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**Titration Problems and Solutions** 1. **Problem 1:** - The titration of 25.00 mL of a sulfuric acid solution of unknown concentration requires 31.22 mL of a 0.1234 M NaOH solution. What is the concentration of the sulfuric acid solution? 2. **Problem 2:** - 10.00 mL of vinegar (mass = 10.05 g) requires 16.28 mL of 0.5120 M NaOH to reach the end point. Calculate the molarity and mass percent of the acetic acid in the vinegar. 3. **Problem 3:** - A 0.1936 g sample of an unknown monoprotic acid requires 15.56 mL of 0.1020 M NaOH solution to reach the end point. What is the molecular mass of the acid? *Note: This exercise is intended for educational purposes and focuses on applying titration concepts to calculate unknown concentrations, molarity, mass percent, and molecular mass in various chemical scenarios.*

**Titration Problems and Solutions** 1. **Problem 1:** - The titration of 25.00 mL of a sulfuric acid solution of unknown concentration requires 31.22 mL of a 0.1234 M NaOH solution. What is the concentration of the sulfuric acid solution? 2. **Problem 2:** - 10.00 mL of vinegar (mass = 10.05 g) requires 16.28 mL of 0.5120 M NaOH to reach the end point. Calculate the molarity and mass percent of the acetic acid in the vinegar. 3. **Problem 3:** - A 0.1936 g sample of an unknown monoprotic acid requires 15.56 mL of 0.1020 M NaOH solution to reach the end point. What is the molecular mass of the acid? *Note: This exercise is intended for educational purposes and focuses on applying titration concepts to calculate unknown concentrations, molarity, mass percent, and molecular mass in various chemical scenarios.*

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
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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**Titration Problems and Solutions** 1. **Problem 1:** - The titration of 25.00 mL of a sulfuric acid solution of unknown concentration requires 31.22 mL of a 0.1234 M NaOH solution. What is the concentration of the sulfuric acid solution? 2. **Problem 2:** - 10.00 mL of vinegar (mass = 10.05 g) requires 16.28 mL of 0.5120 M NaOH to reach the end point. Calculate the molarity and mass percent of the acetic acid in the vinegar. 3. **Problem 3:** - A 0.1936 g sample of an unknown monoprotic acid requires 15.56 mL of 0.1020 M NaOH solution to reach the end point. What is the molecular mass of the acid? *Note: This exercise is intended for educational purposes and focuses on applying titration concepts to calculate unknown concentrations, molarity, mass percent, and molecular mass in various chemical scenarios.*
Transcribed Image Text:**Titration Problems and Solutions** 1. **Problem 1:** - The titration of 25.00 mL of a sulfuric acid solution of unknown concentration requires 31.22 mL of a 0.1234 M NaOH solution. What is the concentration of the sulfuric acid solution? 2. **Problem 2:** - 10.00 mL of vinegar (mass = 10.05 g) requires 16.28 mL of 0.5120 M NaOH to reach the end point. Calculate the molarity and mass percent of the acetic acid in the vinegar. 3. **Problem 3:** - A 0.1936 g sample of an unknown monoprotic acid requires 15.56 mL of 0.1020 M NaOH solution to reach the end point. What is the molecular mass of the acid? *Note: This exercise is intended for educational purposes and focuses on applying titration concepts to calculate unknown concentrations, molarity, mass percent, and molecular mass in various chemical scenarios.*
Expert Solution
Step 1

Hi, as you have posted multiple questions and also not mentioned which one you want us to solve for you. If you want the rest questions to be solved then please resubmit the question and also mention the number of questions.

  • Volume of H2SO4 = 25 mL
  • Volume of NaOH = 31.22 mL
  • Molarity of NaOH = 0.1234 M
Step 2

The balanced reaction is –

2NaOH + H2SO4 →Na2SO4 +2H2O

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