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A solution is prepared by dissolving 0.25 mol of lactic acid and 0.23 mol of sodium lactate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. What is the pH of the solution after the NaOH was added? The K₂ of lactic acid is 1.4 x 10-4. A 3.91 4.00 O 3.63 3.70

A solution is prepared by dissolving 0.25 mol of lactic acid and 0.23 mol of sodium lactate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. What is the pH of the solution after the NaOH was added? The K₂ of lactic acid is 1.4 x 10-4. A 3.91 4.00 O 3.63 3.70

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A solution is prepared by dissolving 0.25 mol of lactic acid and 0.23 mol of sodium lactate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. What is the pH of the solution after the NaOH was added? The K₂ of lactic acid is 1.4 x 10-4. A O 3.91 4.00 O 3.63 O 3.70
Transcribed Image Text:A solution is prepared by dissolving 0.25 mol of lactic acid and 0.23 mol of sodium lactate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. What is the pH of the solution after the NaOH was added? The K₂ of lactic acid is 1.4 x 10-4. A O 3.91 4.00 O 3.63 O 3.70
A 40.00 mL sample of 0.200 M HX is titrated with 0.200 M NaOH. Not surprisingly, it takes 40.00 mL of the NaOH to reach the equivalence point. Determine the pH of the solution the equivalence point. The Ka of HX is 1.0 x 10-9. B 2.85 O 3.00 O 11.15 5.00 O 11.00
Transcribed Image Text:A 40.00 mL sample of 0.200 M HX is titrated with 0.200 M NaOH. Not surprisingly, it takes 40.00 mL of the NaOH to reach the equivalence point. Determine the pH of the solution the equivalence point. The Ka of HX is 1.0 x 10-9. B 2.85 O 3.00 O 11.15 5.00 O 11.00
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