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:
• C6H5NH2 → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: C6H5NH2(aq) + H2O(l) ⇌ C6H5NH3+(aq) + OH-(aq)
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?
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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.