Find the pH of a buffer that consists of 1.3 M sodium phenolate (C6 H5 ONa) and 1.2 M phenol (C6

step 1 Let's look at a buffer that contains 1 .2 molar phenol and 1 .3 molar phenolate. If you have som

Find the pH of a buffer that consists of 1.3 M sodium...

Find the $\mathrm{pH}$ of a buffer that consists of 1.3 $\mathrm{M}$ sodium phenolate $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{ONa}\right)$ and 1.2 $\mathrm{M}$ phenol $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\left(\mathrm{p} K_{\mathrm{a}} \text { of phenol }=\right.$ 10.00$)$

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Key Concepts

pKa

pKa is the negative logarithm of the acid dissociation constant (Ka) and provides a measure of the strength of an acid in solution. It indicates the pH at which the acid is half dissociated, and is used in the Henderson-Hasselbalch equation to relate the concentrations of the acid and its conjugate base to the pH of the buffer.

Acid-Base Equilibrium

Acid-base equilibrium refers to the dynamic balance between the formation of ions in solution when an acid donates a proton and when a base accepts a proton. In buffer systems, this equilibrium between the weak acid and its conjugate base helps to maintain a stable pH by shifting in response to added acids or bases.

Buffer Solutions

Buffer solutions are mixtures of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resist changes in pH when small amounts of acid or base are added. They work by the weak acid neutralizing added bases while the conjugate base neutralizes added acids, maintaining a relatively constant pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a practical formula 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 is essential in calculating the pH of buffer systems.

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