The curve in the figure shows the variation of pH during the course of titration of a weak acid,

step 1 So in this question, we're dealing with a reaction of a base plus H -plus, the hydronium ion in

The curve in the figure shows the variation of pH during the...

The curve in the figure shows the variation of $\mathrm{pH}$ during the course of titration of a weak acid, HA with a strong base $(\mathrm{NaOH})$. At which point in the titration curve is the concentration of the acid equal to that of its conjugate base? (a) Point D (b) Point $\mathrm{E}$ (c) Point C (d) Point $\mathrm{B}$

The curve in the figure shows the variation of $\mathrm{pH}$ during the course of titration of a weak acid, HA with a strong base $(\mathrm{NaOH})$. At which point in the titration curve is the concentration of the acid equal to that of its conjugate base?
(a) Point D
(b) Point $\mathrm{E}$
(c) Point C
(d) Point $\mathrm{B}$

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Key Concepts

Half-Equivalence Point

The half-equivalence point is the phase in a titration where half of the weak acid has been converted to its conjugate base, resulting in equal concentrations of the acid and its conjugate base. This point is significant because the pH at this stage equals the pKa of the weak acid.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a relationship between the pH of a solution, the pKa of the weak acid, and the ratio of the concentrations of the conjugate base and the conjugate acid. It is especially useful at the half-equivalence point, where this ratio becomes 1, simplifying the equation so that pH equals pKa.

Titration Curve

A titration curve graphically represents the change in pH of a solution as a titrant is added. In the context of a weak acid titration with a strong base, the curve typically shows a gradual increase in pH at first, a buffering region, a sharp rise near the equivalence point, and often a leveling off after the equivalence point.

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