In the lab, “Properties of Hydrates,” the purpose was to compare the properties of several well observable hydrates and to determine if dehydration is a reversible or irreversible change. The lab consisted of attaining a pea-size sample of each compound, burning it over a bunsen burner, and comparing the starting mass and the mass lost after the combustion. These results are important to be able to identify a variety of different chemicals that contain water molecules as part of their crystalline structure. Some can be removed by heating (resulting in evaporation) and some remain mostly unchanged. In this lab the answer will be found. Procedure and Observations To begin the lab, first all the correct equipment and materials had to be collected …show more content…
Then an estimated (by trial and error) 1-3 grams of hydrated copper sulfate was added to a crucible with the lid on top. The total mass of the hydrated copper sulfate was recorded by subtracting the total mass of the crucible, lid, and sample from the mass of the crucible and lid (described in table 1.3). By attaching the wire triangle to the ring, the crucible was able to sit securely while having the bunsen burner underneath. Lighting the burner once again, each substance was heated for several minutes until estimated that the compound had changed color. Once a prevalent color change had been observed at approximately 4 minutes (blue green color) the crucible was set on the counter using the tongs to cool for approximately 5 minutes. The appearance after this period resulted in another color change back to white. The crucible, lid, and hydrated copper sulfate was weighed again to calculate the mass of water lost by dehydration (described in table 1.3). This was done by subtracting the final mass by the initial mass of the crucible, lid, and compound. The mass of the crucible would remain unchanged while the mass of the compound would be altered. This trial was repeated 3 times and 1 extra set of data was taken from 2 separate groups to include
B) Briefly describe each method, including the specific types of scientific tools and equipment used. Modified Mercalli Intensity Scale:
Now, they are ready to start the lab. The empty crucible is weighed by and the weight was recorded. Then the students used a disposable pipet and put close to 4.0 grams of their milk sample in their crucible on the scale. The crucible was then placed back on
Metal cations can be identified based on the colors they emitted off when heated in a flame.1 When atoms of the ions that were tested are excited, their electrons move up to higher levels of energy.2 When the electrons relax and return to the original states, they emit photons of specific energy creating wavelengths of light that produces colors.3 The test wire and Bunsen Burner were used to excite the solution in the crucible. The standard metal cations that were tested and their outcomes are as shown in Table 1.
In addition, when heat is applied, 36.1% of water is lost from the hydrate. Using theoretical yield with the average atomic masses, I calculated the molar mass of the copper sulfate hydrate (CuSO4 ᐧ 5H2O) to be 249.685 grams, then found the percentage of water lost from the hydrate by dividing 5 water molecules, 90.0764 grams, with the entire hydrate. After doing that, 36.1% is the actual percentage of water that was lost when heat is applied to the hydrate. However, with the experiments, we had lost only 34.5% of water, so it is important to understand how to determine the percent of water in a hydrate that was lost, but also the error percent because knowing the percent error will help me understand what was done wrong, so next time more accurate results would be concluded. For example, because of the 4.4% error, some of the weight may have been lost due to heat circulating in the evaporating dish after applying heat to the hydrate.
The chemical state of the water varies widely between different classes of hydrates, some of which were so labeled before their chemical structure was understood. 2: Specific to your hydrate. What are common uses of your hydrate? Magnesium sulfate heptahydrate, or MgSO4
Equipment: List the equipment you need to conduct the experiment in alphabetical order. Draw a labeled diagram clearly showing what the equipment is and how it is used, preferably large and easy to understand. Procedure: List the steps you follow to conduct the experiment. -Every
The materials used in day two consisted of the Blood Agar Plate (From Previous Period), one bottle of Catalase Reagent (Hydrogen Peroxide), one Sterile Wooden Applicator Stick, The MSA Plate used in Exercise 26 and one Tube of TSB. When beginning with day two you have to examine the blood agar plate and confirm if you have any pure colonies. You then compare your plate with other students in the lab, and then record the color of your colonies. After observing, evaluate your plate with hemolysis and record your results.
Finding the empirical formula for hydrated copper sulfate using calculations to find the amount of each element present in the copper ion, sulfate ion, and water while also comparing the empirical formula to a literature value. Christian Cooper Alexis Powers CHM1210-18M/Gregory Bowers 11-5-15 Purpose: To begin, there are several different goals, techniques, and claims to note in the experiment involving hydrated copper sulfate. The overall goal of this experiment is to find the empirical formula and compare it with a literature value. Yet, in finding the empirical formula of hydrated copper sulfate, there are several process for it to get through, like finding the percentages of copper, water, and finally sulfate.
A hydrate is a compound, where water molecules are chemically bounded to another compound or element. An anhydrate is the substance remaining after removing water from a hydrate. The hydrate in this lab was Copper Sulfate. The hydrates formula is CuSO4 times xH2O. The purpose of this lab was to pull the water from a hydrate to expose the anhydrate and calculate what the hydrate is by finding the formula for the
The overall purpose of this lab was to develop a lab procedure in order to separate and measure the mass of each containment obtained the provided sample. In addition, this experiment was conducted in order to provide the EPA with a plan to remove all contaminants from a heterogenous mixture which purifies the water, making it accessible for the society. Furthermore, the sample consisted of the following contaminants, sand, rock, wood, plastic, salt, water, and an unknown metal. When it came to separating the contaminants, the wood and plastic were taken out through the use of tweezers, while the rocks were separated by decanting the mixture of sand and rocks from the water.
The objective of the lab was to understand the Law of Conservation of Mass. The Law of Conservation of Mass states that matter can be changed from one form into another, mixtures can be separated or made, and pure substances can be decomposed, but the total amount of mass remains constant. For example, from our experiment in the lab, we observed mass of the mixture of aqueous Sodium Sulfide and aqueous Zinc chloride turned white color. After the filtration, and all the water was evaporated, we measured the mass very close to what we had started at the beginning. The error in mass occurred because of the remained residue (solute) in the beaker.
The objective of the lab Mixed Substances, is to see how properties of individual substances compare with properties of mixed substances. This means comparing one item to a pair of items. The cornstarch is a white, fluffy substance with no smell to it. Also the cornstarch is lightweight and soft to tough. The second substance is water.
The first step of the creation of verdigris was preformed using the following reaction (1): 4CuSO4*5H2O(aq) + 6NH3(aq) CuSO4*3Cu(OH)2(s) + 3(NH4)2SO4(aq) + 14H2O(l) Based on this chemical equation, four moles of hydrated copper sulfate reacted with six moles of ammonia to produce a precipitate of copper sulfate tribasic along with aqueous ammonium sulfate and liquid water. It was known that a chemical reaction was occurring when the ammonia was being added via the color change from light blue to dark blue. The precipitate formed from this solution was acquired via vacuum filtration, which involved the solution being separated from the precipitate via air pressure flowing out of the flask. The air pressure flowing out of the flask was caused by a faucet that was running water which was attached to a tube that was attached to the collection flask.
In this experiment, four white powders were tested. After visually inspecting the powders, Powder A appeared to be white, lumpy, and possessed no lust, Powder B appeared to be white, soft, and lumpy, Powder C appeared to look smooth, white, and soft, and Powder D appeared to be lumpy, solid, and whitish-yellow. The materials that were utilized in this lab were cornstarch, baking powder, baking soda, powdered sugar, spot plate, scoopula, dropper, water, vinegar, iodine, toothpicks, and paper towels. The physical property that was observed was solubility, the ability of something to be dissolved, and the chemical property that was observed, reactivity, is the tendency of a substance to undergo chemical change. Knowing both chemical and physical properties of the substances is important because they give more information about the identities of the substances and back up observations
Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4