EXPERIMENT Determination of Molecular weight: Approximately 0.3 grams of unknown acid is dissolved in 70.0 mL deionized water. The unknown acid solution is then titrated with 0.123 M NaOH (aq). • Initial volume of NaOH in the burette = 50 mL • Final volume of NaOH in the burette = 32 mL • Volume of NaOH used to complete the titration = • Number of moles of NaOH added= 13 135.50 g/mol • Number of moles of unknown acid present = MOLECULAR WEIGHT OF UNKNOWN ACID = Determination of pKa of the weak acid: 9,93

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...
icon
Related questions
Question
CHARACTERIZATION OF A WEAK ACID
In this experiment, we shall perform a titration of an
unknown weak acid (HX(aq)) with NaOH (aq) a strong base.
The net ionic equation of the titration reaction is:
HX(aq) + OH(aq) à H,O(I) + X(aq)
The identity of the unknown can be determined by
comparing its experimental molecular weight and pKa to the
molecular weights and pKa of the weak acids shown in the
table I.
EXPERIMENT
Determination of Molecular weight:
Approximately 0.3 grams of unknown acid is dissolved in
70.0 mL deionized water. The unknown acid solution is then
titrated with 0.123 M NaOH (aq).
50
• Initial volume of NaOH in the burette =
mL
32
• Final volume of NaOH in the burette =
mL
• Volume of NaOH used to complete the titration =
Number of moles of NaOH added = 13
135.50 g/mol
• Number of moles of unknown acid present
MOLECULAR WEIGHT OF UNKNOWN ACID =
Determination of pKa of the weak acid: 9,93
Transcribed Image Text:CHARACTERIZATION OF A WEAK ACID In this experiment, we shall perform a titration of an unknown weak acid (HX(aq)) with NaOH (aq) a strong base. The net ionic equation of the titration reaction is: HX(aq) + OH(aq) à H,O(I) + X(aq) The identity of the unknown can be determined by comparing its experimental molecular weight and pKa to the molecular weights and pKa of the weak acids shown in the table I. EXPERIMENT Determination of Molecular weight: Approximately 0.3 grams of unknown acid is dissolved in 70.0 mL deionized water. The unknown acid solution is then titrated with 0.123 M NaOH (aq). 50 • Initial volume of NaOH in the burette = mL 32 • Final volume of NaOH in the burette = mL • Volume of NaOH used to complete the titration = Number of moles of NaOH added = 13 135.50 g/mol • Number of moles of unknown acid present MOLECULAR WEIGHT OF UNKNOWN ACID = Determination of pKa of the weak acid: 9,93
Expert Solution
steps

Step by step

Solved in 4 steps

Blurred answer
Knowledge Booster
Analytical Processes
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY