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You need a buffer with a pH of 3. The total volume of the buffer must equal 100.00 mL and the final concentration of the acid buffer component must equal 0.150 M. After searching the stockroom, you find the following acids: • Aqueous formic acid, 2.00M concentration, Ka = 1.8x10 %3D • TRIS-HCI, solid acid with a molecular weight of 157.60 g/mol, Ka =8.5x10 • Boric acid, solid acid with a molecular weight of 61.83 g/mol, Ka = 5.8x1010 All three acids can be converted to their respective conjugate bases using 1.00 M NAOH. a. Which buffer system will you use? (Circle one.) Why? Formic acid (HCO,H)/ formate (HCO2') TRISH+/TRIS Boric acid (H;B0;)/dihydrogen borate (H,BO;) Why? b. How many moles of the acid component should be in 100 mL of the buffer solution in order to obtain an acid concentration of0.150 M?

You need a buffer with a pH of 3. The total volume of the buffer must equal 100.00 mL and the final concentration of the acid buffer component must equal 0.150 M. After searching the stockroom, you find the following acids: • Aqueous formic acid, 2.00M concentration, Ka = 1.8x10 %3D • TRIS-HCI, solid acid with a molecular weight of 157.60 g/mol, Ka =8.5x10 • Boric acid, solid acid with a molecular weight of 61.83 g/mol, Ka = 5.8x1010 All three acids can be converted to their respective conjugate bases using 1.00 M NAOH. a. Which buffer system will you use? (Circle one.) Why? Formic acid (HCO,H)/ formate (HCO2') TRISH+/TRIS Boric acid (H;B0;)/dihydrogen borate (H,BO;) Why? b. How many moles of the acid component should be in 100 mL of the buffer solution in order to obtain an acid concentration of0.150 M?

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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You need a buffer with a pH of 3. 6 The total volume of the buffer must equal 100.00 mL and the final concentration of the acid buffer component must equal 0.150 M. After searching the stockroom, you find the following acids: • Aqueous formic acid, 2.00M concentration, Ka = 1.8x104 %3D • TRIS-HCI, solid acid with a molecular weight of 157.60 g/mol, Ka =8.5x10" • Boric acid, solid acid with a molecular weight of 61.83 g/mol, Ka = 5.8x1010 All three acids can be converted to their respective conjugate bases using 1.00 M NAOH. a. Which buffer system will you use? (Circle one.) Why? • Formic acid (HCO2H)/ formate (HCO2) • TRISH+/TRIS • Boric acid (H;BO;)/dihydrogen borate (H2BO3) Why? b. How many moles of the acid component should be in 100 mL of the buffer solution in order to obtain an acid concentration of 0.150 M?
Transcribed Image Text:You need a buffer with a pH of 3. 6 The total volume of the buffer must equal 100.00 mL and the final concentration of the acid buffer component must equal 0.150 M. After searching the stockroom, you find the following acids: • Aqueous formic acid, 2.00M concentration, Ka = 1.8x104 %3D • TRIS-HCI, solid acid with a molecular weight of 157.60 g/mol, Ka =8.5x10" • Boric acid, solid acid with a molecular weight of 61.83 g/mol, Ka = 5.8x1010 All three acids can be converted to their respective conjugate bases using 1.00 M NAOH. a. Which buffer system will you use? (Circle one.) Why? • Formic acid (HCO2H)/ formate (HCO2) • TRISH+/TRIS • Boric acid (H;BO;)/dihydrogen borate (H2BO3) Why? b. How many moles of the acid component should be in 100 mL of the buffer solution in order to obtain an acid concentration of 0.150 M?
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