A chemist titrates 250.0 mL of a 0.2431M dimethylamine ((CH3)₂NH) solution with 0.4945M HNO3 solution at 25 °C. Calculate the pH at equivalence. The pK of dimethylamine is 3.27. 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 HNO3 solution added. pH = X 000 Ar

A chemist titrates 250.0 mL of a 0.2431M dimethylamine ((CH3)₂NH) solution with 0.4945M HNO3 solution at 25 °C. Calculate the pH at equivalence. The pK of dimethylamine is 3.27. 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 HNO3 solution added. pH = X 000 Ar

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 250.0 mL of a 0.0775 M potassium hydroxide (KOH) solution with 0.0631 M HCl 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 HCl solution added. pH =
3. Please help me answer all parts to this chemistry question:
Calculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.5851 M ethylamine (C2H5NH2) solution with 0.8192M HBr solution at 25 °C. Calculate the pH at equivalence. The pK of ethylamine is 3.19. b 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. pH = ] ☑
Calculating the pH at equivalence of a titration
A chemist titrates 190.0 mL of a 0.5701 M methylamine (CH3NH₂) solution with 0.4336M HNO3 solution at 25 °C. Calculate the pH at equivalence. The p K of methylamine is 3.36. 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 HNO3 solution added. -0 pH = X` S
A chemist titrates 130.0mL of a 0.6404M acetic acid (HCH3CO2) solution with 0.7306M 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 0.6712M benzoic acid (HC6H5CO₂) solution with 0.6137M NaOH solution at 25 °C. Calculate the pH at equivalence. The pk of benzoic acid is 4.20. a 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 = X
A 10.0 mL solution of 0.570 M NH3 is titrated with a 0.190 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the K of acids at 25 °C and K₁ of bases at 25 °C tables for additional information. b Part 1 of 4 0.00 mL Added, pH = ☐ x10 Part 2 of 4 10.0 mL Added, pH = ☐ ☐ x10 Part 3 of 4 ☑ ✓ G
A chemist titrates 210.0 mL of a 0.7303M potassium hydroxide (KOH) solution with 0.0877M HNO3 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 HNO3 solution added. pH = X
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
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.