Asked by Alex
If the Kb of a weak base is 2.6 × 10-6, what is the pH of a 0.24 M solution of this base?
Answers
Answered by
DrBob222
Call the weak base ANH2
........ANH2 + HOH ==> ANH3^+ + OH^-
I.......0.24.............0........0
C.........-x.............x........x
E......0.24-x............x.........x
Kb = (ANH3^+()(OH^-)/(ANH2)
Substitute from the ICE chart and solve for x = (OH^-) and convert to pH.
........ANH2 + HOH ==> ANH3^+ + OH^-
I.......0.24.............0........0
C.........-x.............x........x
E......0.24-x............x.........x
Kb = (ANH3^+()(OH^-)/(ANH2)
Substitute from the ICE chart and solve for x = (OH^-) and convert to pH.
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