please help and im really stuck

Calculate the pH of the solution made by adding 0.50mol of HOBr and 0.30mol of KOBr to 1.00L of water The value of Ka for HOBr is 2.0109. Express your answer numerically using two decimal places. You may want to reference (Page) section 16.2 while completing this problem. Calculate the pH of the solution that results from each of the following mixtures. The ionization constants required in this exercise are found in Appendix II, page A-12, of your textbook: The acidity constant Ka of HF is 3.5104. The basicity constant Kb of C2H5NH2 is 5.6104. 160.0mL of 0.24MHF with 220.0mL of 0.31MNaF Express your answer using two decimal places. 185.0mL of 0.11MC2H5NH2 with 280.0mL of 0.20MC2H5NH3Cl Express your answer using two decimal places