|Apr14-12, 02:42 PM||#1|
Oxoacid strengths in aqueous solutions
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?
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