Henderson-Hasselbalch Equation

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on

Jul 24, 2020, 6:28:07 PM

Created by

on

Jun 6, 2014, 8:23:50 PM

`pH = pK' + log( A^- /( HA ))`

`"Acid Dissociation Constant"`

`"Conjugate Base"`

`"Weak Acid"`

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Describes the relationship between pH and the extent of dissociation of a weak acid. When the pH of the solution of a weak acid is equal to the pK' of the acid, then 50% of the acid is in the undissociated form, HA, and 50% is in the dissociated form, H⁺ + A^-.

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