An analytical chemist is titrating 215.6 mL of a 1.000M solution of hydrazoic acid (HN) with a 0.5300M solution of KOH. The pK of hydrazoic acid is 4.72.Calculate the pH of the acid solution after the chemist has added 205.1 mL 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.pH =☑

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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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The answer I got was 13.33 but that's not correct
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
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
Calculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.1528M hypochlorous acid (HC10) solution with 0.7043 M NAOH solution at 25 °C. Calculate the pH at equivalence. The pK, of hypochlorous acid is 7.50. 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 = |
A chemist titrates 50.0 mL of a 0.5456M carbonic acid (H₂CO3) solution with 0.1077M 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. pH = X
An analytical chemist is titrating 189.4 mL of a 0.8600 M solution of cyanic acid (HCNO) with a 0.8700 M solution of NaOH. The PX of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 125.9 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- 0 ?
An analytical chemist is titrating 168.8mL of a 1.100M solution of cyanic acid HCNO with a 0.7700M solution of KOH. The pKa of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 282.6mL 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.
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 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.
A chemist titrates 180.0 mL of a 0.7495M hypochlorous acid (HCIO) solution with 0.5517M NaOH solution at 25 °C. Calculate the pH at equivalence. The PK of hypochlorous acid is 7.50. 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 Ś

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