Question

What is the pH of a 0.24 M diethylamine solution? Kb = 8.6 x 10^-4

Answer 1

Explanation:

$poh = \frac{1}{2} \times pkb - \frac{1}{2} log(c)$

$pkb = - log(kb)$

pkb = 3.066

C is concentration which is 0.24M

Substituting the values the pOH is

1.84.

pH +pOH = 14

pH = 14-1.84

pH= 12.16