Problem: 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.

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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:

% ionization=[OH-][B]initial×100

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:

NX3weak baseproton acceptor
H2O → will act as the weak acidproton donor


Equilibrium reaction:       NX3(aq) + H2O(l)  NX3H+(aq) + OH-(aq)

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Problem Details

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.

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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.