To determine the pH and pOH of a solution of 0.30 M HCl that is 88% ionized, we can use the ionization constant of HCl, which is assumed to be 100% in this case.
Since HCl is a strong acid, it completely dissociates into H+ and Cl- ions. Thus, the concentration of H+ ions in the solution is the same as the concentration of the HCl solution, which is 0.30 M.
pH is defined as the negative logarithm (base 10) of the concentration of H+ ions in a solution. Therefore, the pH of the HCl solution is:
pH = -log[H+] = -log(0.30) ≈ 0.52
Now, since pH + pOH = 14 (at 25 degrees Celsius), we can calculate the pOH:
pOH = 14 - pH = 14 - 0.52 ≈ 13.48
Therefore, the pH of the 0.30 M HCl solution is approximately 0.52, and the pOH is approximately 13.48.