The weak acid HA is 4 % ionized (dissociated) in a 0.10 M solution.
a)What is Ka for this acid?
b) What is the pH of this solution?
concentration = 0.10 M
% ionization = 4 %
a)
% ionization = ([H+] / C ) x 100
4 = ([H+] / 0.10) x 100
[H+] = 4.0 x 10^-3 M
[H+] = sqrt (Ka x C)
4.0 x 10^-3 = sqrt (Ka x 0.10)
Ka = 1.6 x 10^-4
b)
pH = -log [H+]
= -log (4 x 10^-3)
pH = 2.40
The weak acid HA is 4 % ionized (dissociated) in a 0.10 M solution. a)What is...