CH3NH2weak base → proton acceptor• H2O → will certainly 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 must identify if we have the right to remove (–x) from the equation. To perform so, we need to identify the proportion of the initial concentration and Kb:



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Problem Details

Solve an equilibrium trouble (using an ICE table) to calculate the pH of each solution:

a solution that is 0.225 M in CH3NH2 and also 0.120 M in CH3NH3Br

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