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AP Chemistry
8.7 pH and pKa
8.5 Acid-Base Titrations
8.3 Weak Acid and Base Equilibria
IntermediateMCQGraphicalConceptual13.6k
A 2D line graph plotted on a Cartesian coordinate system with light gray gridlines. The horizontal x-axis is labeled 'Volume of 0.10 M NaOH added (mL)' and ranges from 0 to 40 with major tick marks labeled every 5 units: 0, 5, 10, 15, 20, 25, 30, 35, 40. The vertical y-axis is labeled 'pH' and ranges from 0 to 14 with major tick marks labeled every 2 units: 0, 2, 4, 6, 8, 10, 12, 14. A single solid black curve begins at (0, 3.0), rises gradually through the buffer region passing directly through the half-equivalence point at coordinate (12.5, 4.8), exhibits a steep vertical inflection centered at coordinate (25.0, 8.8) where the curve rises sharply from pH 6.5 to 11.0, and levels off asymptotically toward pH 12.5 at 40 mL. No other curves, points, labels, or annotations appear.
Titration curve for the titration of \(25.0\text{ mL}\) of \(\text{HA}\) with \(0.10\text{ M NaOH}\).
A student titrates a \(25.0\text{ mL}\) sample of an unknown weak monoprotic acid, \(\text{HA}\), with a \(0.10\text{ M}\) solution of \(\text{NaOH}\) at \(25\,^{\circ}\text{C}\). The resulting titration curve is shown below.

Based on the titration curve, which of the following correctly identifies the \(\text{p}K_a\) of \(\text{HA}\) and provides the correct chemical justification for why the \(\text{pH}\) at the equivalence point is greater than \(7.0\)?

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