Problem: What is the pH of a 0.25 M solution of C 6H 5NH 2 given that its Kb is 1.8 x 10-6? a. 3.17b. 10.83c. 2.67d. 11.32

FREE Expert Solution

We are being asked to calculate the pH of a 0.25 M solution of C6H5NH2


C6H5NH2 has a low Kb, 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:

C6H5NH2weak baseproton acceptor
H2O → will act as the weak acidproton donor


Equilibrium reaction:        C6H5NH2(aq) + H2O(l)  C6H5NH3+(aq) + OH-(aq)

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Problem Details

What is the pH of a 0.25 M solution of C 6H 5NH 2 given that its Kb is 1.8 x 10-6

a. 3.17
b. 10.83
c. 2.67
d. 11.32

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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.