An aqueous solution of 0.057 M weak acid, HX, has a pH of...

An aqueous solution of $0.057 M$ weak acid, HX, has a pH of $4.65 .$ What is the $\mathrm{pH}$ of the solution if $0.018 \mathrm{~mol}$ of $\mathrm{KX}$ is dissolved in one liter of the weak acid?

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Key Concepts

Acid Dissociation Constant (Ka) and pKa

This concept relates to how a weak acid partially dissociates in solution to produce H+ and its conjugate base. The equilibrium constant for this dissociation (Ka) gives a measure of the acid's strength, and its negative logarithm (pKa) provides a more convenient way to compare acid strengths. Determining pKa from a known pH and concentration is essential for predicting and understanding the behavior of weak acids in various environments.

Buffer Solutions and the Henderson–Hasselbalch Equation

A buffer solution is made up of a weak acid and its conjugate base and is designed to resist substantial pH changes when small amounts of acid or base are added. The Henderson–Hasselbalch equation, which relates pH to pKa and the ratio of the concentrations of the base to the acid, is a key tool in calculating the pH of such buffer systems. This concept is fundamental in chemical equilibria and is widely applied in both laboratory and real-world scenarios to maintain a desired pH.

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