How many moles of water are in copper sulfate hydrate?
Similarly one may ask, how do you find the moles of water in a hydrate?
Divide the mass of water by the molar mass of water to get moles of water. 2.60 g H2 O / (18.00 g/mol H2 O) = 0.144 moles H2 O. Divide the mass of anhydrate by the molar mass of anhydrate to get moles of anhydrate.
Similarly, how many moles of water are there in one mole of hydrated salt?
Divide the mass of your anhydrous (heated) salt sample by the molar mass of the anhydrous compound to get the number of moles of compound present. In our example, 16 grams / 160 grams per mole = 0.1 moles. Divide the mass of water lost when you heated the salt by the molar mass of water, roughly 18 grams per mole.
The chemical formula of a typical hydrated compound, such as copper(II) sulfate pentahydrate, is written as CuSO4•5H2O. The dot in the formula indicates that the two compounds are bound together. Upon heating, the water can be evaporated leaving an anhydrous salt. This process is reversible.