7. Select the diprotic acid as the analyte. a. What is the pH and volume of titrant at the first equivalence point? b. What is the pH and volume of titrant at the second equivalence point? c. Unlike the monoprotic acid titrations (weak or strong), why is [OH-] still-0 after adding 30 mL of titrant? d. What are the values of pKai and pKa2 for this acid? Hint: Recall that pH = pKa when [acid] = [conjugate base] tates) Accessibility: Good to go

7. Select the diprotic acid as the analyte. a. What is the pH and volume of titrant at the first equivalence point? b. What is the pH and volume of titrant at the second equivalence point? c. Unlike the monoprotic acid titrations (weak or strong), why is [OH-] still-0 after adding 30 mL of titrant? d. What are the values of pKai and pKa2 for this acid? Hint: Recall that pH = pKa when [acid] = [conjugate base] tates) Accessibility: Good to go

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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use the titration curve below. 14 12 10 8 4 2 60 70 10 20 30 40 50 80 Volume of Titrant (mL) What is the possible identity of the titrant? a. Strong base b. Strong acid Which of the following stoichiometrically represents the titration curve? а. НА +3 X-Он — Х;А +3 Н,О b. НА +X-ОН — ХА+Н:0 с. Н.А +2X-Он — Х,А + 2 H,0 d. 2 H;A + 3 X(0H), → X;A2 + 6 H,0 Which of the following statement is NOT FALSE regarding the titration curve? a. There are three equivalence points located near pH 2.00, 6.00 and 12.00. b. There are three equivalence points that approximately requires 15.00, 40.00 and 60.00 mL of titrant. c. There are two equivalence points located near pH 6.00 and 12.00. d. There are two equivalence points that approximately requires 25.00 and 50.00 mL of titrant. c. Weak base d. Weak acid Hd
8. What is the pH of a buffer solution made with 1.8M benzoic acid with Ka = 6.5 x 105 and 0.478M sodium benzoate? 9. What is the [H*] for the buffer solution made in #8?
a. What was the concentration of the NaOH? Concentration = м b. What is the pH at the equivalence point? рн - c. Which indicator, bromothymol blue, phenolpl
Which of the following indicators will be the most appropriate to be used for the titration of 15.0 mL 1.0 M H2CO3 with 1.0 M KOH titrant to the second equivalence point ? H2CO3: pKa, 6.35 ; pKaz : 10.33 Select one: O A. Methyl Red, pKa 5.1 O B. Phenol red, pka 7.9 OC. Phenopthalein, pka 9.3 O D. Bromthymol blue, pka 7.0 O E. Methyl Orange, pka 3.7
1. Adding NaCl to: HC₂H₃O₂ + H₂O ↔ C₂H₃O₂⁻ + H₃O⁺ a. reaction shift backward b.reaction shift forward c.no effect d.none of the above 2.A stock solution has a concentration of 0.05 M. Which of the following concentrations might be the concentration of the final solution when diluted? 3.A buffer system with pKa of 6.4. Which of the following pH is reasonable when a base is added to the buffer solution?
In this experiment, the color change from pink/violet to colorless during the titration is caused by: Group of answer choices a.change from MnO4– to Mn2+ b.change from Fe2+ to Fe3+ c.change from H+ to H2O d.the addition of an indicator.
A 25.00 mL of 0.0300 M H;B (pKa, = 5.83, pKa, = 8.64) was titrated with 0.0250 M NaOH. Calculate the pH after addition of the following volumes of titrant: A. 0.00 mL B. 15.00 mL. C. 30.00 mL. D. 50.00 mL. E. 60.00 mL.
6. Using the data in this graph: 12 a. What is the equivalence point? 10 8 b. What is the half-way point of the titration? 6. с. What is the pH at the half- way point? 10 20 30 40 50 Volume Base (mL) 4- 2.
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.
Part 1: A 42.50-mL sample of 0.0527 M HF (Ka = 6.6 10-4) was titrated with a 0.0600-M KOH solution. What would be the equivalence point of this titration? Part 2: (This is the follow-up question of part 1) What would be the pH of the titree solution at the equivalence point? Please solve part 2