Need #28-34

Data:

28. Average K, value for the CH3CO2H solutions (0.25 pts): 29. Average pK, value for the CH3CO2H solutions (0.25 pts): C. Buffer Solutions 30. Concentration of CH3CO2Na after dilution (0.5 pts). M 31. Concentration of CH3CO2H after dilution (0.25 pts) M 32. Theoretical pH of solution in beakers B and D before the addition of HCl or NaOH. (Hint: Use the average K, value calculated for CH3CO2H in #28). (1.0 pt) CHEM 032 Experiment 5: Acid-Base Equilibria, pH, and Buffers Calculations 3, Part C (1.5 pts) Note: you must show work for all calculations to receive full credit. 33. Calculated pH of beaker A after the addition of 6 M HCl. (0.5 pts) 34. Calculated pH of beaker B after the addition of 6 M HCl. (1.0 pt) A. Hydrochloric Acid Solutions 1. Original concentration HCl: 0.1M 2. pH of original HCl solution : 1.47 3. Volume HCl used in dilution: 5.00 mL 4. pH of diluted HCl solution: 2.11 B. Acetic Acid Solutions 5. Original conc. CH3CO2H 0.1 M 6. pH of original CH3CO2H soln 2.85 7. Volume CH3CO2H used 5.00 mL 8. pH of diluted CH3CO2H soln 3.68 C. Buffer Solutions 9. Mass of CH3CO2Na used 4.10 g 10. Original concentration CH3C02H 6 M 11. Volume of CH3CO2H used__8.5 mL 12. Volume of distilled water used 91.5 mL 13. Total volume of buffer solution 100 mL 1.0 mL 14. Volume of 6 M HCl used for addition to beaker A: ___1.0_mL; beaker B: 15. Volume of 6 M NaOH used for addition to beaker C: mL; beaker D: 1.0 1.0 mL Initial pH of Solutions pH of Solutions after additions 16. Beaker A 4.63 1.30 17. Beaker B 4.45 4.12 18. Beaker C 4.60 2.96 19. Beaker D 4.45 4.38