Problem: Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook).0.401 M .

FREE Expert Solution

We’re being asked to calculate the percent ionization of a 0.401 M aqueous solution of hydrazoic acid (HN3).


Recall that the percent ionization is given by:


% ionization=[H+][HA]initial×100


We know the initial concentration of hydrazoic acid (HN3), 0.401 M. We just need to find the concentration of H+ at equilibrium.


Since hydrazoic acid (HN3) has a low Ka value, it’s a weak acid. 

Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). 


The dissociation of HA is as follows:

HN3(aq) + H2O(l)  H3O+(aq) + N3-(aq); Ka = 1.9 × 10–5 

Ka was found in books or the internet.


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Problem Details

Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook).

0.401 M .

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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 Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Halihan's class at OKSTATE.