x10-5. A student is preparing a pH buffer solution with 1.663 M NH3 solution and (NH₂)₂SO4 solid. Please answer the following questions. A. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815 B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1" if the answer is pH = 4.741 ± 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 + 1, please put down "4" if the answer is pH=9.26±10. Please provider your answer below. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.67 buffer solution? The volume of the buffer solution is 250.0 mL. grams S Please provider your answer below. S (0

x10-5. A student is preparing a pH buffer solution with 1.663 M NH3 solution and (NH₂)₂SO4 solid. Please answer the following questions. A. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815 B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1" if the answer is pH = 4.741 ± 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 + 1, please put down "4" if the answer is pH=9.26±10. Please provider your answer below. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.67 buffer solution? The volume of the buffer solution is 250.0 mL. grams S Please provider your answer below. S (0

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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solution. Methylamine is a weak base with K = 4.4 x 104. What mass of A chemistry graduate student is given 125. mL of a 1.80M methylamine (CH₂NH₂): CH3NH₂Cl should the student dissolve in the CH₂NH₂ solution to turn it into a buffer with pH = 10.95? You may assume that the volume of the solution doesn't change when the CH3NH₂Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. M
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10-1
Aa.51.
Buffer Intensity?
O ACIDS AND BASES Calculating the pH of a buffer A solution is prepared at 25 °c that is initially 0.077M in trimethylamine ((CH3)3N), a weak base with K₁=7.4× 10-4, and 0.50M in trimethylammonium Calculate the pH of the solution. Round your answer chloride ((CH3), NHCI) to 2 decimal places. pH = 1/3 X
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A buffer solution is composed of 1.324 g of KH,PO4 and 4.362 g of Naz HPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)