1. Experiment 6 hydrate Operation of bunsen burner and crucible heating When ready, attach the bunsen burner to the gas jet(blue cap). Turn the burner tube to adjust the air and turn the stopcock to adjust the natural gas until there is a blue inner and outer cone (law of definite proportions). A lazy yellow flame indicates the formation of dangerous CO.

2. Experiment 6 hydrate Some ionic compounds such as CuSO 4 ∙ 5 H 2 O are called hydrates. When heated they lose water: CuSO 4 ∙ 5 H 2 O → CuSO 4 + 5 H 2 O CuSO 4 is the anhydrous salt.

3. A chemist heats a sample of the blue solid and observes the following reaction: A. X H 2 0 → A + X H 2 O The chemist collects the following data: Mass of crucible: 21.2443 g Mass of crucible & hydrate (A. X H 2 0 ): 25.4943 g Mass of crucible & anhydrous salt (A): 23.9643 g Molar mass of hydrate = 250 g/mol 1.Calculate the mass of the hydrate. ANS: 4.2500 g 2. Calculate the moles of hydrate. ANS: 0.0170 mol Experiment 6 hydrate

4. Mass of crucible & hydrate(A. X H 2 0):25.4943 g Mass of crucible & anhydrous salt(A): 23.9643 g 3. Calculate the mass of H 2 O. ANS: 1.5300 g 4. Calculate the moles of H 2 O. ANS: 0.0850 mol 5. Calculate the % water. ANS: 6.00% 6. Calculate the moles of water in 1.0 mole of hydrate. See problem #2. ANS: 5 mol water