A hydrate is an ionic compound that contains water molecules in its structure. To determine the formula of a hydrate experimentally, we must calculate...
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Determining the Formula of a Hydrate Chem Worksheet 11-6
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A hydrate is an ionic compound that contains water molecules in its structure. To determine the formula of a hydrate experimentally, we must calculate the mole: mole ratio of the water portion compared to the anhydrate portion. An anhydrate is the substance that remains after the water is removed from a hydrate. When a hydrate is heated the water molecules are driven off as steam, leaving behind the water-free anhydrate. The first step to finding the formula for a hydrate is to record the mass of the hydrate. After heating the hydrate, the mass is determined for the anhydrate that remains. The mass of the water that was present is calculated by finding the difference between Data Table the mass of the hydrate and the mass of the anhydrate. The 4.72 g Mass of hydrate (CaCl2 · xH2O) mass of the water and the mass of the anhydrate are each Mass of anhydrate (CaCl ) 3.56 g 2 converted to moles using their respective molar masses. From Mass of water 1.18 g this a whole number ratio can be determined (see example). Example A calcium chloride hydrate has a mass of 4.72 g. After heating for several minutes the mass of the anhydrate is found to be 3.56 g. Use this information to determine the formula for the hydrate. - find the mass of the water driven off:
mass of hydrate – mass of anhydrate = mass of water 4.72 g – 3.56 g = 1.18 g
- convert the mass of anhydrate to moles:
3.56 g CaCl 2 1 mol CaCl 2 × = 0.0321 mol CaCl 2 1 110.98 g CaCl 2
- convert the mass of water to moles:
1.18 g H 2O 1 mol H 2O × = 0.0655 mol H 2O 1 18.02 g H 2O
- find the mole H2O to mole CaCl2 ratio:
0.0655 mol H 2O 2 mol H 2 O = 0.0321 mol CaCl 2 1 mol CaCl 2
Since the compound contains 2 moles of water for every 1 mole of anhydrate the formula is CaCl2 · 2 H2O
