AP Chemistry 8.7 A Explain the Relationship Between the Predominant Form of a Weak Acid or Base in Solution At a Given Ph and the Questions

For the correct answer and a valid justification, consistent with part (e):
Accept one of the following:
- The conjugate base, $\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{O}_{3}{ }^{-}$. When pH=4, the titration is beyond the half-
equivalence point, where $\left[\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{3}\right]=\left[\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{O}_{3}{ }^{-}\right]$. Thus, $\left[\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{O}_{3}{ }^{-}\right]$must be
greater than $\left[\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{3}\right]$.
- The conjugate base, $\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{O}_{3}{ }^{-}$. Because the pH of the solution is greater than the
$\mathrm{p} K_{a}$ of the acid, the majority of the molecules will be deprotonated.

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