A chemist titrates 20.0 mL of 0.2000 M HBrO (Ka=2.3x10-9) with 0.1000 M NaOH. What is the pH when [HBrO]=[BrO-]? After solving the ice table, I was getting x=2.1446x10^-5 but wasn't sure if that was correct. If so, would I go ahead and -log(x) to get my pOH and then solve 'for pH?