An analytical chemist is titrating 121.0 mL of a 0.3000M solution of isopropylamine ((CH) CHNH, with a 0.6300M solution of HNO2. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 40.1 mL of the HNO, 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, solution added. 2 docimal places

Chemistry: Principles and Reactions
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Chapter14: Equilibria In Acid-base Solutions
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Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...
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An analytical chemist is titrating 121.0 mL of a 0.3000M solution of isopropylamine ((CH3), CHNH2) with a 0.6300M
solution of HNO2. The p K of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added
40.1 mL of the HNO, 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, solution added.
Round your answer to 2 decimal places.
pH =
Check
Explanation
Acces
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Transcribed Image Text:An analytical chemist is titrating 121.0 mL of a 0.3000M solution of isopropylamine ((CH3), CHNH2) with a 0.6300M solution of HNO2. The p K of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 40.1 mL of the HNO, 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, solution added. Round your answer to 2 decimal places. pH = Check Explanation Acces O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy W
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