Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for for pH to 2 decimal places. solution A B C [HO] -6 6.4 X 10 mol/L mol/L 7.6 x 10 8 mol/L PH 0 10.85 0.0 X S ? [H₂O] to to 2 significant digits, and your entries

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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_{
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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