If we use good technique (avoid spills, etc.) them the following will be true: m

Question

If we use good technique (avoid spills, etc.) them the following will be true: mass of hydrate = mass of the residue + mass of the water lost From the data above, calculate the mass of the anhydrous compound (- then residue) and the mass of water lost by subtracting the appropriate masses. Copy the descriptions for the lines you are using from the table. Mass of ___ ___ Mass of ___ - ___ Mass of hydrate(starting material) = ___ Mass of ___ ___ Mass of ___ - ___ Mass of anhydrous compound (residue) = ___ Mass of ___ ___ Mass of ___ - ___ Mass of water lost = ___ Use the data and calculations above to determine the percent water (by mass) in the hydrated compound. If a different sample of your unknown contains 0.815 g of MgSO_4. how many grams of H_2O does it contain? Use the mass percentage information from #2.

Explanation / Answer

Answer to Q1)

% water = mass of water X 100 / Mass of the hydrate

= 0.5483 g X 100 / 1.1492 g

= 47.7%

Answer to Q2)

% Anhydrous MgSO4 = 100 - % water

= 100 – 47.7

= 52.3%

% Anhydrous MgSO4 = mass of Anhydrous MgSO4 X 100 / Mass of MgSO4 hydrate

52.3 = 0.815 g X 100 / Mass of MgSO4 hydrate

Mass of MgSO4 hydrate = 0.815 g X 100 / 52.3

= 1.5583 g

% water = mass of water X 100 / Mass of the MgSO4 hydrate

47.7 = mass of water X 100 / 1.5583 g

Mass of water = 47.7 X 1.5583 / 100

= 0.7433 g

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