How is nitric acid supplied, and how does it react with sulfuric acid?

1 Answer
anor277
Oct 29, 2015

#HNO_3(aq) + H_2O(l) rarr H_3O^+ + NO_3^-#

Explanation:

Concentrated nitric acid as supplied commercially has a density of #1.42# #g*cm^(-3)#, and has a concentration of #15# #mol*L^-1#. It is commonly used as a nitrating agent in organic chemistry in that its reactions with sulfuric acid produces the electrophilic nitrating agent #NO_2^+#, according to the following equation:

#H_2SO_4# #+# #HNO_3# #rarr# #NO_2^+ +HSO_4^-# #+ H_2O#

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