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General Chemistry A: Chapter 17 Acid Base Equilibria Summary Part 2
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Summary of Acid Base Equilibria. Part 2
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Common ion effect Buffer solutions- common ion effect: if - buffer solution: one that
there is another source resists a change in ph
for anion common to one when either small amount
of the ions in an acid/ of oh- or h3o+ is added
base equilibrium, the ph - requires 1 component to
will increase neutralize acid, 1 to
-ie: hf + h2o —> h3o+ + f- neutralize base
& naf —> na+ + f- - 2 opponents can’t
- f- is the neutralize each other
conjugate base, (like w/ strong acid +
therefore ph will strong base)
become more basic - contains a weak acid & its
- ph understood by conjugate both in
applying le chatelier significant and comparable
principle to the weak concentrations
acid or base equilibrium - contains a weak base and
- f- increase means its conjugate both in
shifts left, h3o+ significant and comparable
decrease concentrations
- result of common ion is
the suppression of the Buffer effectiveness
ionization of the weak - effectiveness refers to
acid or base buffers ability to resist ph
change when acid/base added
Ph of a buffer solution - related to relative
- remember: buffers are simply amounts of acid + its
solutions of weak acids/bases conj.
+ significant amount of their - buffer most effective
conjugate when amounts are
- can use ice table to solve, or comparable
Henderson hasselbalch - related to the absolute
equation amount of acid + conj.
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