A chemist prepares a solution of copper (II) fluoride by measuring out of copper (II) fluoride into a volumetric flask and filling the flask to the mark with water. Calculate the concentration in of the chemist's copper (II) fluoride solution. Be sure your answer has the correct number of significant digits.

4.90 * 10⁻³ M

Explanation:

There is some info missing. I think this is the original question.

A chemist prepares a solution of copper (II) fluoride (CuF₂) by measuring out 0.0498 g of copper (II) fluoride into a 100 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's copper (II) fluoride solution. Be sure your answer has the correct number of significant digits.

The molar mass of copper (II) fluoride is 101.54 g/mol. The moles corresponding to 0.0498 grams are:

0.0498 g * (1 mol / 101.54 g) = 4.90 * 10⁻⁴ mol

4.90 * 10⁻⁴ moles of copper (II) fluoride are dissolved in 100 mL (0.100 L) of solution. The molar concentration of copper (II) fluoride is:

4.90 * 10⁻⁴ mol/0.100 L = 4.90 * 10⁻³ M