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Direction: Solve what is being asked. Follow the directions below; All answers, including values used in the solutions, must be rounded to the nearest two decimal places. Always place a zero before the decimal point for values less than 1 | (example: .25 = 0.25) Add trailing zeros to complete your answer to the 2nd decimal place, if necessary | (examples: 62.7 = 62.70; 123 123.00) ● ● ● DO NOT include spaces in between numbers, characters, and decimal points. ● There is NO NEED to write the UNITS Write your answers before the item For answers with exponents, input the base number up to the 2nd decimal place before placing x10^...(examples: 5.31x10^5; 9.60x10^-4) ● Problem 1: A 350-ml buffer solution was prepared by a chemist by mixing 0.135 M CH3COOH and 0.100 M CH3COOK. Accidentally, you added 12 ml of an unlabeled solution to the buffer solution during the experiment. Your groupmate, later on, identified this to be 1.5 M HCI which was mistakenly left unlabeled when she went out to urinate. Compute the following; use the pKb value of 7.62. Atomic weights: K: 39.10 C: 12.01 H: 1.01 CI: 35.45 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? O: 15.99 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?

Direction: Solve what is being asked. Follow the directions below; All answers, including values used in the solutions, must be rounded to the nearest two decimal places. Always place a zero before the decimal point for values less than 1 | (example: .25 = 0.25) Add trailing zeros to complete your answer to the 2nd decimal place, if necessary | (examples: 62.7 = 62.70; 123 123.00) ● ● ● DO NOT include spaces in between numbers, characters, and decimal points. ● There is NO NEED to write the UNITS Write your answers before the item For answers with exponents, input the base number up to the 2nd decimal place before placing x10^...(examples: 5.31x10^5; 9.60x10^-4) ● Problem 1: A 350-ml buffer solution was prepared by a chemist by mixing 0.135 M CH3COOH and 0.100 M CH3COOK. Accidentally, you added 12 ml of an unlabeled solution to the buffer solution during the experiment. Your groupmate, later on, identified this to be 1.5 M HCI which was mistakenly left unlabeled when she went out to urinate. Compute the following; use the pKb value of 7.62. Atomic weights: K: 39.10 C: 12.01 H: 1.01 CI: 35.45 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? O: 15.99 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?

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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Direction: Solve what is being asked. Follow the directions below; All answers, including values used in the solutions, must be rounded to the nearest two decimal places. Always place a zero before the decimal point for values less than 1 | (example: .25 = 0.25) Add trailing zeros to complete your answer to the 2nd decimal place, if necessary | (examples: 62.7 = 62.70; 123 123.00) ● ● ● For answers with exponents, input the base number up to the 2nd decimal place before placing x10^...(examples: 5.31x10^5; 9.60x10^-4) DO NOT include spaces in between numbers, characters, and decimal points. There is NO NEED to write the UNITS Write your answers before the item Problem 1: A 350-ml buffer solution was prepared by a chemist by mixing 0.135 M CH3COOH and 0.100 M CH3COOK. Accidentally, you added 12 ml of an unlabeled solution to the buffer solution during the experiment. Your groupmate, later on, identified this to be 1.5 M HCI which was mistakenly left unlabeled when she went out to urinate. Compute the following; use the pKb value of 7.62. Atomic weights: K: 39.10 C: 12.01 H: 1.01 59. What is the pH of the original buffer solution? 60. What is the pH of the final buffer solution? CI: 35.45 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? O: 15.99 58. What is the number of moles of CH3COOK which participated in the reaction upon adding 12 mL of 1.5 M HCI? 61. What is the final ratio of the CH3COOH and CH3COOK? 62. What is the change in pH in percentage?
Transcribed Image Text:Direction: Solve what is being asked. Follow the directions below; All answers, including values used in the solutions, must be rounded to the nearest two decimal places. Always place a zero before the decimal point for values less than 1 | (example: .25 = 0.25) Add trailing zeros to complete your answer to the 2nd decimal place, if necessary | (examples: 62.7 = 62.70; 123 123.00) ● ● ● For answers with exponents, input the base number up to the 2nd decimal place before placing x10^...(examples: 5.31x10^5; 9.60x10^-4) DO NOT include spaces in between numbers, characters, and decimal points. There is NO NEED to write the UNITS Write your answers before the item Problem 1: A 350-ml buffer solution was prepared by a chemist by mixing 0.135 M CH3COOH and 0.100 M CH3COOK. Accidentally, you added 12 ml of an unlabeled solution to the buffer solution during the experiment. Your groupmate, later on, identified this to be 1.5 M HCI which was mistakenly left unlabeled when she went out to urinate. Compute the following; use the pKb value of 7.62. Atomic weights: K: 39.10 C: 12.01 H: 1.01 59. What is the pH of the original buffer solution? 60. What is the pH of the final buffer solution? CI: 35.45 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? O: 15.99 58. What is the number of moles of CH3COOK which participated in the reaction upon adding 12 mL of 1.5 M HCI? 61. What is the final ratio of the CH3COOH and CH3COOK? 62. What is the change in pH in percentage?
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