Staple this data sheet to the back of your lab report for Experiment 6. Your hyd

Question

Staple this data sheet to the back of your lab report for Experiment 6. Your hydrate is MgSO_4. x H_2 O where X is an integer (your compound 11 has different integer than compound I) Data for Compound 11: Grams of compound used ___3.2337 g Grams of water lost by heating 0.7450 g Hydrate #2: Data for hydrate #2 (supplied on the data slip) Slip Mass of hydrate before heating ____ Mass of residue after heating _____(= anhydrous compound) Loss of mass upon heating ____(= water) A. Calculate moles of the anhydrous compound: B. Calculate moles of water: C. Determine the simplest mole ratio to find the empirical formula: Formula of the hydrate: MgSO_4:___H_2 O

Explanation / Answer

A. Mass of hydrate before heating = 3.2337 g

Grams of water lost by heating = 0.7450 g

Mass of anhydrous = Mass of hydrate before heating - Grams of water lost = 3.2337 - 0.7450 = 2.4887 g

Molar mass of MgSO4 = 120.366 g/mol

Moles of anhydrous compound = mass/molar mass = 2.4887/120.366= 0.02067 moles

B. Moles of water = mass/molar mass = 0.7450/18.015 = 0.04135

C. Ratio of moles of MgSO4 to H2O= 0.02067/0.04135 = 0.5.

Thus for each mole of MgSO4, 2 moles of H2O are present.

MgSO4.2H2O

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