Achemist 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.

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

Explanation:

Moles of  magnesium fluoride  = n

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

Molarity of the solution =

(1 mM = 0.001 M)

1 mole = micro mole

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

the atomic mass is the bottom number on the element.

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