Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Acids and Bases: Interconverting pH and Hydronium Ion Concentration
#### Interconverting pH and Hydronium Ion Concentration
Each row of the table below describes an aqueous solution at about 25 °C.
**Task:** Complete the table. Fill in any missing entries in the second and third columns. Round your entries for \([H_3O^+]\) to 2 significant digits and your entries for pH to 2 decimal places.
<table>
<tr>
<th>Solution</th>
<th>\([\text{H}_3\text{O}^+]\) (mol/L)</th>
<th>pH</th>
</tr>
<tr>
<td>A</td>
<td>6.4 × 10<sup>−6</sup> mol/L</td>
<td></td>
</tr>
<tr>
<td>B</td>
<td></td>
<td>10.85</td>
</tr>
<tr>
<td>C</td>
<td>7.6 × 10<sup>−8</sup> mol/L</td>
<td></td>
</tr>
</table>
#### Explanation
To convert between pH and \([\text{H}_3\text{O}^+]\), use the following equations:
- **pH to \([\text{H}_3\text{O}^+]\):** \([\text{H}_3\text{O}^+] = 10^{-\text{pH}}\)
- **\([\text{H}_3\text{O}^+]\) to pH:** \(\text{pH} = -\log_{10} [\text{H}_3\text{O}^+]\)
Note: Round your entries for \([\text{H}_3\text{O}^+]\) to 2 significant digits and your entries for pH to 2 decimal places.
#### Example Calculation
1. For Solution A:
- Given \([\text{H}_3\text{O}^+]\) = 6.4 × 10<sup>−6</sup> mol/L
- pH = \(-\log_{](https://content.bartleby.com/qna-images/question/e361a5c2-e3a6-4cd8-bee8-5dcb720cb10b/4b7b7d5e-aac9-4165-a884-e0f9ffa82efa/spqlxj8_processed.jpeg)
Transcribed Image Text:### Acids and Bases: Interconverting pH and Hydronium Ion Concentration
#### Interconverting pH and Hydronium Ion Concentration
Each row of the table below describes an aqueous solution at about 25 °C.
**Task:** Complete the table. Fill in any missing entries in the second and third columns. Round your entries for \([H_3O^+]\) to 2 significant digits and your entries for pH to 2 decimal places.
<table>
<tr>
<th>Solution</th>
<th>\([\text{H}_3\text{O}^+]\) (mol/L)</th>
<th>pH</th>
</tr>
<tr>
<td>A</td>
<td>6.4 × 10<sup>−6</sup> mol/L</td>
<td></td>
</tr>
<tr>
<td>B</td>
<td></td>
<td>10.85</td>
</tr>
<tr>
<td>C</td>
<td>7.6 × 10<sup>−8</sup> mol/L</td>
<td></td>
</tr>
</table>
#### Explanation
To convert between pH and \([\text{H}_3\text{O}^+]\), use the following equations:
- **pH to \([\text{H}_3\text{O}^+]\):** \([\text{H}_3\text{O}^+] = 10^{-\text{pH}}\)
- **\([\text{H}_3\text{O}^+]\) to pH:** \(\text{pH} = -\log_{10} [\text{H}_3\text{O}^+]\)
Note: Round your entries for \([\text{H}_3\text{O}^+]\) to 2 significant digits and your entries for pH to 2 decimal places.
#### Example Calculation
1. For Solution A:
- Given \([\text{H}_3\text{O}^+]\) = 6.4 × 10<sup>−6</sup> mol/L
- pH = \(-\log_{
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