I'm trying to figure out how to determine molarity through titration. So we started with about 250mL of 0.1 M NaOH solution. Then we needed to determine how much KHP would be required to neutralize only 25mL of the 0.1 M NaOH solution, which came out to about 0.51g. Then we used 50mL of NaOH solution and dripped it through a drip counter into a solution of KHP (which also had a pH electrode). It turns out that during the several runs, we had an average of about 24.5mL before the solution became neutral, which tells me (off the top of my head) that the actual molarity of the supposed 0.1 M NaOH is actually less... What I can't seem to figure out is how to tell what the actual molarity is. I also need to provide a standard deviation, which I know how to do... it's just getting the average molarity that's boggling the bajesus outa me. Can anyone provide some help per change? This is probably a pretty basic routine for people who aren't knuckleheads at this stuff like myself.