What are the [H3 O^+] and the pH of a benzoic acid-benzoate buffer that consists of 0.33M C6 H5

step 1 Here we have the concentration of the acid and the concentration of the base. And I've written d

What are the [H3 O^+] and the pH of a benzoic acid-benzoate...

What are the $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ and the $\mathrm{pH}$ of a benzoic acid-benzoate buffer that consists of 0.33$M \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}$ and 0.28 $\mathrm{M}$ $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}\left(K_{\mathrm{a}} \text { of benzoic acid }=6.3 \times 10^{-5}\right) ?$

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Key Concepts

Buffer Solutions

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, and works by neutralizing added acids or bases via equilibrium processes.

Acid Dissociation Constant (Ka) and pKa

The acid dissociation constant (Ka) measures the strength of a weak acid in solution, quantifying its tendency to donate protons. pKa, the negative logarithm of Ka, is commonly used because it conveniently represents the acid's strength on a logarithmic scale, with lower pKa indicating a stronger acid.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a straightforward way to calculate the pH of a buffer solution by relating the pH to the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the acid. This formula, pH = pKa + log([base]/[acid]), is fundamental when designing and analyzing buffer systems.

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