**Determining Bromide Ion Concentration via Precipitation of Silver Bromide** The concentration of bromide ions in a solution can be determined through a precipitation reaction involving silver bromide, as shown in the equation below: \[ \text{Ag}^+ (aq) + \text{Br}^- (aq) \rightarrow \text{AgBr} (s) \] **Problem Statement:** A student discovers that 16.11 mL of 0.7730 M silver nitrate is required to precipitate all of the bromide ions in a 10.00 mL sample of an unknown bromide solution. What is the molarity of the bromide ion in the unknown solution? **Solution Steps:** 1. Determine the moles of silver nitrate used: \[ \text{Moles of } \text{AgNO}_3 = \text{Volume (L)} \times \text{Molarity} = 0.01611 \, \text{L} \times 0.7730 \, \text{M} \] 2. Use the stoichiometry of the reaction to find moles of bromide ion, which is in a 1:1 ratio with silver ions. 3. Calculate the molarity of the bromide ion in the unknown solution: \[ \text{Molarity of } \text{Br}^- = \frac{\text{Moles of } \text{Br}^-}{\text{Volume of unknown solution (L)}} = \frac{\text{Moles of } \text{AgNO}_3}{0.01000 \, \text{L}} \] **Interactive Components:** - Input box to enter the calculated molarity. - Buttons: "Submit Answer" and "Retry Entire Group". - Notification: "9 more group attempts remaining". **Note:** Ensure all calculations follow proper unit conversions and stoichiometry principles for accurate results.
**Determining Bromide Ion Concentration via Precipitation of Silver Bromide** The concentration of bromide ions in a solution can be determined through a precipitation reaction involving silver bromide, as shown in the equation below: \[ \text{Ag}^+ (aq) + \text{Br}^- (aq) \rightarrow \text{AgBr} (s) \] **Problem Statement:** A student discovers that 16.11 mL of 0.7730 M silver nitrate is required to precipitate all of the bromide ions in a 10.00 mL sample of an unknown bromide solution. What is the molarity of the bromide ion in the unknown solution? **Solution Steps:** 1. Determine the moles of silver nitrate used: \[ \text{Moles of } \text{AgNO}_3 = \text{Volume (L)} \times \text{Molarity} = 0.01611 \, \text{L} \times 0.7730 \, \text{M} \] 2. Use the stoichiometry of the reaction to find moles of bromide ion, which is in a 1:1 ratio with silver ions. 3. Calculate the molarity of the bromide ion in the unknown solution: \[ \text{Molarity of } \text{Br}^- = \frac{\text{Moles of } \text{Br}^-}{\text{Volume of unknown solution (L)}} = \frac{\text{Moles of } \text{AgNO}_3}{0.01000 \, \text{L}} \] **Interactive Components:** - Input box to enter the calculated molarity. - Buttons: "Submit Answer" and "Retry Entire Group". - Notification: "9 more group attempts remaining". **Note:** Ensure all calculations follow proper unit conversions and stoichiometry principles for accurate results.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Determining Bromide Ion Concentration via Precipitation of Silver Bromide**
The concentration of bromide ions in a solution can be determined through a precipitation reaction involving silver bromide, as shown in the equation below:
\[ \text{Ag}^+ (aq) + \text{Br}^- (aq) \rightarrow \text{AgBr} (s) \]
**Problem Statement:**
A student discovers that 16.11 mL of 0.7730 M silver nitrate is required to precipitate all of the bromide ions in a 10.00 mL sample of an unknown bromide solution. What is the molarity of the bromide ion in the unknown solution?
**Solution Steps:**
1. Determine the moles of silver nitrate used:
\[
\text{Moles of } \text{AgNO}_3 = \text{Volume (L)} \times \text{Molarity} = 0.01611 \, \text{L} \times 0.7730 \, \text{M}
\]
2. Use the stoichiometry of the reaction to find moles of bromide ion, which is in a 1:1 ratio with silver ions.
3. Calculate the molarity of the bromide ion in the unknown solution:
\[
\text{Molarity of } \text{Br}^- = \frac{\text{Moles of } \text{Br}^-}{\text{Volume of unknown solution (L)}} = \frac{\text{Moles of } \text{AgNO}_3}{0.01000 \, \text{L}}
\]
**Interactive Components:**
- Input box to enter the calculated molarity.
- Buttons: "Submit Answer" and "Retry Entire Group".
- Notification: "9 more group attempts remaining".
**Note:**
Ensure all calculations follow proper unit conversions and stoichiometry principles for accurate results.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F144ac4d4-58bf-4a39-b1bc-5bb4c77f8379%2F9d922745-5424-4bcf-8b95-01ed03ad773b%2Fag9j1ap.jpeg&w=3840&q=75)
Transcribed Image Text:**Determining Bromide Ion Concentration via Precipitation of Silver Bromide**
The concentration of bromide ions in a solution can be determined through a precipitation reaction involving silver bromide, as shown in the equation below:
\[ \text{Ag}^+ (aq) + \text{Br}^- (aq) \rightarrow \text{AgBr} (s) \]
**Problem Statement:**
A student discovers that 16.11 mL of 0.7730 M silver nitrate is required to precipitate all of the bromide ions in a 10.00 mL sample of an unknown bromide solution. What is the molarity of the bromide ion in the unknown solution?
**Solution Steps:**
1. Determine the moles of silver nitrate used:
\[
\text{Moles of } \text{AgNO}_3 = \text{Volume (L)} \times \text{Molarity} = 0.01611 \, \text{L} \times 0.7730 \, \text{M}
\]
2. Use the stoichiometry of the reaction to find moles of bromide ion, which is in a 1:1 ratio with silver ions.
3. Calculate the molarity of the bromide ion in the unknown solution:
\[
\text{Molarity of } \text{Br}^- = \frac{\text{Moles of } \text{Br}^-}{\text{Volume of unknown solution (L)}} = \frac{\text{Moles of } \text{AgNO}_3}{0.01000 \, \text{L}}
\]
**Interactive Components:**
- Input box to enter the calculated molarity.
- Buttons: "Submit Answer" and "Retry Entire Group".
- Notification: "9 more group attempts remaining".
**Note:**
Ensure all calculations follow proper unit conversions and stoichiometry principles for accurate results.
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