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The question in the image asks to calculate the mass (in micrograms) of zinc oxalate (\( \text{ZnC}_2\text{O}_4 \)) in a solution. The key information provided is:

- Volume of solution added: \( 0.25 \, \text{L} \)
- Concentration of zinc oxalate solution: \( 9.21 \times 10^{-6} \, \mu M \) (micromolar or \( \mu \text{M} \))
  
To solve this:

### Step 1: Convert concentration from micromolar to molar.
Micromolar (\( \mu \text{M} \)) is \( 10^{-6} \) molar:
\[
9.21 \times 10^{-6} \, \mu \text{M} = 9.21 \times 10^{-12} \, \text{M}
\]

### Step 2: Calculate the number of moles of zinc oxalate.
Using the formula:
\[
\text{moles} = \text{molarity} \times \text{volume}
\]
The molarity is \( 9.21 \times 10^{-12} \, \text{M} \) and the volume is \( 0.25 \, \text{L} \):
\[
\text{moles of ZnC}_2\text{O}_4 = 9.21 \times 10^{-12} \times 0.25 = 2.3025 \times 10^{-12} \, \text{moles}
\]

### Step 3: Convert moles to mass.
To convert moles to mass, we need the molar mass of zinc oxalate. The molar mass of \( \text{ZnC}_2\text{O}_4 \) is:
\[
\text{Zn:} \, 65.38 \, \text{g/mol} + \text{C:} \, 12.01 \times 2 \, \text{g/mol} + \text{O:} \, 16.00 \times 4 \, \text{g/mol} = 125.4 \, \text{g/mol}
\]

Now, convert moles to grams:
\[
\text{mass} = \text{moles} \times \text{molar mass} = 2.3025 \times 10^{-12} \times 125.4 = 2.8896 \times 10^{-10} \, \text{g}
\]

### Step 4: Convert grams to micrograms.
Since \( 1 \, \text{g} = 10^6 \, \mu g \):
\[
\text{mass in micrograms} = 2.8896 \times 10^{-10} \times 10^6 = 0.28896 \, \mu g
\]

### Final Answer:
The mass of zinc oxalate is approximately **0.289 μg** when rounded to three significant figures.

Would you like more details or have any questions?

Here are some related questions:
1. How do you calculate molar mass for more complex compounds?
2. How would the calculation change if the volume of the solution was different?
3. What is the significance of using micromolar concentrations in experiments?
4. How does zinc oxalate dissociate in water, and what are its chemical properties?
5. Why is it important to maintain significant digits in chemical calculations?

**Tip:** Always ensure you are using the correct units, especially when working with concentrations like micromolar or millimolar.

A chemist adds 0.25 L of a 9.21 × 10^(-6) μM zinc oxalate (ZnC2O4) solution to a reaction flask. Calculate the mass in micrograms of zinc oxalate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Learn how to calculate the mass of zinc oxalate (ZnC2O4) in a μM solution based on volume and concentration. Includes detailed stoichiometry and unit conversion steps for microgram calculation. Suitable for college-level chemistry.

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