Consider the titration of50.0 mL of 0.217 M hydrazoic acid (HN3, Ka=2.6 x 10^-5) with 0.183M NaOH. The pH of the soluion before any NaOH is added is____ The answer is 2.62 I cant figure out what to do after you get the moles Solution Concentration of acid = 0.217M [H+] = sqrt (Ka* C) [H+] = 2.37 * 10 ^ -3 so pH = -log([H+]) = 2.624.