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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FREE Expert Solution

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.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofA 0.100 M solution of ethylamine (C 2H5NH2) has a pH of 11.8...as medium difficulty.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Martucci's class at UNM.