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 .

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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 .