- #1
r3dxP
This question appeared on 1986 AP Exam.
1) In water, hydrazoic acid, HN3, is a weak acid that has an equilibrium constant, Ka, equal to 2.8E-5 at 25 degree C. A .300L sample of a .050molar solution of the acid is prepared.
Now.. there is a part d) to this question...
d) To the remaining .150 liter of the original soln, .075L of .100molar NaOH soln is added. Calculate the [OH-] for the resulting solution at 25 degree C.
If you have any clue on how to do this, any help would be greatly appreciated. Thanks.
1) In water, hydrazoic acid, HN3, is a weak acid that has an equilibrium constant, Ka, equal to 2.8E-5 at 25 degree C. A .300L sample of a .050molar solution of the acid is prepared.
Now.. there is a part d) to this question...
d) To the remaining .150 liter of the original soln, .075L of .100molar NaOH soln is added. Calculate the [OH-] for the resulting solution at 25 degree C.
If you have any clue on how to do this, any help would be greatly appreciated. Thanks.