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

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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.
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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