Answer:
The formula of the magnesium halide is MgF₂
Explanation:
All halides, X, produce a salt with Mg with the formula:
MgX₂
<em>-There are 2 moles of the halide ion per mole of Mg-</em>
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With the mass of the MgSO₄ we can find moles of magnesium sulfate = Moles Mg.
With moles of Mg we can know the moles of the halide -1 mole Mg = 2 moles of Halide-
And we can find the mass of Mg in the 0.0776g sample. Subtracting we can find the mass of the halide and, with the mass and moles of the halide we can find its molecular weight and its identity:
<em>Moles MgSO₄ -Molar mass: 120.366g/mol- = Moles Mg:</em>
0.150g * (1mol / 120.366g) = 1.2462x10⁻³ moles Mg
<em>Moles halide:</em>
1.2462x10⁻³ moles Mg * 2 = <em>2.4924x10⁻³ moles Halide</em>
<em>Mass Mg -Molar mass: 24.305g/mol:</em>
1.2462x10⁻³ moles Mg * (24.305g / mol) = 0.0303g Mg
<em>Mass halide:</em>
0.0776g - 0.0303g Mg = <em>0.0473g</em>
<em>Molecular weight of the halide:</em>
0.0473g / 2.4924x10⁻³ moles =
18.98g/mol
This molecular weight is the molecular weight of Fluoride ion, F⁻,
<h3>The formula of the magnesium halide is MgF₂</h3>
