We are being asked to calculate the percent ionization of a 0.325 M aqueous solution of NX3.
Recall that the percent ionization is given by:
We know the initial concentration of NX3, 0.325 M. We just need to find the concentration of OH- at equilibrium.
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 percent ionization of a 0.325 M aqueous solution of NX3?
Express your answer numerically to three significant figures.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
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.