). So, the nitric acid molecule has a net charge of 0 (the positive charge on the nitrogen atom cancels out the negative charge on the oxygen atom). Molecular charges can be delocalized due to resonance in these molecules. Here is a diagram of the nitric acid molecule.
Its density is 1.50g/cm3 and it contains 98% HNO3. The explosives industry frequently uses this grade. The concentration of the anhydrous acid is approximately 21.4 M, and it is not as corrosive or volatile. The reddish-brown colour of RFNA is the result of significant amounts of dissolved nitrogen dioxide (NO2). Red fuming nitric acid has a reduced density of 1.490 g/cm3 due to the dissolved nitrogen dioxide. The addition of hydrogen fluoride (HF) can be used to make an inhibited fuming nitric acid (also referred to as an IWFNA or IRFNA). Metal tanks are coated with this fluoride for corrosion resistance. The flux protects the metal by forming a fluoride layer.
It is possible for a less volatile acid to displace a more volatile acid. The preparation of nitric acid in the laboratory works on this principle.
Unlike sulphuric acid, nitric acid has greater volatility. The metal nitrates displace it with sulfuric acid.
In a round bottom flask, 50 grams of potassium nitrate (KNO3) is combined with 25 ml of concentrated sulfuric acid (H2SO4). A temperature of about 200°C is maintained without exceeding it, as long as the reactants are not overheated.
KNO3 + H2SO4 → KHSO4 + HNO3(Salts of more volatile acids + fewer volatile acids displaced more volatile acids)
In the diagram, you can see the process of cooling and condensing the nitric acid vapours for collection.
Molecular Weight/ Molar Mass
Acids such as nitric acid can turn blue when exposed to light.
Nitrogen dioxide is formed by the decomposition of nitric acid. As a result, it turns brown over time, despite being colourless when in its fresh form.4HNO3 → 4NO2 + O2 + 2H2O
Nitric acid releases hydrogen gas with metals above hydrogen in the metal activity series.
Mg + 2HNO3 → Mg (NO3)2 + H2Mn + 2HNO3 → Mn (NO3)2 + H2
Producing ammonium nitrates is used to manufacture plastic, dye, and fertilizer
TNT and other explosives are made from it
Rockets with liquid fuel use it for oxidation
When it is used in its purest form, it helps remove warts
Electrochemistry uses it as a chemical doping agent
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