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?
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?
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 of an Unknown Monoprotic Acid**
**Problem Statement:**
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?
**Analysis and Explanation:**
In this problem, you are tasked with calculating the molecular mass of an unknown monoprotic acid. A monoprotic acid is an acid that donates one proton (H⁺ ion) per molecule in a reaction.
To find the molecular mass, follow these steps:
1. **Determine Moles of NaOH Used:**
- Use the volume and molarity of the NaOH solution to calculate the number of moles used:
\[
\text{Moles of NaOH} = \text{Volume (L)} \times \text{Molarity (mol/L)}
\]
2. **Equivalence with Acid:**
- Since it’s a monoprotic acid, the moles of NaOH will be equal to the moles of the acid at the endpoint.
3. **Calculate Molecular Mass:**
- The molecular mass (M) of the acid can be calculated using the formula:
\[
M = \frac{\text{Mass of Acid (g)}}{\text{Moles of Acid}}
\]
By applying these principles, you can determine the molecular mass. Remember to convert all measurements to appropriate units (e.g., milliliters to liters) before calculations. Understanding this process is essential for tasks involving titration and stoichiometry.
**Note:**
Always ensure precision in measurements and calculations for accurate results.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb176c34c-6eec-4a55-826b-97aceef00360%2F6a3b577e-f271-4a63-8d1e-eb3171ace713%2Fhggbjef.jpeg&w=3840&q=75)
Transcribed Image Text:**Titration of an Unknown Monoprotic Acid**
**Problem Statement:**
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?
**Analysis and Explanation:**
In this problem, you are tasked with calculating the molecular mass of an unknown monoprotic acid. A monoprotic acid is an acid that donates one proton (H⁺ ion) per molecule in a reaction.
To find the molecular mass, follow these steps:
1. **Determine Moles of NaOH Used:**
- Use the volume and molarity of the NaOH solution to calculate the number of moles used:
\[
\text{Moles of NaOH} = \text{Volume (L)} \times \text{Molarity (mol/L)}
\]
2. **Equivalence with Acid:**
- Since it’s a monoprotic acid, the moles of NaOH will be equal to the moles of the acid at the endpoint.
3. **Calculate Molecular Mass:**
- The molecular mass (M) of the acid can be calculated using the formula:
\[
M = \frac{\text{Mass of Acid (g)}}{\text{Moles of Acid}}
\]
By applying these principles, you can determine the molecular mass. Remember to convert all measurements to appropriate units (e.g., milliliters to liters) before calculations. Understanding this process is essential for tasks involving titration and stoichiometry.
**Note:**
Always ensure precision in measurements and calculations for accurate results.
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