Does Sulfuric acid donate both of it H+ protons?

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Discussion Overview

The discussion centers around the behavior of sulfuric acid (H2SO4) in terms of its ability to donate protons (H+) and the implications of this behavior on its stability and acidity. Participants explore the concepts of acid-base equilibria, the stability of the resulting species, and the definitions of acidity and basicity.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant questions whether sulfuric acid donates both of its protons and discusses the stability of the resulting species based on resonance structures.
  • Another participant notes that while H2SO4 can donate both protons, HSO4- is a weaker acid than H2SO4, emphasizing the role of dissociation equilibria.
  • A participant suggests that HSO4- may not donate its second proton due to stability concerns related to the negative charge.
  • There is a query about whether HSO4- could be considered basic because of its negative charge.
  • One participant argues that the terms "somewhat basic" or "weakly acidic" are relative and do not provide clear descriptions, highlighting the complexity of acid-base behavior.
  • A request for clarification is made regarding why acids do not behave like bases after donating protons.
  • It is mentioned that acids can behave like bases by accepting protons back in reversible reactions.
  • A reminder is provided that all dissociation reactions are reversible, referencing Brønsted-Lowry's theory of acids and bases.

Areas of Agreement / Disagreement

Participants express differing views on the stability of HSO4- and its behavior as an acid or base. The discussion remains unresolved regarding the implications of the negative charge on acidity and basicity, as well as the definitions of these terms.

Contextual Notes

The discussion involves assumptions about the stability of sulfuric acid and its conjugate base, as well as the definitions of acidity and basicity, which may vary based on context. The role of equilibria in acid-base reactions is also a key factor that remains nuanced.

gangsterlover
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H2SO4 + H2O -> HSO4- + H3O+

A question by a noob.

I get the fact that water can act as an acid and as a base. The oxygen "pulls" the hydrogen+ ion away from the sulfuric acid oxygen hydrogen bond an gets one itself and becomes positively charged, therefore a hydronium.

However, I wonder does sulfuric acid donate it`s other proton as well. I see no reason why it wouldn`t I mean it would still be somewhat stable, cause the charge is quite spread out over the 3 oxygen atoms, so more stable more acidic. At least that`s how I am getting it when drawing those resonance structures. When the sulfuric acid molecule would lose both of them, I wonder wouldn`t the sulfuric acid be quite unstable then. And become a base, wouldn`t it just rip out the protons from the oxygen again, because of the size of sulfur in comparison with oxygen.

The oxygen couldn`t accept another proton, but what about another oxygen?

People please help me I am in a mess here :(
If I have stated something from ^^ above please tell me, I am still a underclass rookie.
Thanks.
 
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It can, but HSO4- is a much weaker acid than H2SO4.

It is all about dissociation equilibria. For example at pH=2.0 there is no H2SO4 in the solution (well, some traces), but concentrations of HSO4- and SO42- are identical (so at this particular pH half of HSO4- donated its proton to water).
 
But it tends to not do it because it is less stable than H2SO4? Because of the negative charge right?
 
But would the HS04- become somewhat basic because of the negative charge?
 
To call it somewhat basic or ''weakly acidic'' are relative terms. It doesn't describe very much. The negative charge doesn't indicate whether something is basic or not, there are just general trends which have many exceptions, but hold for a lot of cases.
 
Could you then shortly explain why acids don`t end up like bases when they give up their protons?
 
They do end up like bases in a sense, they will take back a proton if they can. This happens in many reactions
 

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