Why does the OH react with HA and not H3O+?

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In titrating a weak acid (HA) with a strong base, hydroxide ions (OH-) preferentially react with HA rather than hydronium ions (H3O+) for neutralization. This occurs because HA donates protons to water, forming H3O+, but the presence of hydroxide allows for the deprotonation of remaining HA molecules. The reaction of OH- with HA leads to effective neutralization of the weak acid. Hydroxide can deprotonate both weak acids and hydronium ions, but it favors the reaction with HA in this context. Understanding this preference is key to grasping acid-base titration dynamics.
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In titrating HA, the weak acid with a strong base, why does the OH- ions from the strong base react with the HA atom (and neutralize it) rather than say react with the H3O+ to form complete neutralization? Just curious. Thanks.
 
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HA donates protons to water regardless of whether the base is present or not however the hydroxide can neutralize the remaining HA molecules. Ultimately hydroxide is going to prefer the latter over the former.
 
motornoob101 said:
In titrating HA, the weak acid with a strong base, why does the OH- ions from the strong base react with the HA atom (and neutralize it) rather than say react with the H3O+ to form complete neutralization? Just curious.
Thanks.

Hydroxide deprotonates weak acids and hydronium ion alike. In a basic solution, hydroxide abstracts acidic protons from both molecules.
 

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