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b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a 0.4900M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 97.5 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 HNO 3 solution added. Round your answer to 2 decimal places. pH = ☐ An analytical chemist is titrating 187.2 mL of a 0.7600M solution of butanoic acid (HC3H7CO2) with a 1.000M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 157.3 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 ☑ 5

b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a 0.4900M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 97.5 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 HNO 3 solution added. Round your answer to 2 decimal places. pH = ☐ An analytical chemist is titrating 187.2 mL of a 0.7600M solution of butanoic acid (HC3H7CO2) with a 1.000M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 157.3 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 ☑ 5

Chemistry
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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b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a 0.4900M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 97.5 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 HNO 3 solution added. Round your answer to 2 decimal places. pH = ☐
Transcribed Image Text:b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a 0.4900M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 97.5 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 HNO 3 solution added. Round your answer to 2 decimal places. pH = ☐
An analytical chemist is titrating 187.2 mL of a 0.7600M solution of butanoic acid (HC3H7CO2) with a 1.000M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 157.3 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 ☑ 5
Transcribed Image Text:An analytical chemist is titrating 187.2 mL of a 0.7600M solution of butanoic acid (HC3H7CO2) with a 1.000M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 157.3 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 ☑ 5
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