Table 6. Calculations for percent by mass Sample 2 Sample 3 Sample 1 26.071 28.702 28.207 [1] Mass sample (g) [2] Burette reading of NaOH, initial (mL) 1.91 4.78 1.19 [3] Burette reading of N2OH, final (mL) 17.25 22.13 18.24 17.35 [4] Volume of NaOH, dispensed (mL) 17.05 15.34 [5] Molar concentration of NaOH (part A) 0.1077 [6] Mass of acid in sample (g) [7] Percentage by mass in sample (%)
Table 6. Calculations for percent by mass Sample 2 Sample 3 Sample 1 26.071 28.702 28.207 [1] Mass sample (g) [2] Burette reading of NaOH, initial (mL) 1.91 4.78 1.19 [3] Burette reading of N2OH, final (mL) 17.25 22.13 18.24 17.35 [4] Volume of NaOH, dispensed (mL) 17.05 15.34 [5] Molar concentration of NaOH (part A) 0.1077 [6] Mass of acid in sample (g) [7] Percentage by mass in sample (%)
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with #6 and 7 please. The unknown acid type; H3A, and it's molar mass is 192.140
![**Balanced Chemical Equation for Neutralization of Acid with NaOH**
\( \text{H}_3\text{A} + 3\text{NaOH} \rightarrow \text{Na}_3\text{A} + 3\text{H}_2\text{O} \)
**Table 6: Calculations for Percent by Mass**
| | Sample 1 | Sample 2 | Sample 3 |
|--------------------------------|----------|----------|----------|
| **[1] Mass sample (g)** | 28.207 | 26.071 | 28.702 |
| **[2] Burette reading of NaOH, initial (mL)** | 1.19 | 1.91 | 4.78 |
| **[3] Burette reading of NaOH, final (mL)** | 18.24 | 17.25 | 22.13 |
| **[4] Volume of NaOH, dispensed (mL)** | 17.05 | 15.34 | 17.35 |
| **[5] Molar concentration of NaOH (part A)** | 0.1077 | | |
| **[6] Mass of acid in sample (g)** | | | |
| **[7] Percentage by mass in sample (%)** | | | |
---
**Explanation:**
This table presents the calculations for determining the percent by mass of an acid in different samples, using a neutralization reaction with sodium hydroxide (NaOH).
- **[1] Mass sample (g):** The initial mass of each sample.
- **[2] and [3] Burette readings (mL):** Initial and final readings to measure the volume of NaOH used.
- **[4] Volume of NaOH, dispensed (mL):** The volume of NaOH solution dispensed, calculated as the difference between the final and initial burette readings.
- **[5] Molar concentration of NaOH (part A):** Specifies the concentration of the NaOH solution used in Sample 1.
- **[6] and [7]:** These sections are left blank for students to calculate the mass of acid in each sample and the percentage by mass, respectively.
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Transcribed Image Text:**Balanced Chemical Equation for Neutralization of Acid with NaOH**
\( \text{H}_3\text{A} + 3\text{NaOH} \rightarrow \text{Na}_3\text{A} + 3\text{H}_2\text{O} \)
**Table 6: Calculations for Percent by Mass**
| | Sample 1 | Sample 2 | Sample 3 |
|--------------------------------|----------|----------|----------|
| **[1] Mass sample (g)** | 28.207 | 26.071 | 28.702 |
| **[2] Burette reading of NaOH, initial (mL)** | 1.19 | 1.91 | 4.78 |
| **[3] Burette reading of NaOH, final (mL)** | 18.24 | 17.25 | 22.13 |
| **[4] Volume of NaOH, dispensed (mL)** | 17.05 | 15.34 | 17.35 |
| **[5] Molar concentration of NaOH (part A)** | 0.1077 | | |
| **[6] Mass of acid in sample (g)** | | | |
| **[7] Percentage by mass in sample (%)** | | | |
---
**Explanation:**
This table presents the calculations for determining the percent by mass of an acid in different samples, using a neutralization reaction with sodium hydroxide (NaOH).
- **[1] Mass sample (g):** The initial mass of each sample.
- **[2] and [3] Burette readings (mL):** Initial and final readings to measure the volume of NaOH used.
- **[4] Volume of NaOH, dispensed (mL):** The volume of NaOH solution dispensed, calculated as the difference between the final and initial burette readings.
- **[5] Molar concentration of NaOH (part A):** Specifies the concentration of the NaOH solution used in Sample 1.
- **[6] and [7]:** These sections are left blank for students to calculate the mass of acid in each sample and the percentage by mass, respectively.
This structured
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