Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Oxoacid strengths in aqueous solutions

  1. Apr 14, 2012 #1
    Hey there,

    My textbook doesn't expand on this much and I'm unsure if I'm just not seeing some obvious connection; I'd appreciate it if someone could clarify this for me.

    I'm studying the Bronsted-Lowry theory and the strength of binary and ternary acids. I understand how, for example, H2SO4 dissociates in water, but I don't see why the dissociation of that would be any different than say, H2SO3.

    I realize that for some reason, acid strength increases with an increased number of oxygen atoms, but I can't understand why.

    From what I understand, the O-H bonds are broken in water to create an anion and H+, so why would a larger amount of oxygen atoms in a molecule have anything to do with acid strength since the amount of O-H groups remain constant in both molecules (for example, H2SO4 and H2SO3 both have the same amount of O-H groups.)

    What am I misunderstanding or missing?
  2. jcsd
Share this great discussion with others via Reddit, Google+, Twitter, or Facebook

Can you offer guidance or do you also need help?
Draft saved Draft deleted