The given question is incomplete, the complete question is:
A chemist adds 35.0mL of a 6.19 * 10^−4/mmol magnesium fluorideMgF2 solution to a reaction flask. Calculate the mass in micrograms of magnesium fluoride the chemist has added to the flask. Round your answer to
3 significant digits.
Answer:
The correct answer is 1.35 microgram.
Explanation:
Based on the given information,
The volume of magnesium fluoride given is 35 ml, and the concentration of magnesium fluoride is 6.19 × 10⁻⁴ mmol/L.
Now the moles of MgF₂ can be determined by using the formula,
Moles = Concentration × Volume
Moles of MgF₂ = Concentration of MgF₂ × Volume of MgF₂
= 6.19 × 10⁻⁴ mmol/L × 35 ml × L/1000 ml
= 217 × 10⁻⁷ mmol
The molecular mass of magnesium fluoride is 62.3 gram per mole
Thus, the mass of MgF₂ is,
= 217 × 10⁻⁷ mmol × 62.3 g/mol
= 13500 × 10⁻⁷ mg
= 1.35 microgram
