pH of the solution is 10.77.
pH is defined as the negative logarithm of [H+].
Hence, we can calculate the [H+] at equilibrium as follows:
Note that the [OH-] and [H+] of an aqueous solution at 25 0C are related as
Hence, we can calculate the OH- concentration at equilibrium as follows:
Now, we can write the equilibrium reaction of weak base with water as follows:
Given that the initial concentration of B is 0.15 M, we can create the ICE table for the above equilibrium as follows:
Initial, M | 0.15 | 0 | 0 |
Change, M | -x | +x | +x |
Equilibrium, M | 0.15-x | x | x |
Now, we already know the value of x in the ICE table from the pH data as
x = [OH-]=
Hence, we can calculate the base equilibrium constant Kb as follows:
Hence, the Kb of the base is about . (Rounded to three significant figures).
Be sure to answer all parts. Determine the K, of a weak base if a 0.15...
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