Answered: Try to derive the Henderson-Hasselbalch…

Science

Chemistry

Try to derive the Henderson-Hasselbalch Equation for the Carbonic Acid/Bicarbonate Buffer System. and explain each step

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 99QRT: Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it...

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Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.
The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
A buffer solution is prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.
Measure out 50.0 mL 1.0 M CH3COOH and 50.0 mL of 1.0 M NaCH3COO and combine them into a beaker. This is the buffer solution Measure out 50.0 mL of the buffer in part D (that you just made) and pour it into a clean beakerand add 2.0 mL of 1.0 M NaOH to it. What is the calculated/expected pH of this solution after the addition of the NaOH?
Measure out 50.0 mL 1.0 M CH3COOH and 50.0 mL of 1.0 M NaCH3COO and combine them into a beaker. This is the buffer solution Measure out 50.0 mL of the buffer in part D (that you just made) and pour it into a clean beakerand add 2.0 mL of 1.0 M HCl to it. What is the calculated/expected pH of this solution after the addition of the HCl?
Explain why the solubility of a sparingly soluble salt represents an equilibrium system.
e) Provide the chemical equilibrium that describes the carbonic acid buffer system that exists at pH 9.3. Clearly indicate the chemical formulas, identify the weak acid and its conjugate base and the names of the chemical compounds. f) Calculate the ratio of conjugate base/ weak acid at pH 9.3. Show all details of your working out for each individual mathematical manipulation that you apply (skipping steps will receive a deduction). In each step of your working out use the chemical formulas of the compounds that constitute the weak acid and conjugate base. Provide the answer to 3 decimal places, and make sure to round the result accordingly. State the final answer in a complete sentence g) Calculate the concentration of the weak acid and conjugate base for a total buffer concentration of 150 mM at pH 9.3. Show all details of your working out for each individual mathematical manipulation that you do apply (skipping steps will receive a deduction). In each step of your working out use…
All of the following statements concerning acid-base buffers are true EXCEPT A. buffers are resistant to changes in pH when diluted with water. buffers are used as colored indicators in acid-base titrations. B. buffers contain appreciable quantities of a weak acid and its conjugate base. C. buffers are resistant to pH changes upon addition of small quantities of strong acids or bases. D. the pH of a buffer is close to the pKa of the weak acid from which it is made.
Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can “absorb” five times as much acid or base as a 0.1 M buffer for a given pH change. In the next three problems you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. You are given 60 mL of 0.50 M phosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is: Concentration of HPO42−: 0.304 M Molar quantity of HPO42−: 18.2 mmol Concentration of H2PO4−: 0.196 M Molar quantity of H2PO4−: 11.8 mmol c. Take a fresh 60mL of 0.50M pH 6.83 buffer and add 3.7 mL of 1.00 M NaOH. Using the Henderson Hasselback equation to calculate the new pH of the solution.
Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can “absorb” five times as much acid or base as a 0.1 M buffer for a given pH change. In the next three problems you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. You are given 60 mL of 0.50 M phosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is: Concentration of HPO42−: 0.304 M Molar quantity of HPO42−: 18.2 mmol Concentration of H2PO4−: 0.196 M Molar quantity of H2PO4−: 11.8 mmol a. What is the new HPO42−/H2PO4− ratio, and the new pH of the solution? The pKa of H2PO4− is 6.64. Use the Henderson-Hasselbalch equation to calculate the new pH. (Note: You…
Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can “absorb” five times as much acid or base as a 0.1 M buffer for a given pH change. In the next three problems you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. You are given 60 mL of 0.50 M p2hosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is: Concentration of HPO42−: 0.304 M Molar quantity of HPO42−: 18.2 mmol Concentration of H2PO4−: 0.196 M Molar quantity of H2PO4−: 11.8 mmol a. You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H3O+ added as HCl, and the final molar quantity of HPO42- and H2PO42- at equilibrium.