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.
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
2 answers
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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.