Achemist adds of a m copper(ii) fluoride solution to a reaction flask. calculate the mass in micrograms of copper(ii) fluoride the chemist has added to the flask. round your answer to significant digits.

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

i think it is d. e because the next one is igneous.

fdvwsa gfwsargebgeebbfwfwffw gwf   vgwgw gw f gwgw fgw v v dsv dwfff