What is the pH of a liter buffer solution containing 0.6 M sodium acetate and 0.15 M acetic acid

step 1 On 12 .79, we want to find the pH of the buffer solution with 0 .15 molar chloroacetic acid and

What is the pH of a liter buffer solution containing 0.6 M...

What is the $\mathrm{pH}$ of a liter buffer solution containing $0.6 \mathrm{M}$ sodium acetate and $0.15 \mathrm{M}$ acetic acid? The $\mathrm{pk}_{\mathrm{a}}$ for acetic acid equals 4.76 at $25^{\circ} \mathrm{C}$.

Key Concepts

Buffer Solution

A buffer solution is a mixture 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. The ability to maintain a nearly constant pH makes buffer solutions essential in many chemical and biological applications.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is an approximation used to estimate the pH of a buffer solution. It relates the pH to the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the acid. This equation simplifies the process of calculating the pH by converting the acid-base equilibrium into a logarithmic relationship.

Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two species that transform into each other by the gain or loss of a proton. In a buffer solution, the weak acid and its conjugate base work together to neutralize added acids or bases, maintaining the pH of the system. Recognizing these pairs is key to understanding how buffers function and are calculated using the Henderson-Hasselbalch equation.

Acid Dissociation Constant (pKa)

The acid dissociation constant, represented as pKa when expressed in its logarithmic form, quantifies the strength of a weak acid by indicating the pH at which half of the acid is deprotonated. A lower pKa value corresponds to a stronger acid, while a higher pKa indicates a weaker acid. This concept is fundamental in understanding the behavior of weak acids in buffer solutions.

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