I Review | Constants | Periodic Table Part A As a technician in a large pharmaceutical research firm, you need to produce 150. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.98. The pKa of H2PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. • View Available Hint(s) ? Volume of KH2PO4 needed = Value Units

I Review | Constants | Periodic Table Part A As a technician in a large pharmaceutical research firm, you need to produce 150. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.98. The pKa of H2PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. • View Available Hint(s) ? Volume of KH2PO4 needed = Value Units

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 95AE: The active ingredient in aspirin is acetylsalicylic acid. A 2.51-g sample of acetylsalicylic acid...

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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.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
The active ingredient in aspirin is acetylsalicylic acid. A 2.51-g sample of acetylsalicylic acid required 27.36 mL of 0.5106 M NaOH for complete reaction. Addition of 13.68 mL of 0.5106 M HCl to the flask containing the aspirin and the sodium hydroxide produced a mixture with pH = 3.48. Determine the molar mass of acetylsalicylic acid and its Ka value. State any assumptions you must make to reach your answer.
K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic acid with 46.1 mL of 0.182 M sodium acetate. Calculate the pH of this solution at 25C after the addition of 5.82 mL of 0.125 M NaOH.
A titration of 35.0 mL of an unknown tribasic salt, Li₃A, requires 90.00 mL of 0.250 M HCl to reach the 3rd equivalence point. The titration data is shown below: Vol of HCl (mL) 15.00 30.00 45.00 60.00 75.00 90.00 pH 10.45 8.62 6.79 4.86 2.93 1.35 What is the value of Kb₁ of A³⁻?
An aqueous solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka= 6.3 × 10-5for HC7H5O2. Thesolution volume is 5.00 L. What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?
Ka for HPO42- = 4.4 x 10-13. A buffer system of 1.00 mole of Na2HPO4 and 1.00 mole of Na3PO4 to which 0.40 mol of OH- has been added (all in 1.00 L of solution) would have a pH of: Select one: a. 7.40 b. 12.36 c. 12.73 d. 14.60 e. 6.25
Lactobacillus bulgaricus is the main bacterium used in the production of yogurt and requires an acidic environment to grow effectively. To prepare an agar solution of this bacterium, a 100.0 mL 0.100 M buffer solution pH 5.00 must be prepared. The only available reagents in the laboratory are solid benzoic acid (HC6H5COO, MM = 122.12), solid sodium bicarbonate (NaHCO3, MM = 84.01), 1.00 M HCl, and 1.00 M NaOH. Acid dissociation constants: Benzoic acid, HC6H5COO: pKa,1 = 4.19 Carbonic acid, H2CO3: pKa,1 = 6.37, pKa,2 = 10.32 Identify the most appropriate conjugate acid-base pair for the target buffer. Determine the amounts of the acidic and basic species in the buffer (in millimoles).
An aqueous buffer solution of volume 100 cm3 consists of 0.20 M CH3COOH and 0.20 M NaCH3CO2. pKa value of CH3COOH is 4.75. (a) Predict the pH value of this solution. 3 sig. fig. (b) Predict the pH value after adding 9.43 mmol NaOH (note, not mM. Volume is not 1 L) to this buffer solution assuming volume is not changed. 3 sig. fig.