Final answer:
The acid ionization constant (Ka) can be calculated using the equilibrium concentrations of the weak acid and its ions. In this case, the equilibrium mixture has [H3O+] = 0.027 M, [HSO4¯] = 0.29 M, and [SO4²- ] = 0.13 M. To find Ka, we use the equation Ka = [H3O+][A-] / [HA], where A- is the conjugate base of the acid.
Step-by-step explanation:
The acid ionization constant (Ka) can be calculated using the equilibrium concentrations of the weak acid and its ions. In the given equilibrium mixture, the concentration of H3O+ is 0.027 M. To find Ka, we use the equation Ka = [H3O+][A-] / [HA], where A- is the conjugate base of the acid. Since the equilibrium concentrations of HS04- and SO42- are given, we can assume that the acid HA is in the form of HSO4-. Therefore, the equilibrium concentration of [HA] is equal to the concentration of [HSO4-]. Substituting the values into the equation, we have Ka = (0.027 M)(0.13 M) / (0.29 M).