with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after adding 44.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: Determine the molar mass of the weak acid. molar mass= mol pka = g/mol After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pKa of the weak acid.

with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after adding 44.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: Determine the molar mass of the weak acid. molar mass= mol pka = g/mol After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pKa of the weak acid.

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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Question

100%

To a 25.00 mL volumetric flask, a lab technician adds a 0.100 g sample of a weak monoprotic acid, HA, and dilutes to the mark
with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after
adding 44.65 mL of the KOH solution.
Determine the number of moles of the weak acid in the solution.
moles of weak acid:
Determine the molar mass of the weak acid.
molar mass=
pKa
mol
After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pK₁ of the weak acid.
=
g/mol

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