Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: senna on April 04, 2005, 01:58:37 AM
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I have a question that asks to list the acid strength in order of increacing acid strength. The order that I have come up with is NH4, HCN, HPO4 2-, H3O+, HF and finally HCL.
I feel a little confused as to where the HPO4 2- falls into the line up. It is also listed in the next problem that asks to list the bases in increasing strength. The order that I came up for the bases is HPO4 2-, CN-, Cl-, F-, NH3, OH-.
I am confused as to how HPO4 2- can have a ka and kb value and how these numbers relate.
??Do the order of these acids and bases appear correct?
Thank you for your response!
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I am confused as to how HPO4 2- can have a ka and kb value and how these numbers relate.
Very basic fact. You didn't pay attention at school ;)
Let's start with a weak acid HA
HA = H+ + A-
Ka = [H+][A-]/[HA]
What about conjugate base A-? It can react with water:
A- + H2O = HA + OH-
Kb = [HA][OH-]/[A-]
(water concentration moved to Kb by convention)
Multiplying:
Ka * Kb = [H+][A-]/[HA] * [HA][OH-]/[A-]
[HA] and [A-] cancels out:
Ka * Kb = [H+][OH-]
so
Ka * Kb = Kw
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Hi there,
You are contradicting yourself on the relative strengths of the acids and strengths of the bases...I would look up the term conjugate acid.....that should clear up some things.
Chemboy