Asked by Jematormal91
Calculate the pH when 39.0mL of 0.321 of HA is mixed with 39.0mL of 0.321M NaOH where
HA is a monoprotic weak acid with Ka= 7.5x10^-5 M ?
HA is a monoprotic weak acid with Ka= 7.5x10^-5 M ?
Answers
Answered by
DrBob222
The pH is determined by the hydrolysis of the salt.
..........A^- + HOH ==> HA + OH^-
initial..0.160M..........0.....0
change...-x...............x.....x
equil...0.160-x...........x.....x
Kb for A^- = (Kw/Ka for HA) = (x)(x)/(0.160-x
Solve for x = (OH^-)and convert to pH.
..........A^- + HOH ==> HA + OH^-
initial..0.160M..........0.....0
change...-x...............x.....x
equil...0.160-x...........x.....x
Kb for A^- = (Kw/Ka for HA) = (x)(x)/(0.160-x
Solve for x = (OH^-)and convert 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.