Quite effectively, actually. I was pickling a rusted bracket in nitric acid but I left it too long. The bracket was rust-free but the acid continued to eat the steel until it was paper-thin. You are better off using hydrochloric or phosphoric acid if you are prepping steel for painting. Both will open up the metal without eating it up.
It does not so much dissolve it as it oxidizes it. The nitric acid reacts with the iron to produce iron nitrate and hydrogen gas.
6HNO3 + 2Fe --> 2Fe(NO3)3 + 3H2
Iron Oxide is Fe[2]O[3] and Nitric acid is HNO[3]
Nitric acid is oxidizing acid. When it reacts with iron it forms a protective layer of iron oxide over it. So it does not react further.
Nitric acid(HNO3)
I think, concentrated Nitric acid (HNO3)
Sorry i dont know
Iron Oxide is Fe[2]O[3] and Nitric acid is HNO[3]
Nitric acid is oxidizing acid. When it reacts with iron it forms a protective layer of iron oxide over it. So it does not react further.
Nitric acid(HNO3)
I think, concentrated Nitric acid (HNO3)
Sorry i dont know
Examples: nitric acid, sulfuric acid, phosphoric acid, perchloric acid, etc.
iron with concentrated nitric acid no reaction occurs becase of the iron passivity which is due to the oxidizing property of the acid were a layer of the metal oxide is formed which is complete and non porous so it protects the metal from further reaction
Iron is a highly reactive metal and most of the strong acids like sulfuric acid and nitric acid are able to dissolve it. Steel is less reactive than iron because it is an alloy but will get corroded and dissolved in nitric acid solution 50-70 %. See also the link below.
This depends on: - concentration of nitric acid - stirring - temperature - pressure - ratio iron/acid in the beaker - the physical form of iron: powder, granules, chips, etc.
when nitric acid and iron react together Iron Nitrate is formed and hydrogen gas
Products of Iron (Fe) reacting with Nitric Acid(HNO3) depends on temperature of reactants as well as concentration of HNO3. With dilute HNO3 Iron gives Ferrous Nitrate [Fe(NO3)2], water and Nitric oxide(NO). 3Fe + 8HNO3 --> 3Fe(NO3)2 + 4H2O + 2NO With concentrated HNO3 iron gives Ferric nitrate [Fe(NO3)3], water and Nitrogen dioxide(NO2). Fe + 6HNO3 --> Fe(NO3)3 +3H2O + 3NO2 Reaction of iron with concentrated Nitric acid Renders it passive to further reaction due to formation of thin oxide layer on the surface. In all these Reactions Nitric acid acts as an oxidising agent.
The titration must be done in acidic medium to prevent the precipitate of Iron(III) as hydrated oxide (iron hydroxide). Iron (III) is an indicator.