Asked by Jessica
An aqueous solution of a monoprotic acid is prepared. This acid is known to have a pKa of 8.6. If the acid is 37.5% ionized when in solution, what is the pH of the solution?
Not really sure where to start with this question? Thanks in advance
Answers
Answered by
DrBob222
pKa = -log Ka. Solve for Ka.
Then..........HA ==> H^+ + A^-
I.............1.......0.....0
C...........-.375...0.375..0.375
E...........0.625...0.375..0.375
Substitute the E line into the Henderson-Hasselback equation and solve for pH.
Then..........HA ==> H^+ + A^-
I.............1.......0.....0
C...........-.375...0.375..0.375
E...........0.625...0.375..0.375
Substitute the E line into the Henderson-Hasselback equation and solve for pH.
Answered by
Anonymous
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It is the University's task to encourage ethical scholarship and to inform students and staff about the institutional standards of academic behaviour expected of them in learning, teaching and research. Students have a responsibility to maintain the highest standards of academic integrity in their work. Students must not cheat in examinations or other forms of assessment.
It is the University's task to encourage ethical scholarship and to inform students and staff about the institutional standards of academic behaviour expected of them in learning, teaching and research. Students have a responsibility to maintain the highest standards of academic integrity in their work. Students must not cheat in examinations or other forms of assessment.
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