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

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

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Answer 1 · 2015-10-29T18:02:45

$H N O_{3} (a q) + H_{2} O (l) \to H_{3} O^{+} + N O_{3}^{-}$ $HNO_3(aq) + H_2O(l) rarr H_3O^+ + NO_3^-$

Explanation:

Concentrated nitric acid as supplied commercially has a density of $1.42$ $1.42$ $g \cdot c m^{- 3}$ $g*cm^(-3)$ , and has a concentration of $15$ $15$ $m o l \cdot L^{- 1}$ $mol*L^-1$ . It is commonly used as a nitrating agent in organic chemistry in that its reactions with sulfuric acid produces the electrophilic nitrating agent $N O_{2}^{+}$ $NO_2^+$ , according to the following equation:

$H_{2} S O_{4}$ $H_2SO_4$ $+$ $+$ $H N O_{3}$ $HNO_3$ $\to$ $rarr$ $N O_{2}^{+} + H S O_{4}^{-}$ $NO_2^+ +HSO_4^-$ $+ H_{2} O$ $+ H_2O$

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

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