moles of H+ = 0.337 * 0.6303 = 0.2124 moles of OH- = 0.447 * 10^0.02 = 0.46807 Moles of OH- left = 0.46807 - 0.2124 = 0.25566 moles [OH-] = 0.25566 / (0.337 + 0.447) = 0.3261 pOH = - log [OH-] = 0.487 pH = 14 - pOH = 13.513 Solution moles of H+ = 0.337 * 0.6303 = 0.2124 moles of OH- = 0.447 * 10^0.02 = 0.46807 Moles of OH- left = 0.46807 - 0.2124 = 0.25566 moles [OH-] = 0.25566 / (0.337 + 0.447) = 0.3261 pOH = - log [OH-] = 0.487 pH = 14 - pOH = 13.513.