We’re being asked to calculate the pH of a 0.015 M aqueous solution of hydrazoic acid, HN3.
Since 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 HN3 is as follows:
HN3(aq) + H2O(l)⇌ H3O+(aq) + N3–(aq); Ka = 1.9 × 10–5
What is the pH of a 0.015 M aqueous solution of hydrazoic acid (HN 3)
(Ka = 1.9 x 10–5) at 25°C?
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