Understanding Acid Strength: HSO3- vs H2SO3

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    Acid Strength
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Discussion Overview

The discussion revolves around the relative acid strength of HSO3- compared to H2SO3, exploring concepts of electronegativity, bond strength, and pH. Participants also touch on the general principles of acid dissociation and how to rank the pH of various solutions.

Discussion Character

  • Exploratory
  • Debate/contested
  • Conceptual clarification
  • Mathematical reasoning

Main Points Raised

  • One participant questions why HSO3- is considered a stronger acid than H2SO3, suggesting a misunderstanding of acid strength concepts.
  • Another participant states that the strength of an acid relates to how easily it releases hydrogen ions, linking this to pH as a measure of H+ concentration.
  • A participant challenges the initial claim about HSO3- and H2SO3, asserting that increased electronegativity does not necessarily lead to stronger bonds, and thus does not prevent ionization.
  • There is a discussion about the relationship between electronegativity and acid strength, with some arguing that higher electronegativity leads to more ionic character and greater ionization.
  • One participant introduces the idea that acidity is also influenced by the polarity of the molecule and the transition state during dissociation.
  • Another participant reiterates that a stronger acid is one that dissociates more completely into H+ ions, emphasizing the reversible nature of acid dissociation.

Areas of Agreement / Disagreement

Participants express differing views on the strength of HSO3- versus H2SO3, with no consensus reached. There are also conflicting interpretations of how electronegativity affects acid strength and bond strength, indicating ongoing debate.

Contextual Notes

Some statements rely on specific conditions, such as the requirement for H-X to be binary and for X to come from the same period, which may not be universally applicable. Additionally, the discussion includes assumptions about the definitions of acid strength and pH that are not explicitly clarified.

nemzy
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Why is HSO3- a stronger acid then H2SO3?

And also, i know that When the size of an atom X increases, the H-X bonds decreases, meaning the strength of the acid increases since more H+ are ionized.

But when when H-X are more electronegitive, doesn't it mean the bonds between the H-X gets stronger, meaning fewer H+ ionizes?? But this is not the case, the more electrongetive the bond between H-X, the acid strength gets stronger. Is my conceptual idea wrong?

Also, let's say you have solutions of NH3, HCl, NaOH, and HC2H3O2 , all with the same solute concetrations. How would you know rank the pH of these solutions from highest to lowest or vice versa?
 
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from what I know, the pH value is a measure of concentration of H+ ions, but the strength of an acid is how easy an acid releases its hydrogen ions.
 
I don't know about HSO3- and H2SO3, but if you mean HSO4 and H2SO4, then the latter is stronger.

Increased electronegativity doesn't translate to stronger bonds.

Of your list, HCl is the strongest acid, followed by acetic acid, ammonia, and sodium hydroxide.
 
nemzy said:
Why is HSO3- a stronger acid then H2SO3?
other way around then your statement is true. I am assuming you know why if that is the case.

nemzy said:
But when when H-X are more electronegitive, doesn't it mean the bonds between the H-X gets stronger, meaning fewer H+ ionizes?? But this is not the case, the more electrongetive the bond between H-X, the acid strength gets stronger. Is my conceptual idea wrong?
other way around again. your conceptual idea is wrong.

more electronegativity of X means the bond will be more ionic, ie ionization is more favoured. therefore meaning more ionization occurs.

electronegativity increases for X, then the acid strength increases for H-X.

note: H-X must be binary and X must come from the same period for the above statement to hold. because otherwise various different factors will be affecting the bond instead of just a change in electronegativity.
 
Acidity also has to do with polarity of the molecule. Think transition state, of which the product is an H+ ion and the subsequent anion. A transition state with more H+ character will have lower activation energy.


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I think some one already said this but i'll say it again. By 'Strength' I am assuming you mean ph, which is the concentration of H+ ions, therefore if an acid can easily disassociate completely more H+ ions are Formed. ie X-H -> X- + H+, but if the acid only partially disassociates not as many H+ ions are formed. X-H <=> X- + H+ (reversible reaction)
:) that what i was told anyway.

so one acid would be stronger if it dissasosiated into H+ions more that another.
 
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