Subtracting the mass of (flask+water) from the empty flask gives:
95.023 g - 85.135 g = 9.888 grams of water
Dividing this by the given volume of 10.00 mL water gives:
9.888 grams of water / 10.00 mL of water = 0.9888 g/mL of water
Therefore, based on this sample, the density of water is 0.9888 g/mL, which is close to the usually accepted approximation of 1 g/mL.
molar mass of the molecule is 60. Moles=mass/molar mass
92.02g/60=1.53366667mol
1.53mol(3sf)
The traditional method is to heat the compound in an oven, on a hot plate or over a Bunsen burner. Waters of hydration are loosely bound in the compound and can be driven off at temperatures below the melting point of the compound. So the answer is heating.
