nitrates in urine

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Nitrate test
From Wikipedia, the free encyclopedia
For the test to determine the ability of microbes to reduce nitrate to nitrite, see Nitrate reductase test.
A nitrate test is a chemical test used to determine the presence of nitrate ion in solution. Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulphate precipitate with barium.

The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property. Unfortunately, other oxidants present in the analyte may interfere and give erroneous results.

Contents [show]
Ring test[edit]

Nitrate Test by using Brown Ring Test
A common nitrate test, known as the brown ring test[1] can be performed by adding iron(II) sulfate to a solution of a nitrate, then slowly adding concentrated sulfuric acid such that the acid forms a layer below the aqueous solution. A brown ring will form at the junction of the two layers, indicating the presence of the nitrate ion.[2] Note that the presence of nitrite ions will interfere with this test.[3]

The overall reaction is the reduction of the nitrate ion by iron(II) which is oxidised to iron(III) and formation of a nitrosonium complex where nitric oxide is reduced to NO−[4].

2HNO3+ 3H2SO4 + 6FeSO4 —->> 3Fe2(SO4)3 + 2NO + 4H2O
[Fe(H2O)6]SO4 + NO = [Fe(H2O)5(NO)]SO4+ H2O
This test is sensitive up to 2.5 micrograms and a concentration of 1 in 25000 parts. [5]

Devarda's test[edit]
Main article: Devarda's alloy
Devarda's alloy (Copper/Aluminium/Zinc) is a reducing agent. When reacted with nitrate in sodium hydroxide solution, ammonia is liberated. The ammonia formed may be detected by its characteristic odor, and by damp red litmus paper's turning blue, signalling that it is an alkali — very few gases other than ammonia evolved from wet chemistry are alkaline.

3 NO−
3 + 8 Al + 5 OH−
+ 18 H
2O → 3 NH
3 + 8 [Al(OH)
Aluminium is the reducing agent in this reaction.

Diphenylamine test[edit]
Diphenylamine may be used as a wet chemical test for the presence of the nitrate ion. In this test, a solution of diphenylamine and ammonium chloride in sulfuric acid is used. In the presence of nitrates, diphenylamine is oxidized, giving a blue coloration. This reaction has been used to test for organic nitrates as well.,[6] and has found use in gunshot residue kits detecting nitroglycerine and nitrocellulose.[7]

Copper turnings test[edit]
The nitrate ion can easily be identified by heating copper turnings along with concentrated sulphuric acid. Brown, pungent effervescence is observed which turns blue litmus red.

Here sulfuric acid reacts with the nitrate ion to form nitric acid. Nitric acid then reacts with the copper turnings to form nitric oxide. Nitric oxide is thus reduced to nitrogen dioxide (if required)

Cu + 4 HNO
3 → Cu(NO
2 + 2 NO
2 +2H
See also[edit]
Nitrite test
Jump up ^ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
Jump up ^ Mascetta, Joseph A. Barron's How to Prepare for the SAT II: Chemistry, 7th edition. Barron's Educational Series, Inc., 2002. p208.
Jump up ^ Holltzclaw, H; Robinson, W. College Chemistry with qualitative analysis, 8th edition, D. C. Heath and Company:Lexington, MA, 1988, p. 1007.
Jump up ^ Alicja Wanat, Thorsten Schneppensieper, Grażyna Stochel, Rudi van Eldik, Eckhard Bill, and Karl Wieghardt (2002). "Kinetics, Mechanism, and Spectroscopy of the Reversible Binding of Nitric Oxide to Aquated Iron(II). An Undergraduate Text Book Reaction Revisited". Inorganic Chemistry. 41 (1): 4–10. Formerly it was thought that the complex contains Fe(I) and NO+.
Jump up ^; Nilay Ghosh
Jump up ^
Jump up ^ Pamela K. Walker and Philip J. Rodacy (2002). "Field Test Kit for Gunshot Residue Detection" (PDF). Sandia National Laboratories.

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