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Hydrates lecture
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- 2. Hydrate definition A hydrateis a compound that has a specific number of water molecules bound to its atoms
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- 4. Naming Hydrates • Writethe compound and the hydrate connected by a dot Sodium carbonate decahydrate
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- 6. Analyzing a Hydrate •The hydrate can be removed from the compound through heat • Cobalt (II) Chloride is a pink solid that turns deep blue when heated and water is removed (anhydrous form)
- 7. Formula for aHydrate • 1. Determine the number of moles of water associated with one mole of hydrate – 5 g sample of Barium Chloride Hydrate (BaCl2•xH20) – After heating, the weight of the anhydrous sample is 4.26 g – 5 g – 4.26 g = 0.74 g H20 – Determine moles of H20 and BaCl2 ratio
- 8. Hydrate Example • Amass of 2.50 g of blue, hydrated copper sulfate (CuS04•xH20) is placed in a crucible and heated. After heating, 1.59 g white anhydrous copper sulfate remains. What is the formula for the hydrate? Name the hydrate.
- 9. Hydrate Example Cont’d •1. Hydrous copper sulfate is 2.50 g • 2. Anhydrous copper sulfate is 1.59 g • 3. 2.5 g – 1.59 g = 0.91 g of hydrate • 4. 0.91 g water lost, 1.59 g copper sulfate
- 10. Hydrate Example Cont’d •5. Calculate the moles of Copper sulfate and the moles of water lost • 6. Determine the molar ratio • 7. Setup the formula and name it
- 11. Practice Problems-Appendix D •A hydrate is found to have the following percent composition – 48.18% MgS04 and 51.2% H20 – What is the formula and name for this hydrate? MgS04•7H20 Magnesium Sulfate heptahydrate
- 12. Practice Problems-Appendix D •If 11.75 g of the common hydrate cobalt (II) chloride is heated, 9.25 g of anhydrous cobalt chloride remains. What is the formula and name for this hydrate? CoCl2•2H20 Cobalt (II) Chloride dihydrate
- 13. Uses of Hydrates •Drying agents due to hygroscopic nature (absorb water from environment) • Solar energy (Na2S04•10H20)
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