A chemist adds of a magnesium fluoride solution to a reaction flask. Calculate the mass in micrograms of magnesium fluoride the chemist has

Question

A chemist adds of a magnesium fluoride solution to a reaction flask. Calculate the mass in micrograms of magnesium fluoride the chemist has added to the flask. Round your answer to significant digits.

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Sapo 4 years 2021-07-28T21:33:36+00:00 1 Answers 20 views 0

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  1. minhkhang
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    2021-07-28T21:34:44+00:00
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    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

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