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The textbook provides an example of a weak acid as acetic acid, on pg. F75. After providing a chemical equation for the Acid-Base reaction, the textbook claims that "only a small fraction of its molecules undergo deprotonation". Why does only a small fraction of acetic acid undergo deprotonation? How does this tell us whether it is a weak or strong acid?
I believe that the deprotonation has to do with the ability of weak/strong acids to dissociate. Weak acids, such as acetic acids, are known to not dissociate completely while strong acids can dissociate fully in water/aqueous solutions. This means that strong acids can ionize and release a lot of protons (aka deprotonate) while weak acids will release lesser amounts of protons (H+).
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