Hello.
I wanna ask one thing to everyone.
1. Formation of nitrite
I did griess test for check nitrite(NO2-) in the solution.
However, i couldn’t find the reason how they were formed. actually, my method is the thermal plasma, and I assume that the formation of nitrite was started from bond of N and O atom. Therefore, The first state is NO. And then, it reacts with H2O. Finally, I think that they become nitrite as a HNO2 or HNO3.
During this process, is it possible for NO to become a nitrite or nitrate after reaction with H2O ?...
Could you give me some advice or references?..
Thank you so much!
NO2 reacts with H2O and make acid.
2NO2 + H2O --------> 2HNO3
Hi Dr Kim Soonho . Yes in the case of NO2+H2O———> HNO3 . See the kinetics of the reaction in the following RG link: Article Kinetics of the reaction between nitrogen dioxide and water vapour
But in the case of
NO3 + H2O ——-> NH3 + OH.
See the link: https://en.intl.chemicalaid.com/tools/equationbalancer.php?equation=NO3+%2B+H2O+%3D+NH3+%2B+OH
Dear Kim Soonho thank you for posting this interesting technical question. For some basic information about this reaction please have a look at the Wikipedia entry on "Nitrous acid":
https://en.wikipedia.org/wiki/Nitrous_acid
Nitrous acid (HNO2) is the parent acid of nitrite salts. It can be formed by the reaction of N2O3 with water. N2O3 is the reaction product of NO and NO2. Both NO and NO2 are radicals, i.a. they have one unpaired electron so that they can easily combine to afford N2O3. Free nitrous acid is, however, quite unstable and decomposes readily. NO2 can react with water in the presence of oxygen to form nitric acid (see the instructive Wikipedia entry on "Nitric acid"), whereas nitric oxide (NO) alone does not react with water.
Please note that there is no such thing as "NO3". The highest oxidation state of nitrogen is 5, not 6! As a non-existing compound it can also not react with water under formation of NH3.
I hope this helps answering your question. Good luck with your work and best wishes, Frank Edelmann
Dear Chandan Kumar Tiwari thanks for your kind response and question. Please note that in stable (isolable) compounds the highest oxidation state of nitrogen is +5. This means that the last member in the series of nitrogen oxides is N2O5. Sometimes the compound N2O3 with nitrogen in the oxidation state +3 is referred to as "nitrogen trioxide". However, the correct name of this species should be "dinitrogen trioxide".
In sharp sontrast, the compound NO3 ("nitrogen trioxide") is only a transient species, which means that it is highly unstable and cannot be isolated under normal conditions. In this context, please check the following potentially useful literature references:
Nitrogen Trioxide (NO3)
https://www.degruyter.com/database/IUPAC/entry/iupac.62.0442/html
and
Nitrogen trioxide (NO3) quantum yields from nitrogen pentoxide (N2O5) photolysis
Article Nitrogen trioxide (NO3) quantum yields from nitrogen pentoxi...
If the latter article is of interest to you, please check if you can access it through your institution. Unfortunately the paper has not been posted as public full text on RG. The reaction NO3 + H2O = NH3 + OH is thus purely hypothetical. It can perhaps be investigated by calculational methods, but it certainly has no practical importance.
Good luck with your work!
First, NO3 is a very reactive radical and should quickly react with NO (which is also a radical) to form a mixture N2O4 = 2 NO2. Your question whether "is it possible for NO to become a nitrite or nitrate after reaction with H2O ?" has been studied in numerous publications. The correct (but not complete) answer has been given by Chandan Kumar Tiwari .
In addition
NO + NO2 = N2O3
N2O3 + H2O -> 2 HNO2 (nitrous acid)
Nitrous acid (pKa around 3) is unstable and decomposes at low pH. But this is another story.
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