1. A student collected the following data during Lab: Mass of MgCO3 hydrate = 0.9987 g. Constant mass of anhydrous MgCO3 = 0.4831 g How many moles of water were in the MgCO3 hydrate?
1. A student collected the following data during Lab: Mass of MgCO3 hydrate = 0.9987 g. Constant mass of anhydrous MgCO3 = 0.4831 g How many moles of water were in the MgCO3 hydrate?
2. A student uses gravimetric determination to find the water of hydration of a hydrated sample of cobalt (II) sulfate. The student’s sample contained 0.0098459 moles of anhydrous cobalt(II) sulfate (CoSO4) and 0.068921 moles of water (H2O). What is the formula of the cobalt(II) sulfate hydrate?
3. A student has a sample of CaSO4 hydrate and it weighs 0.4813 grams. He heats it strongly to drive off the water of hydration, and after subsequent heatings, the student finds the anhydrous compound has a constant mass of 0.3750 grams. Find the formula of the hydrate.
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