pH = 2.98
or
-log [H+] = 2.98
or
[H+] = 1.047 * 10^-3 M
thus
[CH3COO-] = 1.047 * 10^-3 M
let concentration of acid = x M
thus
Ka = [H+][CH3COO-] / [CH3COOH]
or
1.8 x 10^-5 = 1.047 * 10^-3 * 1.047 * 10^-3 / (x - 1.047 * 10^-3)
or
x = 0.062 M
thus concentration of acid = 0.062 M
An acetic acid solution (Ka= 1.8x10^-5) with an unknown concentration has a pH of 2.98 what...
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