Question about bronstead lowry acids/bases

Question

greatlife44 · Answer

$$HNO_{3} + H_{2}SO_{4} --> NO_{2}^{+}(HSO_{4}^{-} + H_{2}O$$

greatlife44 · Answer

What is the bronstead lowry base in this reaction?

sweetburger · Answer

Pretty rare deal when the strong acid H2SO4 is a base. Bronsted-Lowery bases are any substance that can accept a proton. HNO3 is the base in this equation. Notice that it donated a OH- and its charge became less negative (hence accepted a proton/became more positive) Idk if this explanation will make sense...

greatlife44 · Answer

Yeah, I checked in my book and H2SO4 is acting as the acid and the base is H2NO3. But this is a strange reaction though.

greatlife44 · Answer

hmm I guess I could try to draw this out hopefully this will make some more sense

greatlife44 · Answer

@sweetburger take a look at this. 

Since H2SO4 acts as the acid it donates it's proton to H2SO4

If we draw a resonance structure like this, we can see that HNO3 can accept another proton, but its structure will be different. 

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Now, I think what happens is that in order for this reaction to happen once the oxygen accepts the other proton, the electrons from the oxygen ion come down to expel water and we're left with NO2+ and water. along with HSO4- 


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