Hydrated sodium tetraborate na2b4o7 is commonly called

Question

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.