An analytical chemist is titrating 137.4 mL of a 0.2300M solution of methylamine (CH3NH2) with a 0.1600M solution of HNO3. The pK of methylamine is3.36. Calculate the pH of the base solution after the chemist has added 223.0 mL of the HNO3 solution to it.Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.Round your answer to 2 decimal places.

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Answered: An analytical chemist is titrating…

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...

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An analytical chemist is titrating 129.9mL of a 0.5200M solution of hydrazoic acid HN3 with a 0.2100M solution of NaOH . The pKa of hydrazoic acid is 4.72 . Calculate the pH of the acid solution after the chemist has added 241.9mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.
An analytical chemist is titrating 145.6mL of a 1.100M solution of hydrazoic acid HN3 with a 0.8100M solution of KOH . The pKa of hydrazoic acid is 4.72 . Calculate the pH of the acid solution after the chemist has added 236.7mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
The answer I got was 13.33 but that's not correct
10 An analytical chemist is titrating 180.7 mL of a 0.5200M solution of piperidine (C5H₁0NH) with a 0.8300M solution of HIO3. The p K² of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. G 4 = 0 X 3
5. Please solve the following chemistry problem.
A chemist titrates 90.0 mL of a 0.7050M methylamine (CH3NH₂) solution with 0.5016M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, 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 HBr solution added. pH = x 5 ?
An analytical chemist is titrating 195.5mL of a 0.1800M solution of dimethylamine CH32NH with a 0.4000M solution of HNO3 . The pKb of dimethylamine is 3.27 . Calculate the pH of the base solution after the chemist has added 12.5mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
A chemist titrates 140.0 mL of a 0.1432M butanoic acid (HC3H₂CO₂) solution with 0.5600M KOH solution at 25 °C. Calculate the pH at equivalence. The PK of butanoic acid is 4.82. 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 KOH solution added.
An analytical chemist is titrating 246.3 mL of a 0.8100M solution of butanoic acid (HC3H₂CO₂) with a 0.5500M solution of NaOH. The p K of butanoic acid a is 4.82. Calculate the pH of the acid solution after the chemist has added 429.8 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.
An analytical chemist is titrating 70.8mL of a 0.7400M solution of butanoic acid HC3H7CO2 with a 1.100M solution of KOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 55.5mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
N) with a 0.7800M solution of HNO3. The pK, of trimethylamine An analytical chemist is titrating 123.2 mL of a 0.4600M solution of trimethylamine ((CH3), N) is 4.19. Calculate the pH of the base solution after the chemist has added 86.6 mL of the HNO 3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = ☑
An analytical chemist is titrating 203.4 mL of a 1.000 M solution of hydrazoic acid (HN3) with a 0.2500 M solution of NaOH. The pK of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 405.3 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH pH=0 × 5

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