Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH, CH2),N, with 0.1000 M HCl solution after the following additions of titrant. Note: Reference the K, of bases at 25 °C table for additional information. Part 1 of 3 Be sure your answer has the correct number of significant figures. 11.00 mL: pH G Part 2 of 3 Be sure your answer has the correct number of significant figures. 21.00 mL: pH= Part 3 of 3 Be sure your answer has the correct number of significant figures. 27.00 mL: pH Try again Recheck Save For Later Submit Assignment 2024 McGraw Hill LLC. All Rights Reserved Terms of Use Privacy Center Accessibility B

Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH, CH2),N, with 0.1000 M HCl solution after the following additions of titrant. Note: Reference the K, of bases at 25 °C table for additional information. Part 1 of 3 Be sure your answer has the correct number of significant figures. 11.00 mL: pH G Part 2 of 3 Be sure your answer has the correct number of significant figures. 21.00 mL: pH= Part 3 of 3 Be sure your answer has the correct number of significant figures. 27.00 mL: pH Try again Recheck Save For Later Submit Assignment 2024 McGraw Hill LLC. All Rights Reserved Terms of Use Privacy Center Accessibility B

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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4. In the titration of15.00 mL of 0.200 M HC with 0.100 M NaOH, calculate the pH after the addition of the following volumes of titrant (mL) ; (a) 0.00; (b) 10.00; (c)14.50 ; (d) 15.00; (e) 15.50: (f) 20.00 mL.
Be sure to answer all parts. Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: (a) 30.00 mL pH = (b) 39.40 mL pH = (c) 55.00 mL pH =
ANSWER D and how would the rankings change if...
10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40. Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid. A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.
What is the pH at the equivalence point in the titration of 60.00 mL of 0.200 M HA (a generic acid with K, = (2.26x10^-5)) with 0.400 M NaOH? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
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How many milliliters of 1.27 M NaOH must be added to 275 mL of 0.11 M H₂PO4 to make a buffer solution with a pH of 6.407 Round your answer to 2 significant digits. Note: Reference the pK, of weak acids at 25 °C table for additional information,
100. mL of 0.200 M HC1 is titrated with 0.250 M NaOH.
What is the highest pH that could be used as an effective buffer with B (a generic base) with Kp = (6.46x10^-10) and its chloride salt, HBCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
When 25.00 ml of an unknown monoprotic weak acid was titrated with 0.856 M NaOH, the following series of pH measurements in the region of the equivalence point were collected. Based on the data provided. calculate the concentration, in M, of the weak acid: Report the answer to three places after the decimal. Do not include units pH Titration Data Near Equivalence Point Volume of Solution Added from Buret (mL) pH 10.26 10.78 11.32 11.86 12.37 12.89 6.22 664 10.32 10.97 11:22 11,36