Formula Of Hydrate Lab Report

The second part of this experiment involved measuring out 0.3 grams of the hydrated salt and then finding the mass of the fired crucible, the lid, and the hydrated salt. The value for this measurement was 45.691g for Trial 1 and 48.057g for Trial 2. The hydrated salt was then heated for 10 minutes using a bunsen burner causing water to be released and therefore the mass of the salt to decrease. After being heated for 10 minute the mass of crucible, lid, and the anhydrous salt were 45.620g and 47.945g, for Trial 1 and Trial 2 respectively. The mass of for Trial 1 decreased by 0.071 g and the mass for Trial 2 decreased by 0.112g after being heated for 10 minutes. After making the first mass measurements the crucicle was heated again for 2 minutes to reassure that all the water molecules were removed. The second mass measurement for both trials decreased from the first mass measurement showing that some water

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

The purpose of this lab is to determine the percent of water in a hydrate. I learned that copper sulfate hydrate is blue on its own but, when heat is added it will change color to a dim gray. One error that may have occurred is the failure to zero the scale which would ultimately change the math in the equation. Another error that may occur in this lab is forgetting to wait the recommended amount of cooling time, which would change the mass of the elements. At the end if the lab when we look to the questions, it is also beneficial to look at the notes for the lab because it helps with the setup of equations that may come with the questions, also it is very helpful

The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O.

Fill the rest of the container almost to the top with water and let the mixture separate.

Fulfilling the purpose, after concluding this experiment, the formula of an unknown hydrate was able to be identified. In order to obtain the data needed to develop a response to the purpose, multiple measurements were collected. The mass of an evaporating dish was measured without copper (II) sulfate hydrate (before and after heating), then measured with copper (II) sulfate hydrate before heating and with anhydrous after heating. Initially, the mass of an evaporating dish was recorded, then the dish was heated and the mass was again recorded. Through this additional step of heating, it insured that no excess water remained in the dish which, as a result, would alter the data. Copper (II) sulfate hydrate was added to the dish and the mass was

We were also provided with 6 molar following reagents:  H2SO4  HCl  NH3  NaOH Experimental Methods: We adopted these steps to find out the formula of unknown hydrate: Qualitative analysis: The unknown hydrate (in solution form) was reacted with all given known aqueous solution and reagents separately in separate test tubes and results were noted down in Table No. 1.1. Quantitative Analysis: The number of water molecules were determined by following steps: o Determined the mass of water that has left the compound.

In the experiment, we calculated the percentage of water in 1.5 grams of copper (II) sulfate hydrate by heating it over a Bunsen burner, causing the compound to dehydrate. We then could compare the mass of the hydrate before and after the experiment to determine how much water had been vaporized. Originally, the hydrate inside of the crucible had a total mass of 9.60 grams, but after being heated, the total mass dropped to 9.04 grams. With the crucible alone weighing 8.10 grams, that means that 0.56 grams or 37.33% of water that previously composed the hydrate had completely evaporated from the compound.

This experiment has as purpose the determination of the amount of water present in a hygroscopic ionic compound, also known as hydrates. Therefore, from this experiment a person will get the required knowledge to separate and determine the amount of water present in a compound. The main technique employed in this experiment is the weighing technique. In order to realize this technique, the analytical balance must be tarred and adjusted to the desired units, in this case grams. While doing the measurements, the sensibility of the analytical balance must be taken into account, so act wisely. The analytical balance, the crucible with cover and the lab burner, can be described as the main equipment of this experiment.

Hydrates are inorganic salts that lose water when heated and undergo a color change. The loss of water makes the hydrate anhydrous. Copper chloride hydrate is what will be used in the lab to show what happens when a hydrate is heated which can lead to a better understanding of hydrates as a whole and their reactions that can be observed to discover things about the environment they’re in. After the removal of water from the copper chloride hydrate, the solid ,when reacted with aluminum and filtered, produces elemental copper. Through the understanding of the process used to achieve this, the experiment can be recreated for another hydrate to isolate a different element. By determining the amount of water and copper in the

Leave the mixture to boil until half of it is only left, then strain it, leave it to cool down and store it in the fridge in a glass container.

The purpose of this experiment is to determine the empirical formula also known as the simple formula of a compund known as a hydrate.

In experiment 3, “Hydrates”, tools such as a crucible and a lid will be used and chemicals such as 0.2 grams NiCl2.6H20, 0.2 grams of CuSO4.5H20, 0.2 grams of MgSO4.7H20, 0.2 grams of NaCl, 0.2 grams KAI(SO4)2.12H2O, 0.2 grams CaCl2, 0.4 grams of CuSO4 and 0.5 grams of an unknown hydrate. First off in step A, place 0.2 grams of solid, blue cupric sulfate in a test tube and describe its color and shape essentially determine whether it is a crystalline or powder. Using a test tube holder

Crystals may seem to be dry when an ionic compound is crystallized from an aqueous solution, but when they are heated, the mass decreases as the water is released from the structure of the crystal. As this is performed, the appearance or the color may change. Hydrates are compounds that contain water molecules that are a part of their crystal.

The purpose of this lab is to determine the percent composition of water of the hydrate. Hydrates are solid ionic compounds that contain water that is chemically inside the crystalline structure. An example of such compound is epsom salt. A salt is an ionic compound that forms as a product of a reaction between both acid and base. Water molecules that are incorporated with salt are known as waters of hydration. The waters can be removed from the hydrate with the use of heat, thus, leaving the salt with no water molecules. The remaining amount of salt is referred to as anhydrous. An anhydrate is a substance that has been stripped of their water particles with the use of heat and has since become dehydrated. This experiment shows relevance to