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

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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part A 1. Concentration of Known NiCl2 Stock Solution ___500________ mM Tube Number Blank #1 #2 #3 #4 #5 2. Volume of Known NiCl2 Stock Solution Pipetted Into Tube 0.00 mL 1.50 mL 3.00 mL 4.50 mL 6.00 mL 7.50 mL 3. Volume of Distilled Water Pipetted Into Tube 11.00 mL 9.50 mL 8.00 mL 6.50 mL 5.00 mL 3.50 mL 4. Total Volume of Solution In Tube 11.00 mL 11.00 mL 11.00 mL 11.00 mL 11.00 mL 11.00 mL 5. Diluted Concentration of NiCl2 In Tube ----------- 68.2 mn 136mn 204mn 273mn 341mn 1. Equation for the Best-Fit Straight Line Y=3822x+4.7446 2. Absorbance at λmax for Diluted Unknown 0.87 3. Concentration of NiCl2 in Diluted Unknown 25.693 mM Determine the dilution factor for your diluted unknown U1 based on how you prepared the solutions in Part A. Record this on your report sheet in Part D #4.
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