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