We are being asked to calculate the pOH of a 0.175 M aqueous solution of NX3.
NX3 has a low Kb, 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:
• NX3 → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: NX3(aq) + H2O(l) ⇌ NX3H+(aq) + OH-(aq)
If Kb for NX3 is 4.5×10−6, what is the pOH of a 0.175 M aqueous solution of NX3?
Express your answer numerically.
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