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.

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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.
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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