QUESTION 1Sodium bicarbonate (NaHCO3) dissolves in water by the following reaction:NaHCO3 (s) - Na* (aq) + HCO3 (aq)Ke = 1.3When dissolved in 100 ml of pure water, equilibrium is achieved when 9.6 g NaHCO3 is added. I then try to dissolve NaHCO3 in other aqueous solutions. Which solution will achieve equilibrium with the leastamount of NaHCO3 added?O 1.0 M NaClO 1.0 M KCIO 1.0 M KIQUESTION 2I want to make a pH buffer with a pH of 9.5.From the following given pka and pkh values, which mixture would be best to do so?(Henderson-Hasselbalch equation: pH = pka + log([base)[acid]))Benzoic acid (CGH5COOH): pka = 4.19Pyridine (C5H5N): pKb = 8.77Ammonia (NH3): pkh = 4.751.1 M C5H5N and 0.20 M C5H5NH*O 0.60 M C5H5NO 0.50 M C6H5COOH and 1.0 M C6H5C00.80 M NH3 and 0.45 M NH4+

Answered: Image /qna-images/answer/3f9c1a8d-d1d9-43ce-95e2-6eab21874947.jpg

QUESTION 1 Sodium bicarbonate (NaHCO3) dissolves in water by the following reaction: NaHCO3 (s) + Na* (aq) + HCO3 (aq) K = 1.3 When dissolved in 100 ml of pure water, equilibrium is achieved when 9.6 g NaHCO3 is added. I then try to dissolve NaHCO3 in other aqueous solutions. Which solution will achieve equilibrium with the least amount of NaHCOz added? O 1.0 M NaCI O 1.0 M KCI O 1.0 M KI QUESTION 2 I want to make a pH buffer with a pH of 9.5. From the following given pka and pkh values, which mixture would be best to do so? (Henderson-Hasselbalch equation: pH = pka + log([base)[acid])) Benzoic acid (C6H5COOH): pKka = 4.19 Pyridine (C5H5N): pKh = 8.77 Ammonia (NH3): pKp = 4.75 1.1 M C5H5N and 0.20 M C5H5NH* O 0.60 M C5H5N 0.50 M C6H5COOH and 1.0 M C6H5C" 0.80 M NH3 and 0.45 M NHA+

QUESTION 1 Sodium bicarbonate (NaHCO3) dissolves in water by the following reaction: NaHCO3 (s) + Na* (aq) + HCO3 (aq) K = 1.3 When dissolved in 100 ml of pure water, equilibrium is achieved when 9.6 g NaHCO3 is added. I then try to dissolve NaHCO3 in other aqueous solutions. Which solution will achieve equilibrium with the least amount of NaHCOz added? O 1.0 M NaCI O 1.0 M KCI O 1.0 M KI QUESTION 2 I want to make a pH buffer with a pH of 9.5. From the following given pka and pkh values, which mixture would be best to do so? (Henderson-Hasselbalch equation: pH = pka + log([base)[acid])) Benzoic acid (C6H5COOH): pKka = 4.19 Pyridine (C5H5N): pKh = 8.77 Ammonia (NH3): pKp = 4.75 1.1 M C5H5N and 0.20 M C5H5NH* O 0.60 M C5H5N 0.50 M C6H5COOH and 1.0 M C6H5C" 0.80 M NH3 and 0.45 M NHA+

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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