Just treat it as you would 0.1M soln of NH3.
For the sake of typing let's call the basic form of HEPES, BH2. In water solution this will ionize as
............BH2 + HOH ==> BH3^+ + OH^-
initial....0.1M.............0......0
change......-x.............x.......x
equil......0.1-x............x.......x
Kb = (BH3^+)(OH^-)/(BNH2)
Substitute from the ICE chart above, solve for OH^- and convert to pH.
If you make up a solution of 100 mL of 0.1 M HEPES in the basic form, what will be the pH?
I have no idea where to even start...
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