Acetic acid,(CH_3COOH),has a pK_a of 4.8. Eth | vedclass

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(D) According to the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[A^-]}{[HA]}$.If $pH > pK_a$,the concentration of the conjugate base $[A^

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$CH_3CO_2^{-}$ and $CH_3CH_2OH$

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(D) According to the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[A^-]}{[HA]}$.If $pH > pK_a$,the concentration of the conjugate base $[A^-]$ is greater than the concentration of the acid $[HA]$.If $pH For acetic acid $(CH_3COOH)$ with $pK_a = 4.8$ at $pH = 7.0$:Since $7.0 > 4.8$,the conjugate base $CH_3COO^{-}$ is the major species.For ethanol $(CH_3CH_2OH)$ with $pK_a = 16.0$ at $pH = 7.0$:Since $7.0 Therefore,the major species present are $CH_3COO^{-}$ and $CH_3CH_2OH$.

Acetic acid,$(CH_3COOH)$,has a $pK_a$ of $4.8$. Ethanol,$(CH_3CH_2OH)$,has a $pK_a$ of $16.0$. What are the major species present when acetic acid and ethanol are added to water and the $pH$ is adjusted to $7.0$?

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