Asked by Brian
Calculate the pH of a solution that results from the mixture of 50.0 mL of 0.15 M HCOOH with 75.0 mL of 0.13 M HCOONa. Now, don't forget these solutions are being mixed and you haven't accounted for that yet in the concentrations! Ka for HCOOH is 1.8 x 10-4.
Answers
Answered by
DrBob222
moles HCOOH = M x L = ?
moles HCOONa = M x L = ?
(HCOOH) = moles/total volume.
(HCOONa) = moles/total volume.
Ka = (H^+)(HCOO^-)/(HCOOH)
Solve for (H^+).
(HCOO^-) from above.
(HCOOH) from above.
Convert (H^+) to pH.
This is a buffered solution and you can use the Henderson-Hasselbalch equation if you wish. It is a little simpler because you may use moles/V and not actually determine the concns of each (since the volume cancels).
moles HCOONa = M x L = ?
(HCOOH) = moles/total volume.
(HCOONa) = moles/total volume.
Ka = (H^+)(HCOO^-)/(HCOOH)
Solve for (H^+).
(HCOO^-) from above.
(HCOOH) from above.
Convert (H^+) to pH.
This is a buffered solution and you can use the Henderson-Hasselbalch equation if you wish. It is a little simpler because you may use moles/V and not actually determine the concns of each (since the volume cancels).
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.