A chemist adds 470.0 mL of a 8.8 times 10^-5 mM silver(II) oxide (AgO) solution to a reaction flask. Calculate the mass in micrograms of silver(II) oxide chemist has added to the flask. Round your answer to 2 significant digits.

5.1 μg

Explanation:

Step 1: Given data

Volume of solution (V): 470.0 mL (0.4700 L)

Concentration of the solution (C): 8.8 × 10⁻⁵ mM (8.8 × 10⁻⁸ M)

Step 2: Calculate the moles (n) of AgO added

We will use the following expression.

n = C × V

n = 8.8 × 10⁻⁸ mol/L × 0.4700 L

n = 4.1 × 10⁻⁸ mol

Step 3: Calculate the mass (m) corresponding to 4.1 × 10⁻⁸ moles of AgO

The molar mass of AgO is 123.87 g/mol.

4.1 × 10⁻⁸ mol × 123.87 g/mol = 5.1 × 10⁻⁶ g

Step 4: Convert "m" to micrograms

We will use the conversion factor 1 g = 10⁶ μg.

5.1 × 10⁻⁶ g × 10⁶ μg/1 g = 5.1 μg

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