1. The problem statement, all variables and given/known data A 0.551 L solution of 1.37 M sulfurous acid (Ka1 = 1.5e-2 and Ka2 = 1.0e-7) is titrated with 1.65 M NaOH. What will the pH of the solution be when 0.7549 L of the NaOH has been added? The answer is 7.27. 2. Relevant equations -log(H+)=pH pH = pKa + log(salt/acid) 3. The attempt at a solution I find the moles of the weak acid and strong base. After neutralization the strong base is left over. I find the concentration of the remaining moles of base. Then use -log(OH)=pOH. Then 14-pOH = pH. I keep getting 13.95. This is wrong, and I don't know how to get the right answer.