Measure The Percent Of Water

Using a scoopula, add 5-6 grams of the hydrate into the dish and measure the mass of the hydrate and the dish

2. Used a test tube clamp to held the test tube and gently heated the tube in a laboratory burner flame for about 30 seconds.

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.

In experiment A the results from the precipitation of CaC2O4 H2O from the salt mixture were obtained by weighing the items listed on Table 1 on a scale.

One possible source of error for this experiment is if the anhydride had been exposed to air before measuring because it could have reabsorbed some water vapor in the air. This would cause the ratio of moles of anhydride to moles of water change because there would be less water calculated depending on how much water was actually absorbed back in the anhydride. Another possible source of error is if not all of the water was evaporated from the hydrate. This would also change the ratio of moles of anhydride to moles of water because there would be less water calculated since some of the water’s mass would be accounted for in the mass of the anhydride.

The percent of water can be determined in a hydrate by first determining the mass of the hydrate Copper (II) Sulfate penta-hydrate. The substance will be a deep blue color when it is a hydrate. By heating the substance, water is evaporated, removing the water from the hydrate, making it anyhydrous through a simple decomposition reaction. Evaporation is completed when the substance turns from a blue to a white/ grey color. The mass of the water in a hydrate is determined by subtracting the mass of the hydrate from the mass of the anhydrate. The mass of the water is then divided by the mass of the hydrate, and multiplied by one hundred, resulting in the percent of water in the hydrate, which is 36.35%. The percent error is determined by subtracting

1. Carefully measure the volume of the trapped gas using the graduations (markings) on the side of the container.

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

Fill a test tube about 1/3 full with cold tap water for use in step 34.

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

In this lab, "Gravimetric Methods," students were expected to be able to calculate the mass percentage of an unknown hydrate, describe the process of gravimetric analysis, and put together the equipment needed to evaporate water from the unknown hydrate.   Gravimetric analysis is the process in which an amount of a substance can be found by measuring the mass.  By comparing the masses of two compounds that contain the substance, one can successfully complete a gravimetric analysis.  The initial recorded mass will be different from the final recorded mass since part of the substance evaporates from the container.  By subtracting the initial mass from the final mass, students can determine the amount of the substance that evaporated.  They can

Place the covered crucible into a pipestem triangle, heating gently for 2 minutes. Using a wire tilt the cover to allow air to enter the crucible. Strongly heat the crucible for 10 minutes.

1 ml of water should be added to the first test tube and make a note. In the second test tube, 1 ml of methyl alcohol should be added. In the third test tube, 1 ml of hexane must be added. Lastly, the fourth test tube will be a control.

Measure out one scoop of albumin powder (rich protein) and place it into each individual tube.

This lab was conducted to find the percent water in a hydrate. A hydrate is a compound with water chemically combined to other atoms. The chemical compound tested in this experiment is Copper II Sulfate Pentahydrate, or CuSO4*5H2O, which will break down and release water when heated. The reactant of this reaction begins blue and gradually turns white as the products are produced.