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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

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Similar questions

A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL b. 50.0 mL c. 100.0 mL d. 150.0 mL e. 200.0 mL f. 250.0 mL
The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?