• CH3NH2 → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: CH3NH2(aq) + H2O(l) ⇌ CH3NH3+(aq) + OH-(aq)
Solids and liquids are not included in the expression
Now, we need to determine if we can remove (–x) from the equation. To do so, we need to determine the ratio of the initial concentration and Kb:
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution:
a solution that is 0.225 M in CH3NH2 and 0.120 M in CH3NH3Br
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