What is the pH of a buffer solution containing 0.095 M acetic acid and 0.6 M sodium acetate? The

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 buffer solution containing 0.095 M...

What is the $\mathrm{pH}$ of a buffer solution containing $0.095 \mathrm{M}$ acetic acid and $0.6 \mathrm{M}$ sodium acetate? The dissociation constant of acetic acid is $1.75 \times$ $10^{-5}$ at $25^{\circ} \mathrm{C}$.

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Key Concepts

Acid Dissociation Constant (Ka) and pKa

The acid dissociation constant, Ka, is a quantitative measure of the strength of a weak acid in solution. It represents the equilibrium constant for the dissociation of the acid into its conjugate base and hydrogen ion. The pKa, defined as the negative logarithm of Ka, provides a more convenient scale for comparing acid strengths. Lower pKa values indicate stronger acids, while higher pKa values indicate weaker acids.

Buffer Solutions

A buffer solution is a system that resists changes in pH when small amounts of acids or bases are added. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. Buffers work by the equilibrium established between the acid and its conjugate base, which reacts with added acids or bases to minimize pH changes.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a formula used to estimate the pH of a buffer solution. It relates the pH to the pKa of the acid and the ratio of the concentrations of the conjugate base to the acid. This equation simplifies the calculation of pH in buffer systems by incorporating the logarithmic relationship between acid dissociation and concentration ratios.

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