N the laboratory, a general chemistry student measured the pH of a 0.342 M aqueous solution of ethylamine, C2H5NH2 to be 12.067. Use the information she obtained to determine the Kb for this base.

The value of of the an ethylamine is .

Explanation:

The pH of the solution = 12.067

The pOH of the solution = 14 - pH =14-12.607 =1.933

Initially

0.342 M                              0     0

At equilibrium

(0.342-x)                             x      x

The value of x =

The expression of is given as:

The value of of the an ethylamine is .

b) mutualism

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