In the following example, by changing the titration conditions on a weak acid as compared to a strong acid, a difference at the pre-equivalence regions for the two is evident, while no difference at the post-equivalence regions is observed: 13. HWoak 0.50M HStrong 0.50 M HWoak 0.025 M HStrong 0.025 M pH 7- Caso A pH 7- Case B NaOH volume, ml. NaOH volumo, ml In both Case A and Case B, 0.50 M and 0.025 M acids are titrated with NaOH 0.50 M and NaOH 0.025 M, respectively. Case A corresponds to the weak acid titration (represented as HWeak) and Case B corresponds to the strong acid titration (represented as HStrong). Explain why the pH behavior in Case A is different from Case B in the pre-equivalence region when changing conditions, while they are the same in the post-equivalence region.

In the following example, by changing the titration conditions on a weak acid as compared to a strong acid, a difference at the pre-equivalence regions for the two is evident, while no difference at the post-equivalence regions is observed: 13. HWoak 0.50M HStrong 0.50 M HWoak 0.025 M HStrong 0.025 M pH 7- Caso A pH 7- Case B NaOH volume, ml. NaOH volumo, ml In both Case A and Case B, 0.50 M and 0.025 M acids are titrated with NaOH 0.50 M and NaOH 0.025 M, respectively. Case A corresponds to the weak acid titration (represented as HWeak) and Case B corresponds to the strong acid titration (represented as HStrong). Explain why the pH behavior in Case A is different from Case B in the pre-equivalence region when changing conditions, while they are the same in the post-equivalence region.

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

What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4Cl) in enough water to form 2.50L of solution. The K, of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBr is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H5O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.
7. The pH titration curve of a weak acid, HA, is shown me below. As the titration progresses, HA is converted into its conjugate base, A-. 12 10 8 (a) What is the volume of NaOH at the equivalence point? 2 25 30 35 15 20 volume of NaOH added (mL) 5 10 (b) At what volume (or volumes) is all of the acid present in the protonated (HA) form? (c) At what volume (or volumes) is all of the acid present in the conjugate base (A') form? (d) At what point along the titration will half the original amount of HA have been converted to A-?
1.Determine the pH during the titration of 62.9 mL of 0.360 M hydrocyanic acid (Ka = 4.0×10-10) by 0.360 M KOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 94.4 mL of KOH 2. When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?
4. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid. 2 14.0 13.0 12.0 1.0 5.0 3.0 2.0 00 Titration: pH vs. Volume of Strong Base 2.0 SO Volume of Base Added (ml) 8.0 5. From the graph given in the previous question, determine the pKa of the acid used in the titration. Which of the following acids (hypobromous-HBrO, Formic-HCHO2, Hypochlorus-HCIO, or Periodic-HIO4, or Hydroiodic-HI) is the acid used? Explain how you know. 1.0.0 703
A 1.37 L buffer solution consists of 0.298 M propanoic acid and 0.175 M sodium propanoate. Calculate the pH of the solution following the addition of 0.067 mol HCI. Assume that any contribution of the HCl to the volume of the solution is negligible. The K, of propanoic acid is 1.34 × 10-5. pH =
Calculate the pH for each of the cases in the titration of 35.0 mL of 0.140 M LiOH(aq) with 0.140 M HBr(aq). Note: Enter your answers with two decimal places. before addition of any HBr: after addition of 25.5 mL HBr: after addition of 42.5 mL HBr: after addition of 13.5 mL HBr: after addition of 35.0 mL HBr: after addition of 50.0 mL HBr:
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid: (a) 5.00 mL pH = (b) 29.60 mL pH = (c) 38.00 mL pH =
20
25.00 mL of 0.100 M HCl solution is titrated with a 0.100 M NaOH solution. What is the pH of the solution after the addition of the following strong base? (pH= - log[H3O+] = - log[H+]) a) initially (Before adding NaOH) b) Before the equivalence point (with the addition of 24.00 mL of 0.100 M NaOH) c) At the equivalence point (with the addition of 25.00 mL of 0.100 M NaOH) d) After the equivalence point (with the addition of 26.00 mL of 0.100 M NaOH)
A chemist titrates 110.0 mL of a 0.7452M aniline (C,H,NH,) solution with 0.5088M HCl solution at 25 °C. Calculate the pH at equivalence. The p K, of aniline is 4.87. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = ||
A 1.47 L buffer solution consists of 0.173 M butanoic acid and 0.299 M sodium butanoate. Calculate the pH of the solution following the addition of 0.060 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-. pH =
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL