Anhydrous hydrogen fluoride, HF, has a liquid range from 190 to 292.5 K and, similar to water, it autoionizes with an autoionization constant of ≈ 2 ×10–12.
(a) (3 pts) Write the balanced chemical equilibrium that describes the autoionization of HF(l) using the Brønsted-Lowry perspective. On each side of the chemical equilibrium, identify the (conjugate) acid and the (conjugate) bases.
(b) (1 pt) Write the mass-action expression for the autoionization of HF(l).
(c) (3 pts) Given the autoionization constant, identify the concentration conditions that would make acidic, neutral, and basic solutions of HF(l).
(a) Autoionization of HF:
HF + H2O F- + H3O+
Acid Base Conjugate acid Conjugate base
(b) Mass action expression:
Kc = [F-][H3O+] / [HF]
(c) Autoionization constant:
K = [F-][H3O+]
Acidic : [F-] < [H3O+]
Basic : [F-] > [H3O+]
Neutral : [F-] = [H3O+]
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