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In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH2)3 CNH2, often abbreviated as Tris. At 25 "C, Tris has a pK, of 5.91. The hydrochloride of Tris is (HOCH2), CNH, Cl, which can be abbreviated as TrisHCI. Part A What volume of 10.0 mol L NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHC1? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) 6.7 mL ✓ Correct Previous Answers This procedure represents only one of many ways to prepare a buffer. The exact method chosen depends on the reagents and glassware available as well as the accuracy required for the pH. Part B The buffer from Part A is diluted to 1.00 L. To half of it (500 mL), you add 0.0100 mol of hydrogen ions without changing the volume. What is the pH of the final solution? Express your answer numerically to two decimal places. ▸ View Available Hint(s) pH 7.58 Subm Previous Answers ✓ Correct Part C Notice that even though a significant amount of the strong acid was added to the buffer, the pH did not change drastically since the capacity of the buffer had not been exceeded. What additional volume of 10.0 mol L HCI would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) ΜΕ ΑΣΦ ? mL You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers

In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH2)3 CNH2, often abbreviated as Tris. At 25 "C, Tris has a pK, of 5.91. The hydrochloride of Tris is (HOCH2), CNH, Cl, which can be abbreviated as TrisHCI. Part A What volume of 10.0 mol L NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHC1? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) 6.7 mL ✓ Correct Previous Answers This procedure represents only one of many ways to prepare a buffer. The exact method chosen depends on the reagents and glassware available as well as the accuracy required for the pH. Part B The buffer from Part A is diluted to 1.00 L. To half of it (500 mL), you add 0.0100 mol of hydrogen ions without changing the volume. What is the pH of the final solution? Express your answer numerically to two decimal places. ▸ View Available Hint(s) pH 7.58 Subm Previous Answers ✓ Correct Part C Notice that even though a significant amount of the strong acid was added to the buffer, the pH did not change drastically since the capacity of the buffer had not been exceeded. What additional volume of 10.0 mol L HCI would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) ΜΕ ΑΣΦ ? mL You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers

Chemistry
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...
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In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH2)3 CNH2, often abbreviated as Tris. At 25 °C, Tris has a pK, of 5.91. The hydrochloride of Tris is (HOCH2)3 CNH3 Cl, which can be abbreviated as TrisHCl. Part A What volume of 10.0 mol L-1 NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHC1? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) 6.7 mL Submit Part B Previous Answers Correct This procedure represents only one of many ways to prepare a buffer. The exact method chosen depends on the reagents and glassware available as well as the accuracy required for the pH. The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100 mol of hydrogen ions without changing the volume. What is the pH of the final solution? Express your answer numerically to two decimal places. ▸ View Available Hint(s) pH = 7.58 Submit Previous Answers Part C Correct Notice that even though a significant amount of the strong acid was added to the buffer, the pH did not change drastically since the capacity of the buffer had not been exceeded. What additional volume of 10.0 mol L-¹ HCl would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) ΜΕ ΑΣΦ ? mL You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers
Transcribed Image Text:In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH2)3 CNH2, often abbreviated as Tris. At 25 °C, Tris has a pK, of 5.91. The hydrochloride of Tris is (HOCH2)3 CNH3 Cl, which can be abbreviated as TrisHCl. Part A What volume of 10.0 mol L-1 NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHC1? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) 6.7 mL Submit Part B Previous Answers Correct This procedure represents only one of many ways to prepare a buffer. The exact method chosen depends on the reagents and glassware available as well as the accuracy required for the pH. The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100 mol of hydrogen ions without changing the volume. What is the pH of the final solution? Express your answer numerically to two decimal places. ▸ View Available Hint(s) pH = 7.58 Submit Previous Answers Part C Correct Notice that even though a significant amount of the strong acid was added to the buffer, the pH did not change drastically since the capacity of the buffer had not been exceeded. What additional volume of 10.0 mol L-¹ HCl would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) ΜΕ ΑΣΦ ? mL You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers
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