56. What is the number of moles of HCI contained in the 12-mL solution added? 57. What is the number of moles of CH3COOH which participated in the reaction upon adding 12 mL of 1.5 M HCI? 58. What is the number of moles of CH3COOK which participated in the reaction upon adding 12 mL of 1.5 M HCI? 59. What is the pH of the original buffer solution? 60. What is the pH of the final buffer solution? 61. What is the final ratio of the CH3COOH and CH3COOK? 62. What is the change in pH in percentage?

56. What is the number of moles of HCI contained in the 12-mL solution added? 57. What is the number of moles of CH3COOH which participated in the reaction upon adding 12 mL of 1.5 M HCI? 58. What is the number of moles of CH3COOK which participated in the reaction upon adding 12 mL of 1.5 M HCI? 59. What is the pH of the original buffer solution? 60. What is the pH of the final buffer solution? 61. What is the final ratio of the CH3COOH and CH3COOK? 62. What is the change in pH in percentage?

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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An aqueous solution contains 0.29 M ammonium iodide. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.29 mol HCIO4 0.07 mol Ba(OH)2 0.28 mol NH3 0.14 mol HCIO4 0.28 mol Cal2
6. Which of the following processes will increase the pH of a buffer solution prepared by mixing 0.89 mol HCOOH (formic acid) and 0.76 mol HCOONa (sodium formate) into a 1-L solution? Ka (HCOOH) = 1.8 x 104. %3D a) add some NaCl into the buffer solution. b) add some HCl into the buffer solution. c) add some NaOH into the buffer solution. d) add more water into the buffer solution. e) None of the above.
A buffer is made using 100.0 mL of 0.100 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M NACH3 CH2 COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?
Payli
4. Consider a buffer made by adding 0.050 mol NaC2H302 and 0.040 mol HC2H3O2 to a liter of water. a) What is the pH of this buffer? b) What is the pH after addition of 0.010 mol NaOH? c) What is the pH after addition of 0.010 mol HCI to the original buffer 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?
A buffer is created by adding 0.125 moles of hypobromous acid (HOBr, pKa = 8.65) and 0.475 moles of sodium hypobromite (NaOBr) to 1.00 L of solution.25.00 mL of 0.200 M HCl is then added to the solution.a) What is the pH of the solution after the acid is added?
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 for each of the cases in the titration of 35.0 mL of 0.170 M LiOH(aq) with 0.170 M HCl(aq). Note: Enter your answers with two decimal places. before addition of any HCI: after addition of 21.5 mL HC1: after addition of 45.5 mL HCl: after addition of 13.5 mL HCl: after addition of 35.0 mL HCl: after addition of 50.0 mL HC1: []
Consider the titration of 25.00 mL of 0.250 M NaOH by 0.355 M HCl. Calculate the pH of the solution before the titration and after 5.00 mL of the acid has been added. What volume of the acid is necessary to reach the equivalence point? What is the pH of the solution at the equivalence point?