12 10 8 2 60 70 80 10 20 30 40 50 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. НаА +3 X-ОН — Х;А + 3 H,0 b. НА +X-ОН — ХА+ Н,0 с. Н.А +2X-Он — Х,А +2 Н,0 d. 2 HsA + 3 X(OН) — Х,Аз + 6 Н,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. 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 с. 4. Hd

12 10 8 2 60 70 80 10 20 30 40 50 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. НаА +3 X-ОН — Х;А + 3 H,0 b. НА +X-ОН — ХА+ Н,0 с. Н.А +2X-Он — Х,А +2 Н,0 d. 2 HsA + 3 X(OН) — Х,Аз + 6 Н,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. 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 с. 4. Hd

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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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).
Using Figure 17.11, suggest an indicator to use in each of the following titrations: (a) The weak base pyridine is titrated with HCl. (b) Formic acid is titrated with NaOH. (c) Ethylenediamine, a weak diprotic base, is titrated with HCl. Figure 17.11 Common acid-base indicators. The color changes occur over a range of pH values. Notice that o few indicators hove color changes over two different pH ranges.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Two acids, each approximately 0.01 M in concentration, are titrated separately with a strong base. The adds show the following pH values at the equivalence point: HA, pH = 9.5, and HB, pH = 8.5. (a) Which is the stronger acid, HA or HB? (b) Which of the conjugate bases, A or B, is the stronger base?
Aniline hydrochloride, (C6H5NH3)Cl, is a weak acid. (Its conjugate base is the weak base aniline, C6H5NH2.) The acid can be titrated with a strong base such as NaOH. C6H5NH3+(aq)+OH(aq)C6H5NH2(aq)+H2O(l) Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M NaOH. (Ka for aniline hydrochloride is 2.4 105.) (a) What is the pH of the (C6H5NH3) solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 could be used to detect the equivalence point? (e) Calculate the pH of the solution after adding 10.0, 20.0, and 30.0 mL of base. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.
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
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.