Asked by Amy
The Ka values of maleic acid, HOOCCHCHCOOH, are shown below.
Ka1 1.5 10-2
Ka2 2.6 10-7
A 50.0 mL sample of 0.11 M of maleic acid is titrated with 0.14 M NaOH. Calculate the pH at the following points in the titration curve.
find the first and second eq point pH
i thoguth i was doing it right but i cant get it
Ka1 1.5 10-2
Ka2 2.6 10-7
A 50.0 mL sample of 0.11 M of maleic acid is titrated with 0.14 M NaOH. Calculate the pH at the following points in the titration curve.
find the first and second eq point pH
i thoguth i was doing it right but i cant get it
Answers
Answered by
DrBob222
For the first equivalence point,
(H^+) = sqrt(k1k2)
For the second equivalence point, pH is determined by the hydrolysis of the salt, in this case Na2M
M^-2 + HOH ==> HM^- + OH^-
Write the Keq (Kb) expression, set up an ICE chart, solve for OH^-, convert to pOH, then to pH.
(H^+) = sqrt(k1k2)
For the second equivalence point, pH is determined by the hydrolysis of the salt, in this case Na2M
M^-2 + HOH ==> HM^- + OH^-
Write the Keq (Kb) expression, set up an ICE chart, solve for OH^-, convert to pOH, then to pH.
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.