24. The titration curve of a 0.10-M unknown weak base solution (60.0 mL initially) titrated with 0.10-M HCI is given below. Note that the unknown base is B and its conjugate acid is HB'. Part 1. The pK, value of this unknown base is mostly like to be a) 11.5 b) 9.5 c) 4.5 d) 5.5 e) 7.0 f) none of the above 124 Part 2. At the equivalence point of the titration, the 11 10 correct order of the concentration among different ionic species should be PH a) [H3O*] > [OH] > [HB*] b) [HB'] > [OH]> [H3O*] 2 c) [HB'] > [H3O*] > [OH] 10 30 50 ml of HCI 70 90 110 d) [H3O*] > [HB']> [OH] e) none of the above

24. The titration curve of a 0.10-M unknown weak base solution (60.0 mL initially) titrated with 0.10-M HCI is given below. Note that the unknown base is B and its conjugate acid is HB'. Part 1. The pK, value of this unknown base is mostly like to be a) 11.5 b) 9.5 c) 4.5 d) 5.5 e) 7.0 f) none of the above 124 Part 2. At the equivalence point of the titration, the 11 10 correct order of the concentration among different ionic species should be PH a) [H3O] > [OH] > [HB] b) [HB'] > [OH]> [H3O] 2 c) [HB'] > [H3O] > [OH] 10 30 50 ml of HCI 70 90 110 d) [H3O*] > [HB']> [OH] e) none of the above

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...

See similar textbooks

Similar questions

E)
Please help!!!!
I need help with fill the blanks spaces
Solve correctly please.
Consider the titration of a 20.0 mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine eachof the following. (Ka HC2H3O2 = 1.8 x 10-5) d) the pH at one-half of the equivalence point e) the pH at the equivalence point f) the pH after adding 21.8 mL of base beyond the equivalence point
5 Please answer all questions. Thanks
The molar solubility of PbI2 is 1.46 x 10^-3 M. Calculate the value of Ksp for PbI2. A. 3.11 x 10^-9 B. 4.26 x 10^-6 C. 1.24 x 10^-8 D. 1.46 x 10^-3 E. none of these
I really need help with this review problem thanks
4. You are titrating 50.0 ml of 0.100 M Na:CO, with 0.400 M AGNOS. Calculate the pAg* values.. a) 1.0 ml. before the equivalence point b) at the equivalence point c) 1.0 mL after the equivalence point
A 20.0 mL sample of 0.115M H2SO3 is titrated with 0.1014 M KOH. At what volume (of added base) does each equivalence point occur? a. 25.0mL for the first equivalence point and 50.0mL for the second equivalence point. b. 33.2mL for the first equivalence point and 66.4mL for the second equivalence point. c. 22.7mL for the first equivalence point and 45.4mL for the second equivalence point. d. 20.0mL for the first equivalence point and 40.0mL for the second equivalence point.