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:
• C2H5NH2 → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: C2H5NH2(aq) + H2O(l) ⇌ C2H5NH3+(aq) + OH-(aq)
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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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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