The solubility of AgBrO3 in water at 25 °C is measured to be 1.7 L Round your answer to 2 significant digits. . Use this information to calculate K for AgBrO3.
The solubility of AgBrO3 in water at 25 °C is measured to be 1.7 L Round your answer to 2 significant digits. . Use this information to calculate K for AgBrO3.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![### Solubility and Ksp Calculation
**Problem:**
The solubility of AgBrO₃ in water at 25 °C is measured to be 1.7 g/L. Use this information to calculate the Ksp (solubility product constant) for AgBrO₃.
Round your answer to 2 significant digits.
#### Solution:
1. **Convert solubility from grams per liter to moles per liter:**
- Molar mass of AgBrO₃ = Silver (Ag) + Bromine (Br) + 3 × Oxygen (O)
- Calculate the molar mass using atomic masses: Ag = 107.87 g/mol, Br = 79.90 g/mol, O = 16.00 g/mol.
2. **Calculate concentration in moles per liter:**
- Use the formula:
\[
\text{Concentration (mol/L)} = \frac{\text{Solubility (g/L)}}{\text{Molar mass (g/mol)}}
\]
3. **Determine the Ksp expression:**
For the dissolution of AgBrO₃:
\[
\text{AgBrO}_3(s) \leftrightarrow \text{Ag}^+(aq) + \text{BrO}_3^-(aq)
\]
4. **Calculate Ksp:**
\[
K_{sp} = [\text{Ag}^+][\text{BrO}_3^-]
\]
Since both ions are produced in a 1:1 ratio:
\[
K_{sp} = (S)^2
\]
where \( S \) is the molar solubility of AgBrO₃.
5. **Substitute the concentration found earlier into the equation and calculate Ksp.**
- **Input Box:**
- An input box is provided for entering the calculated Ksp value.
- **Interface Elements:**
- Contains buttons like "Explanation" and "Check" to review or verify the answer.
This problem requires understanding of solubility, molar mass calculations, and equilibrium concepts to solve for Ksp.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcef3f1b2-56cd-4f45-949e-fc7a38ef994c%2F0182a305-850a-4936-9dd6-3ab936b8623e%2F2d66a1c_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Solubility and Ksp Calculation
**Problem:**
The solubility of AgBrO₃ in water at 25 °C is measured to be 1.7 g/L. Use this information to calculate the Ksp (solubility product constant) for AgBrO₃.
Round your answer to 2 significant digits.
#### Solution:
1. **Convert solubility from grams per liter to moles per liter:**
- Molar mass of AgBrO₃ = Silver (Ag) + Bromine (Br) + 3 × Oxygen (O)
- Calculate the molar mass using atomic masses: Ag = 107.87 g/mol, Br = 79.90 g/mol, O = 16.00 g/mol.
2. **Calculate concentration in moles per liter:**
- Use the formula:
\[
\text{Concentration (mol/L)} = \frac{\text{Solubility (g/L)}}{\text{Molar mass (g/mol)}}
\]
3. **Determine the Ksp expression:**
For the dissolution of AgBrO₃:
\[
\text{AgBrO}_3(s) \leftrightarrow \text{Ag}^+(aq) + \text{BrO}_3^-(aq)
\]
4. **Calculate Ksp:**
\[
K_{sp} = [\text{Ag}^+][\text{BrO}_3^-]
\]
Since both ions are produced in a 1:1 ratio:
\[
K_{sp} = (S)^2
\]
where \( S \) is the molar solubility of AgBrO₃.
5. **Substitute the concentration found earlier into the equation and calculate Ksp.**
- **Input Box:**
- An input box is provided for entering the calculated Ksp value.
- **Interface Elements:**
- Contains buttons like "Explanation" and "Check" to review or verify the answer.
This problem requires understanding of solubility, molar mass calculations, and equilibrium concepts to solve for Ksp.
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