If the kb of a weak base is 4.6 × 10-6, what is the ph of a 0.32 m solution of this base?

Assuming that the given base is a weak monoprotic base, the pH of the solution can be calculated as follows:

Write the balanced reaction and ice chart:

          BOH -->  OH- + B+

i           0.32        0         0
c            -x           x          x
e       0.32-x        x          x

Kb = x^2/ (0.32-x)
x = 1.21x10^-3 = [OH-]
pOH = -log[OH-] = -log[1.21x10^-3] = 2.917
pH = 14 - pOH = 14 - 2.917 = 11.08