Asked by anonymous
In a .25 M solution, a weak acid is 3.0% dissociated.
A. calculate the pH of the solution
B. calculate the Ka of the acid
Please explain steps.
A. calculate the pH of the solution
B. calculate the Ka of the acid
Please explain steps.
Answers
Answered by
DrBob222
..............HA ==>H^+ + A^-
initial....0.25M....0......0
change.......-x......x......x
equil......0.25-x....x.....x
If it is 3% dissociated, that means that x = 0.25*0.03 = ?
Substitute into the Ka expression and solve for Ka.
pH = -log(H^+)
initial....0.25M....0......0
change.......-x......x......x
equil......0.25-x....x.....x
If it is 3% dissociated, that means that x = 0.25*0.03 = ?
Substitute into the Ka expression and solve for Ka.
pH = -log(H^+)
Answered by
Kolubah
Please help me solved this problem
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