Determing the Formula of a Hydrate

LAB: DETERMING THE FORMULA OF A HYDRATE Background: Hydrates are ionic compounds (salts) that take up specific amounts of water molecules as part of their crystal structure. This water can be driven off by the application of heat. Since the ratio of the ionic compound to water molecules is always the same, the percentage of water should be the same for each sample. Table salt usually contains a small amount of hydrated calcium sulfate, CaCl2 * H2O, and a hydrated magnesium sulfate, MgCl2*6H2O. On humid days these two impurities absorb moisture and cause the table salt to become wet and to “cake.” To prevent this, some manufacturers add an anti-caking agent such as magnesium silicate, Mg2Si3O8 that forms a hydrate that does not become wet. Purpose: In this lab you will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate you are working with. Safety: Use safety goggles and aprons. Wash your hands thoroughly after handling chemical supplies! Materials: copper (II) sulfate hydrate, electronic balance, evaporating dish, Bunsen burner Procedure: 1. Mass a CLEAN, DRY evaporating dish. Record this mass in the data table. 2. Using a scoopula, measure approximately 4g of copper (II) sulfate hydrate into the evaporating dish and record the exact mass in the data table. Record the initial color of the copper (II) sulfate in the data table. 3. Place the evaporating dish on a clay triangle and set it about 8-10 inches above the Bunsen burner. Light the Bunsen burner. The evaporating dish should be about 3-5 inches above your flame, if it is not, turn off your Bunsen burner and adjust your set up. 4. Observe the contents of the evaporating dish after a few minutes and record your observations in the data table. You may want to use a stirring rod to occasionally move the salt around as it heats. 5. Continue to heat the copper (II) sulfate for about 10 minutes or it has completely lost its blue tint/ until it appears completely light brown/white. This will indicate that all the water has been driven off (evaporated) from the salt. 6. If it still looks clumpy, use your stirring rod to break clumps apart. Be careful; everything is hot! 7. Allow the evaporating dish and compound to cool. NEVER put a HOT dish onto the balance! 8. Mass and record the cooled evaporating dish and compound. 9. Clean out the evaporating dish by adding a little water and disposing the solid waste into the trash. Dry your evaporating dish & put all equipment away. Data Table Mass of evaporating dish Mass of evaporating dish + copper (II) sulfate hydrate (before heating) Initial mass of copper (II) sulfate hydrate (before heating) Initial Color of hydrate Mass of cooled evaporating dish+ Anhydrous copper (II) sulfate (after heating) Final Color of hydrate Final Mass of the anhydrous copper (II) sulfate Mass of water (that evaporated from the original hydrate) Observations when cleaning the evaporating dish Post Lab Questions: You must show ALL WORK in your lab notebook. 1. How does a hydrate differ from something that is aqueous? 2. How many grams of the salt were in the hydrate? 3. How many moles of the salt were in the hydrate? 4. How many grams of water were in the hydrate? How many moles? 5. What percent of water was in the hydrate? (use the masses to answer this) 6. Based on YOUR data, what is the empirical formula for your hydrate? 7. What is your percent error on the accepted percent water of the hydrate (compare to the accepted formula)