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 placingx10^...(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 UNITSWrite your answers before the item Problem 2: Your facilitator asked you to prepare 450 mL of a buffer solution having a pH of 10.45 composed ofAmmonia and Ammonium Chloride. Considering a final salt concentration of 0.123 M, determine the following.pkg = 3.69Atomic weights:N: 14.01H: 1.01CI: 35.45O: 15.9963. What is the volume of Ammonia, in mL, needed to prepare the buffer solution?64. What is the ratio of Ammonium chloride and Ammonia?65. What is the weight, in grams, of Ammonium chloride?66. What is the concentration of the Hydroxyl ion?67. Determine the kb value.68. Determine the mmoles of the salt present in the solution.

Given: Salt concentration/conjugate base = 0.123 M Volume of buffer solution= 450 ml…

Problem 2: Your facilitator asked you to prepare 450 mL of a buffer solution having a pH of 10.45 composed of Ammonia and Ammonium Chloride. Considering a final salt concentration of 0.123 M, determine the following. pkg = 3.69 Atomic weights: N: 14.01 H: 1.01 CI: 35.45 O: 15.99 63. What is the volume of Ammonia, in mL, needed to prepare the buffer solution? 64. What is the ratio of Ammonium chloride and Ammonia? 65. What is the weight, in grams, of Ammonium chloride? 66. What is the concentration of the Hydroxyl ion? 67. Determine the kb value. 68. Determine the mmoles of the salt present in the solution.

Problem 2: Your facilitator asked you to prepare 450 mL of a buffer solution having a pH of 10.45 composed of Ammonia and Ammonium Chloride. Considering a final salt concentration of 0.123 M, determine the following. pkg = 3.69 Atomic weights: N: 14.01 H: 1.01 CI: 35.45 O: 15.99 63. What is the volume of Ammonia, in mL, needed to prepare the buffer solution? 64. What is the ratio of Ammonium chloride and Ammonia? 65. What is the weight, in grams, of Ammonium chloride? 66. What is the concentration of the Hydroxyl ion? 67. Determine the kb value. 68. Determine the mmoles of the salt present in the solution.

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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ANSWER B= 4.99
4
Hh.122.
Is the response below correct, I would belive that pOH = – log (12.7) = 1.103 would be -1.103 Please let me know, as that would change the pH of the final solution Step 1 NaOH ---> Na+ + OH– [NaOH] = 12.7 M = [OH–] So, pOH = – log [OH–] pOH = – log (12.7) = 1.103 Step 2 Since, we know that ; pH + pOH = 14 On substituting the values into it, we get ; pH = 14 – pOH = 14 – 1.103 = 12.897 ≈ 12.9 Hence, The pH will be 12.9.
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