Reference no: EM131089457
Hydrated Crystals Lab Make Up-
You must show all work and answers should be in complete sentences.
1. Summarize the composition of a hydrate
2. Name the compound that has the formula SrCl2 · 6H2O
3. Describe the experimental procedure for determining the formula for a hydrate. Explain the reason for each step.
4. A hydrate contains 0.050 mol of H2O to every 0.00998 mol of ionic compound. Write a generalized formula for a hydrate.
5. Calculate the mass of the water of hydration if a hydrate loses 0.025 mol of water when heated.
6. Arrange these hydrates in order of increasing percent water content: Show work
MgSO4·7H2O, Ba(OH)2·8H2O, and CoCl2·6H2O
7. Explain how a particular hydrate may be used as a means of roughly determining the probability of rain. What are some other uses for hydrates?
8. Use the following data table to determine the formula for a hydrate of barium chloride.
Mass of empty crucible - 21.30 g
Mass of hydrate + crucible - 31.35 g
Initial mass of hydrate - g
Mass after heating - 29.87 g
Mass of anhydrous - g
9. Hydrated sodium tetraborate Na2B4O7 is commonly called borax. Chemical analysis indicates that this hydrate is 52.8% sodium tetraborate and 47.2% water. Determine the formula and name the hydrate.
10. Natural gas hydrates are chemical compounds known as clathrate hydrates. Research natural gas hydrates and write 3 paragraphs on the composition and structure of the compounds, the location of the hydrates, their importance to consumers, and the environmental impact of using these hydrates.
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: Hydrated sodium tetraborate Na2B4O7 is commonly called borax. Chemical analysis indicates that this hydrate is 52.8% sodium tetraborate and 47.2% water. Determine the formula and name the hydrate
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