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

$H N {O}_{3} \left(a q\right) + {H}_{2} O \left(l\right) \rightarrow {H}_{3} {O}^{+} + N {O}_{3}^{-}$
Concentrated nitric acid as supplied commercially has a density of $1.42$ $g \cdot c {m}^{- 3}$, and has a concentration of $15$ $m o l \cdot {L}^{-} 1$. It is commonly used as a nitrating agent in organic chemistry in that its reactions with sulfuric acid produces the electrophilic nitrating agent $N {O}_{2}^{+}$, according to the following equation:
${H}_{2} S {O}_{4}$ $+$ $H N {O}_{3}$ $\rightarrow$ $N {O}_{2}^{+} + H S {O}_{4}^{-}$ $+ {H}_{2} O$