In this experiment you will find the ionization constant for ammonia, a weak base.
I have completed the experiment, and have the following:
Initial concentration of NH3: 3.708mol/L
Initial pH of NH3: 10.26
NH3(aq) + H2O(l) <--> NH4+(aq) + OH-(aq)
pH = -log[H+]
Kb = [NH4+][OH-]/[NH3]
The Attempt at a Solution
I previously had no idea what to do, but now looking at the ICE table I have...
NH3 + H2O <--> NH4 + OH
I 3.708 - 0 0
C -x - +x +x
E 3.708-x x x
Correct me if I'm wrong, but...
Would the E value of NH3 not be 0?
And wouldn't the E values of NH4 and OH be 3.708?