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?

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**Titration Exercises for Determining Concentration and Molecular Mass**

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 endpoint. 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 endpoint. What is the molecular mass of the acid?

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**Explanation:**

This set of problems involves using titration data to calculate various unknowns. Each problem involves an acid being neutralized by a sodium hydroxide (NaOH) solution, where the volume and molarity of the NaOH solution are known. 

- In **Problem 1**, you are tasked with finding the concentration of sulfuric acid. Using the volume and molarity of the NaOH solution, you can determine the moles of NaOH added and use the stoichiometry of the acid-base reaction to find the concentration of H₂SO₄.

- **Problem 2** requires calculating both the molarity and mass percent of acetic acid in vinegar. Here, you'll use the volume of the NaOH solution to find moles of acetic acid and convert that information to determine both its molarity in the solution and its percentage by mass.

- For **Problem 3**, you'll find the molecular mass of an unknown monoprotic acid using the volume and molarity of NaOH titrant used to neutralize a known mass of the acid sample. The relationship between the moles of NaOH and the monoprotic acid will allow for the calculation of molecular weight.

These exercises are essential for understanding titration techniques and applying stoichiometry in real-world laboratory settings.
Transcribed Image Text:**Titration Exercises for Determining Concentration and Molecular Mass** 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 endpoint. 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 endpoint. What is the molecular mass of the acid? --- **Explanation:** This set of problems involves using titration data to calculate various unknowns. Each problem involves an acid being neutralized by a sodium hydroxide (NaOH) solution, where the volume and molarity of the NaOH solution are known. - In **Problem 1**, you are tasked with finding the concentration of sulfuric acid. Using the volume and molarity of the NaOH solution, you can determine the moles of NaOH added and use the stoichiometry of the acid-base reaction to find the concentration of H₂SO₄. - **Problem 2** requires calculating both the molarity and mass percent of acetic acid in vinegar. Here, you'll use the volume of the NaOH solution to find moles of acetic acid and convert that information to determine both its molarity in the solution and its percentage by mass. - For **Problem 3**, you'll find the molecular mass of an unknown monoprotic acid using the volume and molarity of NaOH titrant used to neutralize a known mass of the acid sample. The relationship between the moles of NaOH and the monoprotic acid will allow for the calculation of molecular weight. These exercises are essential for understanding titration techniques and applying stoichiometry in real-world laboratory settings.
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