✓9 10 A chemist titrates 160.0 mL of a 0.4381 M benzoic acid (HC, H,CO₂) solution with 0.2772M NaOH solution at 25 °C. Calculate the pH at equivalence. The pk of benzoic acid is 4.20. pH = Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added.

✓9 10 A chemist titrates 160.0 mL of a 0.4381 M benzoic acid (HC, H,CO₂) solution with 0.2772M NaOH solution at 25 °C. Calculate the pH at equivalence. The pk of benzoic acid is 4.20. pH = Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A chemist titrates 50.0 mL of a 0.6961 M ammonia (NH3) solution with 0.1854M HCl solution at 25 °C. Calculate the pH at equivalence. The pk of ammonia is 4.75. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = X Ś
We have a titration for the titration of 50.0 mL of 0.425 M lactic acid, a monoprotic acid, (Ka = 1.38 x 10^-4) with 0.350 M NaOH. 1. Calculate the exact volume of the NaOH needed (to the correct numbers of sig figs) to reach the equivalence point. 2. Calculate the exact volume of NaOH needed (to the correct numbers of sig figs) to reach the mid point.
A chemist titrates 60.0 mL of a 0.7169M lidocaine (C14H2|NONH) solution with 0.4965 M HNO, solution at 25 °C. Calculate the pH at equivalence. The p Kb of lidocaine is 7.94. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO, solution added. pH %3D
A chemist titrates 180.0mL of a 0.6252M acetic acid HCH3CO2 solution with 0.1719M NaOH solution at 25°C . Calculate the pH at equivalence. The pKa of acetic acid is 4.76 . Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added.
A chemist titrates 160.0 mL of a 0.3349M cyanic acid (HCNO) solution with 0.3751 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK of cyanic acid is 3.46. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = X S ?
A chemist titrates 90.0 mL of a 0.5350M trimethylamine ((CH3)N) solution with 0.1600M HCl solution at 25 °C. Calculate the pH at equivalence. The pK₂ of trimethylamine is 4.19. Round your answer to 2 decimal places. ? Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = ☐ X Ś olo
A chemist titrates 80.0 mL. of a 0.0754 M aniline (C6H5NH2) solution with 0.5961 M HBr solution at 25 °C. Calculate the pH at equivalence. The pKa of aniline is 4.87. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added.
A chemist titrates 100.0 mL of a 0.0621 M hydrobromic acid (HBr) solution with 0.6950M KOH solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = 0 X 5
A chemist titrates 140.0 mL of a 0.4430 M hydrochloric acid (HCI) solution with 0.4963 M NaOH solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. PH =0 × 9
Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 105 mL of a buffer that is 0.260 M in both benzoic acid (CH₂COOH) and its conjugate base (CH₂COO¯). Calculate the maximum volume of 0.270M HCl that can be added to the buffer before its buffering capacity is lost. volume: mL
A chemist titrates 90.0 mL of a 0.2182M acetic acid (HCH3CO₂) solution with 0.8569M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K of acetic acid is 4.76. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. pH = 0 X 3 ?