Asked by Nevaeh
A 25.0 mL sample of 0.125 M pyridine is titrated with 0.100 M HCl.
Calculate the pH at 0 mL of added acid.
Calculate the pH at 0 mL of added acid.
Answers
Answered by
DrBob222
Treat this as just another ammonia, NH3, problem. Remember, NH3 + HOH ==> NH4^+ + OH^- and you know how to solve those problems. This is the same thing.
See here for the structure.
https://en.wikipedia.org/wiki/Pyridine
Let's call pyridine a simple PN. Then
......PN + HOH ==> PNH^+ + OH^-
I.....0.1............0.......0
C.....-x.............x.......x
E....0.1-x...........x.......x
Kb pyr = (PNH^+)(OH-)/(PN)
Substitute the E line and solve for x = (OH^-), then convert to pH.
See here for the structure.
https://en.wikipedia.org/wiki/Pyridine
Let's call pyridine a simple PN. Then
......PN + HOH ==> PNH^+ + OH^-
I.....0.1............0.......0
C.....-x.............x.......x
E....0.1-x...........x.......x
Kb pyr = (PNH^+)(OH-)/(PN)
Substitute the E line and solve for x = (OH^-), then convert to pH.
Answered by
bea
hi I had a similar question too this on an assignment and when I calculated it my pOH was 4.89 and my pH was 9.11 which doesn't seem right and I don't know what I did wrong
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.