A chemist titrates 160.0 mL of a 0.2739M trimethylamine ((CH, N solution with 0.4017M HCI solution at 25 °C. Calculate the pH at equlvalence. ThepK 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 HCI solution added. pH = ||

A chemist titrates 160.0 mL of a 0.2739M trimethylamine ((CH, N solution with 0.4017M HCI solution at 25 °C. Calculate the pH at equlvalence. ThepK 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 HCI solution added. pH = ||

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

dont provide handwriitning solution..
10 11 12 13 14 15 16 17 18 19 20 21 22 A chemist titrates 180.0 mL of a 0.4289 M pyridine (C,H,N) solution with 0.5274M HCI solution at 25 °C. Calculate the pH at equivalence. The p K, of pyridine is 8.77. Round your answer to 2 decimal places. d- 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 = %3D Submit Assignment Continue MacBook Air F12 F10 F9 F8 F7 000 000 * ES F6 F4 esc F2 F3 F1 & *
A chemist titrates 80.0 mL of a 0.8628 M trimethylamine ((CH) N solution with 0.2165 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, 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 HBr solution added. pH =||
Calculate the volume (ml)of concentrated ammonia and the weight (gm) of ammonium chloride respectively to be taken to prepare 100 ml of buffer solution at a pH of 10 if the final concentration of the salt is 0.20 mol. Note that the molar concentration of concentrated ammonia is equal to 14.8 mol/liter, and that the pKb of ammonia is 4.76, and the molecular weight of ammonium :chloride 53.5 g/mole.lt is about
A chemist titrates 70.0mL of a 0.5352M carbonic acid (H2CO3) solution with 0.1825M KOH solution at 25°C. Calculate the pH at equivalence. The pKa of carbonic acid is 3.60. 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.
Subject:
A chemist titrates 120.0 ml. of a 0.7695 M trimethylamine ((CH₂)₂N) solution with 0.1789M HNO, solution at 25 °C. Calculate the pH at equivalence. The PK, 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 HNO, solution added. PH-0
8.00 6.00 1 명 4.00 2.00 2. 0.00 0.02 0.04 0.06 0.08 0.1 Acid Added / mol 22. Curve 1 shows the pH when HCl is added to 1 L of: (A) a solution of 1.0 M CH3COONA and 1.0 M CH3COOH. (B) pure water. a solution of 0.10 M NaCl. 23. Curve 2 shows the pH when HCl is added to 1 L of: FA) a solution of 1.0 M CH3COONA and 1.0 M CH3COOH. (B) a solution of 0.10 M NAOH. (C) pure water.
A chemist titrates 120.0 mL of a 0.3246M cyanic acid (HCNO) solution with 0.2427M NaOH solution at 25 °C. Calculate the pH at equivalence. The p Ka 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 NaOH solution added. pH = [] X Ś
It says that my answers are wrong but it won’t tell me what answers are wrong I thought I did it right please help me.
What is the pH of a buffer solution that is 0.10 M chloroacetic acie, HC2H2ClO2 and 0.15M sodium chloroacetate NaC2H2ClO2? The Ka for HC2H2ClO2 is 1.4x10-3. Express your answer to two decimal places.
A chemist titrates 210.0 mL of a 0.3206M ammonia (NH3) solution with 0.3768 M 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 = 0 X