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

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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}
   \
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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