mam can you explain this
Asked by | 13th Jun, 2008, 10:54: PM
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 (pKa) of −1.4: in aqueous solution, it almost completely (93% at 0.1 mol/L) ionizes into the nitrate ion NO3− and a hydrated proton, known as a hydronium ion, H3O+.
- HNO3 + H2O → H3O+ + NO3-
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.
- C + 4HNO3 → CO2 + 4NO2 + 2H2O
- 3C + 4HNO3 → 3CO2 + 4NO + 2H2O reacting with H2 is to be clarifed, where did you read it!
Answered by | 14th Jun, 2008, 07:49: AM
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