A 10.3-g sample of a diprotic acid requires 180.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid. g/mol Submit Answer [References] Try Another Version I item attempt remaining
A 10.3-g sample of a diprotic acid requires 180.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid. g/mol Submit Answer [References] Try Another Version I item attempt remaining
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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![### Example Chemistry Problem: Determining Molar Mass of a Diprotic Acid
**Problem Statement:**
A 10.3 g sample of a diprotic acid requires 180.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.
**Instructions to Answer:**
Given the information provided:
- Mass of the diprotic acid sample: 10.3 g
- Volume of NaOH solution used: 180.5 mL
- Molarity of NaOH solution: 0.750 M
To find the molar mass of the diprotic acid, follow these steps:
1. **Calculate the moles of NaOH used:**
Convert the volume of NaOH solution from milliliters to liters:
\[
180.5 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.1805 \text{ L}
\]
Use the molarity (M) to find the moles of NaOH:
\[
\text{moles of NaOH} = 0.750 \text{ M} \times 0.1805 \text{ L} = 0.135375 \text{ moles of NaOH}
\]
2. **Determine the moles of the diprotic acid neutralized:**
Since the acid is diprotic (H₂A), it reacts with NaOH in a 1:2 ratio. Thus, the moles of H₂A:
\[
\text{moles of H₂A} = \frac{\text{moles of NaOH}}{2} = \frac{0.135375}{2} = 0.0676875 \text{ moles}
\]
3. **Calculate the molar mass of the diprotic acid:**
The molar mass (M) is calculated by dividing the mass of the acid by the number of moles:
\[
M = \frac{\text{mass of H₂A}}{\text{moles of H₂A}} = \frac{10.3 \text{ g}}{0.0676875 \text{ moles}} \approx 152.16 \text{ g/mol}
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Transcribed Image Text:### Example Chemistry Problem: Determining Molar Mass of a Diprotic Acid
**Problem Statement:**
A 10.3 g sample of a diprotic acid requires 180.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.
**Instructions to Answer:**
Given the information provided:
- Mass of the diprotic acid sample: 10.3 g
- Volume of NaOH solution used: 180.5 mL
- Molarity of NaOH solution: 0.750 M
To find the molar mass of the diprotic acid, follow these steps:
1. **Calculate the moles of NaOH used:**
Convert the volume of NaOH solution from milliliters to liters:
\[
180.5 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.1805 \text{ L}
\]
Use the molarity (M) to find the moles of NaOH:
\[
\text{moles of NaOH} = 0.750 \text{ M} \times 0.1805 \text{ L} = 0.135375 \text{ moles of NaOH}
\]
2. **Determine the moles of the diprotic acid neutralized:**
Since the acid is diprotic (H₂A), it reacts with NaOH in a 1:2 ratio. Thus, the moles of H₂A:
\[
\text{moles of H₂A} = \frac{\text{moles of NaOH}}{2} = \frac{0.135375}{2} = 0.0676875 \text{ moles}
\]
3. **Calculate the molar mass of the diprotic acid:**
The molar mass (M) is calculated by dividing the mass of the acid by the number of moles:
\[
M = \frac{\text{mass of H₂A}}{\text{moles of H₂A}} = \frac{10.3 \text{ g}}{0.0676875 \text{ moles}} \approx 152.16 \text{ g/mol}
\
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