Asked by Anonymous

For a solution that is 0.168M NH3 and 0.106M NH4Cl calculate the following.
[OH-]
[NH4+]
[Cl-]
[H30+]
Answered by DrBob222
pH can be calculated from the Henderson-Hasselbalch equaion.

pOH from pH + pOH = pKw = 14

OH^- from pOH = -log(OH^-)
H3O^+ from pH = -log(H3O^+)
(Cl^-) = NH4Cl
Post your work if you get stuck.
Answered by Anonymous
Using the Henderson-Hasselbalch equation, should i write this:

pH= -log ka + log(0.168/0.106)
PH= -log(5.6*10^-10) + log(0.168/0.106)
PH=9.45
Answered by Anonymous
@DrBob222 .......Thanks. It worked.
Answered by DrBob222
Yes, and 9.45 is correct if Ka is correct. I didn't check that.
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