1. The problem statement, all variables and given/known data 100.0 ml of 0.100 M acetic acid is placed in a flask and is titrated with 0.100 M sodium hydroxide . An appropriate indicator is used. Ka for acetic acid is 1.7 x 10 -5Calculate the pH in the flask at the following points in the titration. a. when no NaOH has been added. b. after 25.0 ml of NaOH is added c. after 50.0 ml of NaOH is added d. after 75.0 ml of NaOH is added e. after 100.0 ml of NaOH is added 2. Relevant equations n/a 3. The attempt at a solution Here is what I have so far. To calculate "a" I think I can use the equation ka=[CH3COON]/[CH3COOH][NaOH] (which uses CH3COOH +NaOH -> CH3COON + H20) and use a table to figure out the equilibrium values. Then plug those values into the formula to get the values of the acid, then figure the pH from there. The part I am not sure on (well two parts) is do I have the equation right, I don't think I do since there isn't an H+ to calculate. The second thing is...how do I factor those different volumes in? And I am sure the 100mL in the beginning matters, but I can't remember how to factor those in.