Histidine has three ionizable groups, with pKa values of 2.1, 6.0 and 9.5. A 1.0L solution of 0.5 M histidine has a pH of 2.1. To this solution, you add 0.5 moles of NaOH. What is the pH of this final solution?
Added by Michael R.
Step 1
At pH 2.1, the first ionizable group (pKa = 2.1) is half-ionized, meaning that 0.25 moles of H+ ions are present in the solution. Show more…
Show all steps
Your feedback will help us improve your experience
Madhur L and 82 other Chemistry 101 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
The precise pKa values for the amino acid Histidine are 1.8, 6.0, and 9.3. What is its isoelectric point (pH at which the charge on the molecule will be zero)? What is the final pH of a solution after 0.04 moles of hydrochloric acid are dissolved in 1 L of pure water? What is the final pH of a solution after 0.04 moles of hydrochloric acid are dissolved in a 1 L solution of 0.1 M MES buffer at pH 6.8 (MES Ka 8.13x 10^-7)?
Adi S.
Use the Henderson-Hasselbalch equation, pH = pKa + Log[base]/[acid], to determine what is the pH of a solution containing 0.70 M H3BO3 and 0.50 M NaH2BO3? (pKa = 9.14)? 8.99 9.29 9.85 8.43
Kyle L.
If histidine has a pKa of 6.0, what is the fraction protonated at pH 5.25 in a 233.7 mM solution of histidine of volume 305.2 mL? Report your answer as a decimal to the nearest 0.001 (so 95% would be entered as 0.950
David C.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD