Asked by Curtis
A buffer solution contains 0.283 M hypochlorous acid and 0.456 M potassium hypochlorite.
If 0.0464 moles of perchloric acid are added to 225 ml of this buffer, what is the pH of the resulting solution ?
(Assume that the volume change does not change upon adding perchloric acid)
pH =
If 0.0464 moles of perchloric acid are added to 225 ml of this buffer, what is the pH of the resulting solution ?
(Assume that the volume change does not change upon adding perchloric acid)
pH =
Answers
Answered by
DrBob222
millimols HOCl = mL x M = 225 x 0.283 = estimated 64.
mmols KOCl = 225 x 0.456 = 103
add 46 mmols HClO4.
..........OCl^- + H^+ ==> HOCl + H2O
I.........64......0........103
add..............46.............
C........-46....-46.........+46
E.........18......0........149
Substitute the E line into the Henderson-Hasselbalch equation and solve for pH. You will need to look up or calculate pKa for HOCl
Note that I have rounded on all of the numbers. You will need to recalculate and obtain more accurate numbers.
mmols KOCl = 225 x 0.456 = 103
add 46 mmols HClO4.
..........OCl^- + H^+ ==> HOCl + H2O
I.........64......0........103
add..............46.............
C........-46....-46.........+46
E.........18......0........149
Substitute the E line into the Henderson-Hasselbalch equation and solve for pH. You will need to look up or calculate pKa for HOCl
Note that I have rounded on all of the numbers. You will need to recalculate and obtain more accurate numbers.
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.