Acid-Base Equilibria
Hey there. I am having trouble with this question.
Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations:
a) 0.250 M
b) 0.0800 M
c) 0.0200 M
** Ka = 1.3 x 10 ^ -5
Could you please show the work. And no power points please.
Thanks in advance!
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Solution Preview
Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations:
a) 0.250 M
b) 0.0800 M
c) 0.0200 M
** Ka = 1.3 x 10 ^ -5
a) 0.250 M
C2H5COOH ↔ H+ + C2H5COO-
Initial 0.25 --- ------
Change -x +x +x
Equilibrium 0.25-x x x
Ka = [H+][ C2H5COO-] / ...
Solution Summary
Acid base equilibria are examined. The percent ionization of propionic acid is calculated.
$2.19