A chemist prepares a solution of copper (II) fluoride (CuF2 by measuring out 0.0498g 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. Round your answer to significant digits.

4.90 * 10⁻³ M

Explanation:

Given data

Mass of copper (II) fluoride (solute) : 0.0498 g Volume of solution: 100 mL = 0.100 L

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

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

The molar concentration of copper (II) fluoride is:

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