Henderson-Hasselbalch Equation

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

$"Acid Dissociation Constant"$

$"Conjugate Base"$

$"Weak Acid"$

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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^-.

Notes

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