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Homework Statement
1. What volume of .022M HCl must be added to the 110ml buffer solution to completely react with the ammonia (NH3) to reach equivalence. Then, what is the pH of this at the equivalence point.
Buffer solution (equilibrium): NH3 + H20 ⇌ NH4+ + OH-
Other Info: .045M NH4+ and .024M NH3
and the pH of the buffer is 8.99
Kb NH3 = 1.8 x 10-5 Not sure if this is needed though.
Homework Equations
Molarity = n(moles)/V(volume in L)
pH = -log[H+]
Brackets means the concentration of the substance on the inside.
Not sure what else, I am sure there's some stoichiometry involved.
The Attempt at a Solution
I'm having a lot of trouble with this one.