Consider a solution formed by mixing 37.0 mL of 0.100 M H2SO4, 35.5 mL of 0.100 M HOCl, 25.0 mL of 0.200 M NaOH, 25.0 mL of 0.100 M Ca(OH)2, and 10.0 mL of 0.150 M KOH. Calculate the pH of this solution.
I started by finding the moles of H+ and OH- present in the solution. I got: .106 M H+ and .192 M OH-. (Multiplied the volume by concentration to find moles, added the moles together and divided by total volume)
I at first thought the pH was just -log(.106) but that's not correct, and I know I'm missing something. I don't know how Ka comes into play either because of the multiple acids present. Thank you in advance.