Question
What is $\mathrm{pH}$ of a liter buffer solution containing $0.4 \mathrm{M}$ benzoic acid and $0.045 M$ sodium benzoate? The $\mathrm{pK}_{\mathrm{a}}$ for benzoic acid equals 4.2 at $25^{\circ} \mathrm{C}$.
Step 1
Step 1: Write the equilibrium equation for the dissociation of benzoic acid: \[ \text{C}_6\text{H}_5\text{COOH} \rightleftharpoons \text{C}_6\text{H}_5\text{COO}^- + \text{H}^+ \] Show more…
Show all steps
Your feedback will help us improve your experience
David Collins and 54 other educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Calculate the $\mathrm{pH}$ of a buffer solution prepared by dissolving $21.46 \mathrm{~g}$ of benzoic acid $\left(\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}\right)$ and $37.68 \mathrm{~g}$ of sodium benzoate in $200.0 \mathrm{~mL}$ of solution.
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 $\mathrm{M}$ $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}\left(K_{\mathrm{a}} \text { of benzoic acid }=6.3 \times 10^{-5}\right) ?$
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$)$
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD