To a 25.00 mL volumetric flask, a lab technician adds a 0.450 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 0.0829 M KOH. She reaches the endpoint after adding 47.75 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: mol Determine the molar mass of the weak acid. molar mass = g/mol After the technician adds 15.65 mL of the KOH solution, the pH of the mixture is 5.61. Determine the pK, of the weak acid. pKa =
To a 25.00 mL volumetric flask, a lab technician adds a 0.450 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 0.0829 M KOH. She reaches the endpoint after adding 47.75 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: mol Determine the molar mass of the weak acid. molar mass = g/mol After the technician adds 15.65 mL of the KOH solution, the pH of the mixture is 5.61. Determine the pK, of the weak acid. pKa =
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 53QAP: The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The...
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Transcribed Image Text:To a 25.00 mL volumetric flask, a lab technician adds a 0.450 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 0.0829 M KOH. She reaches the endpoint
after adding 47.75 mL of the KOH solution.
Determine the number of moles of the weak acid in the solution.
moles of weak acid:
mol
Determine the molar mass of the weak acid.
molar mass =
g/mol
After the technician adds 15.65 mL of the KOH solution, the pH of the mixture is 5.61. Determine the pKa of the weak acid.
pKa =
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