question_answer 1)

The ionization constant of dimethylamine is\[5.4\times {{10}^{-4}}\]. Calculate its degree of ionization in its 0.02 M solution. What percentage of dimethylamine is ionized if the solution is also 0.1 M\[NaOH\]?  

Answer:

Dimethylamine undergoes ionization in aqueous medium as:     association constant may be calculated as: \[{{K}_{b}}=\frac{[(C{{H}_{3}})NH_{2}^{+}][O{{H}^{-}}]}{[(C{{H}_{3}})NH]}=\frac{C\alpha \times C\alpha }{C-C\alpha }\,\,\,\,\,....(i)\] \[=\frac{C{{\alpha }^{2}}}{1-\alpha }\] \[(\because \,1