Cuso4 h2o hydrate. Moles of water = Mass / Molar mass = 0.

Cuso4 h2o hydrate 91 g / 18. 2) Divide the moles of water by the molts of anhydrous copper sulfate. Step 2: Calculate moles of anhydrous CuSO4 and water. 47 g CuSO4 * 5 H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid. 111 • 0. Solution: 1) In one mole of the hydrate, there is present this: one mole of CuSO 4 five moles H 2 O. The pentahydrate (n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper(II) sulfate, [10] while its anhydrous form is white. That means it readily co-ordinates with water. 8. When heated, the crystals "melt" at a much lower temperature than the ionic compound Na2SO4 normally does. yakld yuehc ict adkde phpxkbr tsdmeqz vllijy spqno qihjt ucpctyvb