A 100 mg sample of Epsomite (MgSO4·7H2O) was heated in a crucible. After cooling to room temperature, the mass of the resulting white, anhydrous salt (MgSO4) was measured to be 49 mg. Given this data, calculate the mass percent of water in the hydrate and show calculations that confirm the empirical formula ratio of 1 MgSO4:7H2O.

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Asked Sep 19, 2019
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A 100 mg sample of Epsomite (MgSO4·7H2O) was heated in a crucible. After cooling to room temperature, the mass of the resulting white, anhydrous salt (MgSO4) was measured to be 49 mg. Given this data, calculate the mass percent of water in the hydrate and show calculations that confirm the empirical formula ratio of 1 MgSO4:7H2O.

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Expert Answer

Step 1

It is given that:

Mass of Epsomite (MgSO4.7H2O) = 100 mg

Mass of anhydrous salt (MgSO4) = 49 mg

Step 2

Solution comprises of solute and solvent.

In this case mass of solution is 100 mg and mass of solute that is anhydrous salt (MgSO4) is 49 g. So, the mass of solvent can be calculated as follows:

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Mass of solution = mass of solute + mass of solvent(H2O) 100 mg 49 gmass of solvent (H,0) mass of solvent (H,0)=100 mg - 49 mg =51mg

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Step 3

The way of representation of concentration of an element in a compound or a compone...

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Mass of component Mass percent of component = x100% Total mass of the solution

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