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A 44.4 mL sample of a 0.300 M solution of NaCN is titrated by 0.100 M HC1, K₁ for CN is 2.0 × 10-5. Calculate the pH of the solution: a. prior to the start of the titration pH b. after the addition of 93.2 mL of 0.100 M HCl PH = c. at the equivalence point pH d. after the addition of 173 mL of 0.100 M HCl pH =

A 44.4 mL sample of a 0.300 M solution of NaCN is titrated by 0.100 M HC1, K₁ for CN is 2.0 × 10-5. Calculate the pH of the solution: a. prior to the start of the titration pH b. after the addition of 93.2 mL of 0.100 M HCl PH = c. at the equivalence point pH d. after the addition of 173 mL of 0.100 M HCl pH =

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 44.4 mL sample of a 0.300 M solution of NaCN is titrated by 0.100 M HC1, K₁ for CN is 2.0 × 10-5. Calculate the pH of the solution: a. prior to the start of the titration pH = b. after the addition of 93.2 mL of 0.100 M HCl pH = c. at the equivalence point pH: d. after the addition of 173 mL of 0.100 M HCl pH:
Transcribed Image Text:A 44.4 mL sample of a 0.300 M solution of NaCN is titrated by 0.100 M HC1, K₁ for CN is 2.0 × 10-5. Calculate the pH of the solution: a. prior to the start of the titration pH = b. after the addition of 93.2 mL of 0.100 M HCl pH = c. at the equivalence point pH: d. after the addition of 173 mL of 0.100 M HCl pH:
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