Today in class we learned tht hydrates are ionic compounds that contain an inorganic salt compound loosely bound to water. Putting our knowledge into action we did an experiment today that was meant to determine the emprical formula of a hydrate. In the lab we determined the anhydrous (without water) mass of the hydrate and then compared the original mass with the actual mass of water that should be present.
The materials that we used to conduct this experiment are:
- bunsen burner
- test tubes
- test tube rack
- test tube clamp
- weight scales
The first step we took in conducting our experiment is we filled a test tube with about 1 cm of the hydrate. We then carefully placed the test tube on the scale and recorded the mass of the hydrate and test tube. With extreme cation we proceeded to connect and light our Bunsen burner and adjusted the gas flow until the flame was about 5 cm tall. Afte heating our test tube over the Bunsen burner with the clamps (in and out) for about 5 minutes we carefully re-weighed the test tube.
Our observations were that the mass before heating was:
and the mass after heating was:
Our conclusion was that # amount of water was released during heating and that # percent of the hydrate was water. The actual percent ofwater in the hydrate was 45%. Our percent error was #.
Overall we learned a lot from the first-hand experience and had a great time!
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