Question

A chemist adds 280 mL of a 5.86*10^-4 M copper(II) fluoride solution to a reaction flask... Calculate the mass in MILLIGRAMS of copper(II) fluoride the chemist added to the flask. ROund to 3 sig figs..

Answer 1

We know

Molarity = No. of moles / volume in liters

No. of moles = Molarity X Volume in liters

Moles of Copper(II)floride = volume in liters X molarity

Volume = 280mL = 280/1000 = 0.28L

Moles of Copper(II)floride = 0.28 X 5.86 X 10^-4 = 1.6408 X 10^-4 moles

Mass of Copper(II)floride = No. of moles X Molecular mass

We know No. of moles = mass / Molar mass

mass = Molar mass X No. of moles

Mass of Copper(II)floride =  1.6408 X 10^-4 m X 101.54 = 0.0162g