[HY] = mol of HY / volume in L
= 4.57*10^-3 MOL / 0.085 L
= 0.05376 M
use:
pH = -log [H+]
2.25 = -log [H+]
[H+] = 5.623*10^-3 M
HY dissociates as:
HY -----> H+ + Y-
5.376*10^-2 0 0
5.376*10^-2-x x x
Ka = [H+][Y-]/[HY]
Ka = x*x/(c-x)
Ka = 5.623*10^-3*5.623*10^-3/(0.05376-5.623*10^-3)
Ka = 6.569*10^-4
Answer: 6.57*10^-4
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