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:
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:
• C4H9NH2 → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: C4H9NH2(aq) + H2O(l) ⇌ C4H9NH3+(aq) + OH-(aq)
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?
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