The question is incomplete, here is the complete question.
A chemist adds 345.0 mL of a 0.0013 mM (MIllimolar) copper(II) fluoride solution to a reaction flask.
Calculate the mass in micrograms of copper(II) fluoride the chemist has added to the flask. Be sure your answer has the correct number of significant digits.
Answer : The mass of copper(II) fluoride is, 0.13 mg
Explanation : Given,
Millimolarity of copper (II) fluoride = 0.0013 mM
This means that 0.0013 millimoles of copper (II) fluoride is present in 1 L of solution
Converting millimoles into moles, we use the conversion factor:
1 moles = 1000 millimoles
So,
To calculate the number of moles, we use the equation:
We are given:
Moles of copper (II) fluoride solution =
Molar mass of copper (II) fluoride = 101.5 g/mol
Putting values in above equation, we get:
Converting this into milligrams, we use the conversion factor:
1 g = 1000 mg
So,
Therefore, the mass of copper(II) fluoride is, 0.13 mg