Question
The conjugate acid of aniline has $\mathrm{p} K_{\mathrm{a}}=4.59 ;$ the conjugate acid of 3 -bromoaniline has $\mathrm{p} K_{\mathrm{a}}=3.58$. Which is the stronger base? Explain your answer.
Step 1
59 and the $\mathrm{p} K_{\mathrm{a}}$ of the conjugate acid of 3-bromoaniline is 3.58. We know that for a conjugate acid-base pair, $\mathrm{p} K_{\mathrm{a}} + \mathrm{p} K_{\mathrm{b}} = 14$. Show more…
Show all steps
Your feedback will help us improve your experience
Sima Sarker and 66 other Organic Chemistry 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
Aniline has a $\mathrm{p} K_{a}=4.63 ; 3$ -bromoaniline has a $\mathrm{pK}_{a}=$ 3.58; $\mathrm{p} K_{a}=-\log \left(\boldsymbol{K}_{a}\right)$. Which is the stronger base? Explain your answer.
The $p K_{\mathrm{a}}$ of the conjugate acid of guanidine is $13.6,$ making it one of the strongest neutral organic bases. Offer an explanation.
Write the equation relating $K_{\mathrm{a}}$ for a weak acid and $K_{\mathrm{b}}$ for its conjugate base. Use $\mathrm{NH}_{3}$ and its conjugate acid $\mathrm{NH}_{4}^{+}$ to derive the relationship between $K_{\mathrm{a}}$ and $K_{\mathrm{b}}$.
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD