you will be working originally with 750 mL of a 020 M soluti

you will be working originally with 75.0 mL of a 0.20 M solution of HC4H7O2 (Ka= 1.5 x 10-5 ) 1. Determine the pH of your solution (I got pH= 2.7 with significant figures taken into account, is that right?) 2. Add 85.0 mL of 0.15 M KC4H7O2 to your solution. Find the pH. 3. Add 9.0 mL of 0.100 M HBr to the solution from task #2. Find the pH. 4. In a titration, 5.0 mL of 0.75 M KOH is added to your original solution. Find the pH. 5. What volume of 0.75 M KOH must be added to the original solution to produce a solution which would act as a buffer more than any other time in the titration? What would the pH of the solution be at that point? 6. What volume of 0.75 M KOH must be added to the original solution to reach the equivalence point in the titration? What would the pH of the solution be at that point? 7. If a volume of 25.0 mL of 0.75 M KOH is added to the original solution in a titration, what would the pH of the solution be at that point? 8.If a weak base was used in place of the weak acid in the titration and a strong acid was used in place of the strong base referenced in tasks 4-7 (same volumes, same concentrations) name TWO noteworthy and appropriate similarites in the process in the first scenario [for which you did the work above] compared to this new scenario and TWO noteworthy and appropriate differences as well. PLEASE ANSWER THOROUGHLY AND TRY TO SHOW WORK. THANK YOU!!