We are being asked to calculate the pH for a 0.30 M solution of C6H5NH2.
C6H5NH2 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:
• C6H5NH2 → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: C6H5NH2(aq) + H2O(l) ⇌ C6H5NH3+(aq)(aq) + OH-(aq)
Calculate the pH of a 0.30 M solution of aniline(C6H5NH2 , Kb = 3.8 x 10-10.)
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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.
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Based on our data, we think this problem is relevant for Professor Czader's class at UH.