A chemist prepares a solution of silver(II) oxide (AgO) by measuring out 0.00336 μmol of silver(II) oxide into a 300. mL volumetric flask and filling the fl the mark with water. Calculate the concentration in μmol/L of the chemist's silver(II) oxide solution. Round your answer to 3 significant digits. 0 u mol L x10 X S 1/5
A chemist prepares a solution of silver(II) oxide (AgO) by measuring out 0.00336 μmol of silver(II) oxide into a 300. mL volumetric flask and filling the fl the mark with water. Calculate the concentration in μmol/L of the chemist's silver(II) oxide solution. Round your answer to 3 significant digits. 0 u mol L x10 X S 1/5
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
Chapter1: Chemical Foundations
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![**Title: Calculating Concentration of Silver(II) Oxide Solution**
**Introduction:**
A chemist prepares a solution of silver(II) oxide (AgO) by measuring out 0.00336 μmol of silver(II) oxide into a 300 mL volumetric flask, then filling the flask to the mark with water.
**Objective:**
Calculate the concentration in μmol/L of the chemist's silver(II) oxide solution. Round your answer to three significant digits.
**Step-by-Step Calculation:**
1. **Identify Given Values:**
- Amount of silver(II) oxide: 0.00336 μmol
- Volume of solution: 300 mL
2. **Convert Volume from mL to L:**
- \( 300 \text{ mL} = 0.300 \text{ L} \)
3. **Calculate Concentration:**
- \[ \text{Concentration (μmol/L)} = \frac{\text{Amount of silver(II) oxide (μmol)}}{\text{Volume of solution (L)}} \]
- \[ \text{Concentration} = \frac{0.00336 \text{ μmol}}{0.300 \text{ L}} = 0.0112 \text{ μmol/L} \]
**Rounding:**
Round the concentration to three significant digits: \( 0.0112 \text{ μmol/L} \)
**Conclusion:**
The concentration of the chemist’s silver(II) oxide solution is approximately 0.0112 μmol/L.
**Diagram:**
- The image includes an interactive component to input and calculate the concentration:
- A box labeled "μmol/L" represents where the concentration value is entered.
- Icons for multiplication and resetting calculations are provided for user interaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F119fd9ee-0d86-405f-8fbb-1cd17cdf6dea%2F63b5a7c4-84be-476a-b63f-c6a73e06b446%2F9ro996c_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Calculating Concentration of Silver(II) Oxide Solution**
**Introduction:**
A chemist prepares a solution of silver(II) oxide (AgO) by measuring out 0.00336 μmol of silver(II) oxide into a 300 mL volumetric flask, then filling the flask to the mark with water.
**Objective:**
Calculate the concentration in μmol/L of the chemist's silver(II) oxide solution. Round your answer to three significant digits.
**Step-by-Step Calculation:**
1. **Identify Given Values:**
- Amount of silver(II) oxide: 0.00336 μmol
- Volume of solution: 300 mL
2. **Convert Volume from mL to L:**
- \( 300 \text{ mL} = 0.300 \text{ L} \)
3. **Calculate Concentration:**
- \[ \text{Concentration (μmol/L)} = \frac{\text{Amount of silver(II) oxide (μmol)}}{\text{Volume of solution (L)}} \]
- \[ \text{Concentration} = \frac{0.00336 \text{ μmol}}{0.300 \text{ L}} = 0.0112 \text{ μmol/L} \]
**Rounding:**
Round the concentration to three significant digits: \( 0.0112 \text{ μmol/L} \)
**Conclusion:**
The concentration of the chemist’s silver(II) oxide solution is approximately 0.0112 μmol/L.
**Diagram:**
- The image includes an interactive component to input and calculate the concentration:
- A box labeled "μmol/L" represents where the concentration value is entered.
- Icons for multiplication and resetting calculations are provided for user interaction.
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