Question

please explain all steps if you can!! also how to use the degree of dissociation if possible.

5. In an aqueous solution of an acid (or a base), there is an equilibrium between the acid HA and the products of its dissociation can be described using a dissociation constant: Kg tration. The values of Ka for various acids are known. They show how far the dissociation goes and how strong the acid is. For strong acids, it can be of the order of 10° (molar concentrations are assumed in mol/L, and the units of K are dropped). In calculations, it is often convenient to use the degree of dissociation, a, which is a fraction of the acid molecules that have dissociated. For acetic acid, K = 1.8-105. Evaluate the concentration of hydrogen cations in its 0.010M aqueous solution. Do it rigorously using the degree of dissociation and then approximately assuming that in equilibrium, the concentration of H+and A: HA Ht +A. This equilibrium cHelA") where c is molar concen- CHA) 2 of 3 intact acetic acid molecules is very close to 0.010M. Comment on your findings.

Answer 1

& CH₂ coo +H+ CH₂ cool 0.01 OĎ ta + HV W -X (0.01-x) x x E = 1.8x10-5 (0.1-x) on solving, x=0.00133M = [H+] .L - 0.oolss x10o = 13.3%. gol