A solution with a pH of 8.73 is prepared by adding water to...

A solution with a pH of 8.73 is prepared by adding water to 0.614 mol of NaX to make $2.50 \mathrm{~L}$ of solution. What is the $\mathrm{pH}$ of the solution after 0.219 mol of $\mathrm{HX}$ is added?

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Key Concepts

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a way to relate the pH of a buffer solution to the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the weak acid. This equation is a crucial tool for calculating the pH of buffer solutions after changes in their composition, such as the addition of a known amount of acid or base.

Acid-Base Stoichiometry

Acid-base stoichiometry involves calculating the moles of acid and base present in a solution and understanding how their reaction alters the concentrations of the species that make up a buffer. When an acid is added to a solution containing the conjugate base, it reacts in a 1:1 ratio, changing the composition of the buffer system. This concept is essential for predicting the resulting pH after such an addition.

Buffer Solutions

A buffer solution is a system that resists changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. These components are in equilibrium with each other, allowing the system to neutralize added acids or bases without a significant shift in pH.

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