Question

A chemist adds 380.0mL of a ×9.7510−4mM magnesium fluoride MgF2 solution to a reaction flask. Calculate the micromoles of magnesium fluoride the chemist has added to the flask. Round your answer to 3 significant digits.

Answer 1

0.370 micromoles of magnesium fluoride the chemist has added to the flask.

Step-by-step explanation:

`Molarity=\frac{moles}{\text{Volume of solution(L)}}`

Moles of magnesium fluoride = n

Volume of the solution = 380.0 mL = 0.380 L (1 mL = 0.001 L)

Molarity of the solution =
`9.75* 10^(-4) mM=9.75* 10^(-7) M`

(1 mM = 0.001 M)

`9.75* 10^(-7) M=(n)/(0.380 L)`

`n=3.705* 10^(-7) mol`

1 mole =
`10^6` micro mole

`n=3.705* 10^(-7) * 10^6 \mu mol=0.3705 \mu mol`

0.370 micromoles of magnesium fluoride the chemist has added to the flask.