Problem: A 0.100 M solution of ethylamine (C 2H5NH2) has a pH of 11.87. Calculate the K b for ethylamine.

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We are being asked to calculate the Kb for a 0.100 M solution of ethylamine (C2H5NH2)

Ethylamine (C2H5NH2) is a neutral amine, therefore we know that it is a weak base.


Since we’re dealing with a weak base and Kb is an equilibrium expression, we will have to create an ICE chart to determine the equilibrium concentration of each species:

C2H5NH2weak baseproton acceptor
H2O → will act as the weak acidproton donor


Equilibrium reaction:        C2H5NH2(aq) + H2O(l)  C2H5NH3+(aq) + OH-(aq)

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Problem Details

A 0.100 M solution of ethylamine (C 2H5NH2) has a pH of 11.87. Calculate the K b for ethylamine.

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