3. You need to prepare 100 mL of a 0.200 M acetate buffer at pH 5.00. The pka of acetic acid is 4.756 and the density of liquid acetic acid is 1.049 g/mL. You have pure liquid acetic acid (CH3CO2H; FW = 60.05 g/mol) and pure sodium acetate trihydrate (Na+CH3CO²- 3 H₂O; FW = 136.08 g/mol) available to you to prepare the buffer. a. Calculate the volume (in mL) of liquid acetic acid that must be added to the 100 mL volumetric flask. b. Calculate the mass (in grams) of sodium acetate that you would need to add to the 100 mL flask to prepare 100 mL of a pH 5.00 acetate buffer.

3. You need to prepare 100 mL of a 0.200 M acetate buffer at pH 5.00. The pka of acetic acid is 4.756 and the density of liquid acetic acid is 1.049 g/mL. You have pure liquid acetic acid (CH3CO2H; FW = 60.05 g/mol) and pure sodium acetate trihydrate (Na+CH3CO²- 3 H₂O; FW = 136.08 g/mol) available to you to prepare the buffer. a. Calculate the volume (in mL) of liquid acetic acid that must be added to the 100 mL volumetric flask. b. Calculate the mass (in grams) of sodium acetate that you would need to add to the 100 mL flask to prepare 100 mL of a pH 5.00 acetate buffer.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 125CP: Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to...

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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.)
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The indicator dinitrophenol is an acid with a Ka of 1.1104. In a 1.0104 -M solution, it is colorless in acid and yellow in base. Calculate the pH range over which it goes from 10% ionized (colorless) to 90% ionized (yellow).
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Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to prepare buffered solutions. Calculate the masses of cacodylic acid and sodium cacodylate that should be used to prepare 500.0 mL of a pH = 6.60 buffer so that the buffer has a total of arsenic-containing species equal to 0.25 M, that is, so that: [(CH3)2AsO2H] + [(CH3)2AsO2] = 0.25 M
Lactic acid is a common by-product of cellular respiration and is often said to cause the burn associated with strenuous activity. A 25.0-mL sample of 0.100 M lactic acid (HC3H5O3, pKa = 3.86) is titrated with 0.100 M NaOH solution. Calculate the pH after the addition of 0.0 mL, 4.0 mL, 8.0 mL, 12.5 mL, 20.0 mL, 24.0 mL, 24.5 mL, 24.9 mL, 25.0 mL, 25.1 mL, 26.0 mL, 28.0 mL, and 30.0 mL of the NaOH. Plot the results of your calculations as pH versus milliliters of NaOH added.
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A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.072 M KOH. What volume KOH must be added to give a pH of 5.56? Ka1 = 1.42 × 10–3 and Ka2 = 2.01 × 10–6. Show all of your work on your scratch paper and upload it as a comment to this quiz assignment. Correct!