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

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