Consider a weak acid $\ce$ = pH, the concentrations of protonated and deprotonated species (conjugate acid and base) will be almost equal (exactly equal for ideal solutions). Here, as an example, we have selected acetic acid (CH3COOH) as the weak acid and it is titrated against a strong base NaOH. This module describes the derivation of these two values and describes why the value of 15.7 should not be used. In many organic chemistry textbooks and some biochemistry texts, however, the pKa of water at 25✬ is listed as 15.7. $$\mathrm pK_\mathrm a = -\log K_\mathrm a$$Īcid dissociation constant is the equilibrium constant of the dissociation of ions of an acid in an aqueous solution. In most general chemistry textbooks, the pK a of water at 25 ✬ is listed as 14.0. $\mathrm pK_\mathrm a$ is negative log of the acid dissociation constant ( $K_\mathrm a$).
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