100.0 ml of 0.010M chlorous acid (Ka = 1.2 x 10^-2) is mixed with 200.0 ml of 0.020M hypochlorous acid (Ka = 3.5 x 10^-8). Calculate the pH of the resulting solution.
I am unsure of what to do with the volumes given. I believe that I should find the moles of each acid present and then divide it by the total volume of the solution to find the initial concentrations. So:
.100L (.010 mol HClO2/1 L) = .00100 mol HClO2 / .3000 L = .00333 mol HClO2/L
.200L (.020 mol HOCl/1 L) = .00400 mol HOCl / .3000 L = .0133 mol HOCl/L
Is this the correct way to find the initial concentrations to then make and ICE table and find H+ concentrations?