The ph of 0.1 m c4h9nh2(aq) (butylamine) aqueous solution was measured to be 12.04. what is the value of pkb of butylamine

pkb =2.92

Explanation:

pH is defined as the negative logarithm of the concentration of hydrogen ions.

Thus,  

pH = - log [H⁺]

Given that:- pH = 12.04

Also, pH + pOH = 14  

So, pOH = 14 - 12.04 = 1.96

The expression of the pOH of the calculation of weak base is:-

Where, C is the concentration = 0.1 M

pkb = -log kb = = 2.92

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yes

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