Determining The Chemical Formula For Two Hydrates Through Dehydration

A hydrate is a compound that is bonded with a certain number of water molecules. When heated, the water will be driven out, thus being left with an anhydrate. The anhydrate is the hydrate minus the water. The hydrate must be

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

As a group, we obtained our salt mixture of calcium chloride and potassium oxalate, and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution, leaving the precipitate. Once the precipitate was dried overnight, it was weighed and the mass was measured. Then we calculated the moles of the precipitate.

There are several sources of error to this experiment due to random and systematic errors. The only source of random error was the measurement that we took through the graduated cylinder which was only accurate to the nearest 1%. We took the largest error from this one percent, which was +/- 3. The largest relative error this yielded was only 3%, so this did not affect how precise this experiment was too much. We can still make this more precise by making the masses of the water larger. For example if we started the masses at 300mL and went up by 50mL, the largest error this would yield would be 2% due to the largest error being +/- 5. This would cause smaller errors in the amount of water.

29. When the thermometer reads 40°C, carry the beaker out of the heating apparatus with a beaker tong.

    One possible source of error that can affect the results was that a mercury thermometer was used instead of an electronic one. The use of a mercury

At the beginning of the lab, the crucible is heated. What is the purpose of this step? How would your results (mole ratio of anhydride to water) have changed if you did not pre-heat the crucible? Explain. Feel free to use real numbers to

5. I believe that with a Bunsen burner to dry would have provided more accurate results for the hydration number because the heat can be applied more directly and the time to heat would be faster, giving less room for error in the

Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.

9) Trial E: Remove the syringe and empty the beaker. Add a Thermometer to the beaker. Add 200 mL of Room Temperature water to the beaker and heat with a Bunsen Burner until it reaches 100° C. Remove the Bunsen Burner. Repeat Steps 5 & 6.

The initial magnesium had a mass of 0.06 g while the final compound had a mass of 0.08 g. Magnesium oxide had been formed, and no magnesium should have been lost over the process due to magnesium being unable to form gases or liquids with any of the elements it had been exposed to.

A hydrate is a chemical compound containing salt and water. Depending on the salt, there is a maximum amount of water molecules that can be absorbed by the salt. An anhydrous salt is when the hydrate loses water, which happens when the hydrate is heated

The powdered cobalt oxalate hydrate was weighed to about 0.3 g and placed in a pre-weighed crucible. The crucible and the cobalt oxalate were then heated until the cobalt oxalate decomposed into a stable, black solid, or Co3O4. Once the crucible was sufficiently

Subsequently, two porcelain crucibles were used, weighed, and heated for about 10 minutes and then placed into a desiccator to cool. The two empty porcelain crucibles were first heated because the heat would vaporize any impurities that were originally on the crucible. The first crucible weighed 11.9047 g and the second crucible weighed 12.3735 g. Once the mass of the two crucibles

In this experiment, a saturated calcium sulfate was already made and ready to use. 25.00 mL of this solution was then mixed with 10 mL of an ammonia buffer and 1 drop of