What is the ph of 0.11 m diethylamine, (ch3ch2)2nh, (kb = 8.6 × 10−4)?

Answer : The pH of the solution is, 11.97

Solution :  Given,

Concentration (c) = 0.11 M

Base dissociation constant =

The equilibrium reaction for dissociation of (weak base) is,

initially conc.         0.11                              0             0

At eqm.              (0.11-x)                            x             x 

First we have to calculate the value of 'x'.

Formula used :

Now put all the given values in this formula ,we get:

By solving the terms, we get

Thus, the concentration of hydroxide ion is:

Now we have to calculate the pOH.

Now we have to calculate the pH.

Therefore, the pH of the solution is, 11.97

increased stability in the completion of fluorine's outer shell.