Answer:
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
