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.

sorry idk the answer well to you i have a explaination

explanation: a formula which shows the arrangement of atoms in the molecule of a compound

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !