I'm working on a lab for my chem class and we have to calculate all of the different ion concentrations within some titrations that we did. Here I have to calculate the concentration before anything is added. Na+ + C2H3O2- + H2O → HC2H3O2 + OH- + Na+ the pH is 8.4458 for a 30.0 mL NaC2H3O2 solution. I tried finding the concentration of the Na+ and C2H3O2- ions by: 14.00 - 8.4458 = pOH = 5.55452 then 10-5.55452 = 2.79 X 10-6 which is the OH- concentration. In the Kb? equation this would be x so: 5.3 X 10-6 = (2.79 X 10-6)2/(x-(2.79 X 10-6). Calculating all this through I get 4.25 X 10-6. With the Liters being 30.0 mL I take this concentration and divide it by .0300 L and I get 1.42 X10-4. This just seems incorrect because the Molarity was supposed to be somewhere near 1.0M, what did I do wrong?