Asked by Margaret
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25°C.)
(a) pH = 4.70
(b) pH = 5.26
(c) pH = 5.42
(d) pH = 4.96
(a) pH = 4.70
(b) pH = 5.26
(c) pH = 5.42
(d) pH = 4.96
Answers
Answered by
TK
pKb = 8.77
use the Handerson-Hasselbalch equation
pOH = pKb + log [C5H5NH+]/ [C5H5N]
1
pOH = 14 - 4.50= 9.50
9.50 - 8.77=0.73
10^0.73 = 5.4 = [C5H5NH+]/ [C5H5N]
[C5H5N]/ [C5H5NH+]= 1 / 5.4=0.19
use the Handerson-Hasselbalch equation
pOH = pKb + log [C5H5NH+]/ [C5H5N]
1
pOH = 14 - 4.50= 9.50
9.50 - 8.77=0.73
10^0.73 = 5.4 = [C5H5NH+]/ [C5H5N]
[C5H5N]/ [C5H5NH+]= 1 / 5.4=0.19
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.