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Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution:?
a solution that is 0.195 molL−1 in CH3NH2 and 0.135 molL−1 in CH3NH3Br
Express your answer using two decimal places.
1 Answer
- hcbiochemLv 71 year ago
In this problem, you don't really need to use an ICE table, because the concentrations of the weak base and its conjugate acid are given to you. You do need the Kb for the weak base. I found this value online to be 4.4X10^-4.
Methylamine acts as a base by the equilibrium:
CH3NH2 + H2O <--> CH3NH3+ + OH-
Kb = [CH3NH3+][OH-]/[CH3NH2] = 4.4X10^-4
(0.135)[OH-]/(0.195) = 4.4X10^-4
[OH-] = 6.4X10^-4 M
pOH = 3.20
pH = 14.00 - pOH = 10.80
