Problem: The pH of 0.1 M C 4H9NH2(aq) (butylamine) aqueous solution was measured to be 12.04. What is the value of pKb of butylamine?1. 1.962. 2.933. 2.574. 0.255. 3.506. 2.87

FREE Expert Solution
FREE Expert Solution

We are being asked to calculate the pKb for a 0.1 M solution of C4H9NH2 (butylamine). 

C4H9NH2 (butylamine) is a neutral amine, therefore we know that it is a weak base.


We can calculate the pKb of butylamine from its Kb using the following equation:

pKb=-log Kb


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:

C4H9NH2weak baseproton acceptor
H2O → will act as the weak acidproton donor


Equilibrium reaction:        C4H9NH2(aq) + H2O(l)  C4H9NH3+(aq) + OH-(aq)

View Complete Written Solution
Problem Details

The pH of 0.1 M C 4H9NH2(aq) (butylamine) aqueous solution was measured to be 12.04. What is the value of pKb of butylamine?

1. 1.96

2. 2.93

3. 2.57

4. 0.25

5. 3.50

6. 2.87

Frequently Asked Questions

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 ofThe pH of 0.1 M C 4H9NH2(aq) (butylamine) aqueous solution w...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Jules took 4 minutes and 56 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

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