A 1.384 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES¬K*, MW = 220.29 g/mol) is dissolved in 60.62 mL of water.To the solution, 29.89 mL of HCl is added, resulting in a pH of 6.50. Calculate the concentration of the HCl solution. The pK, of ACES is 6.85. [HCl] = .072 M

A 1.384 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES¬K*, MW = 220.29 g/mol) is dissolved in 60.62 mL of water.To the solution, 29.89 mL of HCl is added, resulting in a pH of 6.50. Calculate the concentration of the HCl solution. The pK, of ACES is 6.85. [HCl] = .072 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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

A 1.384 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES K+, MW = 220.29 g/mol)
dissolved in 60.62 mL of water.To the solution, 29.89 mL of HCl is added, resulting in a pH of 6.50. Calculate the
concentration of the HCl solution. The pKa of ACES is 6.85.
[HCI]
.072
M

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