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.

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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

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