Answer:
0.42 mg
Explanation:
It seems the question is incomplete, however I'll use values that have been found in a web search:
"A chemist adds 55.0 mL of a 1.7x10⁻⁵ M mercury(II) iodide solution to a reaction flask. Calculate the mass in milligrams of mercury(II) iodide the chemist has added to the flask. Round your answer to 2 significant digits."
<u>Keep in mind that while the process of solving the problem remains the same, if the values in your question are different, your answer will differ as well</u>.
First we <u>calculate the moles of mercury (II) iodide</u> (HgI₂):
- 1.7x10⁻⁵M * 55.0 mL = 9.35x10⁻⁴ mmol HgI₂
Then we<u> convert mmol to mg, using the molar mass</u> (454.4 g/mol):
- 9.35x10⁻⁴ mmol HgI₂* 454.4 mg/mmol = 0.42 mg