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

Answer:

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

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 = $9.75\times 10^{-4} mM=9.75\times 10^{-7} M$

(1 mM = 0.001 M)

$9.75\times 10^{-7} M=\frac{n}{0.380 L}$

$n=3.705\times 10^{-7} mol$

1 mole = $10^6$ micro mole

$n=3.705\times 10^{-7} \times 10^6 \mu mol=0.3705 \mu mol$

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